Determine the pH of a solution that is 0.15 M CH3COOH and 0.10 M CH3COONa.

The pH of an aqueous solution of 0.0997 M sodium nitrite, NaNO2, is | (Assume that Ka (HNO₂) = 4.50 × 10−4 .) This solution is

A solution is prepared that is initially 0.087 M in benzoic acid (HC6H5CO2) and 0.11 M in potassium benzoate (KC6H5CO2). Complete the reaction table below, so that you could use it to calculate the pH of this solution. User to stand for the unknown change in [H3O+] You can leave out the M symbol for molarity

Determine the pH of the molecules given in a 1L beaker containing 0.035M solution of the given molecule:  NaNO2,  C6H5CHCOOH, Ba(OH)2. (C6H5CHCOOH, Ka=6.3 x 10^-5, HNO2 Ka= 4.5 x 10^-4, CH3NH2, Kb= 5.0 x 10^-4).

(a) What is the pH of 0.75 M NaF?(b) What is the pH of 0.88 M pyridinium chloride, C₅H₅NHCl?

Given that Ka’s for hydrofluoric acid (HF) and boric acid (H3BO3) are 6.3 × 10^–4and 5.4 × 10^–10, respectively, calculate the pH of the following solutions: (a)The mixture from adding 50 mL 0.2 M HF to 50 mL 0.5 M sodium borate (NaH2BO3).  (b)The mixture from adding an additional 150 mL 0.2 M HF to the solution in (a), i.e., a total of 200 mL 0.2 M HF was added to 50 mL 0.5 M NaH2BO3.

What volume of water must be added to a 26.33 mL solution of a pH = 1.17 solution of HClO4 to raise the pH to 3.53?

The pH of an aqueous solution of 0.458 M pyridine (a weak base with the formula C5H5N) is ?

a) Write the formula for the conjugate base of HPO,2 b) Write the formula for the conjugate acid of NH;

A 100.mL of 0.250 M HNO2 is added to 200.mL of 0.100 M NaNO2. What is the concentration of HNO2 and NaNO2 once two solutions are mixed? What is the pH of this solution? Write a balanced equations showing what happens when NaOH is added, and when HCl is added to solution (b). What is the CHANGE in pH when 50.0 mL of 0.15 M NaOH have been added to solution (b)? What is the CHANGE in pH when 50.0 mL of 0.15 M HCl have been added to solution (b)?