The molar conductances of Ba²⁺ and Cl^- 127 and 76Ω^-1 cm^-1 mol^-1 respectively at infinite dilution. The equivalent conductance of BaCl₂ at infinite dilution will be

1. 139.52

2. 203

3. 279

4. 101.5

An increase in equivalent conductance of a strong electrolyte with dilution is mainly due to

1. increase in ionic mobility of ions

2. 100% ionisation of electrolyte at normal dilution

3. increase in both, i.e. number of ions and ionic mobility of ions

4. increase in number of ions

What will be the molar conductance at infinite dilution for NH₄OH. If at infinite dilution the molar conductances of Ba(OH)₂, BaCl₂ and NH₄Cl are 523.28, 280.0 and 129.8 ohm^-1 cm^-1 mol^-1 respectively.
1. 502.88
2. 373.68
3. 251.44
3. 226.96

At 25° C molar conductance of 0.1 molar aqueous solution of ammonium hydroxide is

9.54 ohm¹cm²mol^-1 and at infinite dilution its molar conductance is 238 ohm¹cm²mol^-1.

The degree of ionisation of ammonium hydroxide at the same concentration and

temperature is

1. 2.080%

2. 20.800%

3. 4.008%

4. 40.800%

Limiting molar conductivity of NH₄OH (i.e Åm(NH₄OH)) is equal to:-

1. Å_m (NH₄Cl)+Å_m(NaCl)-Å_m(NaOH) 

2. Å_m(NaOH)+Å_m(NaCl)-Å_m(NH₄Cl)

3. Å_m(NH₄OH)+Å_m(NH₄Cl)-Å_m(HCl)

4. Å(NH₄Cl)+Å(NaOH)-Å(NaCl)

Kohlrausch's law states that at

(1) finite dilution, each ion makes definite contribution to equivalent conductance of an electrolyte, whatever be the nature of the other ion of the electrolyte.

(2) infinite dilution, each ion makes definite contribution to equivalent conductance of an electrolyte depending on the nature of the other ion of th electrolyte.

(3) infinite dilution, each ion makes definite contribution to conductance of an electrolyte whatever be the nature of the other ion of the electrolyte.

(4) infinite dilution, each ion makes definite contribution to equivalent conductance of an electrolyte, whatever be the nature of the other ion of the electrolyte.

Value of \(\land_{m}^{0}\) for \(\) \(SrCl_{2}\) (strong electrolyte) in water at 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 

Limiting molar conductivity of NH₄OH (i.e., ${\mathrm{\Lambda }}_{\mathrm{m}\left({\mathrm{NH}}_4\mathrm{OH}\right)}^0$ is equal to -

1. ${\mathrm{\Lambda }}_{\mathrm{m}\left(\mathrm{NaOH}\right)}^0+{\mathrm{\Lambda }}_{\mathrm{m}\left(\mathrm{NaCl}\right)}^0-{\mathrm{\Lambda }}_{\mathrm{m}\left(\mathrm{NaOH}\right)}^0$

2. ${\mathrm{\Lambda }}_{\mathrm{m}\left(\mathrm{NaOH}\right)}^0+{\mathrm{\Lambda }}_{\mathrm{m}\left(\mathrm{NaCl}\right)}^0-{\mathrm{\Lambda }}_{\mathrm{m}\left({\mathrm{NH}}_4\mathrm{Cl}\right)}^0$

3. ${\mathrm{\Lambda }}_{\mathrm{m}\left({\mathrm{NH}}_4\mathrm{OH}\right)}^0+{\mathrm{\Lambda }}_{\mathrm{m}\left({\mathrm{NH}}_4\mathrm{Cl}\right)}^0-{\mathrm{\Lambda }}_{\mathrm{m}\left(HCl\right)}^0$

4. ${\mathrm{\Lambda }}_{\mathrm{m}\left({\mathrm{NH}}_4\mathrm{Cl}\right)}^0+{\mathrm{\Lambda }}_{\mathrm{m}\left(\mathrm{NaOH}\right)}^0-{\mathrm{\Lambda }}_{\mathrm{m}\left(\mathrm{NaCl}\right)}^0$

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: