Which of these can not be a Bronsted acid?

1. ${\mathrm{HCO}}_3^{-}$

2. ${\mathrm{HCOO}}^{-}$

3. ${\mathrm{H}}_2{\mathrm{PO}}_3^{-}$

4. ${\mathrm{H}}_3{\mathrm{O}}^{+}$

In ${\mathrm{HS}}^{-},<mspace\; width="1em"></mspace>{\mathrm{I}}^{-},<mspace\; width="1em"></mspace>{\mathrm{RNH}}_2<mspace\; width="1em"></mspace>\mathrm{and}<mspace\; width="1em"></mspace>{\mathrm{NH}}_3$ order of proton accepting tendency will be:

1. ${\mathrm{I}}^{-}>{\mathrm{NH}}_3>{\mathrm{RNH}}_2>{\mathrm{HS}}^{-}$

2. ${\mathrm{HS}}^{-}>{\mathrm{RNH}}_2>{\mathrm{NH}}_3>{\mathrm{I}}^{-}$

3. ${\mathrm{RNH}}_2>{\mathrm{NH}}_3>{\mathrm{HS}}^{-}>{\mathrm{I}}^{-}$

4. ${\mathrm{NH}}_3>{\mathrm{RNH}}_2>{\mathrm{HS}}^{-}>{\mathrm{I}}^{-}$

Which one of the following orders of acid strength is correct?

1. $\mathrm{RCOOH}>\mathrm{HC}\equiv \mathrm{CH}>\mathrm{HOH}>\mathrm{ROH}$

2. $\mathrm{RCOOH}>\mathrm{ROH}>\mathrm{HOH}>\mathrm{HC}\equiv \mathrm{CH}$

3. $\mathrm{RCOOH}>\mathrm{HOH}>\mathrm{ROH}>\mathrm{HC}\equiv \mathrm{CH}$

4. $\mathrm{RCOOH}>\mathrm{HOH}>\mathrm{HC}\equiv \mathrm{CH}>\mathrm{ROH}$

A centinormal solution of a monobasic acid is 100% ionized. Its pH is:

1. 2

2. 4

3. 3

4. 1

The mixture that can act like a buffer is:

1. ${\mathrm{CH}}_3\mathrm{COOH}<mspace\; width="1em"></mspace>+<mspace\; width="1em"></mspace>{\mathrm{CH}}_3\mathrm{COONa}$

2. ${\mathrm{NH}}_4{\mathrm{NO}}_3+{\mathrm{NH}}_4\mathrm{OH}$

3. $50<mspace\; width="1em"></mspace>\mathrm{ml}<mspace\; width="1em"></mspace>0.1<mspace\; width="1em"></mspace>\mathrm{m}<mspace\; width="1em"></mspace>\mathrm{NaCN}+30<mspace\; width="1em"></mspace>\mathrm{ml}<mspace\; width="1em"></mspace>0.1<mspace\; width="1em"></mspace>\mathrm{m}<mspace\; width="1em"></mspace>\mathrm{HCl}$

4. All of the above

Which one of the following statements is not correct?

1. \(Cl^-\) is a Lewis acid

2. The pH of ${10}^{-8}\mathrm{M}<mspace\; width="1em"></mspace>\mathrm{HCl}$ solution is less than 7

3. The ionic product of water at $25°\mathrm{C}$ is ${10}^{-14}<mspace\; width="1em"></mspace>{\mathrm{mol}}^2<mspace\; width="1em"></mspace>{\mathrm{L}}^{-2}$

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

At $90°\mathrm{C}$, pure water has $\left[{\mathrm{H}}_3{\mathrm{O}}^{+}\right]<mspace\; width="1em"></mspace>{\mathrm{=10}}^{-6}<mspace\; width="1em"></mspace>\mathrm{mole}<mspace\; width="1em"></mspace>{\mathrm{litre}}^{-1}.$ 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