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Chapter 17: Problem 38

Predict whether the equivalence point of each of the following titrations is below, above, or at pH 7: (a) benzoic acid titrated with KOH, (b) ammonia titrated with iodic acid, (c) hydroxylamine with hydrochloric acid.

Short Answer

Expert verified
In summary, for the given titrations: (a) Benzoic acid (a weak acid) with KOH (a strong base) results in an equivalence point above pH 7. (b) Ammonia (a weak base) with iodic acid (a strong acid) results in an equivalence point below pH 7. (c) Hydroxylamine (a weak base) with hydrochloric acid (a strong acid) results in an equivalence point below pH 7.

Step by step solution

01

Titration (a) Benzoic acid with KOH

In this case, we have a weak acid (benzoic acid) titrated with a strong base (KOH). According to case 2 mentioned in the analysis, the equivalence point will be above pH 7.
02

Titration (b) Ammonia with iodic acid

Here, we have a weak base (ammonia) titrated with a strong acid (iodic acid). This corresponds to case 3 in the analysis, meaning the equivalence point will be below pH 7.
03

Titration (c) Hydroxylamine with hydrochloric acid

In this titration, we have a weak base (hydroxylamine) being titrated with a strong acid (hydrochloric acid). This is again in line with case 3 mentioned in the analysis, so the equivalence point will be below pH 7. In conclusion: - The equivalence point of titration (a) is above pH 7. - The equivalence point of titration (b) is below pH 7. - The equivalence point of titration (c) is below pH 7.

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Most popular questions from this chapter

How many milliliters of \(0.0750 \mathrm{M} \mathrm{KOH}\) are required to titrate each of the following solutions to the equivalence point: \((\mathbf{a}) 30.0 \mathrm{~mL}\) of \(0.0900 \mathrm{M} \mathrm{HCOOH},\) (b) \(45.0 \mathrm{~mL}\) of \(0.0750 \mathrm{M} \mathrm{HNO}_{3},\) (c) $50.0 \mathrm{~mL}\( of a solution that contains \)3.00 \mathrm{~g}\( of \)\mathrm{HBr}$ per liter?

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