Answer to Question #133441 in General Chemistry for hi

Question #133441
A buffer solution is 0.20M in acetic acid and in sodium acetate. Calculate the change in pH up on adding 1.0ml of 0.10M HCl acid to 10 ml of this solution
1
Expert's answer
2020-09-17T07:16:44-0400

The ICE approach for the equilibrium yields;

CHCO2H+H2OH3O++CH3CO2CHCO_2H+H_2O \leftrightharpoons H_3O^{+}+CH_3CO_2^-

The initial concentration of CH3CO2HCH_3CO_2H =0.20=0.20

Change =x=x

Equilibrium concentration=0.20x= 0.20-x

The initial concentration of CH3CO2CH_3CO_2^-

.=0.20=0.20

Change=x=x

Equilibrium concentration=0.20+x= 0.20+x

Substituting the equilibrium concentration terms into the KaK_a expression, assuming xx\lll 0.200.20 and solving the simplified equation for xx yields

x=1.8×105x= 1.8\times 10^{-5}

[H3O+]=0+x=1.8×105[H_3O^+]=0+x=1.8\times 10^{-5} pH=log[H3O+]=log(1.8×105M)=4.74pH=-log [H_3O^+]=-log (1.8\times 10^{-5}M)=4.74



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