Chemistry, 04.07.2019 08:30, bakerj8395
What volume of 0.307 m naoh must be added to 200.0ml of 0.425m acetic acid (ka = 1.75 x 10-5 ) to produce a buffer of ph = 4.250?
Answers: 1
than hydroxide ions 
. The equilibrium equation shall thus contain protons rather than a combination of water and hydroxide ions as the reacting species.
of the 0.307 
sodium hydroxide solution was added to the acetic acid. Based on previous reasoning, 
is sufficiently small that acetic acid was in excess, and no hydroxide ion has yet been produced in the solution. The solution would thus contain 
moles of acetic acid and 
moles of acetate ions.
denotes an acetic acid molecule and 
denotes an acetate ion. The RICE table below resembles the hydrolysis equilibrium going on within the buffer solution.
. There were no proton in the buffer solution before the hydrolysis of acetic acid. Therefore the table shall have an increase of 
in proton concentration in the third row. Atoms conserve. Thus the concentration increase of protons by 
would correspond to a decrease in acetic acid concentration and an increase in acetate ion concentration by the same amount. That is:
![\text{K}_{a} = [\text{H}^{+}] \cdot [\text{Ac}^{-}] / [\text{HAc}]\\\phantom{\text{K}_{a}} = 10^{-4.250} \times (10^{-4.250} + 0.307 \; x) / (0.085 - 10^{-4.250} - 0.307 \; x)](/tpl/images/0049/5512/989e8.png)
of sodium hydroxide to produce this buffer solution.
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What volume of 0.307 m naoh must be added to 200.0ml of 0.425m acetic acid (ka = 1.75 x 10-5 ) to pr...
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