$\mathrm{Assertion}:$Solubility of $\mathrm{AgBr}$ decreases in the presence of sodium bromide.

$\mathrm{Reason}:$Sodium bromide undergoes hydrolysis in water.

$\mathrm{Assertion}:$ If ${\mathrm{K}}_{\mathrm{sp}}<$ ionic product, precipitate is formed.

$\mathrm{Reason}:$Solubility product $\left({\mathrm{K}}_{\mathrm{sp}}\right)$ is the highest limit of ionic product of the electrolyte in saturated solutions.

Assertion: When an acid or a base is added to water at constant temperature the $\mathrm{pH}$ changes.

Reason: This is due to change in ionic product of water.

$\mathrm{Assertion}:$ For ${\mathrm{H}}_2{\mathrm{SO}}_4, {\mathrm{K}}_{{\mathrm{a}}_1}$ value is much greater than ${\mathrm{K}}_{{\mathrm{a}}_2}$.
$\mathrm{Reason}:$ ${\mathrm{H}}_2{\mathrm{SO}}_4$ is a strong acid.

$\mathrm{Assertion}:$ Solubility of salt of $\mathrm{SB}$ and $\mathrm{WA}$ changes when $\mathrm{pH}$ of the solution is changed.

$\mathrm{Reason}:$ Solubility product $\left({\mathrm{K}}_{\mathrm{sp}}\right)$ depends on $\mathrm{pH}$.

$\mathrm{Assertion}:$$\mathrm{pH}$ of a buffer changes with temperature.

$\mathrm{Reason}:$lonic product of water $\left({\mathrm{K}}_{\mathrm{w}}\right)$ changes with temperature.

$\mathrm{Assertion}:$${\mathrm{H}}_2\mathrm{O}$ is amphoteric in nature.
$\mathrm{Reason}:$${\mathrm{H}}_2\mathrm{O}$ can accept a proton to form ${\mathrm{H}}_3{\mathrm{O}}^{+}$ ion and can donate a proton to form ${\mathrm{OH}}^{-}$ ion.

Assertion: All Arrhenius acids are also Bronsted acids.

Reason: All Bronsted bases are also Lewis bases.

$\mathrm{Assertion}:$ The buffer solution has a capacity to resist the change in $\mathrm{pH}$ value on addition of small amount of acid or base to it.

$\mathrm{Reason}:$ $\mathrm{pH}$ value of buffer solution does not change on dilution or on keeping for long.