Ch.5 - Introduction to Solutions and Aqueous Solutions

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Tro 5th Edition

Ch.5 - Introduction to Solutions and Aqueous Solutions

Problema 43c

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

Problema 44

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) →

Problema 44a

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

Problema 44d

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

Problema 45

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

Problema 45a

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

Problema 45c

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

Problema 46

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

Problema 47a

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

Problema 47b

Write balanced complete ionic and net ionic equations for each reaction. CaS(aq) + CuCl₂(aq) → CuS(s) + CaCl₂(aq)

Problema 47c,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)

Problema 47d

Write balanced complete ionic and net ionic equations for each reaction. d. Na₃PO₄(aq) + NiCl₂(aq) → Ni₃(PO₄)₂(s) + NaCl(aq)

Problema 48a

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

Problema 48a,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)

Problema 48d

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

Problema 49

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.

Problema 50

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.

Problema 51

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

Problema 52

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

Problema 53

Complete and balance each acid–base equation.

a. H₂SO₄(aq) + Ca(OH)₂(aq) →

b. HClO₄(aq) + KOH(aq) →

c. H₂SO₄(aq) + NaOH(aq) →

Problema 54b

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

Problema 56a

Write balanced complete ionic and net ionic equations for each acid–base reaction. a. HI(aq) + RbOH(aq) →

Problema 56b,c

Write balanced complete ionic and net ionic equations for each acid–base reaction.

b. HCHO₂(aq) + NaOH(aq) →

c. HC₂H₃O₂(aq) + LiOH(aq) →

Problema 57

A 25.00-mL sample of an unknown HClO₄ solution requires titration with 22.62 mL of 0.2000 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)

Problema 58

A 30.00-mL sample of an unknown H₃PO₄ solution is titrated with a 0.100 M NaOH solution. The equivalence point is reached when 26.38 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)

Problema 59b

Complete and balance each gas-evolution equation. b. NH₄I(aq) + NaOH(aq) →

Problema 59c

Complete and balance each gas-evolution equation. c. HBr(aq) + Na₂S(aq) →

Problema 60a

Complete and balance each gas-evolution equation. a. HNO₃(aq) + Na₂SO₃(aq) →

Problema 61

Assign oxidation states to each atom in each element, ion, or compound. Ag, Ca²⁺, BaO, H₂S, NO₃^-, CrO₄^2-

Problema 62

Assign oxidation states to each atom in each element, ion, or compound. Cl₂, Fe³⁺, CuCl₂, CH₄, Cr₂O₇^2–, HSO₄^–