Tro - Chemistry: A Molecular Approach 4th Edition - Chapter 4

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Ch.4 - Chemical Quantities & Aqueous Reactions

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Tro 4th Edition

Ch.4 - Chemical Quantities & Aqueous Reactions

Problem 69
A 25.0-mL sample of a 1.20 M potassium chloride solution is mixed with 15.0 mL of a 0.900 M lead(II) nitrate solution and this precipitation reaction occurs: 2 KCl(aq) + Pb(NO3)2(aq) → PbCl2(s) + 2 KNO3(aq). The solid PbCl2 is collected, dried, and found to have a mass of 2.45 g. Determine the limiting reactant and the theoretical yield.
Problem 69c
A 25.0-mL sample of a 1.20 M potassium chloride solution is mixed with 15.0 mL of a 0.900 M lead(II) nitrate solution and this precipitation reaction occurs: 2 KCl(aq) + Pb(NO₃)₂(aq) → PbCl₂(s) + 2 KNO₃(aq) The solid PbCl₂ is collected, dried, and found to have a mass of 2.45 g. Determine the the percent yield.
Problem 70
A 55.0-mL sample of a 0.102 M potassium sulfate solution is mixed with 35.0 mL of a 0.114 M lead(II) acetate solution and this precipitation reaction occurs: K₂SO₄(aq) + Pb(C₂H₃O₂)₂(aq) → 2 KC₂H₃O₂(aq) + PbSO₄(s) The solid PbSO₄ is collected, dried, and found to have a mass of 1.01 g. Determine the limiting reactant, theoretical yield, percent yield.
Problem 71
For each compound (all water soluble), would you expect the resulting aqueous solution to conduct electrical current? a. CsCl b. CH₃OH c. Ca(NO₂)₂ d. C₆H₁₂O₆
Problem 72
Classify each compound as a strong electrolyte or nonelectrolyte. a. MgBr₂ b. C₁₂H₂₂O₁₁ c. Na₂CO₃d. KOH
Problem 73
Determine whether each compound is soluble or insoluble. If the compound is soluble, list the ions present in solution. a. AgNO₃ b. Pb(C₂H₃O₂)₂ c. KNO₃ d. (NH₄)₂S
Problem 74
Determine whether each compound is soluble or insoluble. If the compound is soluble, list the ions present in solution. a. AgI b. Cu₃(PO₄)₂ c. CoCO₃ d. K₃PO₄
Problem 75
Complete and balance the following equation. If no reaction occurs, write “NO REACTION.” NaOH(aq) + FeCl3(aq) → ?
Problem 75a
Complete and balance each equation. If no reaction occurs, write 'NO REACTION.' a. LiI(aq) + BaS(aq)
Problem 75b
Complete and balance each equation. If no reaction occurs, write 'NO REACTION.' b. KCl(aq) + CaS(aq) →
Problem 75c
Complete and balance each equation. If no reaction occurs, write 'NO REACTION.' c. CrBr₂(aq) + Na₂CO₃(aq) →
Problem 76
Complete and balance each equation. If no reaction occurs, write “NO REACTION.” b. NaCl(aq) + Hg2(C2H3O2)2(aq) → c. (NH4)2SO4(aq) + SrCl2(aq) →
Problem 76a
Complete and balance each equation. If no reaction occurs, write 'NO REACTION.' a. NaNO₃(aq) + KCl(aq) →
Problem 76d
Complete and balance each equation. If no reaction occurs, write 'NO REACTION.' d. NH₄Cl(aq) + AgNO₃(aq) →
Problem 77
Write a molecular equation for the precipitation reaction that occurs (if any) when each pair of aqueous solutions is mixed. If no reaction occurs, write “NO REACTION.” 1. lithium sulfate and lead(II) acetate 2. strontium nitrate and potassium iodide
Problem 77a
Write a molecular equation for the precipitation reaction that occurs (if any) when each pair of aqueous solutions is mixed. If no reaction occurs, write 'NO REACTION.' a. potassium carbonate and lead(II) nitrate
Problem 77c
Write a molecular equation for the precipitation reaction that occurs (if any) when each pair of aqueous solutions is mixed. If no reaction occurs, write 'NO REACTION.' c. copper(II) nitrate and magnesium sulfide
Problem 78
Write a molecular equation for the precipitation reaction that occurs (if any) when each pair of aqueous solutions is mixed. If no reaction occurs, write 'NO REACTION.' a. sodium chloride and lead(II) acetate b. potassium sulfate and strontium iodide c. cesium chloride and calcium sulfide d. chromium(III) nitrate and sodium phosphate
Problem 79a
Write balanced complete ionic and net ionic equations for each reaction. a. HCl(aq) + LiOH(aq) → H₂O(l) + LiCl(aq)
Problem 79b
Write balanced complete ionic and net ionic equations for each reaction. b. MgS(aq) + CuCl₂(aq) → CuS(s) + MgCl₂(aq)
Problem 79c,d
Write balanced complete ionic and net ionic equations for each reaction.
c. NaOH(aq) + HC₂H₃O₂(aq) → H₂O(l ) + NaC₂H₃O₂(aq)
d. Na₃PO₄(aq) + NiCl₂(aq) → Ni₃(PO₄)₂(s) + NaCl(aq)
Problem 80a,b,c
Write balanced complete ionic and net ionic equations for each reaction.
a. K₂SO₄(aq) + CaI₂(aq) → CaSO₄(s) + KI(aq)
b. NH₄Cl(aq) + NaOH(aq) → H₂O(l) + NH₃(g) + NaCl(aq)
c. AgNO₃(aq) + NaCl(aq) → AgCl(s) + NaNO₃(aq)
Problem 80a
Write balanced complete ionic and net ionic equations for each reaction. a. K₂SO₄(aq) + CaI₂(aq) → CaSO₄(s) + KI(aq)
Problem 80d
Write balanced complete ionic and net ionic equations for each reaction. d. HC₂H₃O₂(aq) + K₂CO₃(aq) → H₂O(l ) + CO₂(g) + KC₂H₃O₂(aq)
Problem 81
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 and net ionic equations for the reaction of aqueous Hg₂(NO₃)₂ with aqueous sodium chloride to form solid Hg₂Cl₂ and aqueous sodium nitrate.
Problem 82
Lead(II) ions can be removed from solution by precipitation with sulfate ions. Suppose that a solution contains lead(II) nitrate. Write complete ionic and net ionic equations for the reaction of aqueous lead(II) nitrate with aqueous potassium sulfate to form solid lead(II) sulfate and aqueous potassium nitrate.
Problem 83
Write balanced molecular and net ionic equations for the reaction between hydrobromic acid and potassium hydroxide.
Problem 84
Write balanced molecular and net ionic equations for the reaction between nitric acid and calcium hydroxide.
Problem 85
Complete and balance each acid–base equation.
a. H₂SO₄(aq) + Ca(OH)₂(aq) →
b. HClO₄(aq) + KOH(aq) →
c. H₂SO₄(aq) + NaOH(aq) →
Problem 86b
Complete and balance each acid–base equation. b. HC₂H₃O₂(aq) + Ca(OH)₂(aq) →