17. Acid and Base Equilibrium

What is the pH of a solution of 0.20 M HNO2 containing 0.10 M NaNO2 at 25°C, given the Ka of HNO2 is 4.5 × 10⁻⁴?

What is the pH of a solution that contains 0.200 M HF and 0.200 M HCN, given that the Ka of HF is 3.5 x 10^-4 and the Ka of HCN is 4.9 x 10^-10?

What is the pH of the buffer prepared by mixing 200 mL of 0.15 M HNO2 (Ka = 4.0 x 10^-4) and 150 mL of 0.10 M sodium nitrite?

What is the percent dissociation of glycine if the solution has a pH of 8.60 and a pKa of 9.60?

What is the ratio of HCO₃⁻ to H₂CO₃ in blood with a pH of 7.4?

What is the pH of a 0.050 M solution of HNO2 (Ka = 4.6 × 10⁻⁴)?

What is the pH of a 0.050 M solution of HNO2 (Ka = 4.6 × 10^-4)?

At what pH is the side chain of lysine 35% ionized?

Calculate the pH of a 0.250 M CH3NH3I solution, given that the Kb for CH3NH2 is 4.4 x 10^-4.

Consider a 1.0 M solution of a hypothetical weak acid HA whose pKa is 11. Calculate the pH of this solution.

At what pH will alanine exist predominantly in its zwitterionic form, where it is overall uncharged?

What is the pH of a 0.115 M hydrogen chromate ion (HCrO₄⁻) solution, given that the Ka of HCrO₄⁻ is 3.2 x 10⁻⁷?

What is the pH of a 0.040 M solution of benzoic acid, given that the acid dissociation constant (Ka) for benzoic acid is 6.3 x 10^-5?