Tro - Chemistry: A Molecular Approach 6th Edition - Chapter 5

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Ch.5 - Introduction to Solutions and Aqueous Solutions

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Tro 6th Edition

Ch.5 - Introduction to Solutions and Aqueous Solutions

Problem 51a
Complete and balance each equation. If no reaction occurs, write 'NO REACTION.' a. LiI(aq) + BaS(aq)
Problem 51b
Complete and balance each equation. If no reaction occurs, write 'NO REACTION.' b. KCl(aq) + CaS(aq) →
Problem 51c
Complete and balance each equation. If no reaction occurs, write 'NO REACTION.' c. CrBr₂(aq) + Na₂CO₃(aq) →
Problem 52
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 52a
Complete and balance each equation. If no reaction occurs, write 'NO REACTION.' a. NaNO₃(aq) + KCl(aq) →
Problem 52d
Complete and balance each equation. If no reaction occurs, write 'NO REACTION.' d. NH₄Cl(aq) + AgNO₃(aq) →
Problem 53
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 53a
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 53c
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 54
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 55b
Write balanced complete ionic and net ionic equations for each reaction. CaS(aq) + CuCl₂(aq) → CuS(s) + CaCl₂(aq)
Problem 55c,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 55d
Write balanced complete ionic and net ionic equations for each reaction. d. Na₃PO₄(aq) + NiCl₂(aq) → Ni₃(PO₄)₂(s) + NaCl(aq)
Problem 56a,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 56a
Write balanced complete ionic and net ionic equations for each reaction. a. K₂SO₄(aq) + CaI₂(aq) → CaSO₄(s) + KI(aq)
Problem 56d
Write balanced complete ionic and net ionic equations for each reaction. d. HC₂H₃O₂(aq) + K₂CO₃(aq) → H₂O(l ) + CO₂(g) + KC₂H₃O₂(aq)
Problem 57
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 58
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 59
Write balanced molecular and net ionic equations for the reaction between hydrochloric acid and rubidium hydroxide.
Problem 60
Write balanced molecular and net ionic equations for the reaction between nitric acid and magnesium hydroxide.
Problem 62b
Complete and balance each acid–base equation. b. HC₂H₃O₂(aq) + Ca(OH)₂(aq) →
Problem 64b,c
Write balanced complete ionic and net ionic equations for each acid–base reaction.
b. HCHO₂(aq) + NaOH(aq) →
c. HC₂H₃O₂(aq) + LiOH(aq) →
Problem 65
A 15.00-mL sample of an unknown HClO4 solution requires titration with 17.03 mL of 0.1000 M NaOH to reach the equivalence point. What is the concentration of the unknown HClO4 solution? The neutralization reaction is HClO₄(aq) + NaOH(aq) → H₂O(l ) + NaClO₄(aq)
Problem 66
A 25.00-mL sample of an unknown H₃PO₄ solution is titrated with a 0.150 M NaOH solution. The equivalence point is reached when 22.97 mL of NaOH solution is added. What is the concentration of the unknown H₃PO₄ solution? The neutralization reaction is H₃PO₄(aq) + 3 NaOH(aq) → 3 H₂O(l) + Na₃PO₄(aq)
Problem 67
Complete and balance each gas-evolution equation. b. NH₄I(aq) + NaOH(aq) →
Problem 67c
Complete and balance each gas-evolution equation. c. HBr(aq) + Na₂S(aq) →
Problem 68a
Complete and balance each gas-evolution equation. a. HNO₃(aq) + Na₂SO₃(aq) →
Problem 69
Assign oxidation states to each atom in each element, ion, or compound. Ag, Ca²⁺, BaO, H₂S, NO₃^-, CrO₄^2-
Problem 70
Assign oxidation states to each atom in each element, ion, or compound. Cl₂, Fe³⁺, CuCl₂, CH₄, Cr₂O₇^2–, HSO₄^–
Problem 71a
What is the oxidation state of Cr in each compound? a. CrO