Question

1. I mixed 20 mL of .1M CH₃COOH + 20 mL of .1M NaCH₃CO

2. I measured out the 10 mL of my buffer into a vial and measured the pH of my buffer solution to be 4.95.

From there does that mean from my 10 mL of buffer, my moles of acid is 1.12x10^-5M and my moles of base from 10.0 mL of buffer is 8.91x10^-10M?

I got 1.12x10^-5M and 8.91x10^-10M from this:

1. I mixed 20 mL of .1M CH3COOH + 20 mL of .1M NaCH3CO 2. I measured out the 10 mL of my buffer into a vial and measured the pH of my buffer solution to be 4.95. From there does that mean from my 10 mL of buffer, my moles of acid is 1.12x10-5M and my moles of base from 10.0 mL of buffer is 8.91x10-10M? I got 1.12x10-5M and 8.91x10-10M from this: I'm just wondering if these steps are correct.And how would I find the Ka value? I thought I would have to do this:

$14-4.95= 9.05--> 10^{-9.05}=8.91\times 10^{-10}$

And how would I find the K_a value? I thought I would have to do this:

$\frac{(8.91\times 10^{-10})^{2}}{1.12\times 10^{-5}}$ $\frac{(8.91\times 10^{-10})^{2}}{1.12\times 10^{-5}}= 7.09\times 10^{-14}=K_{a}$

I'm just wondering if these steps are correct.

Answer 1

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