Calculate the pH of a 0.0153 M aqueous solution of formic acid (HCOOH, Ka = 1.8×10-4)

Chloroacetic acid, HC 2 H 2 ClO 2 , has a greater acid strength than acetic acid, because the electronegative chlorine atom pulls electrons away from the OOH bond and thus weakens it. Calculate the hydronium ion concentration and the pH of a 0.0020 M solution of chloroacetic acid if Ka is 1.3 * 10 ^ - 3 .

Calculate the pH of a solution prepared by dissolving 0.040 moles of sodium nitrite (NaNO2) in 200 mL of a 0.10 M nitrous acid solution (HNO2, Ka = 5.1 x 10-4).

Calculate the pH of a 0.0325 M hypochlorous acid solution (Ka= 3.0 x 10-8)

The pH of a 0.61 M aqueous solution of HNO2 (Ka = 4.6 × 10–4 at 298 K) is ____.

Calculate the pH of a 0.619 M solution of NaF. The Ka for the weak acid HF is 6.8 × 10-4.

NH3 is a weak base (K, = 1.8 × 10-5) and so the salt NH¼C1 acts as a weak acid. What is the pH of a solution that is 0.088 M in NH,Cl at 25 °C?

Find the pH of a 0.337 M aqueous solution of hydrofluoric acid (HF), for which Ka = 6.8 × 10-4.

Calculate the pH of a solution prepared by dissolving 0.24 mol of benzoic acid (C7H5O2H) and 0.15 mol of sodium benzoate (NaC7H5O2) in water sufficient to yield 1.00 L of solution. The Ka of benzoic acid is 6.50 × 10-5.

Calculate the pH of a solution that is 0.450 M HC2H2O2 and 0.730 M NaC2H3O2. The Ka for acetic acid is 1.80 x 10-5. Does this correspond to an acidic or basic pH?