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) →

Write balanced complete ionic and net ionic equations for each acid–base reaction. a. HBr(aq) + NaOH(aq) → b. HF(aq) + NaOH(aq) → c. HC₂H₃O₂(aq) + RbOH(aq) →

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

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

b. HCHO₂(aq) + NaOH(aq) →

c. HC₂H₃O₂(aq) + LiOH(aq) →

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)

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)

Complete and balance each gas-evolution equation. a. HBr(aq) + NiS(s) → d. HClO₄(aq) + Li₂CO₃(aq) →

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

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

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

Complete and balance each gas-evolution equation. b. HCl(aq) + KHCO₃(aq) → c. HC₂H₃O₂(aq) + NaHSO₃(aq) → d. (NH₄)₂SO₄(aq) + Ca(OH)₂(aq) →

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

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

What is the oxidation state of Cr in each compound? a. CrO

What is the oxidation state of Cr in each compound? b. CrO₃

What is the oxidation state of Cr in each compound? c. Cr₂O₃

What is the oxidation state of Cl in each ion? a. ClO^- b. ClO₂^- c. ClO₃^- d. ClO₄^-

Determine whether each reaction is a redox reaction. For each redox reaction, identify the oxidizing agent and the reducing agent. a. 4 Li(s) + O₂(g) → 2 Li₂O(s) b. Mg(s) + Fe²⁺(aq) → Mg²⁺(aq) + Fe(s)

Determine whether each reaction is a redox reaction. For each redox reaction, identify the oxidizing agent and the reducing agent. c. Pb(NO₃)₂(aq) + Na₂SO₄(aq) → PbSO₄(s) + 2 NaNO₃(aq) d. HBr(aq) + KOH(aq) → H₂O(l) + KBr(aq)

Determine whether each reaction is a redox reaction. For each redox reaction, identify the oxidizing agent and the reducing agent. a. Al(s) + 3 Ag⁺(aq) → Al³⁺(aq) + 3 Ag(s) b. SO₃(g) + H₂O(l) → H₂SO₄(aq) c. Ba(s) + Cl₂(g) → BaCl₂(s) d. Mg(s) + Br₂(l) → MgBr₂(s)