The pH of 10^-8 M HCl solution is:

• 8

• more than 8

• between 6 and 7

• slightly more than 7

Hydroxyl ion concentration of 10^-2 M HCl is

• 1 × 10¹ mol dm^-3

• 1 × 10^-12 mol dm^-3

• 1 × 10^-1 mol dm^-3

• 1 × 10^-14 mol dm^-3

A ligand can also be regarded as

• Lewis acid

• Bronsted base

• Lewis base

• Bronsted acid

314.

Which one of the following salts on being dissolved in water gives pH > 7 at 25°C?

• KCN

• KNO₃

• NH₄Cl

• NH₄CN

Three moles of PCl₃ three moles of PCl₃, and two moles of Cl, are taken in a closed vessel. If at equilibrium the vessel has 1.5 moles of PCl₅ the number of moles of PCl₃, present in it is

• 5

• 3

• 6

• 4.5

For the reaction $2\mathrm{HI} \left(\mathrm{g}\right)\hspace{0.17em}\rightleftharpoons {\mathrm{H}}_2\left(\mathrm{g}\right) + {\mathrm{I}}_2\left(\mathrm{g}\right)\hspace{0.17em}-\mathrm{Q} \mathrm{kJ}$, the equilibrium constant depends upon

• temperature

• pressure

• catalyst

• volume

N₂ + 3H₂ $\rightleftharpoons$2NH₃ + heat.What is the effect of the increase of temperature on the equilibrium of the reaction? 

• Equilibrium is shifted to the left

• Equtlibriumis shifted to the right

• Equilibrium is unaltered

• Reaction rate does not change

30 cc of $\frac{\mathrm{M}}{3}$, 20 cc of $\frac{\mathrm{M}}{2}$ HNO₃ and 40 cc of $\frac{\mathrm{M}}{4}$ NaOH solutions are mixed and the volume was made up to 1 dm³. The pH of the resulting solution is

• 8

• 2

• 1

• 3

10^-6 M NaOH is diluted 100 times. The pH of the diluted base is

• between 7 and 8

• between 5 and 6

• between 6 and 7

• between 10 and 11

2HI (g) $\rightleftharpoons$ H₂ (g) + I₂ (g)

The equilibrium constant of the above reaction is 6.4 at 300 K. If 0.25 mole each of H₂ and I₂ are added to the system, the equilibrium constant will be

• 6.4

• 0.8

• 3.2

• 1.6