Calculate the concentrations of K+ and F− in a 0.19 M KF solution.

Write balanced equations showing how the hydrogen oxalate ion, HC2O4˗, can be both a Bronsted acid and a Bronsted base.

A solution was prepared by 0.250 moles of ammonium chloride to 500.0 mL of 0.35 M ammonia. Given the KB of NH3 is 1.86 × 10^⁻5, determine the pH of the resultant solution. (You may assume the volume is unchanged.)

Calculate the pH of a solution that’s 0.65 M in NaNO2 and 0.40 M in HNO2. (HNO2, Ka = 4.45 × 10–4 ).

What is the pH of a 0.320 M solution of HC₂H₃O₂ (Ka = 1.8 × 10⁻⁵)?

Calculate the pH of a solution resulting from dissolving 23. g of Ba(OH)2 in enough water to make 155 mL of a solution.

Calculate the pH of a 7.4 x 10–4 M solution of Ba(OH)2.

Calculate the hydronium ions concentration, [H3O+ ], for a 0. 01 M HClO4 aqueous solution

Calculate the molarity of an aqueous nitric acid solution if it requires 35.6 mL of 0.165 M NaOH (aq) to neutralize 25.0 mL of the HNO3 (aq) solution.

40) What is the pH of a 0.0140 M Ca(OH)2 solution?