how many moles of sodium acetate must be added to 1L of 0.2M acetic acid to make buffer of pH 5.Ka =1.8×10^-5
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Answer:
Applying Henderson's equation
pH=log
[Acid]
[Salt]
−logK
a
log
[Acid]
[Salt]
=4.5+log1.8×10
−5
=−0.2447
[Salt]=0.5692×[Acid]
[Salt]
[Acid]
=0.063
[Acid]=
1.5692
0.063
=0.040M
no of moles =n=0.04×1=0.04mol
[Salt]=(0.063−0.040)=0.023M
no of moles =n=0.023×1=0.023
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