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

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. 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 hydrochloric acid and rubidium hydroxide.

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.

b. HCHO₂(aq) + NaOH(aq) →

c. HC₂H₃O₂(aq) + LiOH(aq) →

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)

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)

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

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

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? 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)

Predict the products and write a balanced molecular equation for each reaction. If no reaction occurs, write 'NO REACTION.' a. HCl(aq) + Hg₂(NO₃)₂(aq) →

Predict the products and write a balanced molecular equation for each reaction. If no reaction occurs, write 'NO REACTION.' d. aqueous ammonium chloride and aqueous calcium hydroxide

Predict the products and write a balanced molecular equation for each reaction. If no reaction occurs, write 'NO REACTION.' c. liquid pentanol (C₅H₁₂O) and gaseous oxygen

Hard water often contains dissolved Ca²⁺ and Mg²⁺ ions. One way to soften water is to add phosphates. The phosphate ion forms insoluble precipitates with calcium and magnesium ions, removing them from solution. A solution is 0.050 M in calcium chloride and 0.085 M in magnesium nitrate. What mass of sodium phosphate would you add to 1.5 L of this solution to completely eliminate the hard water ions? Assume complete reaction.

An acid solution is 0.100 M in HCl and 0.200 M in H₂SO₄. What volume of a 0.150 M KOH solution would completely neutralize all the acid in 500.0 mL of this solution?

Find the mass of barium metal (in grams) that must react with O₂ to produce enough barium oxide to prepare 1.0 L of a 0.10 M solution of OH^-.

A solution contains Cr³⁺ ions and Mg²⁺ ions. The addition of 1.00 L of 1.51 M NaF solution causes the complete precipitation of these ions as CrF₃(s) and MgF₂(s). The total mass of the precipitate is 49.6 g. Find the mass of Cr³⁺ in the original solution.