Find the $pH$ of a solution formed by mixing equal volumes of $0.1 \text{ M}$ sodium propionate and $0.1 \text{ M}$ propionic acid. (Given: The dissociation constant of propionic acid is $K_a = 1.3 \times 10^{-5}$)
- A$4.89$
- B$5.11$
- C$4.11$
- D$5.89$
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$40 \ mL$ of $0.1 \ M$ ammonia solution is mixed with $20 \ mL$ of $0.1 \ M \ HCl$. What is the $pH$ of the mixture? ($pK_b$ of ammonia solution is $4.74$).
MediumAIIMS 2006
View SolutionStudy the following table:
Buffer Solution Volume (in $mL$) of $0.1 \ M$ Weak acid Volume (in $mL$) of $0.1 \ M$ sodium salt of weak acid $I$ $4.0$ $4.0$ $II$ $4.0$ $40.0$ $III$ $40.0$ $4.0$ $IV$ $0.1$ $10.0$
Which of the two sets of buffer solutions have the least $pH$?
| Buffer Solution | Volume (in $mL$) of $0.1 \ M$ Weak acid | Volume (in $mL$) of $0.1 \ M$ sodium salt of weak acid |
|---|---|---|
| $I$ | $4.0$ | $4.0$ |
| $II$ | $4.0$ | $40.0$ |
| $III$ | $40.0$ | $4.0$ |
| $IV$ | $0.1$ | $10.0$ |
Which of the two sets of buffer solutions have the least $pH$?
DifficultTS EAMCET 2004
View SolutionWhich of the following will form a basic buffer solution?
$100 \ mL$ of a solution contains $0.1 \ M$ $NH_4OH$ and $0.1 \ M$ $NH_4Cl$. The $pH$ of the solution will not change on adding :-
Difficult
View SolutionCalculate the $pH$ of a buffer solution containing $6.1 \times 10^{-2} \ M$ sodium acetate $(CH_3COONa)$ in $1 \ L$ of $0.1 \ M$ acetic acid $(CH_3COOH)$ solution. (Given: $pK_a$ of $CH_3COOH = 4.76$)
Difficult
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