pH Scale

The hydrogen ion concentration of a solution with $\mathrm{pH}$ value $3.69$ is given by

When rain is accompanied by a thunderstorm, the collected rain water will have $\mathrm{pH}$ value

How many times a $0.1 M$ strong monobasic acid solution should be diluted so that pH of the resulting solution is tripled?

Find the $\mathrm{pH}$ of the solution, when $100 \mathrm{mL}$ of $0.10 \mathrm{M}$ $\mathrm{NaOH}$ is mixed with $100 \mathrm{ml}$ of $0.05 \mathrm{M}$ ${\mathrm{CH}}_3\mathrm{COOH}$ solution. 

$40\mathrm{ }\mathrm{mL}$ of oxalic acid reacts with $16\mathrm{ }\mathrm{mL}$ of $0.05\mathrm{M}$ acidified ${\mathrm{KMnO}}_4.$ What is the $\mathrm{pH}$ of $\mathrm{‘}\mathrm{x}\mathrm{’}$ M oxalic acid solution? (Assume that oxalic acid dissociates completely).

On mixing x ml of ${\mathrm{H}}_2\mathrm{O}$, the  $\mathrm{p}\mathrm{H}$ of $1\mathrm{ }\mathrm{m}\mathrm{l}$ of a strong monobasic acid increases by 1 unit .  The value of $\mathrm{x}$ is:

What is the pH of ${10}^{–10}$ M NaOH solution?

What is the $pH$ of ${10}^{–4} M H_{2}S{O}_4$?

When $50\mathrm{ }\mathrm{m}\mathrm{l}$ solution of $\mathrm{p}\mathrm{H}=1$ is mixed with a $50\mathrm{ }\mathrm{m}\mathrm{l}$ solution of $\mathrm{p}\mathrm{H}=2$ than the $\mathrm{p}\mathrm{H}$ of the resultant solution will be nearly -

For the ionisation reaction-
${{\text{RNH}}_2}_{\left(\text{g}\right)}+{\text{H}}_2{\text{O}}_{\left(\mathit{\text{l}}\right)}\rightleftharpoons {{\text{RNH}}_3^{+}}_{\left(\text{aq}\right)}+{{\text{OH}}^{-}}_{\left({\text{aq}}_{}\right)}{\text{ K}}_{eq}{\text{= 8 x 10}}^{\text{-6 }}$ 
 Find the pH of a solution at equilibrium when pressure of RNH₂(g) is 0.5 bar :

$0.08$ mole of $\mathrm{HCl}$ is mixed with $0.1$ mole of ${\mathrm{CH}}_3{\mathrm{NH}}_2\left({\mathrm{K}}_{\mathrm{b}}=5\times {10}^{-4}\right)$ and diluted to one litre. What will be the ${\mathrm{H}}^{+}$ concentration in the solution?

What is the $\mathrm{pH}$ of a solution produced, when an aqueous solution of $\mathrm{pH}=6$ is mixed with an equal volume of an aqueous solution of $\mathrm{pH}=3$?

A solution of $\mathrm{HCl}$ has $\mathrm{pH}=3.$ If one $\mathrm{ml}$ of it is diluted to $1 \mathrm{litre}$, the $\mathrm{pH}$ of the resulting solution will be:

Find the pH of the solution containing $5 \mathrm{mL}$ of $\mathrm{HCL}$ with molarity $\frac{1}{5} \mathrm{M}$ and $10 \mathrm{mL}$ of $\mathrm{NaOH}$ with molarity $\frac{1}{10} \mathrm{M}$: 
 

A decinormal solution of ${\mathrm{NH}}_4\mathrm{OH}$ is $20\mathrm{\%}$ ionized. Find the $\mathrm{pH}$ of the solution.

An aqueous solution of NaOH having density $1.1 \mathrm{kg} / \mathrm{dm}^{3}$ contains 0.02 mole fraction of $\mathrm{NaOH}$ :

The pH of $\mathrm{NaOH}$solution is

A sparingly soluble salt gets precipitated only when the product of concentration of its ions in the solution becomes greater than its solubility product. If the solubility of BaSO₄ in water is 8 × 10^-4 mol dm^-3, if its solubility in 0.01 mol dm^-3 of H₂SO₄ is Y x 10^-5 M. Find X.

The pH of a solution which is three times as acidic as pure water is

What is the pH of a resultant solution produced, when an aqueous solution of $\mathrm{p}\mathrm{H}$ = 6 is mixed with an equal volume of an aqueous solution of $\mathrm{p}\mathrm{H}$ = 3.