After 50.0 mL of a 0.100 M solution of NaOH is added to 50.0 mL of a 0.100 M sol

Question

After 50.0 mL of a 0.100 M solution of NaOH is added to 50.0 mL of a 0.100 M solution of an unknown acid, equilibrium pH is basic. What may be concluded about the identity of the acid? The acid can only be a strong monoprotic acid. The acid can only be a weak monoprotic acid. The acid must be a strong acid, but could be either monoprotic, diprotic. or polyprotic. The acid must be a weak acid, but could be either monoprotic, diprotic, or polyprotic. The acid could be either a strong or weak acid, and could be either a monoprotic, diprotic, orpolyprotic acid

Explanation / Answer

Ans option b the acid must be a weak monoprotic acid.

Given that the volume and molarity of acid and base is same, the acid must be monoprotic because even the base has an acidity of 1. But the equilibrium is basic, which suggests that it should be weak

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