17. Acid and Base Equilibrium

What is the pH of a 0.750 M solution of NaCN (K_a of HCN is 4.9 × 10^-10)?

What is the pH of a 0.320 M solution of Ca(NO₂)₂ (ka of HNO₂ is 4.5 × 10^-4)?

Determine the pH of a solution made by dissolving 6.1 g of sodium cyanide, NaCN, in enough water to make a 500.0 mL of solution. (MW of NaCN = 49.01 g/mol). The K_a value of HCN is 4.9 × 10⁻¹⁰.

An unknown weak base has an initial concentration of 0.750 M with a pH of 8.03. Calculate its equilibrium base constant. 

How can the pH of a solution be calculated if the pOH is known?

The K_b of methylamine is 4.4 x 10^–4. What is the approximate [OH^–] of a 1 M solution of methylamine?

calculate the pH of a 0.10 M solution of hydrazine, N₂H₄ . K_b for hydrazine is 1.3×10⁻⁶ .

What is the [OH⁻] of a 1.40 m solution of pyridine (C₅H₅N, K_b = 1.70 × 10⁻⁹)?

What is the [OH^-] of a 1.40 M solution of pyridine (C₅H₅N, K_b = 1.70 × 10^-9)?

What is the pH of a solution with a hydroxyl ion (OH^-) concentration of 10^-10 M?

The pOH of a solution is 10.75. What is the concentration of OH^– ions in the solution?

Determine the pH of a 0.227 M C₅H₅N solution at 25 °C. The K_b of C₅H₅N is 1.7 x 10^-9.

The pH of 2.65 m CH₃NH_2(aq) is 12.54. determine the value of K_b for methylamine.

An unknown weak base with a concentration of 0.170 M has a ph of 9.42. What is the K_b of this base?

What is the pH of a 0.300 M solution of aniline (C₆H₅NH₂, K_b = 4.3 × 10⁻¹⁰)?