Prepare 100mL of a 0.2M acetate buffer solution of pH =4.76 (using 17.6N acetic acid and...
Prepare 100mL of a 0.2M acetate buffer solution of pH =4.76 (using 17.6N acetic acid and sodium acetate).
a. Calculate the volume of acetic acid and weight of sodium acetate necessary to prepare the buffer solution. pKa of acetic acid is 4.76
Homework Answers
Answer
Volume of 17.6N acetic acid required = 0.568ml
mass of sodium acetate required = 0.8204g
Explanation
mass of
Henderson-Hasselbalch equation is
pH = pKa + log([A-]/[HA])
4.76 = 4.76 + log( [CH3COO-] / [CH3COOH])
log([CH3COO-]/[CH3COOH]) = 0
[CH3COO-]/[CH3COOH] = 1
[CH3COO-]= [CH3COOH]
buffer concentration = 0.2M
[CH3COOH] = 0.1M
[CH3COO-] = 0.1M
Volume of CH3COOH required = 0.1M × 100ml/ 17.6M = 0.568ml
moles of CH3COO- required =( 0.1/1000ml)× 100ml = 0.01mol
moles of CH3COONa required = 0.01mol
mass of CH3COONa required = 0.01mol × 82.04g/mol
mass of CH3COONa required = 0.8204g
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Prepare 100mL of a 0.2M acetate buffer solution of pH =4.76
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