Calculate the number of grams of NaCOOH to be added to 400 mL of a 0.1 M solution of HCOOH to make the pH of the solution equal to 4. Note that the ionization constant of HCOOH is 4-1.74x10 (Na = 23, H = 1, C = 12). , O = 16

What is the pH of a solution that is 0.21 M CH3NH2 (methylamine) and 0.31 M CH3NH3Cl (methylammonium chloride)? (Assume Kw is 1.0 ✕ 10−14.)

What is the concentration of hydroxide ion in a 0.76 M aqueous solution of hydroxylamine, NH2OH? (Assume the value of Kw is 1.0  10-14.)  what is M ? What is the pH ?

Determine the pH of a solution that is 0.50 M in Ch3COOH and 0.75M in NaCH3COO Ka for CH3COOH = 1.8*10^-5

Calculate the pH of a solution containing 0.70 M HC2H3O2 and 0.25 M NaC2H302. The K, for HC,H;0, is 1.8x10-5. pH =

Calculate the pH of a solution that is 0.374 M CH3COOH and 0.489 M CH3COONa. Ka of CH3COOH is 1.8 * 10^-5.

Equal volumes of 0.240 M weak base (Kb=4.0×10−9) and 0.240 M HCl are mixed. Calculate the pH of the resulting solution.

0.653 g of a monoprotic acid (mm = 157 g/mol) is dissolved in water to produce 50.0 mL of a solution with pH = 2.13. Determine the ionization constant of the acid.

The pH of which of the following solutions will decrease by 1.00 pH unit when diluted with water to 10 times its original volume? 0.10 M HCI 0.10 M NAOH 0.10 M CH3COOH 0.10 MCH3COO Na" A mixture of 010 M CH;COOH and 0.10 M CH3COO'Na*

A chemist must prepare 550.0 mL of hydrochloric acid solution with a pH of 1.10 at 25 °C. He will do this in three steps: • Fill a 550.0 mL Vvolumetric flask about halfway with distilled water. • Measure out a small volume of concentrated (9.0M) stock hydrochloric acid solution and add it to the flask. • Fill the flask to the mark with distilled water. Calculate the volume of concentrated hydrochloric acid that the chemist must measure out in the second step. Round your answer to 2 significant digits. OmL Ox10 ?