$A$ weak acid with a dissociation constant of $10^{-5}$ is being titrated with an aqueous $NaOH$ solution. The $pH$ at the point of one-third neutralization of the acid will be:
- A$5 + \log 2 - \log 3$
- B$5 - \log 2$
- C$5 - \log 3$
- D$5 - \log 6$
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The ratio of volumes of $CH_3COOH$ $0.1 \ N$ to $CH_3COONa$ $0.1 \ N$ required to prepare a buffer solution of $pH$ $5.74$ is (Given, $pK_a$ of $CH_3COOH$ is $4.74$)
MediumWBJEE 2015
View SolutionWhich of the following mixtures forms a buffer solution?
Medium
View Solution$A$ solution of $0.1 \ mol$ of $CH_3NH_2$ $(K_b = 5 \times 10^{-4})$ and $0.08 \ mol$ of $HCl$ is diluted to $1 \ L$. The $pOH$ of the resulting solution is $(\log 1.25 = 0.1)$.
The buffer system which helps to maintain the $pH$ of blood between $7.26$ to $7.42$ is:
Buffer solutions have constant acidity and alkalinity because
DifficultAIPMT 2012
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