Ch.4 - Chemical Quantities & Aqueous ReactionsWorksheetSee all chapters
All Chapters
Ch.1 - Intro to General Chemistry
Ch.2 - Atoms & Elements
Ch.3 - Chemical Reactions
BONUS: Lab Techniques and Procedures
BONUS: Mathematical Operations and Functions
Ch.4 - Chemical Quantities & Aqueous Reactions
Ch.5 - Gases
Ch.6 - Thermochemistry
Ch.7 - Quantum Mechanics
Ch.8 - Periodic Properties of the Elements
Ch.9 - Bonding & Molecular Structure
Ch.10 - Molecular Shapes & Valence Bond Theory
Ch.11 - Liquids, Solids & Intermolecular Forces
Ch.12 - Solutions
Ch.13 - Chemical Kinetics
Ch.14 - Chemical Equilibrium
Ch.15 - Acid and Base Equilibrium
Ch.16 - Aqueous Equilibrium
Ch. 17 - Chemical Thermodynamics
Ch.18 - Electrochemistry
Ch.19 - Nuclear Chemistry
Ch.20 - Organic Chemistry
Ch.22 - Chemistry of the Nonmetals
Ch.23 - Transition Metals and Coordination Compounds

Writing Chemical Reactions is based on our understanding of the Solubility Rules

The Chemical Reaction

When writing a chemical reaction our reactants break up into ions and then reassemble to create products. This type of reaction is referred to as a double displacement or metathesis

Writing Chemical Reactions

A balanced molecular equation is an equation showing the neutral forms of compounds. 

All that happens is that soluble ionic compounds separate and become ions in the chemical equation. This represents the total or full ionic equation

Concept #1: Writing Molecular Reactions

Concept #2: Predict whether a reaction occurs, and write the balanced molecular equation, the total and net ionic equations. 

In a balanced molecular equation reactant compounds exist as ions that recombine to form products. 

Concept #3: Total Ionic Equation

In a total ionic equation only the compounds that are aqueous can break up into ions. 

Concept #4: Net Ionic Equation

In a net ionic equation the spectator ions are removed and what remains is the net ionic equation

Remember when asked to write a complete and balanced molecular equation that a reaction only occurs if a solid, liquid or gas is formed as a product. 

Practice: Predict whether a reaction occurs, and write the balanced total and net ionic equations.

Ag2SO4 (aq) + 2 KCl (aq) → 

a) Molecular: Ag2SO4 (aq) + 2 KCl (aq) → K2SO4 (aq) + 2 AgCl (s)

    Total: 2 Ag(aq) + SO42- (aq) + 2 K+ (aq) + 2 Cl- (aq) → K2SO4 (aq) + 2 AgCl (s)

    Net ionic: 2 Ag(aq) + 2 Cl- (aq) → 2 AgCl (s)

b) NO REACTION 

c) Molecular: Ag2SO4 (aq) + 2 KCl (aq) → K2SO4 (aq) + 2 AgCl (s)

    Total: 2 Ag(aq) + SO42- (aq) + 2 K+ (aq) + 2 Cl- (aq) → 2 K(aq) + SO42-(aq) + 2 AgCl (s)

    Net ionic: 2 Ag(aq) + 2 Cl- (aq) → 2 AgCl (s)

d) Molecular: Ag2SO4 (aq) + 2 KCl (aq) → K2SO4 (aq) + 2 AgCl (s)

    Total: 2 Ag(aq) + SO42- (aq) + 2 K+ (aq) + 2 Cl- (aq) → 2 K(aq) + SO42-(aq) + 2 Ag+(aq) + 2 Cl-(aq)

    Net ionic: 2 Ag(aq) + 2 Cl- (aq) → 2 AgCl (s)

If your chemical equation produces only aqueous products then the answer is NO REACTION. 

Practice: Predict whether a reaction occurs, and write the balanced total and net ionic equations.

MgBr(aq) + NaC2H3O(aq) →

a) NO REACTION

b) Molecular: MgBr(aq) + NaC2H3O(aq) → Mg(C2H3O2)2 (aq) + 2 NaBr (s)

    Total: Mg2+(aq) + 2 Br-(aq) + 2 Na+(aq) + C2H3O2-(aq) → Mg2+(aq) + C2H3O2-(aq) + 2 NaBr(s)

    Net ionic: 2 Br-(aq) + 2 Na+(aq) → 2 NaBr (s)

c) Molecular: MgBr(aq) + NaC2H3O(aq) → Mg(C2H3O2)2 (aq) + 2 NaBr (s)

    Total: Mg2+(aq) + 2 Br-(aq) + 2 Na+(aq) + 2 C2H3O2-(aq) → Mg2+(aq) + 2 C2H3O2-(aq) + 2 NaBr (s)

    Net ionic: 2 Br-(aq) + 2 Na+(aq) → 2 NaBr (s)

d) Molecular: MgBr(aq) + NaC2H3O(aq) → Mg(C2H3O2)2 (s) + 2 NaBr (aq)

    Total: Mg2+(aq) + 2 Br-(aq) + 2 Na+(aq) + 2 C2H3O2-(aq) → Mg(C2H3O2)(s) + 2 NaBr (s)

    Net ionic: Mg2+(aq) + 2 C2H3O2-(aq) → Mg(C2H3O2)(s)

Additional Problems
Which are spectator ions in the reaction of aqueous solutions of ammonium perchlorate + sodium bromide A. ammonium and bromide B. sodium and perchlorate C. ammonium and perchlorate D. sodium and bromide E. all are spectator ions
Consider the metathesis reaction between FeF3 and (NH4)2S in water. Write the balanced molecular, total ionic and net ionic equations. Also, identify any spectator ions and include physical states for each equation. Molecular Equation:   Total Ionic Equation:   Net Ionic Equation:   Spectator Ions:
Write balanced molecular and net ionic equations for the following reactions, and identify the gas formed in each.Solid cadmium sulfide reacts with an aqueous solution of sulfuric acid .
Write balanced molecular and net ionic equations for the following reactions, and identify the gas formed in each.Solid magnesium carbonate reacts with an aqueous solution of perchloric acid.
Magnesium carbonate, magnesium oxide, and magnesium hydroxide are all white solids that react with acidic solutions.Write a balanced molecular equation and a net ionic equation for the reaction that occurs when magnesium carbonate reacts with a hydrochloric acid solution.
You choose to investigate some of the solubility guidelines for two ions not listed in the table below, the chromate ion (CrO42 - and the oxalate ion (C2O42-). You are given 0.01 M solutions (A, B, C, D) of four water-soluble salts: Solution Solute Color of Solution A Na2CrO4 Yellow B (NH4)2C2O4 Colorless C AgNO3 Colorless D CaCl2 Colorless When these solutions are mixed, the following observations are made: Experiment Number Solutions Mixed Result 1 A+B No precipitate, yellow solution 2 A+C Red precipitate forms 3 A+D Yellow precipitate forms 4 B+C White precipitate forms 5 B+D White precipitate forms 6 C+D White precipitate forms Write a net ionic equation for the reaction that occurs in each of the experiments. Identify the precipitate formed, if any, in each of the experiments.Write a net ionic equation for the reaction that occurs in the experiment 1.
You choose to investigate some of the solubility guidelines for two ions not listed in the table below, the chromate ion (CrO42 - and the oxalate ion (C2O42-). You are given 0.01 M solutions (A, B, C, D) of four water-soluble salts: Solution Solute Color of Solution A Na2CrO4 Yellow B (NH4)2C2O4 Colorless C AgNO3 Colorless D CaCl2 Colorless When these solutions are mixed, the following observations are made: Experiment Number Solutions Mixed Result 1 A+B No precipitate, yellow solution 2 A+C Red precipitate forms 3 A+D Yellow precipitate forms 4 B+C White precipitate forms 5 B+D White precipitate forms 6 C+D White precipitate forms Write a net ionic equation for the reaction that occurs in each of the experiments. Identify the precipitate formed, if any, in each of the experiments.Identify the precipitate formed, if any, in the experiment 1.
Write balanced molecular and net ionic equations for the following reactions.manganese with dilute sulfuric acid
You choose to investigate some of the solubility guidelines for two ions not listed in the table below, the chromate ion (CrO42 - and the oxalate ion (C2O42-). You are given 0.01 M solutions (A, B, C, D) of four water-soluble salts: Solution Solute Color of Solution A Na2CrO4 Yellow B (NH4)2C2O4 Colorless C AgNO3 Colorless D CaCl2 Colorless When these solutions are mixed, the following observations are made: Experiment Number Solutions Mixed Result 1 A+B No precipitate, yellow solution 2 A+C Red precipitate forms 3 A+D Yellow precipitate forms 4 B+C White precipitate forms 5 B+D White precipitate forms 6 C+D White precipitate forms Write a net ionic equation for the reaction that occurs in each of the experiments. Identify the precipitate formed, if any, in each of the experiments.Identify the precipitate formed, if any, in the experiment 2.
Write balanced molecular and net ionic equations for the following reactions.chromium with hydrobromic acid
You choose to investigate some of the solubility guidelines for two ions not listed in the table below, the chromate ion (CrO42 - and the oxalate ion (C2O42-). You are given 0.01 M solutions (A, B, C, D) of four water-soluble salts: Solution Solute Color of Solution A Na2CrO4 Yellow B (NH4)2C2O4 Colorless C AgNO3 Colorless D CaCl2 Colorless When these solutions are mixed, the following observations are made: Experiment Number Solutions Mixed Result 1 A+B No precipitate, yellow solution 2 A+C Red precipitate forms 3 A+D Yellow precipitate forms 4 B+C White precipitate forms 5 B+D White precipitate forms 6 C+D White precipitate forms Write a net ionic equation for the reaction that occurs in each of the experiments. Identify the precipitate formed, if any, in each of the experiments.Write a net ionic equation for the reaction that occurs in the experiment 3.
Write balanced molecular and net ionic equations for the following reactions.tin with hydrochloric acid
You choose to investigate some of the solubility guidelines for two ions not listed in the table below, the chromate ion (CrO42 - and the oxalate ion (C2O42-). You are given 0.01 M solutions (A, B, C, D) of four water-soluble salts: Solution Solute Color of Solution A Na2CrO4 Yellow B (NH4)2C2O4 Colorless C AgNO3 Colorless D CaCl2 Colorless When these solutions are mixed, the following observations are made: Experiment Number Solutions Mixed Result 1 A+B No precipitate, yellow solution 2 A+C Red precipitate forms 3 A+D Yellow precipitate forms 4 B+C White precipitate forms 5 B+D White precipitate forms 6 C+D White precipitate forms Write a net ionic equation for the reaction that occurs in each of the experiments. Identify the precipitate formed, if any, in each of the experiments.Identify the precipitate formed, if any, in the experiment 3.
Write balanced molecular and net ionic equations for the following reactions.aluminum with formic acid, HCOOH
You choose to investigate some of the solubility guidelines for two ions not listed in the table below, the chromate ion (CrO42 - and the oxalate ion (C2O42-). You are given 0.01 M solutions (A, B, C, D) of four water-soluble salts: Solution Solute Color of Solution A Na2CrO4 Yellow B (NH4)2C2O4 Colorless C AgNO3 Colorless D CaCl2 Colorless When these solutions are mixed, the following observations are made: Experiment Number Solutions Mixed Result 1 A+B No precipitate, yellow solution 2 A+C Red precipitate forms 3 A+D Yellow precipitate forms 4 B+C White precipitate forms 5 B+D White precipitate forms 6 C+D White precipitate forms Write a net ionic equation for the reaction that occurs in each of the experiments. Identify the precipitate formed, if any, in each of the experiments.Write a net ionic equation for the reaction that occurs in the experiment 4.
You choose to investigate some of the solubility guidelines for two ions not listed in the table below, the chromate ion (CrO42 - and the oxalate ion (C2O42-). You are given 0.01 M solutions (A, B, C, D) of four water-soluble salts: Solution Solute Color of Solution A Na2CrO4 Yellow B (NH4)2C2O4 Colorless C AgNO3 Colorless D CaCl2 Colorless When these solutions are mixed, the following observations are made: Experiment Number Solutions Mixed Result 1 A+B No precipitate, yellow solution 2 A+C Red precipitate forms 3 A+D Yellow precipitate forms 4 B+C White precipitate forms 5 B+D White precipitate forms 6 C+D White precipitate forms Write a net ionic equation for the reaction that occurs in each of the experiments. Identify the precipitate formed, if any, in each of the experiments.Identify the precipitate formed, if any, in the experiment 4.
Antacids are often used to relieve pain and promote healing in the treatment of mild ulcers. Write balanced net ionic equations for the reactions between the HCl(aq) in the stomach and each of the following substances used in various antacids.Al(OH)3(s)
You choose to investigate some of the solubility guidelines for two ions not listed in the table below, the chromate ion (CrO42 - and the oxalate ion (C2O42-). You are given 0.01 M solutions (A, B, C, D) of four water-soluble salts: Solution Solute Color of Solution A Na2CrO4 Yellow B (NH4)2C2O4 Colorless C AgNO3 Colorless D CaCl2 Colorless When these solutions are mixed, the following observations are made: Experiment Number Solutions Mixed Result 1 A+B No precipitate, yellow solution 2 A+C Red precipitate forms 3 A+D Yellow precipitate forms 4 B+C White precipitate forms 5 B+D White precipitate forms 6 C+D White precipitate forms Write a net ionic equation for the reaction that occurs in each of the experiments. Identify the precipitate formed, if any, in each of the experiments.Write a net ionic equation for the reaction that occurs in the experiment 5.
Antacids are often used to relieve pain and promote healing in the treatment of mild ulcers. Write balanced net ionic equations for the reactions between the HCl(aq) in the stomach and each of the following substances used in various antacids.MgCO3(s)
You choose to investigate some of the solubility guidelines for two ions not listed in the table below, the chromate ion (CrO42 - and the oxalate ion (C2O42-). You are given 0.01 M solutions (A, B, C, D) of four water-soluble salts: Solution Solute Color of Solution A Na2CrO4 Yellow B (NH4)2C2O4 Colorless C AgNO3 Colorless D CaCl2 Colorless When these solutions are mixed, the following observations are made: Experiment Number Solutions Mixed Result 1 A+B No precipitate, yellow solution 2 A+C Red precipitate forms 3 A+D Yellow precipitate forms 4 B+C White precipitate forms 5 B+D White precipitate forms 6 C+D White precipitate forms Write a net ionic equation for the reaction that occurs in each of the experiments. Identify the precipitate formed, if any, in each of the experiments.Write a net ionic equation for the reaction that occurs in the experiment 6.
Write balanced molecular and net ionic equations for the reactions ofhydrochloric acid with nickel
Antacids are often used to relieve pain and promote healing in the treatment of mild ulcers. Write balanced net ionic equations for the reactions between the HCl(aq) in the stomach and each of the following substances used in various antacids.NaAl(CO3)(OH)2(s)
You choose to investigate some of the solubility guidelines for two ions not listed in the table below, the chromate ion (CrO42 - and the oxalate ion (C2O42-). You are given 0.01 M solutions (A, B, C, D) of four water-soluble salts: Solution Solute Color of Solution A Na2CrO4 Yellow B (NH4)2C2O4 Colorless C AgNO3 Colorless D CaCl2 Colorless When these solutions are mixed, the following observations are made: Experiment Number Solutions Mixed Result 1 A+B No precipitate, yellow solution 2 A+C Red precipitate forms 3 A+D Yellow precipitate forms 4 B+C White precipitate forms 5 B+D White precipitate forms 6 C+D White precipitate forms Write a net ionic equation for the reaction that occurs in each of the experiments. Identify the precipitate formed, if any, in each of the experiments.Identify the precipitate formed, if any, in the experiment 6.
Write balanced molecular and net ionic equations for the reactions ofdilute sulfuric acid with iron (assume iron(II) compound formation)
Antacids are often used to relieve pain and promote healing in the treatment of mild ulcers. Write balanced net ionic equations for the reactions between the HCl(aq) in the stomach and each of the following substances used in various antacids.CaCO3(s)
Write balanced molecular and net ionic equations for the reactions ofhydrobromic acid with magnesium
Write balanced molecular and net ionic equations for the reactions ofacetic acid, CH3COOH, with zinc
Write net ionic equations for the reactions that take place when aqueous solutions of the following substances are mixed.sodium cyanide and nitric acid
Write net ionic equations for the reactions that take place when aqueous solutions of the following substances are mixed.ammonium chloride and sodium hydroxide
Write net ionic equations for the reactions that take place when aqueous solutions of the following substances are mixed.sodium cyanide and ammonium bromide
Write net ionic equations for the reactions that take place when aqueous solutions of the following substances are mixed.potassium hydrogen sulfate and lithium acetate
Write net ionic equations for the reactions that take place when aqueous solutions of the following substances are mixed.sodium hypochlorite and ammonia
A buffer is prepared by adding 21.0 g of sodium acetate (CH3 COONa) to 510 mL of a 0.155 M acetic acid (CH3 COOH) solution.Write the complete ionic equation for the reaction that occurs when a few drops of hydrochloric acid are added to the buffer.
A buffer is prepared by adding 21.0 g of sodium acetate (CH3 COONa) to 510 mL of a 0.155 M acetic acid (CH3 COOH) solution.Write the complete ionic equation for the reaction that occurs when a few drops of sodium hydroxide solution are added to the buffer.
Explain how a molecular equation, a complete ionic equation, and a net ionic equation differ.
Consider two solutions, the first being 50.0 mL of 1.00 M CuSO4 and the second 50.0 mL of 2.00 M KOH. When the two solutions are mixed in a constant-pressure calorimeter, a precipitate forms and the temperature of the mixture rises from 21.5 oC to 27.7 oC.Write net ionic equation for the reaction that occurs when the two solutions are mixed.
Write balanced complete ionic and net ionic equations for each acid–base reaction.Write a balanced complete ionic equation for: HI(aq) + RbOH(aq)
Write balanced complete ionic and net ionic equations for each acid–base reaction.Write a balanced complete ionic equation for: HCHO2(aq) + NaOH(aq)
Write balanced complete ionic and net ionic equations for each acid–base reaction.Write a balanced complete ionic equation for: HC2H3O2(aq) + LiOH(aq)
Write balanced complete ionic and net ionic equations for each acid–base reaction.Write a balanced complete ionic equation for: HBr(aq) + NaOH(aq)
Write balanced complete ionic and net ionic equations for each acid–base reaction.Write a balanced complete ionic equation for: HF(aq) + NaOH(aq)
Write the net ionic equation for the reaction that occurs when a solution of hydrochloric acid (HCl) is mixed with a solution of sodium formate (NaCHO2).
Write balanced complete ionic and net ionic equations for each acid–base reaction.Write a balanced complete ionic equation for: HC2H3O2(aq) + RbOH(aq)
You may want to reference(Pages 126 - 130)Section 4.2 while completing this problem.Identify the spectator ion or ions in this reaction.
You may want to reference(Pages 126 - 130)Section 4.2 while completing this problem.Identify the spectator ion or ions in this reaction.
Enter the net ionic equation, including phases, for the reaction of AgNO3(aq) with K2SO4(aq).
What is the net ionic equation of the reaction of ZnCl 2 with NaOH? Express you answer as a chemical equation including phases.
What is the net ionic equation for the reaction of aqueous sodium hydroxide and aqueous cobalt(II) chloride?a. Na+(aq) + OH–(aq) → NaOH(s)b. Na+(aq) + Cl–(aq) → NaCl(s)c. Co2+(aq) + 2 OH–(aq) → Co(OH)2(s)d. Co2+(aq) + OH–(aq) → CoOH+(s)e. Co2+(aq) + 2 Cl–(aq) → CoCl2(s)  
What is the net ionic equation of the reaction of MgCl  2 with NaOH ? Express your answer as a chemical equation.
What are the spectator ions in the reaction between aqueous hydrobromic acid and aqueous sodium hydroxide?a. Na+ onlyb. H+ and OH–c. Na+ and Br–d. Br– onlye. H+, Br–, Na+, and OH– 
Identify the spectator ions in the following molecular equation.LiCl(aq) + AgNO3(aq)      →       AgCl(s) + LiNO 3(aq)A. Li+ and NO3 -B. Ag+ and Cl-C. Li+ and Cl- D. Ag+ and NO3 - E. no spectator ions 
Write balanced molecular and net ionic equations for the reactions of (a) manganese with dilute sulfuric acid
Write balanced molecular and net ionic equations for the reactions of (b) chromium with hydrobromic acid
Write balanced molecular and net ionic equations for the reactions of (c) tin with hydrochloric acid
Write balanced molecular and net ionic equations for the reactions of (d) aluminum with formic acid, HCOOH.
Write balanced molecular and net ionic equations for the reactions of (a) hydrochloric acid with nickel
Write balanced molecular and net ionic equations for the reactions of (b) dilute sulfuric acid with iron
Write balanced molecular and net ionic equations for the reactions of (c) hydrobromic acid with magnesium
Write balanced molecular and net ionic equations for the reactions of (d) acetic acid, CH3COOH, with zinc.
For the reactions in Exercise 38, write the balanced formula equation, complete ionic equation, and net ionic equation. If no precipitate forms, write “No reaction.”
Write the balanced formula and net ionic equation for the reaction that occurs when the contents of the two beakers are added together. What colors represent the spectator ions in each reaction?
The net ionic equation for the reaction of HCN (aq) and KOH (aq) is _____?a) HCN (aq) + KOH (aq) → H2O (l) + K + (aq) + CN - (aq)b) HCN (aq) + OH - (aq) → H2O (l) +  CN - (aq)c) HCN (aq) + K + (aq) + OH - → H2O (l) +  KCN (aq)d) H+ (aq) + OH - (aq) → H2O (l)e) H + (aq) + CN - (aq) + K + (aq) + OH - → H2O (l) + K + (aq) + CN - (aq) 
Write the balanced formula and net ionic equation for the reaction that occurs when the contents of the two beakers are added together. What colors represent the spectator ions in each reaction?
Magnesium carbonate, magnesium oxide, and magnesium hydroxide are all white solids that react with acidic solutions.Write a balanced molecular equation and a net ionic equation for the reaction that occurs when magnesium hydroxide reacts with a hydrochloric acid solution.
Enter the net ionic equation, including phases, for the reaction of AgNO 3(aq) and KCl(aq).
HBr is a strong electrolyte. HClO is a weak electrolyte. KClO(aq) + HBr(aq) → KBr(aq) + HClO(aq).Write the net ionic equation.
Write the balanced formula and net ionic equation for the reaction that occurs when the contents of the two beakers are added together. What colors represent the spectator ions in each reaction? 
Complete and balance the following neutralization reaction, name the products, and write the net ionic equation. Al(OH)3(s) + 3HCl(aq) → 
Balance the equation:HClO4 (aq) + Mg(OH)2 (s) →a. What is the ionic equation?b. What is the net ionic equation? 
Identify the spectator ions in the following reaction. Na 2CO3(aq) + CaCl2(aq) → 2 NaCl(aq) + CaCO3(s)
Write net ionic equations for the reaction, if any, that occurs when aqueous solutions of the following are mixed.a. chromium(III) chloride and sodium hydroxide
Write net ionic equations for the reaction, if any, that occurs when aqueous solutions of the following are mixed.b. silver nitrate and ammonium carbonate
What is the net ionic equation of the reaction of MgSO 4 with BaCl2? Express your answer as a chemical equation.
Write the complete ionic equation for the reaction (NH 4)2SO4 (aq) + CaS(aq). 
What are the spectator ions when manganese (II) perchlorate mixes with aluminum phosphate?
What is the net ionic equation for the reaction (NH 4)2SO4 (aq) + CaS (aq)a) 2NH4 + (aq) +S -2 (aq) → (NH4)2S(s)b) Ca+2(aq) + SO4 -2 (aq) → CaSO4(s)c) 2NH4 + (aq) + S -2 (aq) + Ca+2(aq) + SO4 -2 (aq) → (NH 4)2S(s) + CaSO4(s)d) There is no net ionic equatione) 2NH4 + (aq) + S -2 (aq) + Ca+2(aq) +SO4 -2 (aq) → (NH 4)2S(aq) + CaSO4(aq) 
Write balanced complete ionic equation for:NH4Cl (aq) + NaOH (aq) → H2O(l) + NH3 (g) + NaCl (aq)Express your answer as a chemical equation. Identify all of the phases in your answer.
Give the net ionic equation for the reaction (if any) that occurs when aqueous solutions of Na2CO3 and HCl are mixed.a) 2 H+(aq) + CO3 2-(aq) H2CO3(s)b) 2 Na+(aq) + CO3 2-(aq) + 2 H+(aq) + 2 Cl-(aq) H2CO3(s) + 2 NaCl(aq)c) 2 H+(aq) + CO3 2-(aq) H2O(l) + CO2(g)d) 2 Na+(aq) + CO3 2-(aq) + 2 H+(aq) + 2 Cl-(aq) H2CO3(s) + 2 Na+(aq) + 2 Cl-(aq)e) No reaction occurs.
Which statement best describes a net ionic equation? a. All substances are shown: as compounds, not ions.b. All substances are shown: as ions if dissolved and compunds if solid.c. All substances EXCEPT spectator ions are shown: as compounds, not ions.d. All substances EXCEPT spectator ions are shown: as ions if dissolved and compunds if solid.e. Only the spectator ions are shown.
__ Ba(OH)2(aq) + __ H2SO4(aq) → __ BaSO4(s) + __ H2O(l)What is the net ionic equation for this reaction ?
Which of the following ions will always be a spectator ion in a precipitation reaction? (a) Cl–, (b) NO3–, (c) NH4+, (d) S2–, (e) SO42–. Explain briefly.
Give the complete ionic equation for the reaction (if any) that occurs when aqueous solutions of lithium sulfide and copper (II) nitrate are mixed.a. Li+(aq) + SO42- (aq) + Cu +(aq) + NO 3- (aq) CuS(s) + Li+(aq) + NO 3- (aq)b. Li+(aq) + S - (aq) + Cu+(aq) + NO 3- (aq) CuS(s) + LiNO 3(aq)c. 2Li+(aq) + S 2- (aq) + Cu 2+(aq) + 2NO 3- (aq) Cu 2+(aq) + S 2- (aq) + 2LiNO 3(s)d. 2Li+(aq) + S 2- (aq) + Cu 2+(aq) + 2NO 3- (aq) CuS(s) + 2Li +(aq) + 2NO 3- (aq)e. No reaction occurs
When 1.0 mol of solid lead nitrate is added to 2.0 mol of aqueous potassium iodide, a yellow precipitate forms. After the precipitate settles to the bottom, does the solution above the precipitate conduct electricity? Explain. Write the complete ionic equation to help you answer this question.
What are the spectator ions in the reaction between aqueous solutions of MgBr 2 and K3PO4?1. Mg2+ and Br –            2. Mg 2+ and PO4 3–3. K+ and PO4 3–            4. K + and Br –
For this question, consider what might happen if a solution of mercury (II) nitrate were to be mixed with a solution of ammonium iodide. You will want to write a balanced equation and a net ionic equation to help you answer the following questions. An ion that is present in the molecular formula but absent in the net ionic equation is said to be a(n): a) participatory ionb) spectator ionc) absent iond) helper ione) none of the above 
You are given a 1.50-g mixture of sodium nitrate and sodium chloride. You dissolve this mixture into 100 mL of water and then add an excess of 0.500 M silver nitrate solution. You produce a white solid, which you then collect, dry, and measure. The white solid has a mass of 0.641 g.b. Write the balanced net ionic equation for the reaction that produces the solid. Include phases and charges.
What is the net ionic equation of the reaction of MgSO 4 with BaCl2?
 What is the net ionic equation of the reaction of MgSO 4 with Pb(NO3)2? Express your answer as a chemical equation including phases.
Write the net ionic equation (including phases) that corresponds to:Fe(ClO4)2(aq) + K2S(aq) → FeS(s) + 2KClO4(aq)
For the reaction: Fe(s) + CuSO4(aq) → FeSO4(aq) + Cu(s)write ionic equation and net ionic equation.
Write the net ionic equation resulting from the mixture of aqueous solutions of silver nitrate (AgNO3) and potassium sulfide (K2S).
Write the balanced formula, complete ionic, and net ionic equations for each of the following acid–base reactions.a. HNO3(aq) + Al(OH3)(s) →
Solutions of calcium hydroxide, Ca(OH)2, and sodium phosphate, Na3PO4, are mixed. Write the balanced complete ionic equation for the reaction.
Write the balanced formula, complete ionic, and net ionic equations for each of the following acid–base reactions.b. HC2H3O2(aq) + KOH(aq) →
Write the balanced formula, complete ionic, and net ionic equations for each of the following acid–base reactions.c. Ca(OH)2(aq) + HCl(aq) →
Give the net ionic equation for the reaction (if any) that occurs when aqueous solutions of H2SO4 and KOH are mixed.a) H+(aq) + OH -(aq) →   H2O(l)b) 2 K+(aq) + SO42-(aq)  →  K2SO4(s)c) H+(aq) + OH -(aq) + 2 K+(aq) + SO 42-(aq)  →   H2O(l) + K2SO4(s)d) H22+(aq) + OH -(aq)  → H2(OH)2 (l)e) No reaction occurs 
Give the net ionic equation for the reaction (if any) that occurs when aqueous solutions of Na2CO3 and HCl are mixed.a) 2 H+(aq) + CO32-(aq) → H2CO3(s)b) 2 Na+(aq) + CO32-(aq) + 2 H+(aq) + 2 Cl -(aq) → H2CO3(s) + 2 NaCl(aq)c) 2 H+(aq) + CO32-(aq) →  H2O(l) + CO2(g)d) 2 Na+(aq) + CO32-(aq) + 2 H+(aq) + 2 Cl -(aq) → H2CO3(s) + 2 Na+(aq) + 2 Cl -(aq) e) No reaction occurs. 
Which ions, if any, are spectator ions in the reaction?AgNO3(aq) + NaCl(aq) → AgCl(s) + NaNO 3(aq) 
Write the balanced formula, complete ionic, and net ionic equations for the reactions that occur when the following are mixed.a. solid silver hydroxide and hydrobromic acid
Write the balanced formula, complete ionic, and net ionic equations for the reactions that occur when the following are mixed.b. aqueous strontium hydroxide and hydroiodic acid
Write balanced complete ionic equation for:NaOH(aq)+HNO3(aq) → H2O(l)+NaNO3(aq)
Write the balanced formula, complete ionic, and net ionic equations for the reactions that occur when the following are mixed.c. solid chromium(III) hydroxide and nitric acid
Write a balanced complete ionic equation and a balanced net ionic equation for the following reaction:Express your answer as a chemical equation. Identify all of the phases in your answer.HCl(aq) + LiOH(aq) → H2O(l) + LiCl(aq)
Name the spectator ions in any reactions that may be involved when each of the following pairs of solutions are mixed. (a) Na2CO3(aq) and MgSO4(aq)
Name the spectator ions in any reactions that may be involved when each of the following pairs of solutions are mixed. (b) Pb(NO3)2(aq) and Na2S(aq)
Name the spectator ions in any reactions that may be involved when each of the following pairs of solutions are mixed. (c) (NH4)3PO4(aq) and CaCl2(aq)
Write balanced net ionic equations for the reactions that occur in each of the following cases. Identify the spectator ion or ions in each reaction. (a) Cr2(SO4)3 (aq) + (NH4)2CO3 (aq) →
Write balanced net ionic equations for the reactions that occur in each of the following cases. Identify the spectator ion or ions in each reaction. (b) Ba(NO3)2 (aq) + K2SO4 (aq) →
Write balanced net ionic equations for the reactions that occur in each of the following cases. Identify the spectator ion or ions in each reaction. (b) Fe(NO3)2 (aq) + KOH (aq) →
Write balanced complete ionic equation and a balanced net ionic equation for the following: Express your answer as a chemical equation. Identify all of the phases in your answer.AgNO3(aq) + NaCl(aq) → AgCl(s) + NaNO 3(aq)
Write the balanced molecular equation (ME) and net ionic equation (NIE) for the following reaction.Be sure to include the correct states in the final equation and charges for ions in the NIE.K2SO4(aq) + CaCl2(aq) →ME: NIE: 
The metal cadmium tends to form Cd 2+ ions. The following observations are made: (i) When a strip of zinc metal is placed in CdCl2(aq), cadmium metal is deposited on the strip. (ii) When a strip of cadmium metal is placed in Ni(NO3)2(aq), nickel metal is deposited on the strip.Write the net ionic equation to explain observation (i).
What is the net ionic equation for: NaOH(aq) + HCl(aq) → NaCl(aq) + H2O(l) 
What are the spectator ions in the following precipitation reaction? (Hint: write the total and net ionic equations first) 2 NaCl(aq) + Pb(NO3)2(aq) → PbCl2(s) + 2 NaNO3(aq) A) Na+,  NO3- B) Pb2+, Cl- C) Na+, Pb2+ D) Pb2+, NO3-
Write the net ionic equation (including phases) that corresponds to:Pb(NO3)2(aq) + K2CO3(aq) → PbCO3(s) + 2KNO3(aq) 
 What is the net ionic equation of the reaction of ZnCl  2 with NaOH? Express your answer as a chemical equation including phases.  
Identify the spectator ion(s) for this reaction occuring in water: Sodium phosphate and calcium chloride are mixed to form sodium chloride and calcium phosphate. 1. Ca2+ and PO43- 2. Na1+, Ca2+, and Cl- 3. Na+ and Cl- 4. Na+ only 5. Cl- only 6. Na+, Cl-, and PO43- 7. Ca2+, Cl-, and PO43-
Identify the spectator ions in the following reaction. AgNO3(aq) + HCl(aq) → HNO3(aq) + AgCl(s) 1. Ag+, Cl− 2. H+, NO3− 3. H+, Cl− 4. Ag+, NO3− 5. There are no spectator ions.
What is the net ionic equation of the reaction of BeCl 2 with NaOH? Express you answer as a chemical equation including phases.
Write the balanced molecular and net ionic equations for each of the following neutralization reactions: (a) Aqueous acetic acid is neutralized by aqueous potassium hydroxide.
Write the balanced molecular and net ionic equations for each of the following neutralization reactions: (b) Solid chromium(Ill) hydroxide reacts with nitric acid.
Write the balanced molecular and net ionic equations for each of the following neutralization reactions: (c) Aqueous hypochlorous acid and aqueous calcium hydroxide react.
Because the oxide ion is basic, metal oxides react readily with acids. (a) Write the net ionic equation for the following reaction: FeO (s) + 2 HClO4 (aq) → Fe(ClO4) (aq) + H2O (l) 
Because the oxide ion is basic, metal oxides react readily with acids.(a) FeO (s) + 2 HClO4 (aq) → Fe(ClO4) (aq) + H2O (l)(b) Based on the equation in part (a), write the net ionic equation for the reaction that occurs between NiO(s) and an aqueous solution of nitric acid.
What is the net ionic equation of the reaction of BeCl 2 with NaOH?
In a reaction between chromium(III) nitrate and sodium phosphate, which of the following are the spectator ions? A. Cr3+, PO43- B. Cr3+, NO3- C. Na+, NO3- D. PO43-, NO3-
As K2O dissolves in water, the oxide ion reacts with water molecules to form hydroxide ions. Write the molecular and net ionic equations for this reaction. Based on the definitions of acid and base, what ion is the base in this reaction? What is the acid? What is the spectator ion in the reaction?
Solid calcium bicarbonate (Ca(HCO3)2) reacts with aqueous hydrochloric acid (HCl) to form aqueous calcium chloride, liquid water, and carbon dioxide gas.Write the balanced molecular equation, complete ionic equation, and net ionic equation for the process. 
Write a balanced molecular equation (ME) and net ionic equation (NIE) for the reactions below. K2CO3(aq) + CaCl2(aq) →ME:NIE:
Define the following reaction between an acid and a base.H+ (aq) + OH - (aq) → H2O (l)a) Molecular equationb) Complete ionic equationc) Net ionic equation 
Complete and balance the equation for gas evolution reactions.(NH4)2SO4(aq) + Ca(OH)2(aq) →
Complete this equation for the reaction of NaHCO 3(s) with HC2H3O2(aq). Include phase symbols. NaHCO3(s)+ HC2H3O2(aq) →
Write balanced molecular equation & net ionic equation for the reaction between nitric acid and calcium hydroxide.
Solid chromium (III) hydroxide reacts with nitrous acid.Express your answer as a balanced net ionic equation. Identify all of the phases in your answer.
The compound chromium(II) nitrate, Cr(NO3)2 is soluble in water. Write the net ionic equation for the dissociation reaction that occurs when solid chromium(II) nitrate dissolves in water.
Write the balanced complete ionic equation forHC2H3O2(aq) + K2CO3(aq) → H2O(l) + CO2(g) + KC2H3O2(aq)Express your answer as a chemical equation. Identify all of the phases in your answer.
Complete and balance the following equations and then write balanced net ionic equations.a. AgNO3(aq)+HCl(aq) ⇌b.NH3(aq)+HCl(aq) ⇌c.Na2CO3(aq)+HNO3(aq) ⇌ 
Write a balanced ionic equation forNa3PO4(aq) + NiCl2(aq) → Ni3(PO4)2(s) + NaCl(aq)
Write balanced molecular equation for the reaction between nitric acid and calcium hydroxide. Express your answer as a chemical equation. Identify all the phases in your answer.
Nutritional biochemists have known for decades that acidic foods cooked in cast-iron cookware can supply significant amounts of dietary iron (ferrous ion).Write a balanced net ionic equation, with oxidation numbers, that supports this fact.
Enter a net ionic equation for the reaction between nitric acid and calcium hydroxide.
Mixtures of CaCl2 and NaCl are used to melt ice on roads. A dissolved 1.9348-g sample of such a mixture was analyzed by using excess Na2C2O4 to precipitate the Ca2+ as CaC2O4. The CaC2O4 was dissolved in sulfuric acid, and the resulting H2C2O4 was titrated with 37.68 mL of 0.1019 M KMnO4 solution.Write the balanced net ionic equation for the precipitation reaction.
Mixtures of CaCl2 and NaCl are used to melt ice on roads. A dissolved 1.9348-g sample of such a mixture was analyzed by using excess Na2C2O4 to precipitate the Ca2+ as CaC2O4. The CaC2O4 was dissolved in sulfuric acid, and the resulting H2C2O4 was titrated with 37.68 mL of 0.1019 M KMnO4 solution.Write the balanced net ionic equation for the titration reaction. (See Sample Problem 4.19.)
The flask represents the products of the titration of 25 mL of sulfuric acid with 25 mL of sodium hydroxide.Write balanced molecular, total ionic, and net ionic equations for the reaction.
Use the following equations to answer the next four questions:i. H2O(s) ⟶ H2O(l)ii. Na+(aq) + Cl−(aq) + Ag+(aq) + NO3−(aq) ⟶ AgCl(s) + Na+(aq) + NO3−(aq)iii. CH3OH(g) + O2(g) ⟶ CO2(g) + H2O(g)iv. 2H2O(l) ⟶ 2H2(g) + O2(g)v. H+(aq) + OH−(aq) ⟶ H2O(l)(d) Which is a net ionic equation?
Complete and balance the following molecular equation.HBr(aq) + Ca(OH)2(aq)  →Write the net ionic equation for it. 
Complete and balance the following molecular equation.Cu(OH)2(s) + HClO4(aq)  →Write the net ionic equation for it. 
Complete and balance the following molecular equation. Al(OH)3(s) + HNO3(aq)  → Write the net ionic equation for it.
A solution contains one or more of the following ions: Ag+, Ca2+, and Cu2+. When sodium chloride is added to the solution, no precipitate forms. When sodium sulfate is added to the solution, a white precipitate forms. The precipitate is filtered off and sodium carbonate is added to the remaining solution, producing a precipitate.Write net ionic equations for the formation of each of the precipitates observed.
A solution contains one or more of the following ions: Hg22+, Ba2+, and Fe2+. When potassium chloride is added to the solution, a precipitate forms. The precipitate is filtered off and potassium sulfate is added to the remaining solution, producing no precipitate. When potassium carbonate is added to the remaining solution, a precipitate forms.Write net ionic equations for the formation of each of the precipitates observed.
Write balanced molecular and net ionic equations for the following reactions, and identify the gas formed in each.(a) solid cadmium sulfide reacts with an aqueous solution of sulfuric acid;
Write balanced molecular and net ionic equations for the following reactions, and identify the gas formed in each.Identify the gas formed in this equation.(b) solid magnesium carbonate reacts with an aqueous solution of perchloric acid.
Write balanced molecular and net ionic equations for each of the following neutralization reactions.Enter the molecular equation representing aqueous acetic acid neutralized by aqueous barium hydroxide.        
You are given a 1.50-g mixture of sodium nitrate and sodium chloride. You dissolve this mixture into 100 mL of water and then add an excess of 0.500 M silver nitrate solution. You produce a white solid, which you then collect, dry, and measure. The white solid has a mass of 0.641 g.Write the balanced net ionic equation for the reaction that produces the solid. Include phases and charges.
Write balanced molecular and net ionic equations for each of the following neutralization reactions.Enter the molecular equation representing solid chromium (III) hydroxide reacting with nitrous acid.        
Write balanced molecular and net ionic equations for each of the following neutralization reactions.Enter the molecular equation representing aqueous nitric acid and aqueous ammonia reacting.
Magnesium carbonate, magnesium oxide, and magnesium hydroxide are all white solids that react with acidic solutions.(A) Write a balanced molecular equation and a net ionic equation for the reaction that occurs when magnesium carbonate reacts with a hydrochloric acid solution.(B) Write a balanced molecular equation and a net ionic equation for the reaction that occurs when magnesium oxide reacts with a hydrochloric acid solution(C) Write a balanced molecular equation and a net ionic equation for the reaction that occurs when magnesium hydroxide reacts with a hydrochloric acid solution.(D) By observing the reactions in parts (A-C), how could you distinguish any of the three magnesium substances from the other two?
Write balanced molecular and net ionic equations for each of the following neutralization reactions.Enter the net ionic equation representing aqueous acetic acid neutralized by aqueous barium hydroxide.        
Write balanced molecular and net ionic equations for each of the following neutralization reactions.Enter the net ionic equation representing solid chromium (III) hydroxide reacting with nitrous acid.    
Write balanced molecular and net ionic equations for each of the following neutralization reactions.Enter the net ionic equation representing aqueous nitric acid and aqueous ammonia reacting.  
Write the balanced formula, complete ionic, and net ionic equations for the following acid–base reaction: HClO4 (aq) + Mg(OH)2 (s) →
Two aqueous solutions contain the ions indicated below.Write balanced molecular, total ionic, and net ionic equations for the reaction that occurs when the solutions are mixed.
Write the balanced formula, complete ionic, and net ionic equations for the following acid–base reaction: HCN (aq) + NaOH (aq) →
Write the balanced formula, complete ionic, and net ionic equations for the following acid–base reaction: HCl (aq) + NaOH (aq) →
Write the balanced formula, complete ionic, and net ionic equations for the following acid–base reaction: HNO3 (aq) + Al(OH)3 (s) →
Write the balanced formula, complete ionic, and net ionic equations for the following acid–base reaction: HC2H3O2 (aq) + KOH (aq) →
Write the balanced formula, complete ionic, and net ionic equations for the following acid–base reaction: Ca(OH)2 (aq) + HCl (aq) →
What is the net ionic equation for the reaction that occurs when aqueous solutions of KOH and ZnCl2 are mixed?
Write balanced molecular and net ionic equations for the reaction:(a) manganese with dilute sulfuric acid,
What is the net ionic equation for the reaction that occurs when aqueous solutions of KOH and HNO3 are mixed?
Write balanced molecular and net ionic equations for the following reactions(b) chromium with hydrobromic acid
What is the net ionic equation for the reaction that occurs when aqueous solutions of KHCO3 and HBr are mixed?
Write balanced molecular and net ionic equations for the following reactions.(c) tin with hydrochloric acid
Write balanced molecular and net ionic equations for the following reactions.(d) aluminum with formic acid, HCOOH
Consider molecular, complete ionic, and net ionic equations.(a) What is the difference between these types of equations?
Consider molecular, complete ionic, and net ionic equations.(b) In what circumstance would the complete and net ionic equations for a reaction be identical?
Write balanced molecular and net ionic equations for the reactions of(a) hydrochloric acid with nickel
Write balanced molecular and net ionic equations for the reactions of(b) dilute sulfuric acid with iron
A reaction cycle for an element is a series of reactions beginning and ending with that element. In the following copper reaction cycle, copper has either a 0 or a +2 oxidation state. Write balanced molecular and net ionic equations for each step.(1) Copper metal reacts with aqueous bromine to produce a greenblue solution.(2) Adding aqueous sodium hydroxide forms a blue precipitate.(3) The precipitate is heated and turns black (water is released).(4) The black solid dissolves in nitric acid to give a blue solution.(5) Adding aqueous sodium phosphate forms a green precipitate.(6) The precipitate forms a blue solution in sulfuric acid.(7) Copper metal is recovered from the blue solution when zinc metal is added
Write balanced molecular and net ionic equations for the reactions of(c) hydrobromic acid with magnesium
Lead ions can be removed from solution by precipitation with sulfate ions. Suppose that a solution contains lead(II) nitrate.Enter the complete ionic equation to show the reaction of aqueous lead(II) nitrate with aqueous potassium sulfate to form solid lead(II) sulfate and aqueous potassium nitrate.
Write balanced molecular and net ionic equations for the reactions of(d) acetic acid, CH3COOH, with zinc
Lead ions can be removed from solution by precipitation with sulfate ions. Suppose that a solution contains lead(II) nitrate.Enter the net ionic equation to show the reaction of aqueous lead(II) nitrate with aqueous potassium sulfate to form solid lead(II) sulfate and aqueous potassium nitrate.
Using the general solubility rules given below, name three reagents that would form precipitates with chloride ion in an aqueous solution. Write the net ionic equation for each of your suggestions.
Using the general solubility rules given below, name three reagents that would form precipitates with calcium ion in an aqueous solution. Write the net ionic equation for each of your suggestions.
Using the general solubility rules given below, name three reagents that would form precipitates with iron(III) ion in an aqueous solution. Write the net ionic equation for each of your suggestions.
Complete the following precipitation reactions with balanced molecular, total ionic, and net ionic equations:Hg2(NO3)2 (aq) + KI (aq) ⟶
Using the general solubility rules given below, name three reagents that would form precipitates with sulfate ion in an aqueous solution. Write the net ionic equation for each of your suggestions.
Complete the following precipitation reactions with balanced molecular, total ionic, and net ionic equations:FeSO4(aq) + Sr(OH)2(aq) ⟶
Using the general solubility rules given below, name three reagents that would form precipitates with mercury(I) ion (Hg22+)in an aqueous solution. Write the net ionic equation for each of your suggestions.
Complete the following precipitation reactions with balanced molecular, total ionic, and net ionic equations:CaCl2(aq) + Cs3PO4(aq) ⟶
Complete the following precipitation reactions with balanced molecular, total ionic, and net ionic equations:Na2S(aq) + ZnSO4(aq) ⟶
Using the general solubility rules given below, name three reagents that would form precipitates with silver ion in an aqueous solution. Write the net ionic equation for each of your suggestions.
A buffer is prepared by adding 11.00 g of ammonium chloride (NH4Cl) to 250 mL of a solution 1.00 M in NH3.Write the complete ionic equation for the reaction that occurs when a few drops of nitric acid are added to the buffer.
A buffer is prepared by adding 11.00 g of ammonium chloride (NH4Cl) to 250 mL of a solution 1.00 M in NH3.Write the complete ionic equation for the reaction that occurs when a few drops of potassium hydroxide solution are added to the buffer.
You may want to reference (Pages 130 - 137)Section 4.3 while completing this problem.Which is the correct net ionic equation for the reaction of aqueous ammonia with nitric acid?(a) NH4+(aq) + H+(aq) → NH52+(aq)(b) NH3(aq) + NO3-(aq) → NH2-(aq) + HNO3(aq)(c) NH2-(aq) + H+(aq) → NH3(aq)(d) NH3(aq) + H+(aq) → NH4+(aq)(e) NH4+(aq) + NO3-(aq) → NH4NO3(aq)
Predict the product(s) and write a balanced equation for each of the following redox reactions:(b) Aluminum + aqueous manganese(II) sulfate ⟶(e) Write a balanced net ionic equation for (b).
Enter a net ionic equation for the reaction that occurs between aqueous HBr and aqueous LiOH.
Predict the product(s) and write a balanced equation for each of the following redox reactions:(d) Aqueous potassium iodide + bromine ⟶(e) Write a balanced net ionic equation for (d).
Enter the net ionic equation for the reaction between HCHO2 (a weak acid) and NaOH.
For each of the following slightly soluble salts, write the net ionic equation, if any, for reaction with acid.MnS
For each of the following slightly soluble salts, write the net ionic equation, if any, for reaction with acid.PbF2
For each of the following slightly soluble salts, write the net ionic equation, if any, for reaction with acid.AuCl3
For each of the following slightly soluble salts, write the net ionic equation, if any, for reaction with acid.Hg2 C2 O4
For each of the following slightly soluble salts, write the net ionic equation, if any, for reaction with acid.CuBr
Mercury(I) ions (Hg22+) can be removed from solution by precipitation with Cl–. Suppose that a solution contains aqueous Hg2(NO3)2.Write complete ionic equation to show the reaction of aqueous Hg2(NO3)2 with aqueous sodium chloride to form solid Hg2Cl2 and aqueous sodium nitrate.
Mercury(I) ions (Hg22+) can be removed from solution by precipitation with Cl–. Suppose that a solution contains aqueous Hg2(NO3)2.Write net ionic equation to show the reaction of aqueous Hg2(NO3)2 with aqueous sodium chloride to form solid Hg2Cl2 and aqueous sodium nitrate.
Enter the net ionic equation for the reaction that occurs when aqueous hydroiodic acid and aqueous calcium sulfide are mixed.
Aqueous hydrogen fluoride (hydrofluoric acid) is used to etch glass and to analyze minerals for their silicon content. Hydrogen fluoride will also react with sand (silicon dioxide).(b) The mineral fluorite (calcium fluoride) occurs extensively in Illinois. Solid calcium fluoride can also be prepared by the reaction of aqueous solutions of calcium chloride and sodium fluoride, yielding aqueous sodium chloride as the other product. Write complete and net ionic equations for this reaction.
With ions shown as spheres and solvent molecules omitted for clarity, the circle illustrates the solid formed when a solution containing K+, Mg2+, Ag+, or Pb2+ (blue) is mixed with one containing ClO4 −, NO3 −, or SO4 2− (yellow).Write a balanced net ionic equation for the reaction.
Consider the following acid-neutralization reactions involving the strong base NaOH(aq):HNO3(aq) + NaOH(aq) → NaNO3(aq) + H2O(l)HCl(aq) + NaOH(aq) → NaCl(aq) + H2O(l)NH4+(aq) + NaOH(aq) → NH3(aq) + Na+(aq) + H2O(l)As we saw in Section 4.3, nitric acid and hydrochloric acid are strong acids. Write net ionic equations for the neutralization of the nitric acid.
Write the molecular, total ionic, and net ionic equations for the following reactions:(a) Ca(OH)2(aq) + HC2H3O2(aq) ⟶
Consider the following acid-neutralization reactions involving the strong base NaOH(aq):HNO3(aq) + NaOH(aq) → NaNO3(aq) + H2O(l)HCl(aq) + NaOH(aq) → NaCl(aq) + H2O(l)NH4+(aq) + NaOH(aq) → NH3(aq) + Na+(aq) + H2O(l)Write net ionic equations for the neutralization of the hydrochloric acid.
Write the molecular, total ionic, and net ionic equations for the following reactions:(b) H3PO4(aq) + CaCl2(aq) ⟶
Consider the following reaction:2HI(aq) + Ba(OH)2(aq) → 2H2O(l) + Ba I2(aq)Enter the complete ionic equation for this reaction.
Enter the net ionic equation for this reaction: 2 HI(aq) + Ba(OH)2(aq) → 2 H2O(l) + BaI2(aq)
The precipitation reaction between 25.0 mL of a solution containing a cation (purple) and 35.0 mL of a solution containing an anion (green) is depicted below (with ions shown as spheres and solvent molecules omitted for clarity).Given the following choices of reactants, write balanced total ionic and net ionic equations that best represent the reaction:KNO3(aq) + CuCl2(aq) ⟶NaClO4(aq) + CaCl2(aq) ⟶Li2SO4(aq) + AgNO3(aq) ⟶NH4Br(aq) + Pb(CH3COO)2(aq) ⟶
The accompanying photo shows the reaction between a solution of Cd(NO3)2 and one of Na2S. Write the net ionic equation for the reaction.
As K2O dissolves in water, the oxide ion reacts with water molecules to form hydroxide ions.Enter the net ionic equation for this reaction.
From the balanced molecular equations, write the complete ionic and net ionic equations for the following:(a) K2C2O4(aq) + Ba(OH)2(aq) ⟶ 2KOH(aq) + BaC2O4(s)
Aluminum sulfate, known as cake alum, has a wide range of uses, from dyeing leather and cloth to purifying sewage. In aqueous solution, it reacts with base to form a white precipitate.Write balanced total and net ionic equations for its reaction with aqueous NaOH.
When the following solutions are mixed together, what precipitate (if any) will form? Write the balanced formula equation, complete ionic equation, and net ionic equation. If no precipitate forms, write “No reaction.”a. FeSO4(aq) + KCl(aq)
When the following solutions are mixed together, what precipitate (if any) will form? Write the balanced formula equation, complete ionic equation, and net ionic equation. If no precipitate forms, write “No reaction.a. Hg2(NO3)2(aq) + CuSO4(aq)
Write the balanced formula and net ionic equation for the reaction that occurs when the contents of the two beakers are added together. What colors represent the spectator ions in the reaction?
From the balanced molecular equations, write the complete ionic and net ionic equations for the following:(b) Pb(NO3)2(aq) + H2SO4(aq) ⟶ PbSO4(s) + 2HNO3(aq)
Write the balanced formula and net ionic equation for the reaction that occurs when the contents of the two beakers are added together. What colors represent the spectator ions in the reaction?
From the balanced molecular equations, write the complete ionic and net ionic equations for the following:(c) CaCO3(s) + H2SO4(aq) ⟶ CaSO4(s) + CO2(g) + H2O(l)
Write balanced complete ionic equation for HCl(aq) + LiOH(aq) → H2O(l) + LiCl(aq)
Write the balanced formula and net ionic equation for the reaction that occurs when the contents of the two beakers are added together. What colors represent the spectator ions in the reaction?
Write balanced complete ionic equation for NaOH(aq) + HC2H3O2(aq) → H2O(l) + NaC2H3O2(aq)
Complete the following acid-base reactions with balanced molecular, total ionic, and net ionic equations:Calcium hydroxide(aq) + acetic acid(aq) ⟶
Write balanced complete ionic equation for Na3PO4(aq) + NiCl2(aq) → Ni3(PO4)2(s) + NaCl(aq)
Write balanced net ionic equation for HCl(aq) + LiOH(aq) → H2O(l) + LiCl(aq)
Write balanced net ionic equation for CaS(aq) + CuCl2(aq) → CuS(s) + CaCl2(aq)
Write balanced net ionic equation for NaOH(aq) + HC2H3O2(aq) → H2O(l) + NaC2H3O2(aq)
Enter the balanced complete ionic equation for K2SO4(aq) + CaI2(aq) → CaSO4 (s) + KI(aq).
Enter the balanced complete ionic equation for NH4Cl(aq) + NaOH(aq) → H2O(l) + NH3(g) + NaCl(aq)
Enter the balanced complete ionic equation for AgNO3(aq) + NaCl(aq) → AgCl(s) + NaNO3(aq)
Enter the balanced complete ionic equation for HCl(aq) + K2CO3(aq) → H2O(l) + CO2(g) + KCl(aq).
When the following solutions are mixed together, what precipitate (if any) will form? Write the balanced formula equation, complete ionic equation, and net ionic equation. If no precipitate forms, write “No reaction.”b. Al(NO3)3(aq) + Ba(OH)2(aq)
Write net ionic equations for the reaction, if any, that occurs when aqueous solutions of the following are mixed: ammonium sulfate and barium nitrate.
Enter the balanced net ionic equation for K2SO4(aq) + CaI2(aq) → CaSO4(s) + KI(aq) .
When the following solutions are mixed together, what precipitate (if any) will form? Write the balanced formula equation, complete ionic equation, and net ionic equation. If no precipitate forms, write “No reaction.”c. CaCl2(aq) + Na2SO4(aq)
Enter the balanced net ionic equation for NH4Cl(aq) + NaOH(aq) → H2O(l) + NH3(g) + NaCl(aq)
Enter the balanced net ionic equation for AgNO3(aq) + NaCl(aq) → AgCl(s) + NaNO3(aq)
Complete the following acid-base reactions with balanced molecular, total ionic, and net ionic equations:Potassium hydroxide (aq) + hydrobromic acid (aq) ⟶
Enter the balanced net ionic equation for HCl(aq) + K2CO3(aq) → H2O(l) + CO2(g) + KCl(aq).
When the following solutions are mixed together, what precipitate (if any) will form? Write the balanced formula equation, complete ionic equation, and net ionic equation. If no precipitate forms, write “No reaction.”d. K2S(aq) + Ni(NO3)2(aq)
Complete the following acid-base reactions with balanced molecular, total ionic, and net ionic equations:Ammonia (aq) + hydrochloric acid (aq) ⟶
Write net ionic equations for the reaction, if any, that occurs when aqueous solutions of the following are mixed: lead(II) nitrate and sodium chloride.
Write balanced net ionic equation for the reaction between hydrobromic acid and potassium hydroxide.
When the following solutions are mixed together, what precipitate (if any) will form? Write the balanced formula equation, complete ionic equation, and net ionic equation. If no precipitate forms, write “No reaction.b. Ni(NO3)2(aq) + CaCl2(aq)
Limestone (calcium carbonate) is insoluble in water but dissolves in aqueous hydrochloric acid. Write balanced total ionic and net ionic equations, showing hydrochloric acid as it actually exists in water and the reaction as a proton-transfer process.
Write net ionic equations for the reaction, if any, that occurs when aqueous solutions of the following are mixed: sodium phosphate and potassium nitrate.
When the following solutions are mixed together, what precipitate (if any) will form? Write the balanced formula equation, complete ionic equation, and net ionic equation. If no precipitate forms, write “No reaction.c. K2CO3(aq) + MgI2(aq)
Zinc hydroxide is insoluble in water but dissolves in aqueous nitric acid. Why? Write balanced total ionic and net ionic equations, showing nitric acid as it actually exists in water and the reaction as a proton-transfer process.
Write net ionic equations for the reaction, if any, that occurs when aqueous solutions of the following are mixed: sodium bromide and rubidium chloride.
When the following solutions are mixed together, what precipitate (if any) will form? Write the balanced formula equation, complete ionic equation, and net ionic equation. If no precipitate forms, write “No reaction.d. Na2CrO4(aq) + AlBr3(aq)
Write net ionic equations for the reaction, if any, that occurs when aqueous solutions of the following are mixed: copper(II) chloride and sodium hydroxide.
Write net ionic equations for the reaction, if any, that occurs when aqueous solutions of the following are mixed: chromium(III) chloride and sodium hydroxide.
Write net ionic equations for the reaction, if any, that occurs when aqueous solutions of the following are mixed: silver nitrate and ammonium carbonate.
Write net ionic equations for the reaction, if any, that occurs when aqueous solutions of the following are mixed: copper(II) sulfate and mercury(I) nitrate.
Write net ionic equations for the reaction, if any, that occurs when aqueous solutions of the following are mixed: strontium nitrate and potassium iodide.
Write balanced net ionic equations for the reactions that occur in each of the following cases. Identify the spectator ion or ions in each reaction.You may want to reference(Pages 126 - 130)Section 4.2 while completing this problem.(a) Cr2(SO4)3(aq) + (NH4)2CO3(aq) →
The drawings below represent aqueous solutions. Solution A is 2.00 L of a 2.00-M aqueous solution of copper(II) nitrate. Solution B is 2.00 L of a 3.00-M aqueous solution of potassium hydroxide.Draw a picture of the solution made by mixing solutions A and B together after the precipitation reaction takes place. Make sure this picture shows the correct relative volume compared to solutions A and B, and the correct relative number of ions, along with the correct relative amount of solid formed.
You are given a 1.50-g mixture of sodium nitrate and sodium chloride. You dissolve this mixture into 100 mL of water and then add an excess of 0.500 M silver nitrate solution. You produce a white solid, which you then collect, dry, and measure. The white solid has a mass of 0.641 g.If you had an extremely magnified view of the solution (to the atomic-molecular level), list the species you would see (include charges, if any).
As K2O dissolves in water, the oxide ion reacts with water molecules to form hydroxide ions.Based on the definitions of acid and base, identify the acid and base in this reaction. Then identify the spectator ion.
4.26You may want to reference(Pages 126 - 130)Section 4.2 while completing this problem.Identify the spectator ion or ions in this reaction.(b) Ba(NO3)2(aq) + K2SO4(aq) → 
4.26You may want to reference(Pages 126 - 130)Section 4.2 while completing this problem.Identify the spectator ion or ions in this reaction.(c) Fe(NO3)2(aq) + KOH(aq) → 
4.26Write balanced net ionic equations for the reactions that occur in each of the following cases. Identify the spectator ion or ions in each reaction.You may want to reference(Pages 126 - 130)Section 4.2 while completing this problem.(b) Ba(NO3)2(aq) + K2SO4(aq) →
4.26Write balanced net ionic equations for the reactions that occur in each of the following cases. Identify the spectator ion or ions in each reaction.You may want to reference(Pages 126 - 130)Section 4.2 while completing this problem.(c) Fe(NO3)2(aq) + KOH(aq) →
Write a balanced chemical equation for the reaction:Na2CO3 + AgNO3 →Include their ionic equations. 
Write a balanced and complete ionic equation.NaOH(aq) + HNO3(aq) → H2O(l) + NaNO3(aq)
Write a balanced chemical equations for the following reactions:Na2CO3 and AgNO3FeSO4 and Pb(NO3)2
Complete and balance each of the following equations for gas-evolution reactions. Identify all of the phases in your answer. Express your answer as a chemical equation. Identify all of the phases in your answer. a. HBr(aq)+NiS(s)→ b. NH4I(aq)+NaOH(aq)→ c. HNO3(aq)+Li2S(aq)→ d. HNO3(aq)+K2CO3(aq)→  
You choose to investigate some of the solubility guidelines for two ions not listed in the table below, the chromate ion (CrO42 -  and the oxalate ion (C2O42-).You are given 0.01 M solutions (A, B, C, D) of four water-soluble salts:SolutionSoluteColor of SolutionANa2CrO4YellowB(NH4)2C2O4ColorlessCAgNO3ColorlessDCaCl2ColorlessWhen these solutions are mixed, the following observations are made:Experiment NumberSolutions MixedResult1A+BNo precipitate, yellow solution2A+CRed precipitate forms3A+DYellow precipitate forms4B+CWhite precipitate forms5B+DWhite precipitate forms6C+DWhite precipitate formsWrite a net ionic equation for the reaction that occurs in each of the experiments. Identify the precipitate formed, if any, in each of the experiments.Write a net ionic equation for the reaction that occurs in the experiment 2.
Complete the following acid-base reactions with balanced molecular, total ionic, and net ionic equations:Cesium hydroxide(aq) + nitric acid(aq) ⟶
Write balanced net ionic equation for Na 3PO4(aq) + NiCl2(aq) → Ni3(PO4)2(s) + NaCl(aq)
You choose to investigate some of the solubility guidelines for two ions not listed in the table below, the chromate ion (CrO42 -  and the oxalate ion (C2O42-).You are given 0.01 M solutions (A, B, C, D) of four water-soluble salts:SolutionSoluteColor of SolutionANa2CrO4YellowB(NH4)2C2O4ColorlessCAgNO3ColorlessDCaCl2ColorlessWhen these solutions are mixed, the following observations are made:Experiment NumberSolutions MixedResult1A+BNo precipitate, yellow solution2A+CRed precipitate forms3A+DYellow precipitate forms4B+CWhite precipitate forms5B+DWhite precipitate forms6C+DWhite precipitate formsWrite a net ionic equation for the reaction that occurs in each of the experiments. Identify the precipitate formed, if any, in each of the experiments.Identify the precipitate formed, if any, in the experiment 5.
For the reactionHBr(aq) + NH3(aq) → ?a. Balance the equation.b. What is the ionic equation?
Be sure to answer all parts.Write ionic and net ionic equations for the following reactions. Be sure to include the states for each species. (a) Na2S (aq) + ZaCl2 (aq) → Total ionic: Net ionic: (b) Mg(NO3)2 (aq) + 2 NaOH (aq) → Total ionic:Net ionic:
2K3PO4 (aq) + 3MgCl2 (aq) → Mg 3(PO4)2 (s) + 6KCl (aq) The molecular equation you determined in Part B is shown above for your convenience. Examine each of the chemical species involved to determine ions that would be present in solution. Be sure to consider both the coefficients and subscripts of the molecular equation, and then write this precipitation reaction in the form of a balanced complete ionic equation. Express your answer as a chemical equation including phases. 
Write the net ionic equation when acetic acid reacts with calcium hydroxide.
The following chemical reaction takes place in aqueous solution: Fe(NO3)2 (aq) + K2S(aq) → FeS(s) + 2KNO3(aq) Write the net ionic equation for this reaction.
Complete and balance the following neutralization reaction, name the products, and write the net ionic equation. Complete and balance the reaction. HBr(aq) + KOH(aq) → Name the products. Write the net ionic equation. H+ + OH- → H2O-(l)
Complete and balance the reaction. Name the products. Is CH3COOH a strong acid or a weak acid? How should it be handled in a net ionic equation? Is Sr(OH)2 a strong base or a weak base? How should it be handled in a net ionic equation? Write the net ionic equation.
The following molecular equation represents the reaction that occurs when aqueous solutions of lead(lI) nitrate and sodium bromide are combined.Pb(NO3)2 (aq) + 2NaBr (aq) → PbBr3 (s) + 2NaNO3 (aq)Write the balanced net ionic equation for the reaction.(Use the lowest possible coefficents. Use the pull-down boxes to specify states such as (aq) or (l). If a box is not needed, leave it blank.) 
One way to determine the concentration of hypochlorite ions (CIO-) in solution is by first reacting them with I- ions. Under acidic conditions the products of this reaction are I_2 and Cl^- ions. Then the l2 produced in the first reaction is titrated with a solution of thiosulfate ions (S2O32-). The products of the titration reaction are S4O62- and I- ions. Write net ionic equations for these two reactions. Write the first one in the upper box. Do not include phases.
What are the spectator ions in the following reaction?2 HCl(aq) + CaCO3(s) → CaCl2(aq) + CO2(g) + H2O(l)
Consider this aqueous reaction. What is the formula for the salt that forms?
Write the net ionic equation (including phases) that corresponds to Cu(NO3)(aq) + Na2CO3(s) + 2NaNO3(aq) 
Write the balanced molecular equation for the neutralization reaction between H2SO4 and KOH in aqueous solution. Phase are optional. 
Identify the spectator ions in the following complete ionic equation. Ba2+ (aq) + 2 I - (aq) + 2 Na+ (aq) + SO42- (aq) → BaSO4 (s) + 2 I - (aq) + 2 Na+ (aq) Express your answers as ions separated by a comma. Do not enter the coefficient.
For the following chemical reaction:  2HBr(aq) + Ba(OH) 2(aq) → 2H2O(l) + BaBr2(aq),  write the net ionic equation, including the phases.
The compound chromium(II) nitrate, Cr(NO3)2 is soluble in water. Write the net ionic equation for the dissociation reaction that occurs when solid chromium(II) nitrate dissolves in water: Use the pull-down boxes to specify states such as (aq) or (s). 
Write net ionic equations for the following reactions Part AMg(s) + CuCl2(aq) → MgCl2(aq) + Cu(s) Express your answer as a chemical equation. Identify all of the phases in your answer. Part B 2KCl(aq) + Pb(NO3)2(aq) → PCl2(s) + 2KNO3(aq) Express your answer as a chemical equation. Identify all of the phases in your answer. Part C 2Cr(NO3)3(aq) + 3Na2S(aq) → Cr2S3(s) + 6NaNO3(aq) Express your answer as a chemical equation. Identify all of the phases in your answer.
What is the net ionic equation of the reaction of MgSO 4 with Ba(NO3)2?
Write a balanced equation for the double-replacement precipitation reaction described, using the smallest possible integer coefficients. A precipitate forms when aqueous solutions of silver (I) nitrate and nickel (II) sulfate are combined. Do not include states such as (s) or (aq). It is not necessary for you to indicate which of the products is the precipitate.
Aluminum carbonate is used in some antacids. Write a balanced net ionic equation for the reaction of aluminum carbonate with hydrochloric acid.
Write a balanced equation for the double-replacement precipitation reaction described, using the smallest possible integer coefficients. A precipitate forms when aqueous solutions of calcium chloride and cobalt(II) sulfate are combined. Do not include states such as (s) or (aq). It is not necessary for you to indicate which of the products is the precipitate.
Write balanced complete ionic equation for CaS(aq) + CuCl2(aq) → CuS(s) + CaCl2(aq)
For the following chemical reaction write the net ionic equation, including the phases. 
 For the following chemical reaction 2HBr(aq) + Ba(OH)2(aq) → 2H2O(l) + BaBr2(aq) write the net ionic equation, including the phases.
For the following chemical reaction HCN(aq) + KOH(aq) → H2O(l) + KCN(aq) write the net ionic equation, including the phases.
Write the net ionic equation (including phases) that corresponds to Zn(NO3)2(aq) + K2S(aq) → ZnS(s) + 2KNO3(aq).
Write a balanced equation for the double-replacement precipitation reaction described, using the smallest possible integer coefficients. A precipitate forms when aqueous solutions of iron(III) nitrate and sodium carbonate are combined. Do not include states such as (s) or (aq). It is not necessary for you to indicate which of the products is the precipitate.
Antacids are often used to relieve pain and promote healing in the treatment of mild ulcers. Write balanced net ionic equations for the reactions between the HCl(aq) in the stomach and each of the following substances used in various antacids.Mg(OH)2(s)
Enter the net ionic equation, including phases, for the reaction of AgNO3(aq) with K2SO4(aq). Solubility Rules are found here.
Complete and balance the molecular equation, including phases, for the reaction of aqueous ammonium bromide, NH4Br, and aqueous lead(II) acetate, Pb(C2H3O2)2. NH4Br(aq) + Pb(C2H3O2)2(aq) → Enter the balanced net ionic equation, including phases, for this reaction. 
Select the spectator ions for the following reaction, Pb(NO3)2 + 2 KCI → PbCI2 + 2KNO3 a. K+(aq), NO3- (aq) b. Pb2+(aq), CI- (aq) c. K+(aq), CI- (aq) d. Pb2+(aq), CI- (aq), K+ (aq), NO3- (aq) e. Pb2+(aq).CI- (aq)
Tartaric acid, H2C4H4O6, has two acidic hydrogens. The acid is often present in wines and precipitates from solution as the wine ages. A solution containing an unknown concentration of the acid is titrated with NaOH. It requires 23.65 mL of 0.3000 M NaOH solution to titrate both acidic protons in 55.00 mL of the tartaric acid solution.Write a balanced net ionic equation for the neutralization reaction.
Consider two solutions, the first being 50.0 mL of 1.00 M CuSO4 and the second 50.0 mL of 2.00 M KOH. When the two solutions are mixed in a constant-pressure calorimeter, a precipitate forms and the temperature of the mixture rises from 21.5 oC to 27.7 oC.Write the complete equation for the reaction that occurs when the two solutions are mixed.
Enter the net ionic equation, including phases, for the reaction of AgNO3(aq) and KCl(aq).
What is the net ionic equation of the reaction of MgCl2 with NaOH? Express your answer as a chemical equation. 
For the following chemical reaction write the net ionic equation, including the phases.HCN(aq) + KOH(aq) → H2O(I) + KCN(aq)
For the following chemical reactionHClO2(aq) + NaOH(aq) → H2O (l) + NaClO2(aq)write the net ionic equation, including phases.
Magnesium carbonate, magnesium oxide, and magnesium hydroxide are all white solids that react with acidic solutions.Write a balanced molecular equation and a net ionic equation for the reaction that occurs when magnesium oxide reacts with a hydrochloric acid solution.