Calculate the pH

What is the pH of a solution containing 0.30 M lactic acid (K₂ = 1.38 x 10-4) and 0.50 M of lactate ion?

Calculate the pH of a 0.100 M solution of lactic acid, for which the Ka value is 1.40 x 10-4.

What is the pH of a solution containing 1.50 M Acetic acid (CH3COOH) (Ka = 1.8 X 10-5) and 2.5 M sodium acetate (NaCH3COO)?

Chloroacetic acid (chemical formula ClCH2CH2COOH) is a weak acid with Ka = 6.3 x 10-5. Calculate the pH of a buffer solution composed of 1.34 MClCH2CH2COOH and 1.58 M ClCH2CH2COO−.?

In a biochemistry laboratory, you are asked to prepare a buffer solution to be used as a solvent for isolation of an enzyme. On the shelf are the following solutions, all 1.00 M: formic acid (Ka = 1.8 × 10-4), acetic acid (Ka = 1.8 × 10-5), sodium formate (NaHCO2), and sodium acetate (NaCH3CO2). Describe how you would prepare 1.0L of a pH = 4.56 buffer solution with total molarity of 0.20 M. Mix together i g of sodium acetate i Lof 1.0 M acetic acid acid, and enough water to make 1.0 L.

Calculate the pH of the solution that results when 15.0 mL of 0.1600 M lactic acid (Ka(CH3 CHOHCOOH) = 1.38 × 10 : 10-4) is a. diluted to 55.0 mL with distilled water. pH = b. mixed with 40.0 mL of 0.0600 M NaOH solution. pH = c. mixed with 40.0 mL of 0.120 M NaOH solution. pH = d. mixed with 40.0 mL of 0.120 M sodium lactate solution. pH =

A solution is prepared at 25 °C that is initially 0.69M in dimethylamine ((CH3)2NH), a weak base with K = 5.4 × 10-4, and 2.4M in dimethylammonium ((CH3)2NH₂CI). Calculate the pH of the solution. Round your answer to 2 decimal places. chloride pH = ☐

The ionization constant of a very weak acid, HA, is 1.9x10-9. Calculate the equilibrium concentrations of H30", A", and HA in a 0.040 M solution of the acid. Determine the concentrations of all species at equilibrium and the solution pH. [H3O"] =| mol/L [A'] =[ mol L [HA] = | mol L pH =

What is the pH for a weak monoprotic acid if a 0.020 M solution of the acid has a Ka of 3.28 x 10-7 ?