NEET Test Series from KOTA - 10 Papers In MS WORD
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Ionic Equilibrium
229566
The conductivity of a $0.05 \mathrm{M}$ solution of a weak monobasic acid is $10^{-3} \mathrm{~S} \mathrm{~cm}^{-1}$. If $\lambda_{\mathrm{m}}$ for weak acid is $500 \mathrm{~S} \mathrm{~cm}^2 \mathrm{~mol}^{-1}$, calculate $K_{\mathrm{a}}$ of weak monobasic acid:
229567
Which of the following is incorrect about $\mathrm{K}_2 \mathrm{Cr}_2 \mathrm{O}_7$ ?
1 It can be prepared from $\mathrm{K}_2 \mathrm{CrO}_4$.
2 It is used in redox titrations.
3 It is stable in both acid \& base.
4 It is orange in colour.
Explanation:
Exp: - Colour of $\mathrm{K}_2 \mathrm{Cr}_2 \mathrm{O}_7$ is orange - $2 \mathrm{Cr}_4^{-2} \stackrel{\text { In acidic medium }}{\mathrm{H}+} \mathrm{Cr}_2 \mathrm{O}_7^{2-}+\mathrm{H}_2 \mathrm{O}$ (Chromate ion) (Dichromate ion) - $\mathrm{K}_2 \mathrm{Cr}_2 \mathrm{O}_7$ is used in redox titrations. - It is stable in both acid \& base this statement is incorrect about $\mathrm{K}_2 \mathrm{Cr}_2 \mathrm{O}_7$.
AIIMS 26 May 2019(Evening)
Ionic Equilibrium
229572
Assertion : $\mathbf{K O H}$ is more soluble in water than $\mathrm{NaOH}$. **Reason :** $\mathrm{NaOH}$ is a stronger base than $\mathrm{KOH}$.
1 If both Assertion and Reason are correct and the Reason is the correct explanation of Assertion.
2 If both Assertion and Reason are correct, but Reason is not the correct explanation of Assertion.
3 If Assertion if correct but Reason is incorrect.
4 If both the Assertion and Reason are incorrect.
Explanation:
$\mathrm{KOH}$ is more soluble in water than $\mathrm{NaOH}$. The ionic size of $\mathrm{Na}^{+}$is smaller than $\mathrm{K}^{+}$. Hence attractive force between $\mathrm{Na}^{+}$and $\mathrm{OH}$ is relatively strong and so ionisation of $\mathrm{NaOH}$ is lower than $\mathrm{KOH}$ which makes $\mathrm{NaOH}$ a weaker base than $\mathrm{KOH}$.
AIIMS-(2011)
Ionic Equilibrium
229573
Assertion : Addition of silver ions to a mixture of aqueous sodium chloride and sodium bromide solution will first precipitate $\mathrm{AgBr}$ rather than AgC1. **Reason:** $\mathrm{K}_{5 p}$ of $\mathrm{AgCl}>\mathrm{K}_{5 p}$ of $\mathrm{AgBr}$.
1 If both Assertion and Reason are correct and the Reason is the correct explanation of Assertion.
2 If both assertion and Reason are correct, but Reason is not the correct explanation of assertion.
3 If Assertion is correct but Reason is incorrect.
4 If both the Assertion and Reason are incorrect.
Explanation:
We know that, The solubility product of $\mathrm{AgBr}=5 \times 10^{-13}$ and $\mathrm{AgCl}=$ $5 \times 10^{-10}$ Hence, $\mathrm{K}_{\text {sp }}$ of $\mathrm{AgCl}<\mathrm{K}_{\text {sp }}$ of $\mathrm{AgBr}$ Hence, when we add silver ion to a mixture of aqueous sodium chloride and sodium bromide solution, $\mathrm{AgBr}$ will percipitate first.
229566
The conductivity of a $0.05 \mathrm{M}$ solution of a weak monobasic acid is $10^{-3} \mathrm{~S} \mathrm{~cm}^{-1}$. If $\lambda_{\mathrm{m}}$ for weak acid is $500 \mathrm{~S} \mathrm{~cm}^2 \mathrm{~mol}^{-1}$, calculate $K_{\mathrm{a}}$ of weak monobasic acid:
229567
Which of the following is incorrect about $\mathrm{K}_2 \mathrm{Cr}_2 \mathrm{O}_7$ ?
1 It can be prepared from $\mathrm{K}_2 \mathrm{CrO}_4$.
2 It is used in redox titrations.
3 It is stable in both acid \& base.
4 It is orange in colour.
Explanation:
Exp: - Colour of $\mathrm{K}_2 \mathrm{Cr}_2 \mathrm{O}_7$ is orange - $2 \mathrm{Cr}_4^{-2} \stackrel{\text { In acidic medium }}{\mathrm{H}+} \mathrm{Cr}_2 \mathrm{O}_7^{2-}+\mathrm{H}_2 \mathrm{O}$ (Chromate ion) (Dichromate ion) - $\mathrm{K}_2 \mathrm{Cr}_2 \mathrm{O}_7$ is used in redox titrations. - It is stable in both acid \& base this statement is incorrect about $\mathrm{K}_2 \mathrm{Cr}_2 \mathrm{O}_7$.
AIIMS 26 May 2019(Evening)
Ionic Equilibrium
229572
Assertion : $\mathbf{K O H}$ is more soluble in water than $\mathrm{NaOH}$. **Reason :** $\mathrm{NaOH}$ is a stronger base than $\mathrm{KOH}$.
1 If both Assertion and Reason are correct and the Reason is the correct explanation of Assertion.
2 If both Assertion and Reason are correct, but Reason is not the correct explanation of Assertion.
3 If Assertion if correct but Reason is incorrect.
4 If both the Assertion and Reason are incorrect.
Explanation:
$\mathrm{KOH}$ is more soluble in water than $\mathrm{NaOH}$. The ionic size of $\mathrm{Na}^{+}$is smaller than $\mathrm{K}^{+}$. Hence attractive force between $\mathrm{Na}^{+}$and $\mathrm{OH}$ is relatively strong and so ionisation of $\mathrm{NaOH}$ is lower than $\mathrm{KOH}$ which makes $\mathrm{NaOH}$ a weaker base than $\mathrm{KOH}$.
AIIMS-(2011)
Ionic Equilibrium
229573
Assertion : Addition of silver ions to a mixture of aqueous sodium chloride and sodium bromide solution will first precipitate $\mathrm{AgBr}$ rather than AgC1. **Reason:** $\mathrm{K}_{5 p}$ of $\mathrm{AgCl}>\mathrm{K}_{5 p}$ of $\mathrm{AgBr}$.
1 If both Assertion and Reason are correct and the Reason is the correct explanation of Assertion.
2 If both assertion and Reason are correct, but Reason is not the correct explanation of assertion.
3 If Assertion is correct but Reason is incorrect.
4 If both the Assertion and Reason are incorrect.
Explanation:
We know that, The solubility product of $\mathrm{AgBr}=5 \times 10^{-13}$ and $\mathrm{AgCl}=$ $5 \times 10^{-10}$ Hence, $\mathrm{K}_{\text {sp }}$ of $\mathrm{AgCl}<\mathrm{K}_{\text {sp }}$ of $\mathrm{AgBr}$ Hence, when we add silver ion to a mixture of aqueous sodium chloride and sodium bromide solution, $\mathrm{AgBr}$ will percipitate first.
229566
The conductivity of a $0.05 \mathrm{M}$ solution of a weak monobasic acid is $10^{-3} \mathrm{~S} \mathrm{~cm}^{-1}$. If $\lambda_{\mathrm{m}}$ for weak acid is $500 \mathrm{~S} \mathrm{~cm}^2 \mathrm{~mol}^{-1}$, calculate $K_{\mathrm{a}}$ of weak monobasic acid:
229567
Which of the following is incorrect about $\mathrm{K}_2 \mathrm{Cr}_2 \mathrm{O}_7$ ?
1 It can be prepared from $\mathrm{K}_2 \mathrm{CrO}_4$.
2 It is used in redox titrations.
3 It is stable in both acid \& base.
4 It is orange in colour.
Explanation:
Exp: - Colour of $\mathrm{K}_2 \mathrm{Cr}_2 \mathrm{O}_7$ is orange - $2 \mathrm{Cr}_4^{-2} \stackrel{\text { In acidic medium }}{\mathrm{H}+} \mathrm{Cr}_2 \mathrm{O}_7^{2-}+\mathrm{H}_2 \mathrm{O}$ (Chromate ion) (Dichromate ion) - $\mathrm{K}_2 \mathrm{Cr}_2 \mathrm{O}_7$ is used in redox titrations. - It is stable in both acid \& base this statement is incorrect about $\mathrm{K}_2 \mathrm{Cr}_2 \mathrm{O}_7$.
AIIMS 26 May 2019(Evening)
Ionic Equilibrium
229572
Assertion : $\mathbf{K O H}$ is more soluble in water than $\mathrm{NaOH}$. **Reason :** $\mathrm{NaOH}$ is a stronger base than $\mathrm{KOH}$.
1 If both Assertion and Reason are correct and the Reason is the correct explanation of Assertion.
2 If both Assertion and Reason are correct, but Reason is not the correct explanation of Assertion.
3 If Assertion if correct but Reason is incorrect.
4 If both the Assertion and Reason are incorrect.
Explanation:
$\mathrm{KOH}$ is more soluble in water than $\mathrm{NaOH}$. The ionic size of $\mathrm{Na}^{+}$is smaller than $\mathrm{K}^{+}$. Hence attractive force between $\mathrm{Na}^{+}$and $\mathrm{OH}$ is relatively strong and so ionisation of $\mathrm{NaOH}$ is lower than $\mathrm{KOH}$ which makes $\mathrm{NaOH}$ a weaker base than $\mathrm{KOH}$.
AIIMS-(2011)
Ionic Equilibrium
229573
Assertion : Addition of silver ions to a mixture of aqueous sodium chloride and sodium bromide solution will first precipitate $\mathrm{AgBr}$ rather than AgC1. **Reason:** $\mathrm{K}_{5 p}$ of $\mathrm{AgCl}>\mathrm{K}_{5 p}$ of $\mathrm{AgBr}$.
1 If both Assertion and Reason are correct and the Reason is the correct explanation of Assertion.
2 If both assertion and Reason are correct, but Reason is not the correct explanation of assertion.
3 If Assertion is correct but Reason is incorrect.
4 If both the Assertion and Reason are incorrect.
Explanation:
We know that, The solubility product of $\mathrm{AgBr}=5 \times 10^{-13}$ and $\mathrm{AgCl}=$ $5 \times 10^{-10}$ Hence, $\mathrm{K}_{\text {sp }}$ of $\mathrm{AgCl}<\mathrm{K}_{\text {sp }}$ of $\mathrm{AgBr}$ Hence, when we add silver ion to a mixture of aqueous sodium chloride and sodium bromide solution, $\mathrm{AgBr}$ will percipitate first.
NEET Test Series from KOTA - 10 Papers In MS WORD
WhatsApp Here
Ionic Equilibrium
229566
The conductivity of a $0.05 \mathrm{M}$ solution of a weak monobasic acid is $10^{-3} \mathrm{~S} \mathrm{~cm}^{-1}$. If $\lambda_{\mathrm{m}}$ for weak acid is $500 \mathrm{~S} \mathrm{~cm}^2 \mathrm{~mol}^{-1}$, calculate $K_{\mathrm{a}}$ of weak monobasic acid:
229567
Which of the following is incorrect about $\mathrm{K}_2 \mathrm{Cr}_2 \mathrm{O}_7$ ?
1 It can be prepared from $\mathrm{K}_2 \mathrm{CrO}_4$.
2 It is used in redox titrations.
3 It is stable in both acid \& base.
4 It is orange in colour.
Explanation:
Exp: - Colour of $\mathrm{K}_2 \mathrm{Cr}_2 \mathrm{O}_7$ is orange - $2 \mathrm{Cr}_4^{-2} \stackrel{\text { In acidic medium }}{\mathrm{H}+} \mathrm{Cr}_2 \mathrm{O}_7^{2-}+\mathrm{H}_2 \mathrm{O}$ (Chromate ion) (Dichromate ion) - $\mathrm{K}_2 \mathrm{Cr}_2 \mathrm{O}_7$ is used in redox titrations. - It is stable in both acid \& base this statement is incorrect about $\mathrm{K}_2 \mathrm{Cr}_2 \mathrm{O}_7$.
AIIMS 26 May 2019(Evening)
Ionic Equilibrium
229572
Assertion : $\mathbf{K O H}$ is more soluble in water than $\mathrm{NaOH}$. **Reason :** $\mathrm{NaOH}$ is a stronger base than $\mathrm{KOH}$.
1 If both Assertion and Reason are correct and the Reason is the correct explanation of Assertion.
2 If both Assertion and Reason are correct, but Reason is not the correct explanation of Assertion.
3 If Assertion if correct but Reason is incorrect.
4 If both the Assertion and Reason are incorrect.
Explanation:
$\mathrm{KOH}$ is more soluble in water than $\mathrm{NaOH}$. The ionic size of $\mathrm{Na}^{+}$is smaller than $\mathrm{K}^{+}$. Hence attractive force between $\mathrm{Na}^{+}$and $\mathrm{OH}$ is relatively strong and so ionisation of $\mathrm{NaOH}$ is lower than $\mathrm{KOH}$ which makes $\mathrm{NaOH}$ a weaker base than $\mathrm{KOH}$.
AIIMS-(2011)
Ionic Equilibrium
229573
Assertion : Addition of silver ions to a mixture of aqueous sodium chloride and sodium bromide solution will first precipitate $\mathrm{AgBr}$ rather than AgC1. **Reason:** $\mathrm{K}_{5 p}$ of $\mathrm{AgCl}>\mathrm{K}_{5 p}$ of $\mathrm{AgBr}$.
1 If both Assertion and Reason are correct and the Reason is the correct explanation of Assertion.
2 If both assertion and Reason are correct, but Reason is not the correct explanation of assertion.
3 If Assertion is correct but Reason is incorrect.
4 If both the Assertion and Reason are incorrect.
Explanation:
We know that, The solubility product of $\mathrm{AgBr}=5 \times 10^{-13}$ and $\mathrm{AgCl}=$ $5 \times 10^{-10}$ Hence, $\mathrm{K}_{\text {sp }}$ of $\mathrm{AgCl}<\mathrm{K}_{\text {sp }}$ of $\mathrm{AgBr}$ Hence, when we add silver ion to a mixture of aqueous sodium chloride and sodium bromide solution, $\mathrm{AgBr}$ will percipitate first.