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How much NaOH (in moles) must be added to 1 L of a buffer solution that a 1.8 M in acetic acid and 1.2 M in sodium acetate to result in buffer solution of pH 5.22. Assume volume to remain constant.

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A buffer solution is that solution which resists the change in its pH when small amount of acid or base is added to it. Acetate buffer is composed of weak acid and its salt with strong base in a specific concentration .

As per question, the required pH of buffer is 5.22, concentration of acetic acid = 1.8 M, concentration of sodium acetate = 1.2 MpKa of acetic acid = 1.8 x 10-5, pKa = -log (1.8 x 10-5) = 4.75According to Henderson Hasselbalch equation for acetate buffer,&nbsp;&nbsp;

Let the moles of NaOH to be added = xRequired ratio of [sodium acetate]:[acetic acid] = 2.95As the NaOH added will react with acetic acid to form sodium acetate, [sodium acetate] will increase while [acetic...

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How much NaOH (in moles) must be added to 1 L of a buffer solution that a 1.8 M in acetic acid and 1.2 M in sodium acetate to result in buffer solution of pH 5.22. Assume volume to remain constant.

How much NaOH (in moles) must be added to 1 L of a buffer solution that a 1.8 M in acetic acid and 1.2 M in sodium acetate to result in buffer solution of pH 5.22. Assume volume to remain constant.

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