When a base is dissolved in water,it produces a hydroxide ion concentration of $0.05 \ mol/L$. Therefore,this solution will be.......

$0.1 \ (M) \ HCl$ and $0.1 \ (M) \ H_2SO_4$ each of volume $2 \ mL$ are mixed and the volume is made up to $6 \ mL$ by adding $2 \ mL$ of $0.01 \ (N) \ NaCl$ solution. The $pH$ of the resulting mixture is

If the $pH$ of a solution is $2$,its normality will be

Calculate the $pOH$ of $0.10 \ M \ HCl$ solution.

What is the concentration of hydrogen $[H^{+}]$ ions in $0.01 \, M \, HCl$?

$x \ mg$ of $Mg(OH)_2$ (molar mass $= 58 \ g/mol$) is required to be dissolved in $1.0 \ L$ of water to produce a $pH$ of $10.0$ at $298 \ K$. The value of $x$ is $........... mg$ ($Nearest$ $integer$). ($Given$: $Mg(OH)_2$ is assumed to dissociate completely in $H_2O$)