Which of the following solutions does not act | vedclass

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(C) buffer solution is a mixture of a weak acid and its conjugate base (acidic buffer) or a weak base and its conjugate acid (basic buffer).$H_3PO_4 +

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$NH_4Cl + HCl$

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(C) buffer solution is a mixture of a weak acid and its conjugate base (acidic buffer) or a weak base and its conjugate acid (basic buffer).$H_3PO_4 + NaH_2PO_4$ is a mixture of a weak acid and its salt,which forms an acidic buffer.$NaHCO_3 + H_2CO_3$ is a mixture of a weak acid and its salt,which forms an acidic buffer.$CH_3COOH + CH_3COONa$ is a mixture of a weak acid and its salt,which forms an acidic buffer.$NH_4Cl + HCl$ consists of a weak base salt $(NH_4Cl)$ and a strong acid $(HCl)$. $A$ mixture of a strong acid and a salt of a weak base does not form a buffer solution.

Which of the following solutions does not act as a buffer?

Similar Questions

An acidic buffer solution is prepared by mixing a proportionate quantity of

The $pH$ of a buffer solution obtained by mixing $50 \ mL$ of $0.1 \ M$ $NH_4OH$ and $25 \ mL$ of $2.0 \ M$ $NH_4Cl$ is ($pK_b$ of $NH_4OH$ is $4.8$).

$A$ buffer solution of $100 \ mL$ has a $pH$ value of $4$. When $1 \ mL$ of dilute $HCl$ is added to it,what happens to the $pH$ of the buffer solution?

What is the value of $[H^{+}]$ when $0.1 \ mol$ of $CH_3NH_2$ is mixed with $0.08 \ mol$ of $HCl$? Given $K_b = 5 \times 10^{-4}$.

Which of the following would produce a buffer solution when mixed in equal volumes?

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