Ch.4 - Chemical Quantities & Aqueous ReactionsSee 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

Whether you use the term molarity, concentration or solubility they all represent the maximum amount of solute that can successfully be dissolved in a solvent. 

Understanding the Solubility Rules

Concept #1: The Rules for the Solubility of a compound

Certain positive ions combine with negative ions to form either a liquid, aqueous, solid or gaseous compound. The Solubility Rules help us determine which form is created. 

Concept #2: The meaning of the terms soluble and aqueous

Saying a compound is soluble means that the compound will dissolve into aqueous ions in a solvent. These ions can conduct electricity and are called electrolytes

Concept #3: The meaning of the terms insoluble and precipitate

Saying a compound is insoluble means that the compound will not dissolve into aqueous ions and forms a solid called a precipitate, which will not conduct electricity. 

Additional Problems
In each of the following instances two solutions are mixed together. Which reaction will lead to the formation of a precipitate? a) potassium carbonate solution + calcium hydroxide solution b) hydrochloric acid solution + strontium hydroxide solution c) calcium nitrate solution + lithium chloride solution d) ammonium chloride solution + copper (II) acetate solution e) None of the above reactions will lead to formation of a precipitate
If you take an ionic compound, dissolve it into water, and then carry out the following steps: I. Add 50 mL of 2.0 M Ca(NO 3)2 solution. This produces a white precipitate. II. Next add 50 mL of 2.0 M HCl solution. This causes the precipitate to dissolve and produces a lot of bubbles, but no apparent odor Which of the following anions (from the original ionic compound) would be consistent with these results. a) OH - b) SO4 2- c) S 2- d) CO3 2- e) PO4 3-
Separate samples of a solution of an unknown salt are treated with dilute solutions of HBr, H2SO4, and NaOH. A precipitate forms in all three cases. Which of the following cations could the solution contain:   a) Pb2+ b) Ba2+ c) Na+
Which of the following reagents could be used to separate the two cations from a solution containing Cobalt (I) nitrate and sodium hydroxide?   a) Ca(C2H3O2)2 b) Sc(NO3)3 c) BaCO3 d) LiClO4 e) NaNO3
Which one of the following reactions does not produce a precipitate? a) 2LiI (aq) + BaS (aq) → b) Pb(NO3)2 (aq) + 2NaCl (aq) → c) Li2CO3 (aq) + CaS (aq) → d) NH4Br (aq) + AgNO3 (aq) →
Equal volumes of 1.00M of NaCl and 1.00M Pb(NO 3)2 are mixed. Which statement below best describes what happens?   a. All the Pb(NO3)2 precipitates and excess NaCl remains. b. All the chloride ions in the NaCl are precipitates as PbCl 2. c. No nitrate ions remain in solution. d. No sodium ions remain in solution. e. No Pb2+ ions remain in solution.
The following aqueous solutions are mixed: 1.00M NaCl(aq) and 1.00M KNO 3(aq). Which statement is true?   a. No reaction occurs since all possible species are soluble in water. b. No reaction occures since NaCl and KNO 3 are both insoluble to begin with. c. NaNO3 precipitates from the solution d. KCl precipitates from the solution e. None of the above statements is true. 
Which of the following reagents could be used to separate the two anions from a solution containing magnesium nitrate and cesium hydroxide? a)    NH4CN b)    NaCl c)    KNO3 d)    ZnBr2 e)    CsBrO3
Which of the following reagents could be used to separate the two cations from a solution containing Lead (IV) acetate and cesium permanganate? a)    Sr(NO3)2 b)    TiC2H3O2 c)    K2S d)    NaClO4 e)    KNO3
Which is the most satisfactory solvent for alumina, Al 2O3, in the electrolytic process for the preparation of aluminum? a) liquid water, H2O b) molten cryolite, Na 3AlF6 c) molten bauxite, Al2O3 with other oxides d) molten sodium chloride, NaCl
What is the identity of the insoluble solid that is formed when sodium carbonate reacts with aqueous hydrochloric acid? a) no solid form is formed b) NaCl c) NaO d) NaOH e) H2CO3
Predict the identity of the precipitate that forms when aqueous solutions of BaCl 2 and K2SO4 are mixed. a) barium chloride (BaCl2) b) potassium chloride (KCl) c) barium sulfate (BaSO4) d) potassium sulfate (K2SO4) e) no precipitate is formed
Some Pb(NO3)2 (aq) and KI (aq) are combined and a yellow precipitate forms. Which of the following has the highest concentration in the supernatant?   a) K+ (aq) b) NO3 - (aq) c) Pb2+ (aq) d) I- (aq) e) It depends on what was the limiting reactant
Which ion may form a scummy precipitate with ordinary soap? a) HCO3- b) CO32- c) Na+ d) Ca2+
The SOLUBILITY of a compound represents the maximum amount of solute that dissolves in a solvent.  
You may want to reference (Pages 126 - 130) Section 4.2 while completing this problem.Enter a balanced equation for the reaction of KOH and Cu(NO3)2.
You may want to reference (Pages 126 - 130) Section 4.2 while completing this problem.Enter a balanced equation for the reaction of Na2S and CdSO4.
Does a reaction occur when an aqueous solution of NiCl2(aq) is added to a test tube containing strips of metallic zinc?
Does a reaction occur when NiCl2(aq) is added to a test tube containing Zn(NO3)2(aq)?
A solution of 116 mL of 0.180 M KOH is mixed with a solution of 260 mL of 0.210 M NiSO4.Write the balanced chemical equation for the reaction that occurs.
The accompanying photo shows the reaction between a solution of Cd(NO3)2 and one of Na2S. You may want to reference (Pages 138 - 144) Section 4.4 while completing this problem.What ions remain in solution?
Which ions remain in solution, unreacted, after each of the following pairs of solutions is mixed?potassium carbonate and magnesium sulfate
Which ions remain in solution, unreacted, after each of the following pairs of solutions is mixed?lead nitrate and lithium sulfide
Which ions remain in solution, unreacted, after each of the following pairs of solutions is mixed?ammonium phosphate and calcium chloride
As K2O dissolves in water, the oxide ion reacts with water molecules to form hydroxide ions. You may want to reference (Pages 131 - 137) Section 4.3 while completing this problem.Enter the molecular equation for this reaction.
You may want to reference (Pages 168 - 174) Section 4.8 while completing this problem.Write balanced molecular equation for the reaction between nitric acid and calcium hydroxide.
A hydrochloric acid solution will neutralize a sodium hydroxide solution. Look at the following molecular views showing one beaker of HCl and four beakers of NaOH. Which NaOH beaker will just neutralize the HCl beaker? Begin by writing a balanced chemical equation for the neutralization reaction.
You may want to reference (Pages 126 - 130) Section 4.2 while completing this problem.Enter a balanced equation for the reaction of NaCH3COO (also written as NaC2H3O2) and HCl.
A sample of 5.55 g of Mg(OH)2 is added to 25.2 mL of 0.180 M HNO3.Write the chemical equation for the reaction that occurs.
What is an acid-base reaction?
You may want to reference (Pages 168 - 174) Section 4.8 while completing this problem.Enter a molecular equation for the reaction that occurs between aqueous HBr and aqueous LiOH.
Will precipitation occur when the following solutions are mixed?Na2CO3 and AgNO3
Will precipitation occur when the following solutions are mixed?NaNO3 and NiSO4
Will precipitation occur when the following solutions are mixed?FeSO4 and Pb(NO3)2
Will precipitation occur when the following solutions are mixed?Write a balanced chemical equation for the reaction. Na2CO3 and AgNO3
Will precipitation occur when the following solutions are mixed?Write a balanced chemical equation for the reaction. FeSO4 and Pb(NO3)2
You may want to reference (Pages 126 - 130) Section 4.2 while completing this problem.Identify the precipitate (if any) that forms when NaCH3COO (also written as NaC2H3O2) and HCl are mixed.        
You may want to reference (Pages 126 - 130) Section 4.2 while completing this problem.Identify the precipitate (if any) that forms when KOH and Cu(NO3)2 are mixed.        
A precipitation reaction.Which ions remain in solution after PbI2 precipitation is complete?
You may want to reference (Pages 126 - 130) Section 4.2 while completing this problem.Identify the precipitate (if any) that forms when Na2S and CdSO4 are mixed.    
You are presented with a white solid and told that due to careless labeling it is not clear if the substance is barium chloride, lead chloride, or zinc chloride. When you transfer the solid to a beaker and add water, the solid dissolves to give a clear solution. Next a Na2SO4(aq) solution is added and a white precipitate forms. What is the identity of the unknown white solid?
You know that an unlabeled bottle contains an aqueous solution of one of the following: AgNO3, CaCl2, or Al2(SO4)3. A friend suggests that you test a portion of the solution with Ba(NO3)2 and then with NaCl solutions.According to your friend’s logic, which of these chemical reactions could occur, thus helping you identify the solution in the bottle?
What is a precipitation reaction?
How can you predict whether a precipitation reaction will occur upon mixing two aqueous solutions?
You may want to reference (Pages 163 - 166) Section 4.6 while completing this problem.Enter an equation for the precipitation reaction that occurs (if any) when solutions of ammonium chloride and iron(III) nitrate are mixed.
You may want to reference (Pages 163 - 166) Section 4.6 while completing this problem.Enter an equation for the precipitation reaction that occurs (if any) when solutions of sodium hydroxide and copper(II) bromide are mixed.
A solution of 116 mL of 0.180 M KOH is mixed with a solution of 260 mL of 0.210 M NiSO4.What precipitate forms?
Separate samples of a solution of an unknown salt are treated with dilute solutions of HBr, H2SO4, and NaOH. A precipitate forms in all three cases.Which of the following cations could be present in the unknown salt solution: K+, Pb2+, Ba2+?
Consider the generic ionic compounds with the formulas A2X and BY2 and the following solubility rules: A2X soluble; BY2 soluble; AY insoluble; BX soluble. Assume A+ ions are circles, B2+ ions are squares, X2- ions are trianges, and Y- ions are diamonds. Solutions of the two compounds (A2X and BY2) can be represented as follows: Draw a molecular level representation showing the result of mixing the two solutions given.
Consider the generic ionic compounds with the formulas A2X and BY2 and the following solubility rules: A2X soluble; BY2 soluble; AY insoluble; BX soluble. Assume A+ ions are circles, B2+ ions are squares, X2- ions are trianges, and Y- ions are diamonds. Solutions of the two compounds (A2X and BY2) can be represented as follows: Write an equation to represent the reaction.
Three solutions are mixed together to form a single solution; in the final solution, there are 0.2 mol Pb(CH3COO)2, 0.1 mol Na2S, and 0.1 mol CaCl2 present.What solid(s) will precipitate?
The accompanying photo shows the reaction between a solution of Cd(NO3)2 and one of Na2S. You may want to reference (Pages 138 - 144) Section 4.4 while completing this problem.What is the identity of the precipitate?
By analogy to examples given in the text, predict what gas forms when Na2SO3(s) reacts with HCl(aq).
What is a gas-evolution reaction?
What reactant types give rise to gas-evolution reactions?
You may want to reference (Pages 168 - 174) Section 4.8 while completing this problem.Enter a molecular equation for the gas-evolution reaction that occurs when aqueous hydrobromic acid and aqueous potassium sulfite are mixed.
Which of the following is a precipitation reaction?a) Zn (s) + 2 AgNO3 (aq)      →       2 Ag (s) + Zn(NO 3) 2 (aq)b) 2 LiI (aq) + Hg 2(NO3)2 (aq)      →       Hg 2I2 (s) + 2 LiNO3 (aq)c) HCl (aq) + KOH (aq)      →       KCl (aq) + H  2O (l)d) NaCl (aq) + LiI (aq)      →       NaI (aq) + LiCl (aq)e) None of the above. 
Write a molecular equation for the precipitation reaction that occurs (if any) when the following solutions are mixed. If no reaction occurs, write NO REACTION.copper(II) bromide and lead (II) acetate
Write a molecular equation for the precipitation reaction that occurs (if any) when the following solutions are mixed. If no reaction occurs, write NO REACTION.Express your answers as a chemical equation. Identify all of the phases in your answer.a. sodium chloride and lead (II) acetateb. potassium sulfate and strontium iodidec. chromium (III) nitrate and sodium phosphate 
When the following solutions are mixed together, what precipitate (if any) will form?a. FeSO4(aq) + KCl(aq)
Write a balanced chemical equation for the reaction of aqueous solutions of magnesium chloride and potassium phosphate.a. MgCl2(aq) + K3PO4(aq) → K3Mg(s) + PO4Cl2(aq)b. 3 MgCl2(aq) + 2 K3PO4(aq) → 3 K2Mg(s) + 2 PO4Cl3(aq)c. MgCl(aq) + KPO4(aq) → MgPO4(s) + KCl(aq)d. MgCl2(aq) + 2 KPO4(aq) → Mg(PO4)2(s) + 2 KCl(aq)e. 3 MgCl2(aq) + 2 K3PO4(aq) → Mg3(PO4)2(s) + 6 KCl(aq)  
What gas is produced if (NH4)2SO4 is reacted with Ca(OH)2?A. SO2B. H2C. O2D. NH3E. H2S
When the following solutions are mixed together, what precipitate (if any) will form?b. Al(NO3)3(aq) + Ba(OH)2(aq)
When the following solutions are mixed together, what precipitate (if any) will form?c. CaCl2(aq) + Na2SO4(aq)
When the following solutions are mixed together, what precipitate (if any) will form?d. K2S(aq) + Ni(NO3)2(aq)
When the following solutions are mixed together, what precipitate (if any) will form?a. Hg2(NO3)2(aq) + CuSO4(aq)
When the following solutions are mixed together, what precipitate (if any) will form?b. Ni(NO3)2(aq) + CaCl2(aq)
When the following solutions are mixed together, what precipitate (if any) will form?c. K2CO3(aq) + MgI2(aq)
When the following solutions are mixed together, what precipitate (if any) will form?d. Na2CrO4(aq) + AlBr3(aq)
Predict the precipitate in the reaction between sodium phosphate and calcium chloride.A. Ca(PO4)2B. Ca3(PO4)2C. NaClD. Na2Cl
What product(s) form in the following neutralization reaction?H2SO4(aq) + Ba(OH)2(aq) →
The mixing of which pair of reactants will result in a precipitation reaction?a. Na2SO4(aq) + KNO3(aq)b. NH4Br(aq) + Kl(aq)c. LiClO4(aq) + (NH4)2S(aq)d. Cu(NO3)2(aq) + Li3PO4(aq)
Suppose that aqueous solutions of barium nitrate and potassium carbonate are mixed. What is the name of the compound or compounds that precipitate?
Consider separate aqueous solutions of HCl and H 2SO4 with the same molar concentrations. You wish to neutralize an aqueous solution of NaOH. For which acid solution would you need to add more volume (in milliliters) to neutralize the base?a. the HCl solutionb. the H2SO4 solutionc. You need to know the acid concentrations to answer this question.d. You need to know the volume and concentration of the NaOH solution to answer this question.e. c and dExplain.
a. Write the balanced equation for the reaction of aqueous Pb(ClO 3)2 with aqueous NaI. Include phases.b. What mass of precipitate will form if 1.50 L of concentrated Pb(ClO 3)2 is mixed with 0.500 L of 0.250 M NaI? Assume the reaction goes to completion.
Which of the following metathesis reactions will occur, i.e. has (have) a driving force?i) NaC2H3O2 (aq) and HCl (aq) →ii) NaOH (aq) and HCl (aq) →iii) AgNO3 (aq) and Ca(C2H3O2)2 →iv) KOH (aq) and Fe(NO3)2 →v) Cr2(SO4)3 (aq) and (NH4)2CO3 (aq) →a) i, iib) i, ii, iiic) i, ii, ivd) ii,ve) i, ii, iv, v 
The mixing of which pair of reactants will result in a precipitation reaction?a. Mg(NO3)2(aq) + K2CO3(aq)b. Na2SO4(aq) + Cu(NO3)2(aq)c. LiClO4(aq) + (NH4)2S(aq)d. NH4Cl(aq) + NH4I(aq)
Write a balanced equation to show the reaction of sulfurous acid with lithium hydroxide to form water and lithium sulfite.
Consider the double displacement reaction of calcium nitrate with potassium sulfide. Which response identifies all of the products formed and no others?1. CaSN and PO22. Ca and S and K and H2 O3. CaSO2 and K3 N4. None of the other answers is correct5. CaSO3 and KNO26. CaSO3 and KNO37. CaSO4 and PNO38. CaS and KNO39. CaN3 and K2O and SO2
Calcium hydride reacts with water to form calcium hydroxide (aqueous) and hydrogen gas.Write a balanced chemical equation for the reaction.Express your answer as a balanced chemical equation. Identify all of the phases in your answer.
Express your answer as a chemical equation. Enter NO REACTION if no reaction occurs. Identify all of the phases in your answer.(NH4)2SO4(aq) + SrCl2(aq) →BaI2(aq) + AgNO3(aq) → 
Write a molecular equation for the precipitation reaction that occurs (if any) when the following solutions are mixed. If no reaction occurs, write NO REACTION.sodium chloride and lead (II) acetatea. NaCl + 2Pb(C2H3O2)2 → 2NaC2H3O2 + PbCl2b. 2NaCl + Pb(C2H3O2)2 → 2NaC2H3O2 + PbCl2c. NaCl + Pb(C2H3O2)2 → NaC2H3O2 + PbCl2d. No reaction.
Write net ionic equations for the reaction, if any, that occurs when aqueous solutions of the following are mixed.c. 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.d. strontium nitrate and potassium iodide
Separate samples of a solution of an unknown soluble ionic compound are treated with KCl, Na2SO4, and NaOH. A precipitate forms only when Na 2SO4 is added. Which cations could be present in the unknown soluble ionic compound?
Write a molecular equation for the precipitation reaction that occurs (if any) when the following solutions are mixed. If no reaction occurs, write NO REACTION.potassium sulfate and strontium iodidea. K2SO4 + SrI2 → 2Kl + SrSO4b. K2SO4 + SrI2 → KI + SrSO4c. 2K2SO4 + SrI2 → 2KI + SrSO4d. No reaction.
A sample may contain any or all of the following ions: Hg 22+, Ba2+, and Mn2+.a. No precipitate formed when an aqueous solution of NaCl was added to the sample solution.b. No precipitate formed when an aqueous solution of Na2SO4 was added to the sample solution.c. A precipitate formed when the sample solution was made basic with NaOH.Which ion or ions are present in the sample solution?
Write a balanced equation describing the neutralization of sodium hydroxide with sulfuric acid. In the balanced equation, what is the sum of the coefficients.A. 6B. 4C. 5D. 7E. 8
Write a molecular equation for the precipitation reaction that occurs (if any) when the following solutions are mixed. If no reaction occurs, write NO REACTION.chromium (III) nitrate and sodium phosphatea. Cr(NO3)3 + Na3PO4 → CrPO4 + NaNO3b. Cr(NO3)3 + 3Na3PO4 → CrPO4 + 3NaNO3c. Cr(NO3)3 + Na3PO4 → CrPO4 + 3NaNO3d. No reaction.
Complete and balance each of the following equations for gas-evolution reactions. Express your answer as a chemical equation. Identify all of the phases in your answer. HNO3(aq) + Na2SO3(aq)→
Complete and balance each of the following equations for gas-evolution reactions. Express your answer as a chemical equation. Identify all of the phases in your answer. HBr(aq) + NaHCO3(aq)→
What kind of reaction occurs when you mix aqueous solutions of barium sulfide and sulfuric acid? a) Neutralization b) Gas evolution c) Precipitation d) Precipitation and gas evolution
Many years ago, it was common to find small toys in boxes of breakfast cereal. One of these toys was a little submarine that had a compartment on the bottom for some baking soda (NaHCO3). On the top was another compartment connected to the first one with a small tube. This one was to be filled with vinegar (CH3COOH). After filling both containers and tightly covering them, the submarine was allowed to sink (usually in the bathtub with dirty children) to the bottom of the water where the vinegar then mixed with the baking soda. Which of the following answers describes the chemistry of the reaction that occurred as the submarine slowly rose to the surface?
Complete and balance each of the following equations for gas-evolution reactions. Express your answer as a chemical equation. Identify all of the phases in your answer. HC2H3O2(aq) + NaHSO3(aq)→
An interesting use of copper oxide is as a black surface coating in devices that collect solar energy. A thin layer of CuO transmits infrared radiation but not shorter wavelength radiation. It is degraded by acid rain primarily HNO3. Write an equation for what happens. 
Complete and balance each of the following equations for gas-evolution reactions. Express your answer as a chemical equation. Identify all of the phases in your answer. (NH4)2SO4(aq) + Ca(OH)2(aq)→
Write balanced molecular and net ionic equation for the following reaction, and identify the gas formed.Solid cadmium sulfide reacts with an aqueous solution of sulfuric acid. Express your answer as a balanced net ionic equation. Identify all of the phases in your answer.
Write balanced molecular and net ionic equation for the following reaction, and identify the gas formed.Solid magnesium carbonate reacts with an aqueous solution of perchloric acid. Express your answer as a balanced net ionic equation. Identify all of the phases in your answer.
Complete and balance:CrBr2(aq)+AgNO3(aq) →KCl(aq)+Pb(C2H3O2)2(aq) →NaOH(aq)+(NH4)2SO4(aq) →Express your answer as a chemical equation. Enter NO REACTION if no reaction occurs. Identify all of the phases in your answer. 
Write balanced molecular equation for the following reaction, and identify the gas formed.Solid magnesium carbonate reacts with an aqueous solution of perchloric acid. Express your answer as a balanced chemical equation. Identify all of the phases in your answer.
Complete and balance the following neutralization reactions.HC2H3O2(aq) + Ca(OH)2(aq) →Express your answer as a chemical equation. Identify all of the phases in your answer.
The labels have fallen off two bottles, one containing Mg(NO3)2 and the other containing Pb(NO3)2. You have a bottle of dilute H 2SO4. How could you use it to test a portion of each solution to identify which solution is which?
For each reaction, identify the precipitate or lack thereof. 2NaCI(aq) + Ba(OH)2 (aq) → BaCI2 + 2NaOH a) BaCI2 b) NaOH c) no precipitate
Complete the following reaction. Express your answer as a chemical equation. Enter NO REACTION  if no reaction occurs. NaOH(aq) + (NH4)2SO4(aq)  →
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.In the balanced equation, the coefficient in front of the mercury compound on the left side of the equation and the ammonium compound on the right side of the equation will bea) 1 and 1, respectivelyb) 1 and 2, respectivelyc) 2 and 1, respectivelyd) 2 and 4, respectively 
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.a. 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).
Complete and balance the following reaction:H3PO4(aq) + KOH(aq) →
Complete and balance the equation: Al2(SO4)3 (aq) + AgNO3 (aq) →
Complete and balance each of the following equations for acid-base reactions. Express your answer as a chemical equation. Identify all of the phases in your answer. a) HBr(aq) + LiOH(aq) →   b) H2SO4(aq) + Ba(OH)2(aq) →  
2 Al(NO3)3 + 3 Na 2CO3 → Al2(CO3)3 + 6 NaNO3Which product is precipitate?If 0.400 moles of aluminum nitrate is reacted with 0.700 moles of sodium carbonate, how many moles of precipitate will be formed? 
What acid and what strong base would react in aqueous solution to produce the following salts in the formula equation? Write the balanced formula equation for each reaction.a. potassium perchlorate
What acid and what strong base would react in aqueous solution to produce the following salts in the formula equation? Write the balanced formula equation for each reaction.b. cesium nitrate
For each reaction, identify the precipitate or lack thereof.  FeCl2(aq) + (NH4)2SO4(aq) → FeSO4 + 2NH4Cl a) FeSO4 b) NH4Cl c) no precipiate
A salt is obtained as a reaction between a. a base and an acid. b. an acid and oxygen. c. a nonmetal and a metal. d. a base and water.
What acid and what strong base would react in aqueous solution to produce the following salts in the formula equation? Write the balanced formula equation for each reaction.c. calcium iodide
Which substances are always produced in an acid-base neutralization reaction? Check all that apply. a) a salt b) a base c) water d) a gas e) an acid
Will precipitation occur when the following solutions are mixed? If so, write a balanced chemical equation for the reaction. (a) Na2CO3 and AgNO3
Will precipitation occur when the following solutions are mixed? If so, write a balanced chemical equation for the reaction. (b) NaNO3 and NiSO4
Will precipitation occur when the following solutions are mixed? If so, write a balanced chemical equation for the reaction. (c) FeSO4 and Pb(NO3)2
Identify the precipitate (if any) that forms when the following solutions are mixed, and write a balanced equation for each reaction. (a) Ni(NO3)2 and NaOH
Complete and balance each of the following equations. If no reaction occurs, write no reaction. a. NaOH(aq) + FeBr3(aq) →   b. BaCl2(aq) + AgNO3(aq) →   c. Na2CO3(aq) + CoCl2(aq) →   d. K2S(aq) + BaCl2(aq) → Express your answer as a chemical equation. Enter no reaction if no precipitate is formed.
Identify the precipitate (if any) that forms when the following solutions are mixed, and write a balanced equation for each reaction. (b) NaOH and K2SO4
Identify the precipitate (if any) that forms when the following solutions are mixed, and write a balanced equation for each reaction. (c) Na2S and Cu(CH3COO)2.
For the reactionAl2(SO4)3(aq) + AgNO3(aq) →express your answer as a chemical equation. Enter NO REACTION if no reaction occurs. Identify all of the phases in your answer.
Separate samples of a solution of an unknown salt are treated with dilute solutions of HBr, H2SO4, and NaOH. A precipitate forms in all three cases. Which of the following cations could the solution contain: K+, Pb2+, Ba2+? 
Separate samples of a solution of an unknown ionic compound are treated with dilute AgNO3, Pb(NO3)2, and BaCl2. Precipitates form in all three cases. Which of the following could be the anion of the unknown salt: Br–, CO32–, NO3–?
Complete and balance each of the following equations for gas evolution reactions.Express your answer as a chemical equation. Identify all of the phases in your answer.a. HClO4(aq) + K2CO3(aq)→b. HC2H3O2(aq) + LiHSO3(aq)→c. (NH4)2SO4(aq) + Ca(OH)2(aq)→d. HCl(aq) + ZnS(s)→
You know that an unlabeled bottle contains a solution of one of the following: AgNO 3, CaCl2, or Al2(SO4)3. A friend suggests that you test a portion of the solution with Ba(NO 3)2 and then with NaCl solutions. Explain how these two tests together would be sufficient to determine which salt is present in the solution.
Which product or set of products would correctly complete this reaction?Al2(SO4)3 (s) + H2O (l) →A. Al23+ (aq) + (SO4)32- (aq)B. Al2(SO4)3 (s) + H2O (l)C. Al2(SO4)3 (aq)D. 2Al3+ (aq) + 3 SO42- (aq)E. This reaction would not occur.
Hard water contains Ca2+, Mg2+, and Fe2+, which interfere with the action of soap and leave an insoluble coating on the insides of containers and pipes when heated. Water softeners replace these ions with Na+. If 1500 L of hard water contains 0.020 M Ca 2+, and 0.0040 M Mg2+, how many moles of Na+ are needed to replace these ions?
Complete and balance: HCl(aq) + ZnS(s) →Express your answer as a chemical equation. Identify all of the phases in your answer.  
Which component correctly completes this reaction, once the equation would be balanced?2 HClO4 (aq) + Ba(OH)2 (aq) → 2 H2O (l) +A. Ba(ClO4)2 (aq)B. 2 Ba(ClO4)2 (aq)C. BaCl2 (aq)D. 2 BaCl2 (aq)E. This reaction would not occur.
Consider this table of experimental data. In each case, two aqueous solutions were thoroughly mixed, and a small amount of organic solvent was then added, forming a separate layer in the reaction mixture.What conclusion can be drawn from these observations?(A) Iodine is able to displace bromide ion, but not chloride ion.(B) Chlorine is able to displace both bromide and iodide ion.(C) Both chlorine and bromine are able to displace iodine ion.(D) Neither chlorine and bromine are able to displace iodide ion.                                                     
Ca(NO3)2(aq)+KCl(aq) →Express your answer as a chemical equation. Write no reaction if no reaction occurs. Identify all of the phases in your answer. 
Complete the reaction:KBr(aq) + Na2CO3(aq)→Express your answer as a chemical equation. Identify all of the phases in your answer.
A 25.0 mL sample of 0.15 M silver nitrate, AgNO 3, is reacted with a 3.58 g sample of calcium chloride, CaCl2, (M= 111.0). Which of the following statements is true? a) Silver nitrate is the limiting reactant and calcium nitrate precipitates. b) Silver nitrate is the limiting reactant and silver chloride precipitates. c) Calcium chloride is the limiting reactant and calcium nitrate precipitates. d) Calcium chloride is the limiting reactant and silver chloride precipitates.
Write a balanced chemical equation for the reaction.FeSO4 and Pb(NO3)2Express your answer as a chemical equation. Identify all of the phases in your answer.
Which of the following is a neutralization reaction?a. KCl + NaNO3 → KNO3 + NaClb. HNO3 + KOH → H2O + KNO3c. H2O + SO3 → H2SO4d. 4Na + O2 → 2Na2Oe. 2NO2 → 2NO + O2
Write a molecular equation for the precipitation reaction that occurs (if any) when the following solutions are mixed. If no reaction occurs, write NO REACTION.sodium nitrate and lead (II) acetatelithium sulfide and strontium iodidealuminum sulfate and sodium phosphate
Write the balanced equation for the reaction of aqueous Pb(ClO 3)2 with aqueous NaI. Include phases. What mass of precipitate will form if 1.50 L of concentrated Pb(ClO 3)2 is mixed with 0.500 L of 0.150 M NaI? Assume the reaction goes to completion.
What precipitate is most likely formed from a solution containing Ba+2, Na+ , OH - , CO3 2- ?a) Na2CO3b) BaCO3c) NaOHd) Ba(OH)2
Complete and balance each of the following equations for gas-evolution reactions:a. HCl(aq) + K2SO3(aq) →b. HBr(aq) + NaHCO3(aq) →
Complete and balance the equation:HI(aq)+Sr(OH)2(aq) Express your answer as a chemical equation. Identify all of the phases in your answer.  
Determine whether each of the following compounds is soluble or insoluble? HgI2, CaCO3, AlPO4, K3PO4
A 100.0-mL aliquot of 0.200 M aqueous potassium hydroxide is mixed with 100.0 mL of 0.200 M aqueous magnesium nitrate. Write a balanced chemical equation for any reaction that occurs.
Complete the following reaction:HC2H3O2 + NaOH →
You may want to reference (Pages 163 - 166) section 4.6 while completing this problem.Complete and balance each of the following equations. If no reaction occurs, enter NO REACTION.NaNO3(aq) + KCl(aq) →
You may want to reference (Pages 163 - 166) section 4.6 while completing this problem.Complete and balance each of the following equations. If no reaction occurs, enter NO REACTION.NaCl(aq) + Hg2(C2H3O2)2(aq) →
You may want to reference (Pages 163 - 166) section 4.6 while completing this problem.Complete and balance each of the following equations. If no reaction occurs, enter NO REACTION.(NH4)2SO4(aq) + SrCl2(aq) →
You may want to reference (Pages 163 - 166) section 4.6 while completing this problem.Complete and balance each of the following equations. If no reaction occurs, enter NO REACTION.NH4Cl(aq) + AgNO3(aq) →
Predict the products of each of these reactions and write balanced molecular equations for each. If no reaction occurs, write NO REACTION.aqueous ammonium chloride and aqueous lead(II) nitrate
Predict the products of each of these reactions and write balanced molecular equations for each. If no reaction occurs, write NO REACTION.aqueous ammonium chloride and aqueous calcium hydroxide
Predict the products of each of these reactions and write balanced molecular equations for each. If no reaction occurs, write NO REACTION.liquid pentanol (C5H12O) and gaseous oxygen
Predict the products of each of these reactions and write balanced molecular equations for each. If no reaction occurs, write NO REACTION.aqueous strontium sulfide and aqueous copper(II) sulfate
Complete and balance the following acid-base equations:(a) HCl gas reacts with solid Ca(OH)2(s).
Complete and balance the following acid-base equations:(b) A solution of Sr(OH)2 is added to a solution of HNO3.
Complete and balance the following acid-base equations:(a) A solution of HClO4 is added to a solution of LiOH.
Complete and balance the following acid-base equations:(b) Aqueous H2SO4 reacts with NaOH.
Complete and balance the following acid-base equations:(c) Ba(OH)2 reacts with HF gas.
Complete and balance the equations for the following acid-base neutralization reactions. If water is used as a solvent, write the reactants and products as aqueous ions. In some cases, there may be more than one correct answer, depending on the amounts of reactants used.(a) Mg(OH)2(s) + HClO4(aq) ⟶
Complete and balance the equations for the following acid-base neutralization reactions. If water is used as a solvent, write the reactants and products as aqueous ions. In some cases, there may be more than one correct answer, depending on the amounts of reactants used.(b) SO3(g) + H2O(l) ⟶      (assume an excess of water and that the product dissolves)
Complete and balance the equations for the following acid-base neutralization reactions. If water is used as a solvent, write the reactants and products as aqueous ions. In some cases, there may be more than one correct answer, depending on the amounts of reactants used.(c) SrO(s) + H2SO4(l) ⟶
Calcium propionate is sometimes added to bread to retard spoilage. This compound can be prepared by the reaction of calcium carbonate, CaCO3, with propionic acid, C2H5CO2H, which has properties similar to those of acetic acid. Write the balanced equation for the formation of calcium propionate.
Complete and balance the equations of the following reactions, each of which could be used to remove hydrogen sulfide from natural gas:(a) Ca(OH)2(s) + H2S(g) ⟶
Complete and balance the equations of the following reactions, each of which could be used to remove hydrogen sulfide from natural gas:(b) Na2CO3(aq) + H2S(g) ⟶
Which of the following pairs of aqueous solutions will form a precipitate when mixed? a. Li2S + HI b. MgCl2 + KOH c. K2CO3 + HNO3 d. HF+ LiOH e. All of these solution pairs will produce a precipitate.
Complete and balance each of the following equations. If no reaction occurs, write NO REACTION.LiI(aq) + BaS(aq) →
Complete and balance each of the following equations. If no reaction occurs, write NO REACTION.KCl(aq) + CaS(aq) →
Complete and balance each of the following equations. If no reaction occurs, write NO REACTION.CrBr2(aq) + Na2CO3(aq) →
Complete and balance each of the following equations. If no reaction occurs, write NO REACTION.NaOH(aq) + FeCl3(aq) →
Write a molecular equation for the precipitation reaction that occurs (if any) when the following solutions are mixed. If no reaction occurs, write NO REACTION.potassium carbonate and lead(II) nitrate
Write a molecular equation for the precipitation reaction that occurs (if any) when the following solutions are mixed. If no reaction occurs, write NO REACTION.lithium sulfate and lead(II) acetate
Write a molecular equation for the precipitation reaction that occurs (if any) when the following solutions are mixed. If no reaction occurs, write NO REACTION.copper(II) nitrate and sodium sulfide
Write a molecular equation for the precipitation reaction that occurs (if any) when the following solutions are mixed. If no reaction occurs, write NO REACTION.strontium nitrate and potassium iodide
Write a molecular equation for the precipitation reaction that occurs (if any) when the following solutions are mixed. If no reaction occurs, write NO REACTION.sodium chloride and lead (II) acetate
Write a molecular equation for the precipitation reaction that occurs (if any) when the following solutions are mixed. If no reaction occurs, write NO REACTION.potassium sulfate and strontium iodide
Write a molecular equation for the precipitation reaction that occurs (if any) when the following solutions are mixed. If no reaction occurs, write NO REACTION.chromium (III) nitrate and sodium phosphate
Complete and balance each of the following equations for acid-base reactions.H2SO4(aq) + Ca(OH)2(aq) →
Complete and balance each of the following equations for acid-base reactions.HClO4(aq) + KOH(aq) →
Complete and balance each of the following equations for acid-base reactions.H2SO4(aq) + NaOH(aq) →
Which of the following pairs of aqueous solutions will form a precipitate when mixed? a. HCl + LiOH b. MgCl2 + KOH c. Li2S + HCl d. K2CO3 + HNO3 e. All of these solution pairs will produce a precipitate
Write the balanced formula equation for the acid–base reaction that occur when the following are mixed: potassium hydroxide (aqueous) and nitric acid.
Write the balanced formula equation for the acid–base reaction that occur when the following are mixed: barium hydroxide (aqueous) and hydrochloric acid.
Write the balanced formula equation for the acid–base reaction that occur when the following are mixed: perchloric acid [HClO4 (aq)] and solid iron(III) hydroxide.
Write the balanced formula equation for the acid–base reaction that occur when the following are mixed: solid silver hydroxide and hydrobromic acid.
Write the balanced formula equation for the acid–base reaction that occur when the following are mixed: aqueous strontium hydroxide and hydroiodic acid.
What acid and what base would react in aqueous solution so that potassium perchlorate appear as product in the formula equation? Write the balanced formula equation for the reaction.
What acid and what base would react in aqueous solution so that cesium nitrate appear as product in the formula equation? Write the balanced formula equation for the reaction.
What acid and what base would react in aqueous solution so that calcium iodide appear as product in the formula equation? Write the balanced formula equation for the reaction.
Some of the substances commonly used in stomach antacids are MgO, Mg(OH) 2, and Al(OH)3. Write a balanced equation for the neutralization of hydrochloric acid by each of these substances.
Some of the substances commonly used in stomach antacids are MgO, Mg(OH) 2, and Al(OH)3. Which of these substances will neutralize the greatest amount of 0.10 M HCl per gram?
Determine whether each of the following compounds is soluble or insoluble. For the soluble compounds, write the ions formed when the salt dissolves in water. a. (NH4)2S b. CuCO3 c. ZnS d. Pb(C2H3O2)2
Complete and balance each of the following equations for acid-base reactions. a. H3PO4(aq) + Sr(OH)2(aq) → b. HC2H3O2(aq) + Ca(OH)2(aq) → c. HCl(aq) + Ba(OH)2(aq) →
A sample may contain any or all of the following ions: Hg 22+, Ba2+, and Mn2+.a. No precipitate formed when an aqueous solution of NaCl was added to the sample solution.b. No precipitate formed when an aqueous solution of Na 2SO4 was added to the sample solution.c. A precipitate formed when the sample solution was made basic with NaOH.Which ion or ions are present in the sample solution?
A 100.0-mL aliquot of 0.200 M aqueous potassium hydroxide is mixed with 100.0 mL of 0.200 M aqueous magnesium nitrate. What precipitate forms?
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).Identify the solid.
What precipitate (if any) will form from the following reaction?FeSO4 (aq) + KCl (aq)
What precipitate (if any) will form from the following reaction?Al(NO3)3 (aq) + Ba(OH)2 (aq)
What precipitate (if any) will form from the following reaction?CaCl2 (aq) + Na 2SO4 (aq)
What precipitate (if any) will form from the following reaction?K2S (aq) + Ni(NO3)2 (aq)
What precipitate (if any) will form from the following reaction?Hg2(NO3)2 (aq) + CuSO4 (aq)
What precipitate (if any) will form from the following reaction?Ni(NO3)2 (aq) + CaCl2 (aq)
What precipitate (if any) will form from the following reaction?K2CO3 (aq) + MgI2 (aq)
What precipitate (if any) will form from the following reaction?Na2CrO4 (aq) + AlBr2 (aq)
Give an example how Fe(OH)3 (s) could be produced using a precipitation reaction. Write the balanced formula equation for the reaction.
Give an example how Hg2Cl2 (s) could be produced using a precipitation reaction. Write the balanced formula equation for the reaction.
Give an example how PbSO4 (s) could be produced using a precipitation reaction. Write the balanced formula equation for the reaction.
Give an example how BaCrO4 (s) could be produced using a precipitation reaction. Write the balanced formula equation for the reaction.
Complete and balance each of the following equations for gas-evolution reactions.HBr(aq) + NiS(s) →
Complete and balance each of the following equations for gas-evolution reactions.NH4I(aq) + NaOH(aq) →
Complete and balance each of the following equations for gas-evolution reactions.HBr(aq) + Na2S(aq) →
Complete and balance each of the following equations for gas-evolution reactions.HClO4(aq) + Li2CO3(aq) →
Complete and balance each of the following equations for gas-evolution reactions.HNO3(aq) + Na2SO3(aq) →
Complete and balance each of the following equations for gas-evolution reactions.HCl(aq) + KHCO3(aq) →
Complete and balance each of the following equations for gas-evolution reactions.HC2H3O2(aq) + NaHSO3(aq) →
Complete and balance each of the following equations for gas-evolution reactions.(NH4)2SO4(aq) + Ca(OH)2(aq) →
Write formulas for the acid and indicated valid that could be used to prepare each of the following salts: a. BaCl2 (solid is an oxide) b. MgSO4 (solid is a carbonate) c. KBr (solid is a hydroxide) 
Part 1 (1 point)Complete and balance the reaction. Al(OH)3 (s) + HCl (aq) →Part 2 (1 point)Water is one of the products formed. Write the name (not the chemical formula) for the other product.
Write the balanced neutralization reaction between H2SO and KOH in aqueous solution. Phases are optional. H2SO4 + 2KOH → K2SO4 + 2H2O0.750 L of 0.420 M H2SO4 is mixed with 0.700 L of 0.220 M KOH. What concentration of sulfuric acid remains after neutralization?
This question has multiple parts. Work on all the aprts to get the most points.Write a balanced molecular equation to represent the neutralization reaction between HBr and each of the following bases: (Use the lowest possible coefficients. Use the pull-down boxes to specify states such as (aq) or (s). If a box is not needed, leave it blank.) a. Mg(OH)2 b. Cr(OH)3 c. Fe(OH)2
If 37.85 mL of 0.170 M nitric acid neutralizes 53.0 mL of ammonia, what is the molarity of the base?HNO3 (aq) + NH4OH (aq) → NH4 NO3 (aq) + H2O(l)Express your answer to three significant figures and include the appropriate units.
Consider this aqueous reaction. HNO3(aq) + Ba(OH)2(aq) → What is the formula for the salt that forms?
Which of the following compounds is insoluble in water? A. LiCO3 B. FeCO3. C. Na2CO3 D. K2CO3 E. (NH4)2CO3.
Which of the following ions forms the fewest insoluble salts? a. Al3+ b. Cl- c. NH4+ d. OH- e. Mg2+
Identify the precipitate(s) of the reaction that occurs when a silver nitrate solution is mixed with a sodium chloride solution. Check all that apply. sodium nitrate, silver chloridesilver nitrate, sodium chloride
Write a balanced chemical equation for the following neutralization reaction producing a soluble salt Phosphoric acid neutralizes a potassium hydroxide solution.
Predict whether the following compounds are soluble or insoluble in water.