A chemistry student needs to standardize a fresh solution of sodium hydroxide. He carefully weighs out 297.mg of oxalic acid H2C2O4 , a diprotic acid that can be purchased inexpensively in high purity, and dissolves it in 250.mL of distilled water. The student then titrates the oxalic acid solution with his sodium hydroxide solution. When the titration reaches the equivalence point, the student finds he has used 127.4mL of sodium hydroxide solution. Calculate the molarity of the student's sodium hydroxide solution. Be sure your answer has the correct number of significant digits

3. Consider the titration Ba(OH)2 (aq) + 2 HNO3 (aq)→ Ba(NO3)2 (aq) + 2 H2O (1).The equivalence point is reached when 18.91 mL of 0.200 M HNO3 is titrated into 25.00 mL of the Ba(OH)2 solution. Calculate the molarity of the Ba(OH)2 solution. Be sure to account for the stoichiometry of the reaction. 4. In a titration of KOH solution, 0.0742 g of KHP is weighed into a flask and dissolved in deionized water. The equivalence point of the titration is reached when 7.05 mL of KOH solution is added to the KHP solution. a) How many moles of KHP are in the solution? b) How many moles of KOH will have to be titrated to neutralize the KHP? c) What is the molarity of the KOH solution?

You have a 39.2 mL sample of hydrochloric acid (HCl) of unknown concentration. A titration is performed with 1.48 M sodium hydroxide (NaOH), and find 3.81 x 10-2 L are required to reach the equivalence point . What is the hydrochloric acid concentration?

An analytical chemist weighs out 0.026 g of an unknown monoprotic acid into a 250 mL volumetric flask and dilutes to the mark with distilled water. She then titrates this solution with 0.0700 M NaOH solution. When the titration reaches the equivalence point, the chemist finds she has added 3.8 mL of NaOH solution. Calculate the molar mass of the unknown acid. Be sure your answer has the correct number of significant digits. g x10 mol