What mass of sodium benzoate should be added to 160.0mL of a 0.16M benzoic acid solution in order to obtain a buffer with a pH of 4.25?
Express your answer using two significant figures.
Ka of benzoic acid = 6.3*10^-5
Ka = 6.3*10^-5
pKa = - log (Ka)
= - log(6.3*10^-5)
= 4.201
use formula for buffer
pH = pKa + log ([C6H5COOH]/[C6H5COONa])
4.25 = 4.2007 + log ([C6H5COOH]/[C6H5COONa])
log ([C6H5COOH]/[C6H5COONa]) = 0.0493
[C6H5COOH]/0.16 = 1.1203
[C6H5COOH] = 0.1793
volume , V = 1.6*10^2 mL
= 0.16 L
use:
number of mol,
n = Molarity * Volume
= 0.1793*0.16
= 2.868*10^-2 mol
Molar mass of C6H5COOH,
MM = 7*MM(C) + 6*MM(H) + 2*MM(O)
= 7*12.01 + 6*1.008 + 2*16.0
= 122.118 g/mol
use:
mass of C6H5COOH,
m = number of mol * molar mass
= 2.868*10^-2 mol * 1.221*10^2 g/mol
= 3.502 g
Answer: 3.5 g
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