Titrations of Diprotic and Polyprotic Acids

For the following polyprotic acid questions: Citric acid (H3C6H5O6)          K a1 = 8.4 x 10–4            K a2 = 1.8 x 10–5            K a3 = 4.0 x 10–6 Oxalic acid (H2C2O4)             K a1 = 6.5 x 10–2            K a2 = 6.1 x 10–5Sketch a titration curve of the complete titration oxalic acid with NaOH. Label the important points on the curve and list the dominant species present at each of these points.

What anion is present at the first equivalence point in the titration of H  3PO4 with NaOH?a. H2PO4-b. HPO42-c. PO43-d. PO33-e. P3-

Match the following descriptions of titration curves with the diagrams.strong base added to poly-protic acid

On the polyprotic weak acid/strong base titration curve below, label the following points. a) The point where the pH corresponds to a solution of H2A in water. b) The point where the pH corresponds to a solution of HA- in water. c) The point where the pH corresponds to a solution of A2- in water. d) The point where pH = pKa1. e) The point where pH = pKa2.

The following plot below shows a titration curve for the titration of 1.00 L of 1.00 M diprotic acid H2A with NaOH. Which point(s) a-d represent(s) the H 2X/HX - buffer region?(a) point a(b) point b(c) point c(d) point d(e) points a and c

This is the pH curve for titration of a triprotic acid with NaOH.Only the first two equivalence points can be observed. What is the most likely identity of the acid?Refer to the pKa values provided below.Answer Choices:A. ascorbic acidB. citric acidC. phosphoric acidD. telluric acid

The flask shown here contains 0.365 g of acid and a few drops of phenolphthalein indicator dissolved in water. The buret contains 0.220 M NaOH. What volume (mL) of base is needed to reach the end point of the titration? What is the molar mass (g/mol) of the acid (assuming it is diprotic and that the end point corresponds to the second equivalence point)?

Consider these three titrations: (i) the titration of 25.0 mL of a 0.100 M monoprotic weak acid with 0.100 M NaOH (ii) the titration of 25.0 mL of a 0.100 M diprotic weak acid with 0.100 M NaOH (iii) the titration of 25.0 mL of a 0.100 M strong acid with 0.100 M NaOH Which of the following statements is true? All three titrations have the same pH at their first equivalence point.All three titrations require the same volume of NaOH to reach their first equivalence point. All three titrations have the same the initial pH. 

Enter your answer in the provided box. If 29.11 mL of a standard 0.4926 M NaOH solution is required to neutralize 47.58 mL of H  2SO4, what is the molarity of the acid solution?

You are given solutions of HCl and NaOH and must determine their concentrations. You use 67.9 mL of NaOH to titrate 100. mL of HC1 and 32.5 mL of NaOH to titrate 50.0 mL of 0.0782 M H2SO4. Find the unknown concentrations. 

What is the molarity of a solution that contains 0.958 g of H 3PO4 in 140. mL of solution? How many milliliters of this solution could be completely neutralized by 10.59 mL of 0.449 M NaOH? 

If 32.0 mL of a 0.166 M NaOH solution is required to titrate 16.5 mL of a solution of H2SO4, what is the molarity of the H2SO4 solution? H2SO4 (aq) + 2NaOH (aq) → 2H2O (l) + Na2SO4 (aq) Express your answer with the appropriate units.