What is the molar solubility (in M) of silver chromate (Ag₂CrO₄) in water? Hint: Ksp of Ag₂CrO₄ = 1.1 × 10⁻12

What happens when a small amount of HCl is added to a buffer solution containing NH₃ and NH₄Cl?

Consider the following titration curve graphs: Which of the titration curves best represents the results for a strong base titrated with a strong acid?

A 1.00 L buffer solution is made with 0.500 mol of ammonia (NH₃) and 0.600 mol of ammonium chloride (NH₄Cl).The pKa of NH₄⁺ is 9.25. What is the pH of the solution after the addition of 0.100 mol of HCl. Hint:  Assume no change in volume upon addition of HCl

What is the pH of a buffer made from 0.45 mol of HCN and 0.20 mol of NaCN in 2.0 L of solution? Hint: The Ka of hydrogen cyanide, HCN, is 4.9 × 10⁻10.

Which of the following titrations would produce a solution with a basic pH at equivalence point?

Which of the following titrations would produce a solution with an acidic pH at the equivalence point?

What is the pH of a buffer made from 0.15 mol of HF and 0.55 mol of KF in 2.0 L of solution? Hint: The Ka of hydrofluoric acid, HF, is 6.8 × 10⁻4.

In which of the following aqueous solutions would you expect the solubility of Fe(OH)₃ to be the greatest? Hint: Consider the factors that affect solubility.

What is the molar solubility (in M) of magnesium hydroxide (Mg(OH)₂) in water? Hint: Ksp of Mg(OH)₂ = 1.5 × 10⁻11