Question

Part A. Calculate the volume lf 0.210-M NaOH solution needed to completely neutralize 89.1 mL of a 0.310-M solution of the diprotic acid H2C2O4

Part B. You wish to make a 0.202 M Hydrochloric acid solution from a stock solution of 3.00 M hydrochloric acid. How much concdntrated acid must you add to obtain a total volume of 50.0 mL of the dilute solution?

Part C. an aqueous solution of barium hydroxide is standarized by titration with a 0.143 M solution of hydrobromic acid. If 12.1 mL of base are required to neutralize 20.2 mL of acid, what is the molarity of the barium hydroxide solution?

Part D. an aqueous solution of nitric acid is standardized by titration with a 0.108 M solution of barium hydroxide. If 22.0 mL of base are required to neutralize 25.9 mL of the acid, what is the molarity of the nitric acid solution?

discard part b .. the question was,

what volume of a 0.143 M barium hydroxide solution is required to neutralize 12.1 mL of a 0.252 M hydrobric acid solution

Answer 1

Part A.

Part B.

Part C.

Part D.