# Which of the following mixtures will form a buffer solution?

## Which of the following mixtures will form a buffer solution: $a .$ ${H}_{2} S {O}_{4} \left(a q\right)$ and $N a O H \left(a q\right)$ $b .$ ${H}_{3} P {O}_{4}$ and $N a H C {O}_{3} \left(a q\right)$ $c .$ ${H}_{3} C - C {O}_{2} H \left(a q\right)$ and and half an equiv of $N a O H$. $d .$ $N {H}_{4}^{+}$ and and half an equiv of $N a O H$?

Mar 6, 2017

$\text{A buffer solution is formed when appreciable............}$

#### Explanation:

A buffer solution is formed when appreciable quantities of a weak acid and its conjugate base are mixed together in aqueous solution. A buffer acts to resist GROSS changes in $p H$.

So looking at your list, $a .$ has strongish acid, strong base;

$b .$ strongish acid, weak base;

$c .$ weak acid, and a half equiv strong base;

$d .$ weak acid, and a half equiv strong base.

Solutions $c .$ and $d .$ will form a buffer.

Their $p H$ will be given by the buffer equation:

$p H = p {K}_{a} + {\log}_{10} \left(\frac{\left[{A}^{-}\right]}{\left[H A\right]}\right)$

For more of the same on buffers, see this link.