Provide a balanced chemical equation for the dissociation of each compound:

a) Na₃PO_4,  b) K₂CrO_4,  c) MgCl_2,  d) Al(NO₃)_3,  e) HNO_3,  f) K₂SO_4,  g) Ca(NO₂)_2,  h) Mg(C₂H₃O₂)_2,  i) Na₂CO_3,  j) (NH₄)₂SO_4,  k) HClO_4,  l) NaHSO_3, 

Write balanced complete ionic and net ionic equations for each reaction:

a) K₂SO₄(aq) + CaCl₂(aq) →CaSO₄(s) + 2KCl(aq)

b) Na₂S(aq) + 2HBr(aq) → 2NaBr(aq) + H₂S(g)

c) NH₄Cl(aq) + KOH(aq) → KaCl(aq) + H₂O(l) + NH₃(g)

d) Na₂CO₃(s) + H₂SO₄(aq) → Na₂SO₄(aq) + CO₂(g)+ H₂O(l)

e) AgNO₃(aq) + NaI(aq) → Agl(s) + NaNO₃(aq)

f) HBr(aq) + KOH(aq) → KBr(aq) + H₂O(l)

g) HC₂H₃O₂(aq) + Na₂CO₃(aq) → NaC₂H₃O₂(aq) + CO₂(g) + H₂O(l)

h) LiOH(aq) + HC₂H₃O₂(aq) → LiC₂H₃O₂(aq) + H₂O(l)

i) HCl(aq) + NH₃(aq) → NH₄Cl(aq)

j) 2K₃PO₄(aq) + 3BaCl₂(aq) → Ba₃(PO₄)₂(s) + 6KCl(aq)

Complete and balance each of the following molecular equations in aqueous solution:

a) AgNO₃(aq) + CaCl₂(aq) →

b) HNO₃(aq) + Na₂CO₃(aq) →

c) K₂CO₃(s) + HClO₃(aq) →

d) Al(OH)₃(s) + HBr(aq) →

e) H₃PO₄(aq) + Fe(OH)₃(s) →

f) BaCl₂(aq) + K₂SO₄(aq) →

Calculate the molarity of each ion in the following solutions:

a) 0.150 M NaNO₃
b) 0.250 M K₂SO₄
c) 0.280 M Ca(NO₃)₂
d) 0.350 M AlCl₃

Which solution contains more chloride ions assuming complete solubility of salts?

a) 0.140 M NaCl or 0.060 M AlCl₃
b) 0.250 M BaCl₂ or 0.250 M MgCl₂
c) 0.250 M MgCl₂ or 0.450 M KCl

How many ml of 1.80 M MgBr₂ is necessary to precipitate all the silver ions in 600.0 mL of 0.80 M AgNO₃ solution?

How many ml of 2.70 M K₂SO₄ is required to precipitate all the barium ions in 500. mL of 0.650 M BaCl₂ solution?

27.0 mL of a NaOH solution was needed to neutralize 0.326 g of KHP (KHC₈H₄O₄). What is the molarity of the NaOH solution?

What volume of 0.150 M calcium hydroxide is required to neutralize 250.0 mL of 0.0350 M sulfuric acid?

How many mL of 0.250 M HCl will neutralize 60.00 mL of 0.060 M Ba(OH)₂?

What is the mass in grams of AgCl precipitate if 20.0 mL of 0.150 M AgNO₃ is added to 45.0 mL of 0.250 M MgCl₂?

How many mL of 0.600 M K₂SO₄ was added to 400.0 mL of 0.500 M BaCl₂ solution if 31.2 g of precipitate was collected?

When a 42.0-mL sample of a 0.85 M sodium chloride solution is mixed with 17.0 mL of a 0.650 M lead(II) nitrate solution, 2.45 g of a precipitate is formed:

2NaCl(aq) + Pb(NO₃)₂(aq) → PbCl₂(s) + 2NaNO₃(aq)

What are the theoretical and the percent yields of the reaction?

A 4.598-g sample of acetylsalicylic acid (the active ingredient in aspirin) was dissolved in water. It took 35.6 mL of a 0.717 M NaOH solution to neutralize the acid. Determine the molar mass of the acid considering that it is a monoprotic acid.

A student prepared a solution by dissolving 2.40-g mixture of calcium nitrate and calcium chloride. To this, a solution of silver nitrate was added dropwise until the mass of the precipitate stayed constant at 0.584 g. Determine the mass percent of calcium nitrate in the mixture.