Molecular Equations

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

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+

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. 

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-

What are the primary products of the neutralization reaction between an acid and a base? A. H2O and salt B. CO2 and H2O C. CO2 and protons D. H2O and hydroxide ions

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) →

When glucose, C6H12O6, is completely oxidized with excess oxygen, what are the products? a) H2O2 and CO2 b) H2O and CO2 c) H2O2 and CO d) H2O and CO

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

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

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 

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. 

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 solutionb) hydrochloric acid solution + strontium hydroxide solutionc) calcium nitrate solution + lithium chloride solutiond) ammonium chloride solution + copper (II) acetate solutione) None of the above reactions will lead to formation of a precipitate

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 

Which ion may form a scummy precipitate with ordinary soap?a) CO32-b) HCO3-c) Ca2+d) Na+

Predict the precipitate in the reaction between sodium phosphate and calcium chloride.A. Ca(PO4)2B. Ca3(PO4)2C. NaClD. Na2Cl

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?

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–?

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.

When the following solutions are mixed together, what precipitate (if any) will form?a. FeSO4(aq) + KCl(aq)

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?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)

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?

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?

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).

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

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)  

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.

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.

Which substances are always produced in an acid-base neutralization reaction? Check all that apply.a) a saltb) a basec) waterd) a gase) an acid

For each reaction, identify the precipitate or lack thereof.2NaCI(aq) + Ba(OH)2 (aq) → BaCI2 + 2NaOHa) BaCI2b) NaOHc) no precipitate

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)

What salt is produced in each of the following neutralization reactions?a. HNO3(aq) + KOH(aq) → H 2O(l) + ?b. HNO3(aq) + Ca(OH)2(aq) → H2O(l) + ?c. HCl(aq) + Ca(OH)2(aq) → H2O(l) + ?d. HCl(aq) + KOH(aq) → H 2O(l) + ?

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)

What salt is produced in the following reaction?HNO3(aq) + KOH(aq) → H2O(l) + ?

What salt is produced in the following reaction?HNO3(aq) + Ca(OH)2(aq) → H2O(l) + ?

What salt is produced in the following reaction?HCl(aq) + Ca(OH)2(aq) → H2O(l) + ?

What salt is produced in the following reaction?HCl(aq) + KOH(aq) → H2O(l) + ?

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 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.

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.

What are products for this reaction? Ba(OH)2 + H2O →

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.

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?

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)2b) Sc(NO3)3c) BaCO3d) LiClO4e) NaNO3

Suppose that aqueous solutions of barium nitrate and potassium carbonate are mixed. What is the name of the compound or compounds that precipitate?

Consider this aqueous reaction. HNO3 (aq) + Ba(OH)2(aq) →What is the formula for the salt that forms?

Identify the precipitation and non-precipitation reactionsa. 4P + 5O2 → 2P2O5b. H2O2 + NaIO → NaI + H 2O + O2c. Ba(NO3)2 + MgSO4 → BaSO4 + Mg(NO3)2d. Hg2(C2H3O2)2 + 2NaBr → Hg 2Br2 + 2NaC2H3O2e. 2KI + Pb(NO3)2 → PbI2 + 2KNO3f. HCI + NaOH → NaCI + H 2Og. HBr + NaOH → NaBr + H 2O

For each reaction, identify the precipitate or lack thereof. FeCl2(aq) + (NH4)2SO4(aq) → FeSO4 + 2NH4Cla) FeSO4b) NH4Clc) no precipitate

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?a. Hg2(NO3)2(aq) + CuSO4(aq)

Part B. When the following reaction occurs:H3PO4(aq) + Ca(OH)2(aq) →What is the formula for the salt formed? Express your answer as a chemical formula.Reactions in water solution can be classified based on the driving force that converts reactants to product. The three classes are precipitation reactions, acid-base neutralization reactions, and oxidation-reduction reactions.• In precipitation reactions a solid product forms from aqueous reactants. The product can be predicted by using solubility rules.• In acid-base neutralization reactions an acid (proton donor) reacts with a base (proton acceptor) to form an ionic salt and sometimes water. You can recognize this type of reaction by the presence of an acid and base in the reactants.• In oxidation-reduction reactions (or redox for short) electrons are transferred between reactants. So you will always see changes in oxidation number within this type of reaction.