330467
Molar conductance of \(\mathrm{KCl}\) increases slowly with decrease in concentration because of
1 Increase in degree of ionisation
2 Increase in total number of current carrying species
3 Weakening of interionic attractions and increase in ionic mobilities
4 Increase in hydration of ions.
Explanation:
\(\mathrm{KCl}\) is a strong electrolyte and on dilution inter ionic attractions weakens as a result ionic mobilities increase. So, molar conductance increases slowly on dilution.
CHXII03:ELECTROCHEMISTRY
330468
The conductivity of \({\mathrm{0.1 \mathrm{~mol} \mathrm{~L}^{-1}\, \mathrm{KCl}}}\) solution is \({\mathrm{1.41 \times 10^{-3} \mathrm{~S} \mathrm{~cm}^{-1}}}\). What is its molar conductivity (in \({\mathrm{\mathrm{S} \mathrm{~cm}^{2} \mathrm{~mol}^{-1}}}\) )?
330469
Which of the following statements is correct for an electrolytic solution upon dilution?
1 Conductivity increases.
2 Conductivity decreases.
3 Molar conductance decreases but equivalent conductance increases.
4 Molar conductance increases while equivalent conductance decreases.
Explanation:
Number of ions per unit volume decreases, hence conductivity decreases.
CHXII03:ELECTROCHEMISTRY
330452
The molar conductivity for electrolytes \({\mathrm{A}}\) and \({\mathrm{B}}\) are plotted against \({\mathrm{C^{1 / 2}}}\) as shown below. Electrolytes A and B respectively are
1 A - Weak electrolyte B - Strong electrolyte
2 A - Weak electrolyte B - Weak electrolyte
3 A - Strong electrolyte B - Weak electrolyte
4 A - Strong electrolyte B - Strong electrolyte
Explanation:
\({\mathrm{\Lambda_{\mathrm{m}}}}\) increases continously with dilution for weak electrolytes (A) and for strong electrolytes, no much change is noticed with dilution (B). So, the correct option is (1).
JEE Main - 2024
CHXII03:ELECTROCHEMISTRY
330453
Assertion : \({{\rm{\Lambda }}_{\rm{m}}}\) for weak electrolytes shows at a sharp increase when the electrolytic solution is diluted. Reason : For weak electrolytes degree of dissociation increases with dilution of solution.
1 If both the assertion and reason are true and reason is a true explanation of the assertion
2 If both the assertion and reason are true but the reason is not the correct explanation of assertion
3 If the assertion is true but reason is false
4 If assertion is false but reason is true.
Explanation:
Assertion and reason are true and the reason is the correct explanation of the assertion. Molar conductivity of weak electrolytic solution increases on dilution, because as we add excess water to increase the dilution degree of dissociation increases with lead to increase in number of ions in the solution. Thus, \({{\rm{\Lambda }}_{\rm{m}}}\) show a very sharp increase. So, the option (1) is correct.
330467
Molar conductance of \(\mathrm{KCl}\) increases slowly with decrease in concentration because of
1 Increase in degree of ionisation
2 Increase in total number of current carrying species
3 Weakening of interionic attractions and increase in ionic mobilities
4 Increase in hydration of ions.
Explanation:
\(\mathrm{KCl}\) is a strong electrolyte and on dilution inter ionic attractions weakens as a result ionic mobilities increase. So, molar conductance increases slowly on dilution.
CHXII03:ELECTROCHEMISTRY
330468
The conductivity of \({\mathrm{0.1 \mathrm{~mol} \mathrm{~L}^{-1}\, \mathrm{KCl}}}\) solution is \({\mathrm{1.41 \times 10^{-3} \mathrm{~S} \mathrm{~cm}^{-1}}}\). What is its molar conductivity (in \({\mathrm{\mathrm{S} \mathrm{~cm}^{2} \mathrm{~mol}^{-1}}}\) )?
330469
Which of the following statements is correct for an electrolytic solution upon dilution?
1 Conductivity increases.
2 Conductivity decreases.
3 Molar conductance decreases but equivalent conductance increases.
4 Molar conductance increases while equivalent conductance decreases.
Explanation:
Number of ions per unit volume decreases, hence conductivity decreases.
CHXII03:ELECTROCHEMISTRY
330452
The molar conductivity for electrolytes \({\mathrm{A}}\) and \({\mathrm{B}}\) are plotted against \({\mathrm{C^{1 / 2}}}\) as shown below. Electrolytes A and B respectively are
1 A - Weak electrolyte B - Strong electrolyte
2 A - Weak electrolyte B - Weak electrolyte
3 A - Strong electrolyte B - Weak electrolyte
4 A - Strong electrolyte B - Strong electrolyte
Explanation:
\({\mathrm{\Lambda_{\mathrm{m}}}}\) increases continously with dilution for weak electrolytes (A) and for strong electrolytes, no much change is noticed with dilution (B). So, the correct option is (1).
JEE Main - 2024
CHXII03:ELECTROCHEMISTRY
330453
Assertion : \({{\rm{\Lambda }}_{\rm{m}}}\) for weak electrolytes shows at a sharp increase when the electrolytic solution is diluted. Reason : For weak electrolytes degree of dissociation increases with dilution of solution.
1 If both the assertion and reason are true and reason is a true explanation of the assertion
2 If both the assertion and reason are true but the reason is not the correct explanation of assertion
3 If the assertion is true but reason is false
4 If assertion is false but reason is true.
Explanation:
Assertion and reason are true and the reason is the correct explanation of the assertion. Molar conductivity of weak electrolytic solution increases on dilution, because as we add excess water to increase the dilution degree of dissociation increases with lead to increase in number of ions in the solution. Thus, \({{\rm{\Lambda }}_{\rm{m}}}\) show a very sharp increase. So, the option (1) is correct.
330467
Molar conductance of \(\mathrm{KCl}\) increases slowly with decrease in concentration because of
1 Increase in degree of ionisation
2 Increase in total number of current carrying species
3 Weakening of interionic attractions and increase in ionic mobilities
4 Increase in hydration of ions.
Explanation:
\(\mathrm{KCl}\) is a strong electrolyte and on dilution inter ionic attractions weakens as a result ionic mobilities increase. So, molar conductance increases slowly on dilution.
CHXII03:ELECTROCHEMISTRY
330468
The conductivity of \({\mathrm{0.1 \mathrm{~mol} \mathrm{~L}^{-1}\, \mathrm{KCl}}}\) solution is \({\mathrm{1.41 \times 10^{-3} \mathrm{~S} \mathrm{~cm}^{-1}}}\). What is its molar conductivity (in \({\mathrm{\mathrm{S} \mathrm{~cm}^{2} \mathrm{~mol}^{-1}}}\) )?
330469
Which of the following statements is correct for an electrolytic solution upon dilution?
1 Conductivity increases.
2 Conductivity decreases.
3 Molar conductance decreases but equivalent conductance increases.
4 Molar conductance increases while equivalent conductance decreases.
Explanation:
Number of ions per unit volume decreases, hence conductivity decreases.
CHXII03:ELECTROCHEMISTRY
330452
The molar conductivity for electrolytes \({\mathrm{A}}\) and \({\mathrm{B}}\) are plotted against \({\mathrm{C^{1 / 2}}}\) as shown below. Electrolytes A and B respectively are
1 A - Weak electrolyte B - Strong electrolyte
2 A - Weak electrolyte B - Weak electrolyte
3 A - Strong electrolyte B - Weak electrolyte
4 A - Strong electrolyte B - Strong electrolyte
Explanation:
\({\mathrm{\Lambda_{\mathrm{m}}}}\) increases continously with dilution for weak electrolytes (A) and for strong electrolytes, no much change is noticed with dilution (B). So, the correct option is (1).
JEE Main - 2024
CHXII03:ELECTROCHEMISTRY
330453
Assertion : \({{\rm{\Lambda }}_{\rm{m}}}\) for weak electrolytes shows at a sharp increase when the electrolytic solution is diluted. Reason : For weak electrolytes degree of dissociation increases with dilution of solution.
1 If both the assertion and reason are true and reason is a true explanation of the assertion
2 If both the assertion and reason are true but the reason is not the correct explanation of assertion
3 If the assertion is true but reason is false
4 If assertion is false but reason is true.
Explanation:
Assertion and reason are true and the reason is the correct explanation of the assertion. Molar conductivity of weak electrolytic solution increases on dilution, because as we add excess water to increase the dilution degree of dissociation increases with lead to increase in number of ions in the solution. Thus, \({{\rm{\Lambda }}_{\rm{m}}}\) show a very sharp increase. So, the option (1) is correct.
330467
Molar conductance of \(\mathrm{KCl}\) increases slowly with decrease in concentration because of
1 Increase in degree of ionisation
2 Increase in total number of current carrying species
3 Weakening of interionic attractions and increase in ionic mobilities
4 Increase in hydration of ions.
Explanation:
\(\mathrm{KCl}\) is a strong electrolyte and on dilution inter ionic attractions weakens as a result ionic mobilities increase. So, molar conductance increases slowly on dilution.
CHXII03:ELECTROCHEMISTRY
330468
The conductivity of \({\mathrm{0.1 \mathrm{~mol} \mathrm{~L}^{-1}\, \mathrm{KCl}}}\) solution is \({\mathrm{1.41 \times 10^{-3} \mathrm{~S} \mathrm{~cm}^{-1}}}\). What is its molar conductivity (in \({\mathrm{\mathrm{S} \mathrm{~cm}^{2} \mathrm{~mol}^{-1}}}\) )?
330469
Which of the following statements is correct for an electrolytic solution upon dilution?
1 Conductivity increases.
2 Conductivity decreases.
3 Molar conductance decreases but equivalent conductance increases.
4 Molar conductance increases while equivalent conductance decreases.
Explanation:
Number of ions per unit volume decreases, hence conductivity decreases.
CHXII03:ELECTROCHEMISTRY
330452
The molar conductivity for electrolytes \({\mathrm{A}}\) and \({\mathrm{B}}\) are plotted against \({\mathrm{C^{1 / 2}}}\) as shown below. Electrolytes A and B respectively are
1 A - Weak electrolyte B - Strong electrolyte
2 A - Weak electrolyte B - Weak electrolyte
3 A - Strong electrolyte B - Weak electrolyte
4 A - Strong electrolyte B - Strong electrolyte
Explanation:
\({\mathrm{\Lambda_{\mathrm{m}}}}\) increases continously with dilution for weak electrolytes (A) and for strong electrolytes, no much change is noticed with dilution (B). So, the correct option is (1).
JEE Main - 2024
CHXII03:ELECTROCHEMISTRY
330453
Assertion : \({{\rm{\Lambda }}_{\rm{m}}}\) for weak electrolytes shows at a sharp increase when the electrolytic solution is diluted. Reason : For weak electrolytes degree of dissociation increases with dilution of solution.
1 If both the assertion and reason are true and reason is a true explanation of the assertion
2 If both the assertion and reason are true but the reason is not the correct explanation of assertion
3 If the assertion is true but reason is false
4 If assertion is false but reason is true.
Explanation:
Assertion and reason are true and the reason is the correct explanation of the assertion. Molar conductivity of weak electrolytic solution increases on dilution, because as we add excess water to increase the dilution degree of dissociation increases with lead to increase in number of ions in the solution. Thus, \({{\rm{\Lambda }}_{\rm{m}}}\) show a very sharp increase. So, the option (1) is correct.
330467
Molar conductance of \(\mathrm{KCl}\) increases slowly with decrease in concentration because of
1 Increase in degree of ionisation
2 Increase in total number of current carrying species
3 Weakening of interionic attractions and increase in ionic mobilities
4 Increase in hydration of ions.
Explanation:
\(\mathrm{KCl}\) is a strong electrolyte and on dilution inter ionic attractions weakens as a result ionic mobilities increase. So, molar conductance increases slowly on dilution.
CHXII03:ELECTROCHEMISTRY
330468
The conductivity of \({\mathrm{0.1 \mathrm{~mol} \mathrm{~L}^{-1}\, \mathrm{KCl}}}\) solution is \({\mathrm{1.41 \times 10^{-3} \mathrm{~S} \mathrm{~cm}^{-1}}}\). What is its molar conductivity (in \({\mathrm{\mathrm{S} \mathrm{~cm}^{2} \mathrm{~mol}^{-1}}}\) )?
330469
Which of the following statements is correct for an electrolytic solution upon dilution?
1 Conductivity increases.
2 Conductivity decreases.
3 Molar conductance decreases but equivalent conductance increases.
4 Molar conductance increases while equivalent conductance decreases.
Explanation:
Number of ions per unit volume decreases, hence conductivity decreases.
CHXII03:ELECTROCHEMISTRY
330452
The molar conductivity for electrolytes \({\mathrm{A}}\) and \({\mathrm{B}}\) are plotted against \({\mathrm{C^{1 / 2}}}\) as shown below. Electrolytes A and B respectively are
1 A - Weak electrolyte B - Strong electrolyte
2 A - Weak electrolyte B - Weak electrolyte
3 A - Strong electrolyte B - Weak electrolyte
4 A - Strong electrolyte B - Strong electrolyte
Explanation:
\({\mathrm{\Lambda_{\mathrm{m}}}}\) increases continously with dilution for weak electrolytes (A) and for strong electrolytes, no much change is noticed with dilution (B). So, the correct option is (1).
JEE Main - 2024
CHXII03:ELECTROCHEMISTRY
330453
Assertion : \({{\rm{\Lambda }}_{\rm{m}}}\) for weak electrolytes shows at a sharp increase when the electrolytic solution is diluted. Reason : For weak electrolytes degree of dissociation increases with dilution of solution.
1 If both the assertion and reason are true and reason is a true explanation of the assertion
2 If both the assertion and reason are true but the reason is not the correct explanation of assertion
3 If the assertion is true but reason is false
4 If assertion is false but reason is true.
Explanation:
Assertion and reason are true and the reason is the correct explanation of the assertion. Molar conductivity of weak electrolytic solution increases on dilution, because as we add excess water to increase the dilution degree of dissociation increases with lead to increase in number of ions in the solution. Thus, \({{\rm{\Lambda }}_{\rm{m}}}\) show a very sharp increase. So, the option (1) is correct.
