In the titration of 50.0 mL of 1.0 M methylamine, CH3NH2 (Kb=4.4 x 10-4), with 0.50 M HCl, calculate the pH under the following conditions: after 50.0 mL of 0.50 M HCl has been added at the equivalence point

Determine the mass of solid NaCH₃COO that must be dissolved in an existing 500.0 mL solution of 0.200 M CH₃COOH to form a buffer with a pH equal to 5.00. The value of Ka for CH₃COOH is 1.8 × 10⁻⁵. Based on the information provided, set up a RICE/ICE Table to answer the question. Let x represent the original concentration of CH₃COOH in the water.

4) a) Determine the mass (in grams) of sodium formate that must be added to 1.00 L of 0.180 M formic acid to prepare a buffer with a pH = 3.50. Assume there is no change in volume upon addition of the sodium formate. b) Write the predominant chemical reaction that occurs when 0.050 mol of HClO4 is added to 1.00 L of the buffer prepared in part a and calculate the pH of the solution.

Calculate the pH at the equivalence point in titrating 0.090 M solutions of each of the following with 0.064 M NaOH. (a) hydrochloric acid (HCI) pH = (b) hypolodous acid (HIO), K₂ = 2.3e-11 pH = (c) phenol (HC6H5O), Ka 1.3e-10 PH