Molar conductivities $(\wedge {°}_m)$ at infinite dilution of
NaCl, HCl, and $C{H}_{3}COONa$ are 126.4, 425.9, and 91.0 S cm² mol^-1 respectively.
 $(\wedge {°}_m)$  for $C{H}_{3}COOH$  will be: 

\(\Lambda _{m(NH_{4}OH)}^{o}\) is equal to -
1. \(\Lambda _{m(NH_{4}OH)}^{o} \ + \ \Lambda _{m(NH_{4}Cl)}^{o} \ - \ \Lambda _{m(HCl)}^{o}\)
2. \(\Lambda _{m(NH_{4}Cl)}^{o} \ + \ \Lambda _{m(NaOH)}^{o} \ - \ \Lambda _{m(NaCl)}^{o}\)
3. \(\Lambda _{m(NH_{4}Cl)}^{o} \ + \ \Lambda _{m(NaCl)}^{o} \ - \ \Lambda _{m(NaOH)}^{o}\)
4. \(\ \Lambda _{m(NaOH)}^{o} \ + \ \Lambda _{m(NaCl)}^{o}\ - \ \Lambda _{m(NH_{4}Cl)}^{o}\)

The resistance of a conductivity cell containing 0.001M KCl solution at 298 K is 1500 Ω. The cell constant if conductivity of 0.001 M KCl solution at 298 K is 0.146 ×10^-3  S cm^-1 will be: 

1. 0.32 cm^-1

2. 0.47 cm

3. 0.22 cm^-1

4. 0.23 cm

The resistance of a cell containing 0.001 M KCl solution at 298 K is 1500 Ω. The conductivity is 0.146 × 10^–3 S cm^–1. The cell constant would be-

$1.$ $0.12$ ${\mathrm{cm}}^{-1}$

$2.$ $0.56$ ${\mathrm{cm}}^{-1}$

$3.$ $0.22$ ${\mathrm{cm}}^{-1}$

$4.$ $1.36$ ${\mathrm{cm}}^{-1}$

The molar conductance of $\frac{\mathrm{M}}{32}$ solution of a weak monobasic acid is 8.0 ohm^-1 cm² and at infinite dilution is 400 ohm^-1 cm². The dissociation constant of this acid is: 

Kohlrausch's law states that at:

Value of ${{\wedge }_m}^0$ for $$ $SrC{l}_2$ (strong electrolyte) in water at $\mathrm{25 }°C$ from the data below is:

1. 270 Ω^-1 cm² mol^-1                                                     

2. 260 Ω^-1 cm² mol^-1 

3. 250 Ω^-1 cm² mol^-1                                                    

4. 255 Ω^-1 cm² mol^-1 

Consider the following graph of molar conductivity of KCl solution at different concentrations. 

 

The value of limiting molar conductivity for KCl is 150.0 S cm² mol^-1. The value of the slope at point A will be :