Acidic buffer is mixture of weak acid and its salt with strong base, similarly, basic buffer is a mixture of weak base and its salt with strong acid. Hence, $50 \mathrm{~mL} 0.1 \mathrm{M} \mathrm{CH} \mathrm{CH}_3 \mathrm{COOH}+100 \mathrm{~mL} 0.1 \mathrm{M} \mathrm{NaOH}$ does not constitute a buffer solution. Because in this case millimoles of acid are less than that the strong base, which after reaction with strong base gives salt. Now, the solution contains only strong base and salt but no weak acid. Hence, no buffer is formed.
CG PET-2009
Ionic Equilibrium
229736
Heat of neutralisation of $\mathrm{NH}_4 \mathrm{OH}$ and HCl is
1 equal to $13.7 \mathrm{kcal}$
2 more than $13.7 \mathrm{kcal}$
3 less than $13.7 \mathrm{kcal}$
4 more than one is correct
Explanation:
The heat of neutralization is the amount of heat evolved when one gram equivalent of an acid is neutralised by one gram equivalent of a base in dilute solution. $\mathrm{NH}_4 \mathrm{OH}$ is a weak base. Heat of neutralization $<13.7$ $\mathrm{Kcal}$. The heat released in the neutralization of a weak base or a weak acid by a strong acid or a strong base, respectively is less than $13.7 \mathrm{Kcal}$.
CG PET-2004
Ionic Equilibrium
229737
In the combustion of $2.0 \mathrm{~g}$ of methane, $25 \mathrm{kcal}$ heat is liberated, heat of combustion of methane would be
1 $100 \mathrm{kcal}$
2 $200 \mathrm{kcal}$
3 $300 \mathrm{kcal}$
4 $400 \mathrm{kcal}$
Explanation:
$\mathrm{CH}_4+2 \mathrm{O}_2 \rightarrow \mathrm{CO}_2+2 \mathrm{H}_2 \mathrm{O}$ Molecular weight of $\mathrm{CH}_4=12+4=16$ $\therefore$ On the combustion of $2.0 \mathrm{gm}$ of methane $=25.0 \mathrm{kcal}$. $\therefore$ On the combustion of $16.0 \mathrm{gm}=\frac{25 \times 16}{2}=200 \mathrm{kcal}$.
CG PET-2004
Ionic Equilibrium
229738
Which of the following mixtures forms an acid buffer?
Acid buffer $\Rightarrow$ Weak Acid + Strong Base Match in option (a) $\mathrm{NaOH}+\mathrm{HCl}\left(\begin{array}{l}\mathrm{NaOH} \text { strong Base and } \\ \mathrm{HCl} \text { is strong Acid }\end{array}\right)$ (b) $\mathrm{CH}_3 \mathrm{COOH}+\mathrm{CH}_3 \mathrm{COONa}\left(\begin{array}{l}\mathrm{CH}_3 \mathrm{COOH} \text { is weak acid and } \\ \mathrm{CH}_3 \mathrm{COONa} \text { is a strong base }\end{array}\right)$ So, option (b) is correct.
CG PET-2004
Ionic Equilibrium
229740
An aqueous solution of $1 \mathrm{M} \mathrm{NaCl}$ and $1 \mathrm{M} \mathrm{HCl}$ is
1 not a buffer but $\mathrm{pH}<7$
2 not a buffer but $\mathrm{pH}>7$
3 a buffer with $\mathrm{pH}<7$
4 a buffer with $\mathrm{pH}>7$
Explanation:
$\mathrm{NaCl}$ is not the case of buffer $\mathrm{NaCl}$ is salt of strong acid and strong base. $\mathrm{NaCl}+\mathrm{H}_2 \mathrm{O} \quad \mathrm{NaOH}+\mathrm{HCl}$ aqueous $\mathrm{NaCl}$, itself exact neutral solution $\mathrm{HCl}+\mathrm{H}_2 \mathrm{O} \square \mathrm{H}_3 \mathrm{O}^{+}+\mathrm{Cl}^{-}$ make solution acidic. So, not a buffer but $\mathrm{pH}<7$
Acidic buffer is mixture of weak acid and its salt with strong base, similarly, basic buffer is a mixture of weak base and its salt with strong acid. Hence, $50 \mathrm{~mL} 0.1 \mathrm{M} \mathrm{CH} \mathrm{CH}_3 \mathrm{COOH}+100 \mathrm{~mL} 0.1 \mathrm{M} \mathrm{NaOH}$ does not constitute a buffer solution. Because in this case millimoles of acid are less than that the strong base, which after reaction with strong base gives salt. Now, the solution contains only strong base and salt but no weak acid. Hence, no buffer is formed.
CG PET-2009
Ionic Equilibrium
229736
Heat of neutralisation of $\mathrm{NH}_4 \mathrm{OH}$ and HCl is
1 equal to $13.7 \mathrm{kcal}$
2 more than $13.7 \mathrm{kcal}$
3 less than $13.7 \mathrm{kcal}$
4 more than one is correct
Explanation:
The heat of neutralization is the amount of heat evolved when one gram equivalent of an acid is neutralised by one gram equivalent of a base in dilute solution. $\mathrm{NH}_4 \mathrm{OH}$ is a weak base. Heat of neutralization $<13.7$ $\mathrm{Kcal}$. The heat released in the neutralization of a weak base or a weak acid by a strong acid or a strong base, respectively is less than $13.7 \mathrm{Kcal}$.
CG PET-2004
Ionic Equilibrium
229737
In the combustion of $2.0 \mathrm{~g}$ of methane, $25 \mathrm{kcal}$ heat is liberated, heat of combustion of methane would be
1 $100 \mathrm{kcal}$
2 $200 \mathrm{kcal}$
3 $300 \mathrm{kcal}$
4 $400 \mathrm{kcal}$
Explanation:
$\mathrm{CH}_4+2 \mathrm{O}_2 \rightarrow \mathrm{CO}_2+2 \mathrm{H}_2 \mathrm{O}$ Molecular weight of $\mathrm{CH}_4=12+4=16$ $\therefore$ On the combustion of $2.0 \mathrm{gm}$ of methane $=25.0 \mathrm{kcal}$. $\therefore$ On the combustion of $16.0 \mathrm{gm}=\frac{25 \times 16}{2}=200 \mathrm{kcal}$.
CG PET-2004
Ionic Equilibrium
229738
Which of the following mixtures forms an acid buffer?
Acid buffer $\Rightarrow$ Weak Acid + Strong Base Match in option (a) $\mathrm{NaOH}+\mathrm{HCl}\left(\begin{array}{l}\mathrm{NaOH} \text { strong Base and } \\ \mathrm{HCl} \text { is strong Acid }\end{array}\right)$ (b) $\mathrm{CH}_3 \mathrm{COOH}+\mathrm{CH}_3 \mathrm{COONa}\left(\begin{array}{l}\mathrm{CH}_3 \mathrm{COOH} \text { is weak acid and } \\ \mathrm{CH}_3 \mathrm{COONa} \text { is a strong base }\end{array}\right)$ So, option (b) is correct.
CG PET-2004
Ionic Equilibrium
229740
An aqueous solution of $1 \mathrm{M} \mathrm{NaCl}$ and $1 \mathrm{M} \mathrm{HCl}$ is
1 not a buffer but $\mathrm{pH}<7$
2 not a buffer but $\mathrm{pH}>7$
3 a buffer with $\mathrm{pH}<7$
4 a buffer with $\mathrm{pH}>7$
Explanation:
$\mathrm{NaCl}$ is not the case of buffer $\mathrm{NaCl}$ is salt of strong acid and strong base. $\mathrm{NaCl}+\mathrm{H}_2 \mathrm{O} \quad \mathrm{NaOH}+\mathrm{HCl}$ aqueous $\mathrm{NaCl}$, itself exact neutral solution $\mathrm{HCl}+\mathrm{H}_2 \mathrm{O} \square \mathrm{H}_3 \mathrm{O}^{+}+\mathrm{Cl}^{-}$ make solution acidic. So, not a buffer but $\mathrm{pH}<7$
Acidic buffer is mixture of weak acid and its salt with strong base, similarly, basic buffer is a mixture of weak base and its salt with strong acid. Hence, $50 \mathrm{~mL} 0.1 \mathrm{M} \mathrm{CH} \mathrm{CH}_3 \mathrm{COOH}+100 \mathrm{~mL} 0.1 \mathrm{M} \mathrm{NaOH}$ does not constitute a buffer solution. Because in this case millimoles of acid are less than that the strong base, which after reaction with strong base gives salt. Now, the solution contains only strong base and salt but no weak acid. Hence, no buffer is formed.
CG PET-2009
Ionic Equilibrium
229736
Heat of neutralisation of $\mathrm{NH}_4 \mathrm{OH}$ and HCl is
1 equal to $13.7 \mathrm{kcal}$
2 more than $13.7 \mathrm{kcal}$
3 less than $13.7 \mathrm{kcal}$
4 more than one is correct
Explanation:
The heat of neutralization is the amount of heat evolved when one gram equivalent of an acid is neutralised by one gram equivalent of a base in dilute solution. $\mathrm{NH}_4 \mathrm{OH}$ is a weak base. Heat of neutralization $<13.7$ $\mathrm{Kcal}$. The heat released in the neutralization of a weak base or a weak acid by a strong acid or a strong base, respectively is less than $13.7 \mathrm{Kcal}$.
CG PET-2004
Ionic Equilibrium
229737
In the combustion of $2.0 \mathrm{~g}$ of methane, $25 \mathrm{kcal}$ heat is liberated, heat of combustion of methane would be
1 $100 \mathrm{kcal}$
2 $200 \mathrm{kcal}$
3 $300 \mathrm{kcal}$
4 $400 \mathrm{kcal}$
Explanation:
$\mathrm{CH}_4+2 \mathrm{O}_2 \rightarrow \mathrm{CO}_2+2 \mathrm{H}_2 \mathrm{O}$ Molecular weight of $\mathrm{CH}_4=12+4=16$ $\therefore$ On the combustion of $2.0 \mathrm{gm}$ of methane $=25.0 \mathrm{kcal}$. $\therefore$ On the combustion of $16.0 \mathrm{gm}=\frac{25 \times 16}{2}=200 \mathrm{kcal}$.
CG PET-2004
Ionic Equilibrium
229738
Which of the following mixtures forms an acid buffer?
Acid buffer $\Rightarrow$ Weak Acid + Strong Base Match in option (a) $\mathrm{NaOH}+\mathrm{HCl}\left(\begin{array}{l}\mathrm{NaOH} \text { strong Base and } \\ \mathrm{HCl} \text { is strong Acid }\end{array}\right)$ (b) $\mathrm{CH}_3 \mathrm{COOH}+\mathrm{CH}_3 \mathrm{COONa}\left(\begin{array}{l}\mathrm{CH}_3 \mathrm{COOH} \text { is weak acid and } \\ \mathrm{CH}_3 \mathrm{COONa} \text { is a strong base }\end{array}\right)$ So, option (b) is correct.
CG PET-2004
Ionic Equilibrium
229740
An aqueous solution of $1 \mathrm{M} \mathrm{NaCl}$ and $1 \mathrm{M} \mathrm{HCl}$ is
1 not a buffer but $\mathrm{pH}<7$
2 not a buffer but $\mathrm{pH}>7$
3 a buffer with $\mathrm{pH}<7$
4 a buffer with $\mathrm{pH}>7$
Explanation:
$\mathrm{NaCl}$ is not the case of buffer $\mathrm{NaCl}$ is salt of strong acid and strong base. $\mathrm{NaCl}+\mathrm{H}_2 \mathrm{O} \quad \mathrm{NaOH}+\mathrm{HCl}$ aqueous $\mathrm{NaCl}$, itself exact neutral solution $\mathrm{HCl}+\mathrm{H}_2 \mathrm{O} \square \mathrm{H}_3 \mathrm{O}^{+}+\mathrm{Cl}^{-}$ make solution acidic. So, not a buffer but $\mathrm{pH}<7$
Acidic buffer is mixture of weak acid and its salt with strong base, similarly, basic buffer is a mixture of weak base and its salt with strong acid. Hence, $50 \mathrm{~mL} 0.1 \mathrm{M} \mathrm{CH} \mathrm{CH}_3 \mathrm{COOH}+100 \mathrm{~mL} 0.1 \mathrm{M} \mathrm{NaOH}$ does not constitute a buffer solution. Because in this case millimoles of acid are less than that the strong base, which after reaction with strong base gives salt. Now, the solution contains only strong base and salt but no weak acid. Hence, no buffer is formed.
CG PET-2009
Ionic Equilibrium
229736
Heat of neutralisation of $\mathrm{NH}_4 \mathrm{OH}$ and HCl is
1 equal to $13.7 \mathrm{kcal}$
2 more than $13.7 \mathrm{kcal}$
3 less than $13.7 \mathrm{kcal}$
4 more than one is correct
Explanation:
The heat of neutralization is the amount of heat evolved when one gram equivalent of an acid is neutralised by one gram equivalent of a base in dilute solution. $\mathrm{NH}_4 \mathrm{OH}$ is a weak base. Heat of neutralization $<13.7$ $\mathrm{Kcal}$. The heat released in the neutralization of a weak base or a weak acid by a strong acid or a strong base, respectively is less than $13.7 \mathrm{Kcal}$.
CG PET-2004
Ionic Equilibrium
229737
In the combustion of $2.0 \mathrm{~g}$ of methane, $25 \mathrm{kcal}$ heat is liberated, heat of combustion of methane would be
1 $100 \mathrm{kcal}$
2 $200 \mathrm{kcal}$
3 $300 \mathrm{kcal}$
4 $400 \mathrm{kcal}$
Explanation:
$\mathrm{CH}_4+2 \mathrm{O}_2 \rightarrow \mathrm{CO}_2+2 \mathrm{H}_2 \mathrm{O}$ Molecular weight of $\mathrm{CH}_4=12+4=16$ $\therefore$ On the combustion of $2.0 \mathrm{gm}$ of methane $=25.0 \mathrm{kcal}$. $\therefore$ On the combustion of $16.0 \mathrm{gm}=\frac{25 \times 16}{2}=200 \mathrm{kcal}$.
CG PET-2004
Ionic Equilibrium
229738
Which of the following mixtures forms an acid buffer?
Acid buffer $\Rightarrow$ Weak Acid + Strong Base Match in option (a) $\mathrm{NaOH}+\mathrm{HCl}\left(\begin{array}{l}\mathrm{NaOH} \text { strong Base and } \\ \mathrm{HCl} \text { is strong Acid }\end{array}\right)$ (b) $\mathrm{CH}_3 \mathrm{COOH}+\mathrm{CH}_3 \mathrm{COONa}\left(\begin{array}{l}\mathrm{CH}_3 \mathrm{COOH} \text { is weak acid and } \\ \mathrm{CH}_3 \mathrm{COONa} \text { is a strong base }\end{array}\right)$ So, option (b) is correct.
CG PET-2004
Ionic Equilibrium
229740
An aqueous solution of $1 \mathrm{M} \mathrm{NaCl}$ and $1 \mathrm{M} \mathrm{HCl}$ is
1 not a buffer but $\mathrm{pH}<7$
2 not a buffer but $\mathrm{pH}>7$
3 a buffer with $\mathrm{pH}<7$
4 a buffer with $\mathrm{pH}>7$
Explanation:
$\mathrm{NaCl}$ is not the case of buffer $\mathrm{NaCl}$ is salt of strong acid and strong base. $\mathrm{NaCl}+\mathrm{H}_2 \mathrm{O} \quad \mathrm{NaOH}+\mathrm{HCl}$ aqueous $\mathrm{NaCl}$, itself exact neutral solution $\mathrm{HCl}+\mathrm{H}_2 \mathrm{O} \square \mathrm{H}_3 \mathrm{O}^{+}+\mathrm{Cl}^{-}$ make solution acidic. So, not a buffer but $\mathrm{pH}<7$
Acidic buffer is mixture of weak acid and its salt with strong base, similarly, basic buffer is a mixture of weak base and its salt with strong acid. Hence, $50 \mathrm{~mL} 0.1 \mathrm{M} \mathrm{CH} \mathrm{CH}_3 \mathrm{COOH}+100 \mathrm{~mL} 0.1 \mathrm{M} \mathrm{NaOH}$ does not constitute a buffer solution. Because in this case millimoles of acid are less than that the strong base, which after reaction with strong base gives salt. Now, the solution contains only strong base and salt but no weak acid. Hence, no buffer is formed.
CG PET-2009
Ionic Equilibrium
229736
Heat of neutralisation of $\mathrm{NH}_4 \mathrm{OH}$ and HCl is
1 equal to $13.7 \mathrm{kcal}$
2 more than $13.7 \mathrm{kcal}$
3 less than $13.7 \mathrm{kcal}$
4 more than one is correct
Explanation:
The heat of neutralization is the amount of heat evolved when one gram equivalent of an acid is neutralised by one gram equivalent of a base in dilute solution. $\mathrm{NH}_4 \mathrm{OH}$ is a weak base. Heat of neutralization $<13.7$ $\mathrm{Kcal}$. The heat released in the neutralization of a weak base or a weak acid by a strong acid or a strong base, respectively is less than $13.7 \mathrm{Kcal}$.
CG PET-2004
Ionic Equilibrium
229737
In the combustion of $2.0 \mathrm{~g}$ of methane, $25 \mathrm{kcal}$ heat is liberated, heat of combustion of methane would be
1 $100 \mathrm{kcal}$
2 $200 \mathrm{kcal}$
3 $300 \mathrm{kcal}$
4 $400 \mathrm{kcal}$
Explanation:
$\mathrm{CH}_4+2 \mathrm{O}_2 \rightarrow \mathrm{CO}_2+2 \mathrm{H}_2 \mathrm{O}$ Molecular weight of $\mathrm{CH}_4=12+4=16$ $\therefore$ On the combustion of $2.0 \mathrm{gm}$ of methane $=25.0 \mathrm{kcal}$. $\therefore$ On the combustion of $16.0 \mathrm{gm}=\frac{25 \times 16}{2}=200 \mathrm{kcal}$.
CG PET-2004
Ionic Equilibrium
229738
Which of the following mixtures forms an acid buffer?
Acid buffer $\Rightarrow$ Weak Acid + Strong Base Match in option (a) $\mathrm{NaOH}+\mathrm{HCl}\left(\begin{array}{l}\mathrm{NaOH} \text { strong Base and } \\ \mathrm{HCl} \text { is strong Acid }\end{array}\right)$ (b) $\mathrm{CH}_3 \mathrm{COOH}+\mathrm{CH}_3 \mathrm{COONa}\left(\begin{array}{l}\mathrm{CH}_3 \mathrm{COOH} \text { is weak acid and } \\ \mathrm{CH}_3 \mathrm{COONa} \text { is a strong base }\end{array}\right)$ So, option (b) is correct.
CG PET-2004
Ionic Equilibrium
229740
An aqueous solution of $1 \mathrm{M} \mathrm{NaCl}$ and $1 \mathrm{M} \mathrm{HCl}$ is
1 not a buffer but $\mathrm{pH}<7$
2 not a buffer but $\mathrm{pH}>7$
3 a buffer with $\mathrm{pH}<7$
4 a buffer with $\mathrm{pH}>7$
Explanation:
$\mathrm{NaCl}$ is not the case of buffer $\mathrm{NaCl}$ is salt of strong acid and strong base. $\mathrm{NaCl}+\mathrm{H}_2 \mathrm{O} \quad \mathrm{NaOH}+\mathrm{HCl}$ aqueous $\mathrm{NaCl}$, itself exact neutral solution $\mathrm{HCl}+\mathrm{H}_2 \mathrm{O} \square \mathrm{H}_3 \mathrm{O}^{+}+\mathrm{Cl}^{-}$ make solution acidic. So, not a buffer but $\mathrm{pH}<7$