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Consider the titration of a 38.0 ml sample of 0.175 mol/L HBr with 0.205 mol/L KOH. The pH at the equivalence point.

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Final answer:

The equivalence point pH for a titration between a strong acid and a strong base is 7.00, as they completely neutralize each other.

Step-by-step explanation:

The question involves determining the pH at the equivalence point of a titration between a strong acid, hydrobromic acid (HBr), and a strong base, potassium hydroxide (KOH). To find the pH at the equivalence point for the titration of a strong acid with a strong base, we know that the solution will be neutral, thus having a pH of 7.00. This is because the hydroxide ions (OH-) from the KOH will completely neutralize the hydrogen ions (H+) from the HBr, forming water (H2O).The pH at the equivalence point in the titration of a strong acid with a strong base is 7.00. This is because at the equivalence point, equal amounts of acid and base have reacted and formed water, resulting in a neutral solution. Therefore, the pH of the solution will be 7.00.

User Sam Ritchie
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