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?

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).

Determine the pH of a buffer solution prepared by dissolving 0.20 mol of formic acid (HCHO) and 0.80 mol of sodium formate (NaCHO) in enough water to make 1.0 L of solution. The pKa of formic acid is 3.75.

What is the pH of a 0.10 M solution of H₂SO₃, given that its pKₐ is 1.77 and the change in concentration is small?

What is the pH of the solution when 20.00 mL of 0.1563 M aniline hydrochloride (C6H5NH3+Cl-) is titrated with 15.00 mL of 0.1249 M NaOH? (Ka for aniline = 2.40 x 10^-5)

What is the pH of a 0.090 M H2CO3 solution, given that the first dissociation constant (Ka1) is 4.3×10^-7 and the second dissociation constant (Ka2) is 5.6×10^-11?