229762
The buffering action of an acidic buffer is maximum when its $\mathrm{pH}$ is equal to
1 5
2 7
3 1
4 $\mathrm{pK}_{\mathrm{a}}$
Explanation:
Buffer capacity of an acidic buffer is maximum when the ratio of HA to $\mathrm{A}^{-}$is unity since, $\mathrm{pH}$ of acidic buffer ltbr. $=\mathrm{pK}_{\mathrm{a}}+\log \frac{\left[\mathrm{A}^{-}\right]}{[\mathrm{HA}]}$ For maximum buffer capacity $[\mathrm{A}]=[\mathrm{HA}]$ $\therefore \quad \mathrm{pH}=\mathrm{pK}_{\mathrm{a}}$
UPTU/UPSEE-2009
Ionic Equilibrium
229733
Which of the following can form buffer solution?
1 aq. $\mathrm{NH}_3+\mathrm{NH}_4 \mathrm{OH}$
2 $\mathrm{KOH}+\mathrm{HNO}_3$
3 $\mathrm{NaOH}+\mathrm{HCl}$
4 $\mathrm{K} 1+\mathrm{KOH}$
Explanation:
Ammonia is a weak base and a salt containing its conjugate acid, the ammonium cantion , such as $\mathrm{NH}_4 \mathrm{OH}$ functions as a buffer solution when they are present together in a solutions.
BITSAT-2017
Ionic Equilibrium
229714
Which of the following would produce a buffer solution when mixed in equal volumes?
1 $1 \mathrm{M} \mathrm{CH} \mathrm{CHOH}_3 \mathrm{CO}$ and $0.5 \mathrm{M} \mathrm{NaOH}$
2 $1 \mathrm{M} \mathrm{CH}_3 \mathrm{COOH}$ and $0.5 \mathrm{M} \mathrm{HCl}$
3 $1 \mathrm{M} \mathrm{NH}_4 \mathrm{OH}$ and $0.5 \mathrm{M} \mathrm{NaOH}$
4 $1 \mathrm{M} \mathrm{NH}_4 \mathrm{OH}$ and $0.5 \mathrm{M} \mathrm{HCl}$
Explanation:
$\mathrm{CH}_3 \mathrm{COOH}+\mathrm{NaOH} \rightarrow \mathrm{CH}_3 \mathrm{COONa}+\mathrm{H}_2 \mathrm{O}$ Hence, weak acid, $\mathrm{CH}_3 \mathrm{COOH}$ and its salt with strong base, $\mathrm{CH}_3 \mathrm{COONa}$ act as acidic buffer.
**AP EAMCET (Engg.)- 2001
Ionic Equilibrium
229711
The solutions which tend to keep the concentration of hydrogen ions constant even when small amount of strong acid or strong base are added to them, are known as
1 Acidic solution
2 Alkaline solution
3 Buffer solution
4 Ideal solution
Explanation:
Buffer solution is an aqueous solution consisting of a mixture of a weak acid and its conjugate base. Buffer solution resist the change in its $\mathrm{pH}$ value on adding a small amount of an acid or base.
229762
The buffering action of an acidic buffer is maximum when its $\mathrm{pH}$ is equal to
1 5
2 7
3 1
4 $\mathrm{pK}_{\mathrm{a}}$
Explanation:
Buffer capacity of an acidic buffer is maximum when the ratio of HA to $\mathrm{A}^{-}$is unity since, $\mathrm{pH}$ of acidic buffer ltbr. $=\mathrm{pK}_{\mathrm{a}}+\log \frac{\left[\mathrm{A}^{-}\right]}{[\mathrm{HA}]}$ For maximum buffer capacity $[\mathrm{A}]=[\mathrm{HA}]$ $\therefore \quad \mathrm{pH}=\mathrm{pK}_{\mathrm{a}}$
UPTU/UPSEE-2009
Ionic Equilibrium
229733
Which of the following can form buffer solution?
1 aq. $\mathrm{NH}_3+\mathrm{NH}_4 \mathrm{OH}$
2 $\mathrm{KOH}+\mathrm{HNO}_3$
3 $\mathrm{NaOH}+\mathrm{HCl}$
4 $\mathrm{K} 1+\mathrm{KOH}$
Explanation:
Ammonia is a weak base and a salt containing its conjugate acid, the ammonium cantion , such as $\mathrm{NH}_4 \mathrm{OH}$ functions as a buffer solution when they are present together in a solutions.
BITSAT-2017
Ionic Equilibrium
229714
Which of the following would produce a buffer solution when mixed in equal volumes?
1 $1 \mathrm{M} \mathrm{CH} \mathrm{CHOH}_3 \mathrm{CO}$ and $0.5 \mathrm{M} \mathrm{NaOH}$
2 $1 \mathrm{M} \mathrm{CH}_3 \mathrm{COOH}$ and $0.5 \mathrm{M} \mathrm{HCl}$
3 $1 \mathrm{M} \mathrm{NH}_4 \mathrm{OH}$ and $0.5 \mathrm{M} \mathrm{NaOH}$
4 $1 \mathrm{M} \mathrm{NH}_4 \mathrm{OH}$ and $0.5 \mathrm{M} \mathrm{HCl}$
Explanation:
$\mathrm{CH}_3 \mathrm{COOH}+\mathrm{NaOH} \rightarrow \mathrm{CH}_3 \mathrm{COONa}+\mathrm{H}_2 \mathrm{O}$ Hence, weak acid, $\mathrm{CH}_3 \mathrm{COOH}$ and its salt with strong base, $\mathrm{CH}_3 \mathrm{COONa}$ act as acidic buffer.
**AP EAMCET (Engg.)- 2001
Ionic Equilibrium
229711
The solutions which tend to keep the concentration of hydrogen ions constant even when small amount of strong acid or strong base are added to them, are known as
1 Acidic solution
2 Alkaline solution
3 Buffer solution
4 Ideal solution
Explanation:
Buffer solution is an aqueous solution consisting of a mixture of a weak acid and its conjugate base. Buffer solution resist the change in its $\mathrm{pH}$ value on adding a small amount of an acid or base.
229762
The buffering action of an acidic buffer is maximum when its $\mathrm{pH}$ is equal to
1 5
2 7
3 1
4 $\mathrm{pK}_{\mathrm{a}}$
Explanation:
Buffer capacity of an acidic buffer is maximum when the ratio of HA to $\mathrm{A}^{-}$is unity since, $\mathrm{pH}$ of acidic buffer ltbr. $=\mathrm{pK}_{\mathrm{a}}+\log \frac{\left[\mathrm{A}^{-}\right]}{[\mathrm{HA}]}$ For maximum buffer capacity $[\mathrm{A}]=[\mathrm{HA}]$ $\therefore \quad \mathrm{pH}=\mathrm{pK}_{\mathrm{a}}$
UPTU/UPSEE-2009
Ionic Equilibrium
229733
Which of the following can form buffer solution?
1 aq. $\mathrm{NH}_3+\mathrm{NH}_4 \mathrm{OH}$
2 $\mathrm{KOH}+\mathrm{HNO}_3$
3 $\mathrm{NaOH}+\mathrm{HCl}$
4 $\mathrm{K} 1+\mathrm{KOH}$
Explanation:
Ammonia is a weak base and a salt containing its conjugate acid, the ammonium cantion , such as $\mathrm{NH}_4 \mathrm{OH}$ functions as a buffer solution when they are present together in a solutions.
BITSAT-2017
Ionic Equilibrium
229714
Which of the following would produce a buffer solution when mixed in equal volumes?
1 $1 \mathrm{M} \mathrm{CH} \mathrm{CHOH}_3 \mathrm{CO}$ and $0.5 \mathrm{M} \mathrm{NaOH}$
2 $1 \mathrm{M} \mathrm{CH}_3 \mathrm{COOH}$ and $0.5 \mathrm{M} \mathrm{HCl}$
3 $1 \mathrm{M} \mathrm{NH}_4 \mathrm{OH}$ and $0.5 \mathrm{M} \mathrm{NaOH}$
4 $1 \mathrm{M} \mathrm{NH}_4 \mathrm{OH}$ and $0.5 \mathrm{M} \mathrm{HCl}$
Explanation:
$\mathrm{CH}_3 \mathrm{COOH}+\mathrm{NaOH} \rightarrow \mathrm{CH}_3 \mathrm{COONa}+\mathrm{H}_2 \mathrm{O}$ Hence, weak acid, $\mathrm{CH}_3 \mathrm{COOH}$ and its salt with strong base, $\mathrm{CH}_3 \mathrm{COONa}$ act as acidic buffer.
**AP EAMCET (Engg.)- 2001
Ionic Equilibrium
229711
The solutions which tend to keep the concentration of hydrogen ions constant even when small amount of strong acid or strong base are added to them, are known as
1 Acidic solution
2 Alkaline solution
3 Buffer solution
4 Ideal solution
Explanation:
Buffer solution is an aqueous solution consisting of a mixture of a weak acid and its conjugate base. Buffer solution resist the change in its $\mathrm{pH}$ value on adding a small amount of an acid or base.
229762
The buffering action of an acidic buffer is maximum when its $\mathrm{pH}$ is equal to
1 5
2 7
3 1
4 $\mathrm{pK}_{\mathrm{a}}$
Explanation:
Buffer capacity of an acidic buffer is maximum when the ratio of HA to $\mathrm{A}^{-}$is unity since, $\mathrm{pH}$ of acidic buffer ltbr. $=\mathrm{pK}_{\mathrm{a}}+\log \frac{\left[\mathrm{A}^{-}\right]}{[\mathrm{HA}]}$ For maximum buffer capacity $[\mathrm{A}]=[\mathrm{HA}]$ $\therefore \quad \mathrm{pH}=\mathrm{pK}_{\mathrm{a}}$
UPTU/UPSEE-2009
Ionic Equilibrium
229733
Which of the following can form buffer solution?
1 aq. $\mathrm{NH}_3+\mathrm{NH}_4 \mathrm{OH}$
2 $\mathrm{KOH}+\mathrm{HNO}_3$
3 $\mathrm{NaOH}+\mathrm{HCl}$
4 $\mathrm{K} 1+\mathrm{KOH}$
Explanation:
Ammonia is a weak base and a salt containing its conjugate acid, the ammonium cantion , such as $\mathrm{NH}_4 \mathrm{OH}$ functions as a buffer solution when they are present together in a solutions.
BITSAT-2017
Ionic Equilibrium
229714
Which of the following would produce a buffer solution when mixed in equal volumes?
1 $1 \mathrm{M} \mathrm{CH} \mathrm{CHOH}_3 \mathrm{CO}$ and $0.5 \mathrm{M} \mathrm{NaOH}$
2 $1 \mathrm{M} \mathrm{CH}_3 \mathrm{COOH}$ and $0.5 \mathrm{M} \mathrm{HCl}$
3 $1 \mathrm{M} \mathrm{NH}_4 \mathrm{OH}$ and $0.5 \mathrm{M} \mathrm{NaOH}$
4 $1 \mathrm{M} \mathrm{NH}_4 \mathrm{OH}$ and $0.5 \mathrm{M} \mathrm{HCl}$
Explanation:
$\mathrm{CH}_3 \mathrm{COOH}+\mathrm{NaOH} \rightarrow \mathrm{CH}_3 \mathrm{COONa}+\mathrm{H}_2 \mathrm{O}$ Hence, weak acid, $\mathrm{CH}_3 \mathrm{COOH}$ and its salt with strong base, $\mathrm{CH}_3 \mathrm{COONa}$ act as acidic buffer.
**AP EAMCET (Engg.)- 2001
Ionic Equilibrium
229711
The solutions which tend to keep the concentration of hydrogen ions constant even when small amount of strong acid or strong base are added to them, are known as
1 Acidic solution
2 Alkaline solution
3 Buffer solution
4 Ideal solution
Explanation:
Buffer solution is an aqueous solution consisting of a mixture of a weak acid and its conjugate base. Buffer solution resist the change in its $\mathrm{pH}$ value on adding a small amount of an acid or base.
