Assume that 30.0 mL of a 0.10 M solution of a weak base B
that ac...

Question

Assume that 30.0 mL of a 0.10 M solution of a weak base B
that accepts one proton is titrated with a 0.10 M solution
of the monoprotic strong acid HA. (c) Is the pH 7, less than 7, or more than 7 at the equivalence point?

Accepted Answer

Hello everyone today, we're at the following problem when at 12.5 mL of 0.125 moller weak base B is tight, traded with 0.125 molar of a mono product. Strong acid H A is the PH at the equivalence point less than equal to or greater than seven. So first, we're gonna show what this reaction looks like. We have our B or a base being added to our acid and this is going to form our base with a proton or the hydrogen ion and our subsequent acid. So at the equivalence point, when we add a mono product, strong acid mono product meeting, we just have one proton or one H. Adam, this is going to completely neutralize the weak base. So we can say that the moles of B are going to equal the moles of H A or acid. And so the mixture is going to be left with a conjugate acid, which is our B H. And ultimately, we can conclude that the PH is going to be less than seven. And so once again, when we have a weak base and a strong acid, you can think of it as if we have a week and a strong, which would win out and it's going to be a strong. And so in this case, it's a strong acid. So the solution is going to be overall acidic, which means having a ph less than seven. And with that, we've answered the question overall, I hope this helped. And until next time.

Assume that 30.0 mL of a 0.10 M solution of a weak base B that accepts one proton is titrated with a 0.10 M solution of the monoprotic strong acid HA. (c) Is the pH 7, less than 7, or more than 7 at the equivalence point?

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