In a titration of 73.0 mL of a 0.500 M solution of a diprotic acid HC,H,O, (malonic acid) with 0.255 M NaOH, how many grams of NaOH are required to reach the second equivalence point? (MW_NaOH = 39.997 g/mol)

If you are going to prepare 100 ml each of the following two (2) buffers: • Buffer 1 will have a concentration of 0.2 M and a pH of 4.4 • Buffer 2 will have a concentration of 0.15 M and a pH of 8.9The buffering systems available to you are • dihydrogen phosphate/ hydrogen phosphate pKa= 6.8 • Tris-HCl/ Tris base pKa = 8.1 • acetic acid/ acetate pKa =4.8 What buffering system would you use for buffer 1 and buffer 2? why?

Aspirin (C 9H 8O 4) is a weak monoprotic acid (K a = 3.3 x 10-4). You are analyzing a samplefor a pharmaceutical company with a quantitative titration and dissolve 10 tablets, eachcontaining 200 mg of aspirin, in 150 mL of water.a) Determine the pH of this solution.b) Determine the pH of the solution after you have added 20.0 mL of 0.500 M NaOH.

When 30 .00 mL of 0.1011 M HCl in 50 mL of deionized water is titrated against 0.09889 M NaOH, the pH increases. What is the volume (in mL) of NaOH required to reach the equivalence point and a pH of 7.00? Find the pH when the volume of NaOH added is 0.02 mL less than the volume required to reach the equivalence point. Find the pH when the volume of NaOH added is 0.01 mL less than the volume required to reach the equivalence point. Find the pH when the volume of NaOH added is 0.02 mL more than the volume required to reach the equivalence point. Comment on the significance of the changes in pH values in relation to the increments of sodium hydroxide added when going “through” the end point. Define equivalence point. For a weak base/strong acid titration, is the pH at the equivalence point <, >, or equal to 7?