The equilibrium constant (K_p) for the decomposition of water is given by:

${\mathrm{H}}_2\mathrm{O}\left(\mathrm{g}\right)\to {\mathrm{H}}_2\left(\mathrm{g}\right)+\frac{1}{2}{\mathrm{O}}_2\left(\mathrm{g}\right)$

Which one of the following is correct option?
[α = degree of dissociation & p = pressure of the reaction mixture at equilibrium]

1. ${\mathrm{K}}_{\mathrm{p}}=\frac{{\mathrm{\alpha }}^3{\mathrm{P}}^{{\displaystyle \frac{1}{2}}}}{\sqrt{2}}$

2. ${\mathrm{K}}_{\mathrm{p}}=\frac{{\mathrm{\alpha }}^3{\mathrm{P}}^{{\displaystyle \frac{3}{2}}}}{(1-\mathrm{\alpha }){(2+\mathrm{\alpha })}^{{\displaystyle \frac{1}{2}}}}$

3. ${\mathrm{K}}_{\mathrm{p}}=\frac{{\mathrm{\alpha }}^3{\mathrm{P}}^{{\displaystyle \frac{1}{2}}}}{(1+\mathrm{\alpha }){(2-\mathrm{\alpha })}^{{\displaystyle \frac{1}{2}}}}$

4. ${\mathrm{K}}_{\mathrm{p}}=\frac{{\mathrm{\alpha }}^{3/2}{\mathrm{P}}^{1/2}}{(1-\mathrm{\alpha }){(2+\mathrm{\alpha })}^{1/2}}$

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 \(HS^-, I^-, RNH_2, \ and\ NH_3\) the 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?

At \(90^\circ \text C,\) pure water has \([H_3O^+]=10^{-6}~\text{mole litre}^{-1}.\) What is the value of \(K_w\) at \(90^\circ \text C?\)
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