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.

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.

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

Classify each compound as a strong electrolyte or nonelectrolyte. a. MgBr₂ b. C₁₂H₂₂O₁₁ c. Na₂CO₃ d. KOH

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

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

Complete and balance each equation. If no reaction occurs, write 'NO REACTION.' a. LiI(aq) + BaS(aq)

Complete and balance each equation. If no reaction occurs, write 'NO REACTION.' b. KCl(aq) + CaS(aq) →

Complete and balance each equation. If no reaction occurs, write 'NO REACTION.' c. CrBr₂(aq) + Na₂CO₃(aq) →

Complete and balance each equation. If no reaction occurs, write 'NO REACTION.' a. NaNO₃(aq) + KCl(aq) →

Complete and balance each equation. If no reaction occurs, write 'NO REACTION.' d. NH₄Cl(aq) + AgNO₃(aq) →

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

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

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

Write balanced complete ionic and net ionic equations for each reaction. a. HCl(aq) + LiOH(aq) → H₂O(l) + LiCl(aq)

Write balanced complete ionic and net ionic equations for each reaction. b. MgS(aq) + CuCl₂(aq) → CuS(s) + MgCl₂(aq)

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)

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)

Write balanced complete ionic and net ionic equations for each reaction. a. K₂SO₄(aq) + CaI₂(aq) → CaSO₄(s) + KI(aq)

Write balanced complete ionic and net ionic equations for each reaction. d. HC₂H₃O₂(aq) + K₂CO₃(aq) → H₂O(l ) + CO₂(g) + KC₂H₃O₂(aq)

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.

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.

Write balanced molecular and net ionic equations for the reaction between hydrobromic acid and potassium hydroxide.

Write balanced molecular and net ionic equations for the reaction between nitric acid and calcium hydroxide.

Complete and balance each acid–base equation.

a. H₂SO₄(aq) + Ca(OH)₂(aq) →

b. HClO₄(aq) + KOH(aq) →

c. H₂SO₄(aq) + NaOH(aq) →

Complete and balance each acid–base equation. b. HC₂H₃O₂(aq) + Ca(OH)₂(aq) →