Predict whether the equivalence point of each of the following titrations is below, above, or at pH 7: (a) NaHCO₃ titrated with NaOH (c) KOH titrated with HBr.

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1. Identify the nature of the acid and base involved in each titration. For (a), NaHCO3 is a weak acid (bicarbonate ion acts as an acid) and NaOH is a strong base. For (c), KOH is a strong base and HBr is a strong acid.
2. Understand that the equivalence point pH depends on the strength of the acid and base. In a titration of a weak acid with a strong base, the equivalence point will be above pH 7 due to the formation of a basic salt.
3. For (a), since NaHCO3 is a weak acid and NaOH is a strong base, the equivalence point will be above pH 7. This is because the bicarbonate ion will be converted to carbonate ion, which is basic.
4. For (c), both KOH and HBr are strong, so the equivalence point will be at pH 7. This is because the neutralization of a strong acid with a strong base results in a neutral solution.
5. Summarize the findings: (a) The equivalence point is above pH 7 due to the weak acid and strong base combination. (c) The equivalence point is at pH 7 due to the strong acid and strong base combination.