229720
The Henderson's equation for a basic buffer is
1 $\mathrm{pOH}=\mathrm{pK}_{\mathrm{b}}+\log \frac{[\text { Salt }]}{[\text { Base }]}$
2 $\mathrm{pOH}=\mathrm{pK}_{\mathrm{b}}-\log \frac{[\text { Salt }]}{[\text { Base }]}$
3 $\mathrm{pOH}=\mathrm{pK}_{\mathrm{b}}+\log \frac{[\text { Base }]}{[\text { Salt }]}$
4 $\mathrm{pOH}=\mathrm{pK}_{\mathrm{b}}+\frac{[\text { Salt }]}{[\text { Base }]}$
Explanation:
The Henderson's equation for a basic buffer is $\mathrm{pOH}=\mathrm{pK}_{\mathrm{b}}+\log \frac{[\text { Salt }]}{[\text { Base }]} \& \mathrm{pH}=14-\mathrm{pOH}$
Manipal-2018
Ionic Equilibrium
229721
Which of the following is a buffer solution?
Buffer solution is made by taking a solution of weak base $\left(\mathrm{NH}_4 \mathrm{OH}\right)$ and one of its salt with strong acid $\left(\mathrm{NH}_4 \mathrm{Cl}\right)$ [or weak acid and its salt]. It resists a change in $\mathrm{pH}$ upon addition of small amount of strong acid or strong base. Therefore (d) is a buffer solution.
COMEDK-2016
Ionic Equilibrium
229712
Which of the following solutions cannot act as a buffer?
$\mathrm{HCl}+\mathrm{NH}_4 \mathrm{Cl}$ cannot act as a buffer because it is a mixture of strong acid and weak base.
AP-EAMCET-1998
Ionic Equilibrium
229719
Which among the following pairs constitute a buffer?
1 $\mathrm{LiOH} \& \mathrm{LiCl}$
2 $\mathrm{HNO}_3 \& \mathrm{NH}_4 \mathrm{NO}_3$
3 $\mathrm{HNO}_2 \& \mathrm{NaNO}_2$
4 $\mathrm{HBr} \& \mathrm{KBr}$
Explanation:
As we know that, $\mathrm{HNO}_2$ is a weak acid and $\mathrm{NaNO}_2$ is salt of that weak acid and strong base $(\mathrm{NaOH})$. So, both pair of $\mathrm{HNO}_2$ and $\mathrm{NaNO}_2$ formed the buffer solution.
Shift-I
Ionic Equilibrium
229729
Which one of the following statements is not correct?
1 The $\mathrm{pH}$ of $1.0 \times 10^{-8} \mathrm{M} \mathrm{HCl}$ is less than 7
2 The ionic product of water at $25^{\circ} \mathrm{C}$ is $1.0 \times 10^{-14} \mathrm{~mol}^2 \mathrm{~L}^{-2}$
3 $\mathrm{Cl}^{-}$is a Lewis acid
4 Bronsted Lowry theory cannot explain the acidic character of $\mathrm{AlCl}_3$
Explanation:
Chlorine $\left(\mathrm{Cl}^{-}\right)$is a Lewis base because it octet is complete and tendency to give an electros.
229720
The Henderson's equation for a basic buffer is
1 $\mathrm{pOH}=\mathrm{pK}_{\mathrm{b}}+\log \frac{[\text { Salt }]}{[\text { Base }]}$
2 $\mathrm{pOH}=\mathrm{pK}_{\mathrm{b}}-\log \frac{[\text { Salt }]}{[\text { Base }]}$
3 $\mathrm{pOH}=\mathrm{pK}_{\mathrm{b}}+\log \frac{[\text { Base }]}{[\text { Salt }]}$
4 $\mathrm{pOH}=\mathrm{pK}_{\mathrm{b}}+\frac{[\text { Salt }]}{[\text { Base }]}$
Explanation:
The Henderson's equation for a basic buffer is $\mathrm{pOH}=\mathrm{pK}_{\mathrm{b}}+\log \frac{[\text { Salt }]}{[\text { Base }]} \& \mathrm{pH}=14-\mathrm{pOH}$
Manipal-2018
Ionic Equilibrium
229721
Which of the following is a buffer solution?
Buffer solution is made by taking a solution of weak base $\left(\mathrm{NH}_4 \mathrm{OH}\right)$ and one of its salt with strong acid $\left(\mathrm{NH}_4 \mathrm{Cl}\right)$ [or weak acid and its salt]. It resists a change in $\mathrm{pH}$ upon addition of small amount of strong acid or strong base. Therefore (d) is a buffer solution.
COMEDK-2016
Ionic Equilibrium
229712
Which of the following solutions cannot act as a buffer?
$\mathrm{HCl}+\mathrm{NH}_4 \mathrm{Cl}$ cannot act as a buffer because it is a mixture of strong acid and weak base.
AP-EAMCET-1998
Ionic Equilibrium
229719
Which among the following pairs constitute a buffer?
1 $\mathrm{LiOH} \& \mathrm{LiCl}$
2 $\mathrm{HNO}_3 \& \mathrm{NH}_4 \mathrm{NO}_3$
3 $\mathrm{HNO}_2 \& \mathrm{NaNO}_2$
4 $\mathrm{HBr} \& \mathrm{KBr}$
Explanation:
As we know that, $\mathrm{HNO}_2$ is a weak acid and $\mathrm{NaNO}_2$ is salt of that weak acid and strong base $(\mathrm{NaOH})$. So, both pair of $\mathrm{HNO}_2$ and $\mathrm{NaNO}_2$ formed the buffer solution.
Shift-I
Ionic Equilibrium
229729
Which one of the following statements is not correct?
1 The $\mathrm{pH}$ of $1.0 \times 10^{-8} \mathrm{M} \mathrm{HCl}$ is less than 7
2 The ionic product of water at $25^{\circ} \mathrm{C}$ is $1.0 \times 10^{-14} \mathrm{~mol}^2 \mathrm{~L}^{-2}$
3 $\mathrm{Cl}^{-}$is a Lewis acid
4 Bronsted Lowry theory cannot explain the acidic character of $\mathrm{AlCl}_3$
Explanation:
Chlorine $\left(\mathrm{Cl}^{-}\right)$is a Lewis base because it octet is complete and tendency to give an electros.
NEET Test Series from KOTA - 10 Papers In MS WORD
WhatsApp Here
Ionic Equilibrium
229720
The Henderson's equation for a basic buffer is
1 $\mathrm{pOH}=\mathrm{pK}_{\mathrm{b}}+\log \frac{[\text { Salt }]}{[\text { Base }]}$
2 $\mathrm{pOH}=\mathrm{pK}_{\mathrm{b}}-\log \frac{[\text { Salt }]}{[\text { Base }]}$
3 $\mathrm{pOH}=\mathrm{pK}_{\mathrm{b}}+\log \frac{[\text { Base }]}{[\text { Salt }]}$
4 $\mathrm{pOH}=\mathrm{pK}_{\mathrm{b}}+\frac{[\text { Salt }]}{[\text { Base }]}$
Explanation:
The Henderson's equation for a basic buffer is $\mathrm{pOH}=\mathrm{pK}_{\mathrm{b}}+\log \frac{[\text { Salt }]}{[\text { Base }]} \& \mathrm{pH}=14-\mathrm{pOH}$
Manipal-2018
Ionic Equilibrium
229721
Which of the following is a buffer solution?
Buffer solution is made by taking a solution of weak base $\left(\mathrm{NH}_4 \mathrm{OH}\right)$ and one of its salt with strong acid $\left(\mathrm{NH}_4 \mathrm{Cl}\right)$ [or weak acid and its salt]. It resists a change in $\mathrm{pH}$ upon addition of small amount of strong acid or strong base. Therefore (d) is a buffer solution.
COMEDK-2016
Ionic Equilibrium
229712
Which of the following solutions cannot act as a buffer?
$\mathrm{HCl}+\mathrm{NH}_4 \mathrm{Cl}$ cannot act as a buffer because it is a mixture of strong acid and weak base.
AP-EAMCET-1998
Ionic Equilibrium
229719
Which among the following pairs constitute a buffer?
1 $\mathrm{LiOH} \& \mathrm{LiCl}$
2 $\mathrm{HNO}_3 \& \mathrm{NH}_4 \mathrm{NO}_3$
3 $\mathrm{HNO}_2 \& \mathrm{NaNO}_2$
4 $\mathrm{HBr} \& \mathrm{KBr}$
Explanation:
As we know that, $\mathrm{HNO}_2$ is a weak acid and $\mathrm{NaNO}_2$ is salt of that weak acid and strong base $(\mathrm{NaOH})$. So, both pair of $\mathrm{HNO}_2$ and $\mathrm{NaNO}_2$ formed the buffer solution.
Shift-I
Ionic Equilibrium
229729
Which one of the following statements is not correct?
1 The $\mathrm{pH}$ of $1.0 \times 10^{-8} \mathrm{M} \mathrm{HCl}$ is less than 7
2 The ionic product of water at $25^{\circ} \mathrm{C}$ is $1.0 \times 10^{-14} \mathrm{~mol}^2 \mathrm{~L}^{-2}$
3 $\mathrm{Cl}^{-}$is a Lewis acid
4 Bronsted Lowry theory cannot explain the acidic character of $\mathrm{AlCl}_3$
Explanation:
Chlorine $\left(\mathrm{Cl}^{-}\right)$is a Lewis base because it octet is complete and tendency to give an electros.
229720
The Henderson's equation for a basic buffer is
1 $\mathrm{pOH}=\mathrm{pK}_{\mathrm{b}}+\log \frac{[\text { Salt }]}{[\text { Base }]}$
2 $\mathrm{pOH}=\mathrm{pK}_{\mathrm{b}}-\log \frac{[\text { Salt }]}{[\text { Base }]}$
3 $\mathrm{pOH}=\mathrm{pK}_{\mathrm{b}}+\log \frac{[\text { Base }]}{[\text { Salt }]}$
4 $\mathrm{pOH}=\mathrm{pK}_{\mathrm{b}}+\frac{[\text { Salt }]}{[\text { Base }]}$
Explanation:
The Henderson's equation for a basic buffer is $\mathrm{pOH}=\mathrm{pK}_{\mathrm{b}}+\log \frac{[\text { Salt }]}{[\text { Base }]} \& \mathrm{pH}=14-\mathrm{pOH}$
Manipal-2018
Ionic Equilibrium
229721
Which of the following is a buffer solution?
Buffer solution is made by taking a solution of weak base $\left(\mathrm{NH}_4 \mathrm{OH}\right)$ and one of its salt with strong acid $\left(\mathrm{NH}_4 \mathrm{Cl}\right)$ [or weak acid and its salt]. It resists a change in $\mathrm{pH}$ upon addition of small amount of strong acid or strong base. Therefore (d) is a buffer solution.
COMEDK-2016
Ionic Equilibrium
229712
Which of the following solutions cannot act as a buffer?
$\mathrm{HCl}+\mathrm{NH}_4 \mathrm{Cl}$ cannot act as a buffer because it is a mixture of strong acid and weak base.
AP-EAMCET-1998
Ionic Equilibrium
229719
Which among the following pairs constitute a buffer?
1 $\mathrm{LiOH} \& \mathrm{LiCl}$
2 $\mathrm{HNO}_3 \& \mathrm{NH}_4 \mathrm{NO}_3$
3 $\mathrm{HNO}_2 \& \mathrm{NaNO}_2$
4 $\mathrm{HBr} \& \mathrm{KBr}$
Explanation:
As we know that, $\mathrm{HNO}_2$ is a weak acid and $\mathrm{NaNO}_2$ is salt of that weak acid and strong base $(\mathrm{NaOH})$. So, both pair of $\mathrm{HNO}_2$ and $\mathrm{NaNO}_2$ formed the buffer solution.
Shift-I
Ionic Equilibrium
229729
Which one of the following statements is not correct?
1 The $\mathrm{pH}$ of $1.0 \times 10^{-8} \mathrm{M} \mathrm{HCl}$ is less than 7
2 The ionic product of water at $25^{\circ} \mathrm{C}$ is $1.0 \times 10^{-14} \mathrm{~mol}^2 \mathrm{~L}^{-2}$
3 $\mathrm{Cl}^{-}$is a Lewis acid
4 Bronsted Lowry theory cannot explain the acidic character of $\mathrm{AlCl}_3$
Explanation:
Chlorine $\left(\mathrm{Cl}^{-}\right)$is a Lewis base because it octet is complete and tendency to give an electros.
229720
The Henderson's equation for a basic buffer is
1 $\mathrm{pOH}=\mathrm{pK}_{\mathrm{b}}+\log \frac{[\text { Salt }]}{[\text { Base }]}$
2 $\mathrm{pOH}=\mathrm{pK}_{\mathrm{b}}-\log \frac{[\text { Salt }]}{[\text { Base }]}$
3 $\mathrm{pOH}=\mathrm{pK}_{\mathrm{b}}+\log \frac{[\text { Base }]}{[\text { Salt }]}$
4 $\mathrm{pOH}=\mathrm{pK}_{\mathrm{b}}+\frac{[\text { Salt }]}{[\text { Base }]}$
Explanation:
The Henderson's equation for a basic buffer is $\mathrm{pOH}=\mathrm{pK}_{\mathrm{b}}+\log \frac{[\text { Salt }]}{[\text { Base }]} \& \mathrm{pH}=14-\mathrm{pOH}$
Manipal-2018
Ionic Equilibrium
229721
Which of the following is a buffer solution?
Buffer solution is made by taking a solution of weak base $\left(\mathrm{NH}_4 \mathrm{OH}\right)$ and one of its salt with strong acid $\left(\mathrm{NH}_4 \mathrm{Cl}\right)$ [or weak acid and its salt]. It resists a change in $\mathrm{pH}$ upon addition of small amount of strong acid or strong base. Therefore (d) is a buffer solution.
COMEDK-2016
Ionic Equilibrium
229712
Which of the following solutions cannot act as a buffer?
$\mathrm{HCl}+\mathrm{NH}_4 \mathrm{Cl}$ cannot act as a buffer because it is a mixture of strong acid and weak base.
AP-EAMCET-1998
Ionic Equilibrium
229719
Which among the following pairs constitute a buffer?
1 $\mathrm{LiOH} \& \mathrm{LiCl}$
2 $\mathrm{HNO}_3 \& \mathrm{NH}_4 \mathrm{NO}_3$
3 $\mathrm{HNO}_2 \& \mathrm{NaNO}_2$
4 $\mathrm{HBr} \& \mathrm{KBr}$
Explanation:
As we know that, $\mathrm{HNO}_2$ is a weak acid and $\mathrm{NaNO}_2$ is salt of that weak acid and strong base $(\mathrm{NaOH})$. So, both pair of $\mathrm{HNO}_2$ and $\mathrm{NaNO}_2$ formed the buffer solution.
Shift-I
Ionic Equilibrium
229729
Which one of the following statements is not correct?
1 The $\mathrm{pH}$ of $1.0 \times 10^{-8} \mathrm{M} \mathrm{HCl}$ is less than 7
2 The ionic product of water at $25^{\circ} \mathrm{C}$ is $1.0 \times 10^{-14} \mathrm{~mol}^2 \mathrm{~L}^{-2}$
3 $\mathrm{Cl}^{-}$is a Lewis acid
4 Bronsted Lowry theory cannot explain the acidic character of $\mathrm{AlCl}_3$
Explanation:
Chlorine $\left(\mathrm{Cl}^{-}\right)$is a Lewis base because it octet is complete and tendency to give an electros.