Which one of the following statements is not correct?

1. Cl - is a Lewis acid

2. the pH of ${10}^{-8}\mathrm{M} \mathrm{HCl}$ solution is less than 7.

3. the ionic product of water at $25°\mathrm{C}$ is ${10}^{-14} {\mathrm{mol}}^2 {\mathrm{L}}^{-2}$

4. Bronsted-Lowry theory could not explain the acidic character of ${\mathrm{AlCl}}_3.$

At $90°\mathrm{C}$, pure water has $\left[{\mathrm{H}}_3{\mathrm{O}}^{+}\right] {10}^{-6} \mathrm{mole} {\mathrm{litre}}^{-1}.$ What is the value of ${\mathrm{K}}_{\mathrm{w}}$ at $90°\mathrm{C}$?

1. ${10}^{-8}$

2. ${10}^{-6}$

3. ${10}^{-12}$

4. ${10}^{-14}$

Of the given anions, the strongest bronsted base is

1. ${\mathrm{ClO}}_4^{-}$

2. ${\mathrm{ClO}}_3^{-}$

3. ${\mathrm{ClO}}_2^{-}$

4. ${\mathrm{ClO}}^{-}$

The pH of a ${10}^{-8}$ molar solution of HCl in water is

1. -8

2. 8

3. between 6 and 7

4. between 7 and 8

An acid buffer solution can be prepared by mixing the solutions of:

1. Sodium chloride and sodium hydroxide

2. Sulphuric acid and sodium sulphate

3. Ammonium chloride and ammonium nitrate

4. Ammonium acetate and acetic acid

For the reaction, ${\mathrm{H}}_2\left(\mathrm{g}\right)+{\mathrm{I}}_2\left(\mathrm{g}\right)\leftrightarrow 2\mathrm{HI}\left(\mathrm{g}\right)$ the equilibrium constant K_p changes with

1. Catalyst

2. Temperature

3. Total pressure

4. The amounts of H₂ and I₂ present

The best indicator for detection of end point in titration of a weak acid and strong base is

1. methyl red (5 to 6)

2. methyl orange (3 to 4)

3. phenolphthalein (8 to 9.6)

4. bromothymol blue (6 to 7.5)

The compound that is not a Lewis acid is-

1.  CCl₄ 

2. BeCl₂ 

3. BF₃

4. AlCl₃

The conjugate acid of ${\mathrm{NH}}_2^{-}$ is

1. ${\mathrm{NH}}_4^{+}$

2. ${\mathrm{NH}}_3$

3. ${\mathrm{NH}}_2\mathrm{OH}$

4. ${\mathrm{N}}_2{\mathrm{H}}_4$

The pH of the neutralization point of 0.1 N ammonium hydroxide with 0.1 N HCl is

1. 1

2. 6

3. 9

4. 7