HCN is a weak acid (?a=6.20×10^−10) , so the salt, KCN , acts as a weak base. What is the pH of a solution that is 0.0525 M in KCN at 25 °C?

The acid ionization constant for a certain monoprotic acid (HA) is 4.52×10−5. What is the pH of a 0.35 M solution of this acid?

3. H̟CO, 2Ħ+HCO,¯ K, = 4.3 × 10-7 HCO, H* + Co, K, = 5.6 × 10-" The acid dissociation constants for the reactions above are given at 25°C. (a) What is the pH of a 0.050-molar solution of H,CO, at 25°C? (b) What is the concentration of CO,- ions in the solution in (a)? (c) How would the addition of each of the following substances affect the pH of the solution in (a)? (i) HCl (ii) NaHCO, (iii) NaOH (iv) NaCl

The pH of an aqueous solution of 0.149 M potassium acetate, (Assume that KCH3COO, is K. (HCH3COO) = 1.80 × 10-5.) This solution is

What is the pH of the solution that results from mixing 75 mL of 0.50 M NH 3(aq) and 75 mL of 0.50 HCl(aq) at 25 °C? ( K b for NH 3 = 1.8 × 10 –5)

Calculate the pOH of 0.716 M anilinium hydrochloride (C6H5NH3Cl) solution in water, given that Kb for aniline is 3.83 × 10-4.

What is the concentration of hydroxide ion in a 0.45 M aqueous solution of hydroxylamine, NH2OH? (Assume the value of Kw is 1.0 ✕ 10−14.) M What is the pH?

Calculate the pH and the pOH of an aqueous solution that is 0.045 M in HCI(aq) and 0.055 M in HBr(aq) at 25 °C. pH = РОН