Malonic acid, H2C3H2O4 (aq), is a diprotic acid, so 2 moles of hydroxide ions are required per mole of malonic acid for complete neutralization. A.) Write the balanced chemical equation for the reaction of malonic acid with potassium hydroxide. B.) Calculate the molar concentration of the malonic acid if 38.17 mL of 0.315 M potassium hydroxide was required to neutralize 25.0 mL of malonic acid to a phenolphthalein end point.   C.) Calculate the mass percent concentration of malonic acid using the molar concentration calculated in part b and assuming the density of the solution is 1.01 g/mL.

H2. Titrations are performed by a scientist in the laboratory as follows: a solution of deuterated hydrochloric acid contains 1.08 g DCl in 750 ml of deionised, distilled water. An average amount of 14.95 ml of the DCl(aq) solution is titrated with 25.0 ml of Ca(OH)2 to produce an endpoint (as determined by an appropriate indicator). What is the molarity of the Ca(OH)2 solution? You must include all of your calculations    Please give typed answer

A 0.261 g sample of NaHC2O4 (one acidic proton) required 17.5 mL of sodium hydroxide solution for complete reaction. Determine the molar concentration of the sodium hydroxide solution.

A 25.00 mL sample of acetic acid (CH3COOH) is titrated to the equivalence using 31.08 mL of 0.1978 M NaOH. What is the balanced neutralization chemical reaction? What is the molarity of the acetic acid in the original sample?