Given i) 10 ml 5% acetic acid sln ii) 10 ml 5% acetic acid sln mixed with 30 ml

Question

Given

i) 10 ml 5% acetic acid sln

ii) 10 ml 5% acetic acid sln mixed with 30 ml water

1. What is the equivalence point volume for each when titrated with 0.2 M NaOH?

2. What is the pH of the equivalence point of the two solutions if you titrate with 0.3 M NaOH?

I'm really unsure of my answer, for 1, wouldn't you add the same amount, 40 ml, of NaOH to either solution because the equivalance point is simply when there are equal moles?

for 2i, i did the two ice boxes, set my final equation, kw/ka=kb=x^2/.22M and got pH = 9, but again, am really unsure.

Thank you for your help!

Explanation / Answer

the basic concept is that we have to equate the equivalent of acid = equivalent of base

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