17. Acid and Base Equilibrium

What is the pH of a solution formed by mixing 140.0 mL of 0.25 M HF with 225.0 mL of 0.31 M NaF, given that the Ka of hydrofluoric acid (HF) is 6.8 x 10^-4?

Calculate the pH at 25°C of a solution prepared by adding 50.0 mL of 1.60 M NaOH solution to 0.500 L of 0.0850 M HC5H3O3. Furoic acid (HC5H3O3) has a Ka value of 6.76×10⁻⁴ at 25°C.

Calculate the pH at 25°C of a 0.21 M solution of a weak acid that has Ka = 9.2 x 10⁻⁶.

Calculate the pH of a 0.03 M aqueous solution of a weak acid, HA, with a pKa of 3.39.

Calculate the pH of a 0.03 M aqueous solution of a weak acid, HA, that has a pKa of 3.39.

What is the pH of a 0.10 M solution of hypochlorous acid (HOCl) given that the acid dissociation constant (Ka) is 3.0 x 10^-8?

Calculate the pH of a 0.300 M NaHCOO solution, given that the Ka for HCOOH is 1.8 x 10^-4.

Calculate the pH of a 0.800 M NaCH3CO2 solution. Ka for acetic acid, CH3CO2H, is 1.8 × 10^-5.

Calculate the pH of a buffer that contains 1.5 M CH3COOH and 1.3 M NaCH3COO. Given that the acid dissociation constant (Ka) for CH3COOH is 1.8 x 10^-5.

What is the percent ionization of a 0.16 M benzoic acid solution in a solution containing 0.28 M sodium benzoate, given that the Ka of benzoic acid is 6.3 x 10^-5?

Consider the titration of 25.00 mL of 0.150 M hydrazoic acid (Ka = 1.90 x 10^-5) with 0.200 M NaOH. (Hydrazoic acid is HN3, not to be confused with ammonia, NH3) What is the pH of the hydrazoic acid solution prior to beginning the titration?

What is the pH of a 0.16 M NH4Cl solution, given that the Kb for NH3 is 1.76 × 10⁻⁵?

What is the pH of a 0.1 M solution of acetic acid (CH3COOH) given that its acid dissociation constant (Ka) is 1.8 x 10^-5?

Determine the pH of a 0.036 M solution of formic acid (HCO2H), given that the acid dissociation constant (Ka) is 1.8 x 10^-4. The dissociation reaction is: HCO2H (aq) ⇌ H+ (aq) + HCO2- (aq).

What is the pH of a 0.461 M benzoic acid (C6H5CO2H) solution if the acid dissociation constant (Ka) is 6.5 x 10^-5?