Monochloroacetic acid, HC₂H₂ C1O₂, is a skin irritant that is used in "chemical peels" intended to remove the top layer of dead skin from the face and ultimately improve the complexion. The value of Ka for monochloroacetic acid is 1.35 x 10-³. Calculate the pH of a 0.12-M solution of monochloroacetic acid.

A chemist must prepare 800.0 mL of potassium hydroxide solution with a pH of 12.30 at 25 °C. He will do this in three steps: ⚫ Fill a 800.0 mL volumetric flask about halfway with distilled water. • Weigh out a small amount of solid potassium hydroxide and add it to the flask. • Fill the flask to the mark with distilled water. Calculate the mass of potassium hydroxide that the chemist must weigh out in the second step. Round your answer to 2 significant digits.

A chemist dissolves 522. mg of pure potassium hydroxide in enough water to make up 120. mL of solution. Calculate the pH of the solution. (The temperature of the solution is 25 °C.) Round your answer to 3 significant decimal places. x10 5

A chemist dissolves 359. mg of pure sodium hydroxide in enough water to make up 110. mL of solution. Calculate the pH of the solution. (The temperature of the solution is 25 °C.) Round your answer to 3 significant decimal places. x10 X Ś

A chemist dissolves 163. mg of pure nitric acid in enough water to make up 360. mL of solution. Calculate the pH of the solution. Round your answer to 3 significant decimal places. 0 x10 X 5

Unit 2: Chemical Systems & Equilibrium Butanoic acid, C3H₂COOH, gives rancid butter its distinctive odour. Calculate the pH of 0.020 mol/L solution of butanoic acid. K₂ = 1.51 x 10-5

A chemist dissolves 204. mg of pure barium hydroxide in enough water to make up 170. mL of solution. Calculate the pH of the solution. (The temperature of the solution is 25 °C.) Round your answer to 3 significant decimal places. 0 x10 X Ś

A chemist dissolves 215. mg of pure sodium hydroxide in enough water to make up 190. mL of solution. Calculate the pH of the solution. (The temperature of the solution is 25 °C.) Round your answer to 3 significant decimal places. ☐ x10 G

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 .

A chemist dissolves 339. mg of pure hydroiodic acid in enough water to make up 180. mL of solution. Calculate the pH of the solution. Round your answer to 3 significant decimal places. Ú x10 ×