BrCH2COOH→BrCH2COO−+H+\space \space \space BrCH_2COOH \to BrCH_2COO^- +H^+ BrCH2COOH→BrCH2COO−+H+
at t=0 c 0 0
at t=T c(1−α)c(1-\alpha)c(1−α) cαc \alphacα cαc\alphacα
Concentration of H+H^+H+ is given by cαc \alphacα
Where α\alphaα is the degree of ionisation.
[H+]=cα=0.1×0.123=1.23×10−2[H^+]=c \alpha =0.1 \times 0.123=1.23 \times 10^{-2}[H+]=cα=0.1×0.123=1.23×10−2 M
pH=−log[H+]=−log[1.23×10−2]=1.91pH=-log[H^+]=-log[1.23 \times 10^{-2}]=1.91pH=−log[H+]=−log[1.23×10−2]=1.91
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