IS 11-15, Refer to the titration curve below for questions through )4 5.0 11. Th

Question

IS 11-15, Refer to the titration curve below for questions through )4 5.0 11. The titration curve shown above describes the (a) titration of a diprotic acid. (b) titration of a monoprotic base. (c) titration of a diprotic base. (d) titration of a monoprotic acid. the titration began with 100.0 mL of solution (before titrant was added) and the 12. If titrant is 0100 M strong acid or base, what is the concentration of analyte in the origthal solution? (a) 1.00 M(b) 0.100 M ( 0.0100 M (d) 0,00100 M 13. What is pKai for the conjugate acid of the analyte? a) 7.0(b) 11.0 () 4.4 (d) 8.8 14 At the first equivalence point in the titration curve above, the pH can be determined by assuming there is (a) a weak base in solution. (b) a weak acid in solution. (c) a buffer with HA and (d) a solution of the intermediate in the form of HA

Explanation / Answer

11.

When no titrant is added pH > 7, so it is a base.

There are two equivalence points on the curve, it is diprotic.

Option (c)

12.

We observe that equivalence point occurs for each 10 mL of titrant added.

M1 V1 = M2 V2

Molarity of analyte in original solution, M2 = 0.01 M

Option (c)

13.

At half of equivalence point = 5 mL

pOH = pKb1

or pH = pKa1 of conjugate acid

At 5 mL, pH = 11 = pKa1 of conjugate acid.

14.

At first equivalence point of a base (say B(OH)2), we have BOH+ in the solution.

We can assume it is a weak base in solution to determine pH.

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