NEET Test Series from KOTA - 10 Papers In MS WORD
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Ionic Equilibrium
229569
Which of the following is the strongest base?
1 $\mathrm{H}_2^{+}$
2 $\mathrm{H}$
3 $\mathrm{HCO}_3^{-}$
4 $\mathrm{H}^{-}$
Explanation:
$\mathrm{HCO}_3^{-}$is a strongest base. A stronger base liberates more $\mathrm{OH}^{-}$when dissolved in an aqueous solution and has a $\mathrm{pH}$ value of more than 7 . So, $\mathrm{HCO}_3^{-}$acts as a base when reacting with the compound that is more acidic than it i.e. $\mathrm{HCl}$. This is because a stronge acid has more ability to donate the proton.
AIIMS-1996
Ionic Equilibrium
229571
**Assertion:** $\mathrm{H}_2 \mathrm{O}$ shows amphoteric nature. **Reason:** According to Bronsted theory, it acts as acid with $\mathrm{NH}_3$ and a base with $\mathrm{H}_2 \mathrm{~S}$.
1 If both Assertion and Reason are correct and 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:
Water has the ability to act as an acid as well as a base i.e. It behaves as an amphoteric substance. In Bronsted sense it act as an acid with $\mathrm{NH}_3$ and base with $\mathrm{H}_2 \mathrm{~S}$. $\mathrm{H}_2 \mathrm{O}(\mathrm{l})+\mathrm{NH}_3$ (aq)?? $\mathrm{OH}^{-}(\mathrm{aq})+\mathrm{NH}_4^{+}(\mathrm{aq})$ $\mathrm{H}_2 \mathrm{O}(\mathrm{l})+\mathrm{H}_2 \mathrm{~S}(\mathrm{aq})$ ? $\mathrm{qu} \mathrm{H}_3 \mathrm{O}^{+}$(aq) $+\mathrm{HS}^{-}$(aq)
AIIMS 26 May 2019(Morning)
Ionic Equilibrium
229576
$\mathrm{pK}_{\mathrm{a}}$ value of four acids are given below. The strongest acid is:
1 4.0
2 3.5
3 2.5
4 2
Explanation:
We know that acidic strength $\propto \mathrm{K}_{\mathrm{n}} \propto \frac{1}{\mathrm{pK}_2}$ Hence acid with lowest $\mathrm{pKa}$ value will be strongest acid. In this question minimum $\mathrm{pKa}$ value is 2 . Hence, It is a strongest acid.
BCECE-2004]
Ionic Equilibrium
229577
Which is Lewis acid?
1 $\mathrm{C}_2 \mathrm{H}_5 \mathrm{OH}$
2 $\mathrm{BF}_3$
3 $\mathrm{Cl}^{-}$
4 $\mathrm{NH}_3$
Explanation:
Lewis acids are those which can accept a pair of non-bonding electron pair. Hence $\mathrm{BF}_3$ is accept electron pair it is Lewis acid. Lewis base are those which can donate a pair of $\mathrm{e}^{-}$pair $\mathrm{C}_2 \mathrm{H}_5 \mathrm{OH}, \mathrm{Cl}^{-}, \mathrm{NH}_3$ all are donate $\mathrm{e}^{-}$pair. Hence, It is a Lewis base.
229569
Which of the following is the strongest base?
1 $\mathrm{H}_2^{+}$
2 $\mathrm{H}$
3 $\mathrm{HCO}_3^{-}$
4 $\mathrm{H}^{-}$
Explanation:
$\mathrm{HCO}_3^{-}$is a strongest base. A stronger base liberates more $\mathrm{OH}^{-}$when dissolved in an aqueous solution and has a $\mathrm{pH}$ value of more than 7 . So, $\mathrm{HCO}_3^{-}$acts as a base when reacting with the compound that is more acidic than it i.e. $\mathrm{HCl}$. This is because a stronge acid has more ability to donate the proton.
AIIMS-1996
Ionic Equilibrium
229571
**Assertion:** $\mathrm{H}_2 \mathrm{O}$ shows amphoteric nature. **Reason:** According to Bronsted theory, it acts as acid with $\mathrm{NH}_3$ and a base with $\mathrm{H}_2 \mathrm{~S}$.
1 If both Assertion and Reason are correct and 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:
Water has the ability to act as an acid as well as a base i.e. It behaves as an amphoteric substance. In Bronsted sense it act as an acid with $\mathrm{NH}_3$ and base with $\mathrm{H}_2 \mathrm{~S}$. $\mathrm{H}_2 \mathrm{O}(\mathrm{l})+\mathrm{NH}_3$ (aq)?? $\mathrm{OH}^{-}(\mathrm{aq})+\mathrm{NH}_4^{+}(\mathrm{aq})$ $\mathrm{H}_2 \mathrm{O}(\mathrm{l})+\mathrm{H}_2 \mathrm{~S}(\mathrm{aq})$ ? $\mathrm{qu} \mathrm{H}_3 \mathrm{O}^{+}$(aq) $+\mathrm{HS}^{-}$(aq)
AIIMS 26 May 2019(Morning)
Ionic Equilibrium
229576
$\mathrm{pK}_{\mathrm{a}}$ value of four acids are given below. The strongest acid is:
1 4.0
2 3.5
3 2.5
4 2
Explanation:
We know that acidic strength $\propto \mathrm{K}_{\mathrm{n}} \propto \frac{1}{\mathrm{pK}_2}$ Hence acid with lowest $\mathrm{pKa}$ value will be strongest acid. In this question minimum $\mathrm{pKa}$ value is 2 . Hence, It is a strongest acid.
BCECE-2004]
Ionic Equilibrium
229577
Which is Lewis acid?
1 $\mathrm{C}_2 \mathrm{H}_5 \mathrm{OH}$
2 $\mathrm{BF}_3$
3 $\mathrm{Cl}^{-}$
4 $\mathrm{NH}_3$
Explanation:
Lewis acids are those which can accept a pair of non-bonding electron pair. Hence $\mathrm{BF}_3$ is accept electron pair it is Lewis acid. Lewis base are those which can donate a pair of $\mathrm{e}^{-}$pair $\mathrm{C}_2 \mathrm{H}_5 \mathrm{OH}, \mathrm{Cl}^{-}, \mathrm{NH}_3$ all are donate $\mathrm{e}^{-}$pair. Hence, It is a Lewis base.
229569
Which of the following is the strongest base?
1 $\mathrm{H}_2^{+}$
2 $\mathrm{H}$
3 $\mathrm{HCO}_3^{-}$
4 $\mathrm{H}^{-}$
Explanation:
$\mathrm{HCO}_3^{-}$is a strongest base. A stronger base liberates more $\mathrm{OH}^{-}$when dissolved in an aqueous solution and has a $\mathrm{pH}$ value of more than 7 . So, $\mathrm{HCO}_3^{-}$acts as a base when reacting with the compound that is more acidic than it i.e. $\mathrm{HCl}$. This is because a stronge acid has more ability to donate the proton.
AIIMS-1996
Ionic Equilibrium
229571
**Assertion:** $\mathrm{H}_2 \mathrm{O}$ shows amphoteric nature. **Reason:** According to Bronsted theory, it acts as acid with $\mathrm{NH}_3$ and a base with $\mathrm{H}_2 \mathrm{~S}$.
1 If both Assertion and Reason are correct and 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:
Water has the ability to act as an acid as well as a base i.e. It behaves as an amphoteric substance. In Bronsted sense it act as an acid with $\mathrm{NH}_3$ and base with $\mathrm{H}_2 \mathrm{~S}$. $\mathrm{H}_2 \mathrm{O}(\mathrm{l})+\mathrm{NH}_3$ (aq)?? $\mathrm{OH}^{-}(\mathrm{aq})+\mathrm{NH}_4^{+}(\mathrm{aq})$ $\mathrm{H}_2 \mathrm{O}(\mathrm{l})+\mathrm{H}_2 \mathrm{~S}(\mathrm{aq})$ ? $\mathrm{qu} \mathrm{H}_3 \mathrm{O}^{+}$(aq) $+\mathrm{HS}^{-}$(aq)
AIIMS 26 May 2019(Morning)
Ionic Equilibrium
229576
$\mathrm{pK}_{\mathrm{a}}$ value of four acids are given below. The strongest acid is:
1 4.0
2 3.5
3 2.5
4 2
Explanation:
We know that acidic strength $\propto \mathrm{K}_{\mathrm{n}} \propto \frac{1}{\mathrm{pK}_2}$ Hence acid with lowest $\mathrm{pKa}$ value will be strongest acid. In this question minimum $\mathrm{pKa}$ value is 2 . Hence, It is a strongest acid.
BCECE-2004]
Ionic Equilibrium
229577
Which is Lewis acid?
1 $\mathrm{C}_2 \mathrm{H}_5 \mathrm{OH}$
2 $\mathrm{BF}_3$
3 $\mathrm{Cl}^{-}$
4 $\mathrm{NH}_3$
Explanation:
Lewis acids are those which can accept a pair of non-bonding electron pair. Hence $\mathrm{BF}_3$ is accept electron pair it is Lewis acid. Lewis base are those which can donate a pair of $\mathrm{e}^{-}$pair $\mathrm{C}_2 \mathrm{H}_5 \mathrm{OH}, \mathrm{Cl}^{-}, \mathrm{NH}_3$ all are donate $\mathrm{e}^{-}$pair. Hence, It is a Lewis base.
229569
Which of the following is the strongest base?
1 $\mathrm{H}_2^{+}$
2 $\mathrm{H}$
3 $\mathrm{HCO}_3^{-}$
4 $\mathrm{H}^{-}$
Explanation:
$\mathrm{HCO}_3^{-}$is a strongest base. A stronger base liberates more $\mathrm{OH}^{-}$when dissolved in an aqueous solution and has a $\mathrm{pH}$ value of more than 7 . So, $\mathrm{HCO}_3^{-}$acts as a base when reacting with the compound that is more acidic than it i.e. $\mathrm{HCl}$. This is because a stronge acid has more ability to donate the proton.
AIIMS-1996
Ionic Equilibrium
229571
**Assertion:** $\mathrm{H}_2 \mathrm{O}$ shows amphoteric nature. **Reason:** According to Bronsted theory, it acts as acid with $\mathrm{NH}_3$ and a base with $\mathrm{H}_2 \mathrm{~S}$.
1 If both Assertion and Reason are correct and 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:
Water has the ability to act as an acid as well as a base i.e. It behaves as an amphoteric substance. In Bronsted sense it act as an acid with $\mathrm{NH}_3$ and base with $\mathrm{H}_2 \mathrm{~S}$. $\mathrm{H}_2 \mathrm{O}(\mathrm{l})+\mathrm{NH}_3$ (aq)?? $\mathrm{OH}^{-}(\mathrm{aq})+\mathrm{NH}_4^{+}(\mathrm{aq})$ $\mathrm{H}_2 \mathrm{O}(\mathrm{l})+\mathrm{H}_2 \mathrm{~S}(\mathrm{aq})$ ? $\mathrm{qu} \mathrm{H}_3 \mathrm{O}^{+}$(aq) $+\mathrm{HS}^{-}$(aq)
AIIMS 26 May 2019(Morning)
Ionic Equilibrium
229576
$\mathrm{pK}_{\mathrm{a}}$ value of four acids are given below. The strongest acid is:
1 4.0
2 3.5
3 2.5
4 2
Explanation:
We know that acidic strength $\propto \mathrm{K}_{\mathrm{n}} \propto \frac{1}{\mathrm{pK}_2}$ Hence acid with lowest $\mathrm{pKa}$ value will be strongest acid. In this question minimum $\mathrm{pKa}$ value is 2 . Hence, It is a strongest acid.
BCECE-2004]
Ionic Equilibrium
229577
Which is Lewis acid?
1 $\mathrm{C}_2 \mathrm{H}_5 \mathrm{OH}$
2 $\mathrm{BF}_3$
3 $\mathrm{Cl}^{-}$
4 $\mathrm{NH}_3$
Explanation:
Lewis acids are those which can accept a pair of non-bonding electron pair. Hence $\mathrm{BF}_3$ is accept electron pair it is Lewis acid. Lewis base are those which can donate a pair of $\mathrm{e}^{-}$pair $\mathrm{C}_2 \mathrm{H}_5 \mathrm{OH}, \mathrm{Cl}^{-}, \mathrm{NH}_3$ all are donate $\mathrm{e}^{-}$pair. Hence, It is a Lewis base.
