The specific conductance (K) of 0.02 M aqueous acetic acid solution at 298 K is $1.65 \times {10}^{-4}$ S ${\mathrm{cm}}^{-1}$. The degree of dissociation of acetic acid is [Given: Equivalent conductance at infinite dilution of ${\mathrm{H}}^{+}$ = 349.1 S ${\mathrm{cm}}^2$ ${\mathrm{mol}}^{-1}$ and ${\mathrm{CH}}_3{\mathrm{COO}}^{-}$ = 40.9 S ${\mathrm{cm}}^2$ ${\mathrm{mol}}^{-1}$)

1.  0.021

2.  0.21

3.  0.012

4.  0.12

The specific conductance of 0.01 M solution of a weak monobasic acid is 0.20 x 10^-3 S cm^-1. The dissociation constant of the acid is-

[Given  ${\Lambda }_{\mathrm{HA}}^{\infty }$ = 400 S ${\mathrm{cm}}^2$ ${\mathrm{mol}}^{-1}$]

Equivalent conductance of saturated ${\mathrm{BaSO}}_4$ solution is 400 ${\mathrm{ohm}}^{-1} {\mathrm{cm}}^{2 }{\mathrm{equivalent}}^{-1}$ and it's specific conductance is $8 \times {10}^{-5} {\mathrm{ohm}}^{-1} {\mathrm{cm}}^{-1}$; hence solubility product ${\mathrm{K}}_{\mathrm{sp}} \mathrm{of} {\mathrm{BaSO}}_4$ is : 

1.  $4 \times {10}^{-8} {\mathrm{M}}^2$

2.  $1 \times {10}^{-8} {\mathrm{M}}^2$

3.  $2 \times {10}^{-4} {\mathrm{M}}^2$

4.  $1 \times {10}^{-4} {\mathrm{M}}^2$

$$
For the Cell \(Pt(s)|| Br^-(aq)(0.010M)| Br_2(l)|| H^+(aq) (0.0030M) |H_2(g) (1 bar) | Pt(s)\)

If the concentration of ${\mathrm{Br}}^{-}$ becomes 2 times and the concentration of ${\mathrm{H}}^{+}$ becomes half of the initial value, then emf of the cell

1.  Doubles

2.  Four times

3.  Eight times

4.  Remains the same

Adding powdered lead and iron to a solution that is 1.0 molar each in ${\mathrm{Pb}}^{2+}$ and ${\mathrm{Fe}}^{2+}$ ions, would result to a reaction in which

     $\begin{array}{rl}& {\mathrm{E}}_{{\mathrm{Fe}}^{2+}/\mathrm{Fe}}^{\circ }=-0.44\mathrm{V}\\ & {\mathrm{E}}_{{\mathrm{Pb}}^{2+}/\mathrm{Pb}}^0=-0.13\mathrm{V}\end{array}$

1.  Conc. of both ${\mathrm{Pb}}^{2+}$ and ${\mathrm{Fe}}^{2+}$ are increased

2.  More lead and iron are formed

3.  More of iron and ${\mathrm{Pb}}^{2+}$ ions are formed

4.  More of lead and ${\mathrm{Fe}}^{2+}$ ions are formed

The specific conductance of the saturated solution of AgCl is $1.2 \times {10}^{-6} {\Omega }^{-1} c{m}^{-1}$. Molar conductance at infinite dilution of AgCl is $119 {\Omega }^{-1} c{m}^2 mo{l}^{-1}$. The solubility of AgCl in mole/L is

1.  $0.5 \times {10}^{-5} M$

2.  $1.04 \times {10}^{-5} M$

3.  $1.5 \times {10}^{-5} M$

4.  $2 \times {10}^{-5} M$

For a reaction,  A(s) + 2B⁺ $\to$ A²⁺ + 2B(s) ; K_C  has been found to be 10¹². The  ${\mathrm{E}}_{\mathrm{cell}}^{°}$ is
1. 0.354 V

2. 0.708V

3. 0.0098 V

4. 1.36V

Which of the following solutions has the highest equivalent conductance?

1. 0.01 M NaCl

2. 0.05 M NaCl

3. 0.005 M NaCl

4. 0.02 M NaCl

How many coulombs of electric charge must pass through acidulated water in order to release 22.4 litre of H₂ at N.T.P?

1  65900 coulomb

2  193000 coulomb

3  96500 coulomb

4  96500 faraday

Given the following molar conductivities at ${25}^{°}C:, HCl 426 {\Omega }^{-1} c{m}^2 mo{l}^{-1};$
$$$NaCl 126 {\Omega }^{-1} c{m}^2 mo{l}^{-1}; NaC (sodium coronate)$$83 {\Omega }^{-1} c{m}^2 mo{l}^{-1}$.  what is the ionization constant of crotonic acid? If the conductivity of a 0.001 M crotonic acid solution is 3.83$\times$${10}^{-5} {\Omega }^{-1}c{m}^{-1}$?

(1) ${10}^{-5}$                 (2) $1.11\times {10}^{-5}$

(3) $1.11\times {10}^{-4}$      (4)0.01