When equal volumes of 0.1 M NaOH and 0.01 M HCl are mixed, the pH of the resulting solution will be:

The pOH of a solution at 25 °C that contains 1×10^-10 M of hydronium ions is:

The pH of a solution made by mixing 50 mL of 0.01 M barium hydroxide solution with 50 mL of H₂O is

The pH of neutral water at $25°\mathrm{C}$ is 7.0. As the temperature increases, ionisation of water increases. However, the concentration of H⁺ ions and OH^- ions is equal. What will be the pH of pure water at 60°C ?

The concentration of hydrogen ion in a sample of soft drink is $3.8$ $\times {10}^{-3}$ $\mathrm{M}$. The  pH of the soft drink will be:

The number of ${\mathrm{H}}^{\oplus }$ ions present in 1 ml of a solution whose pH= 4 , is given as:

($N_A=$ $Avogadro\text{'}s$ $number$)

1. ${10}^{-7}{N}_A$

2. ${10}^{-8}{N}_A$

3. ${10}^{-16}{N}_A$

4. ${10}^{-14}{N}_A$

When 0.1 mol of CH₃NH₂ $({\mathrm{K}}_{\mathrm{b}}=5\times {10}^{-4})$ is mixed with 0.08 mol of HCl and diluted to 1 L, the H⁺ ion concentration in the solution will be :

1. $8\times {10}^{-11}$ $\mathrm{M}$

2. $6\times {10}^{-5}$ $\mathrm{M}$

3. $1.6\times {10}^{-11}$ $\mathrm{M}$

4. $8\times {10}^{-2}$ $\mathrm{M}$

The pH of 0.1 M solution of the following compounds increases in the order of -

1. $\mathrm{NaCl}<{\mathrm{NH}}_4\mathrm{Cl}<\mathrm{NaCN}<\mathrm{HCl}$

2. $\mathrm{HCl}<{\mathrm{NH}}_4\mathrm{Cl}<\mathrm{NaCl}<\mathrm{NaCN}$

3. $\mathrm{NaCN}<{\mathrm{NH}}_4\mathrm{Cl}<\mathrm{NaCl}<\mathrm{HCl}$

4. $\mathrm{HCl}<\mathrm{NaCl}<\mathrm{NaCN}<{\mathrm{NH}}_4\mathrm{Cl}$