How much hcl must be added to a liter of buffer that is 1. 5 m in acetic acid and 0. 70 m in sodium acetate to result in a buffer ph of 4. 01?]

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01-04-2022
Chemistry

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How much hcl must be added to a liter of buffer that is 1. 5 m in acetic acid and 0. 70 m in sodium acetate to result in a buffer ph of 4. 01?]

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okpalawalter8 okpalawalter8 · Answer 1 · 2022-04-06T05:55:47-04:00

For a liter of a buffer that is 1. 5 m in acetic acid and 0. 70 m in sodium acetate, and with a result in a buffer pH of 4.01, the moles of HCl required is mathematically given as x=0.313mol

What is the result in a buffer ph of 4. 01?

Generally, the equation for the pH is mathematically given as

pH=pKa+logsalt/acid

Generally, the equation for the Chemical Reaction is mathematically given as

HCl+CH3CooNa---->NaCl+CH3OOH

Therefore

4.01=4.74+log\frac{0.8-x}{1.3+x}

-0.52=log\frac{0.8-x}{1.3+x}

x=0.313mol

In conclusion, The moles of HCl required is

x=0.313mol

What is pH?

pH is the potential of hydrogen and is given as,

[tex]\rm pH =\rm pKa + log \dfrac{salt}{acid}[/tex]

The chemical reaction is given as,

[tex]\rm HCl+CH_{3}COONa \rightarrow NaCl+CH_{3}OOH[/tex]

Given,

pH =4.01

pKa = 4.74

Concentration of salt = 0.8 - x

Concentration of acid = 1.3 + x

Substituting values in the pH formula:

[tex]\begin{aligned} 4.01 &= 4.74 + \rm log \dfrac{(0.8 - x)}{ (1.3 + x)}\\\\-0.52 &= \rm log \dfrac{(0.8 - x)}{ (1.3 + x)}\\\\&= 0.313 \;\rm mol\end{aligned}[/tex]

Therefore, 0.313 moles of HCl are needed.

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What is the result in a buffer ph of 4. 01?

What is pH?

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