The addition of small amounts of either acid or base to a buffer solution causes only small changes in $pH$ because the buffer solution
- ADoes not contain either $H_3O^{+}$ or $OH^{-}$
- BContains large amounts of both $H_3O^{+}$ and $OH^{-}$
- CReacts with the added acid or base
- DContains a strong acid and the salt of the same strong acid
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MediumNEET 2022
View SolutionWhich of the following would produce a buffer solution when mixed in equal volumes?
Which of the following mixtures is called an acidic buffer?
Medium
View SolutionAqueous solutions of $HNO_3$,$KOH$,$CH_3COOH$,and $CH_3COONa$ of identical concentrations are provided.
The pair$(s)$ of solutions which form a buffer upon mixing is(are):
$A$. $HNO_3$ and $CH_3COOH$
$B$. $KOH$ and $CH_3COONa$
$C$. $HNO_3$ and $CH_3COONa$
$D$. $CH_3COOH$ and $CH_3COONa$
The pair$(s)$ of solutions which form a buffer upon mixing is(are):
$A$. $HNO_3$ and $CH_3COOH$
$B$. $KOH$ and $CH_3COONa$
$C$. $HNO_3$ and $CH_3COONa$
$D$. $CH_3COOH$ and $CH_3COONa$
What will be the change in $pH$ by adding $0.1 \ M \ NH_4Cl$ to $0.1 \ M \ NH_4OH$ (weak base) solution? (Given: $K_b$ of $NH_4OH = 1.77 \times 10^{-5}$)
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