314501
When 0.1 mole of an acid is added to 2 lit of a buffer solution, the \(\mathrm{pH}\) of the buffer decreases by 0.5. The buffer capacity of the solution is
1 0.6
2 0.4
3 0.2
4 0.1
Explanation:
Buffer capacity \(\rm {=\dfrac{\text { no.of moles of an acid added per lit solution }}{p H \text { change }}}\) 0.1 mole of an acid is added to \(\mathrm {2 \mathrm{~L}}\) of a buffer. \(\mathrm {1 \mathrm{~L}}\) of a buffer contains how many moles \(\mathrm {=\dfrac{1 \times 0.1}{2}=0.05}\) \(\mathrm {\mathrm{pH}}\) change \(\mathrm {=0.5}\) \(\mathrm {\therefore}\) Buffer capacity \(\mathrm {=\dfrac{0.05}{0.5}=0.1}\).
CHXI07:EQUILIBRIUM
314502
Buffer capacity of a buffer solution is \(x\), the volume of \({\text{1 M NaOH}}\) added to \(100 \mathrm{~mL}\) of this solution if the change of \(\mathrm{pH}\) by 1 is
1 \({\text{0}}{\text{.1x mL}}\)
2 \({\text{10x mL}}\)
3 \({\text{100x mL}}\)
4 \({\text{x mL}}\)
Explanation:
Moles of \(\mathrm {\mathrm{NaOH}}\) required for \(\mathrm {1 \mathrm{~L}}\) solution \(\mathrm {=}\) \(\mathrm {x}\) Moles of \(\mathrm {\mathrm{NaOH}}\) required for \(\mathrm {100 \mathrm{~mL}}\) of solution \(\mathrm {=0.1 x}\) Now, \(\mathrm {0.1 x=1 \times \mathrm{V}}\) and \(\mathrm {\mathrm{V}=100 x \mathrm{~mL}}\)
CHXI07:EQUILIBRIUM
314503
Assertion : Buffer solutions are composed of strong acids and strong bases. Reason : It maintains the \(\mathrm{pH}\) to a constant value of 7.4.
1 Both Assertion and Reason are correct and Reason is the correct explanation of the Assertion.
2 Both Assertion and Reason are correct but Reason is not the correct explanation of the Assertion.
3 Assertion is correct but Reason is incorrect.
4 Assertion is incorrect but reason is correct.
Explanation:
Both Assertion and Reason are false as buffer solutions are made by mixing weak acid with its salt of strong base or by mixing weak base with its salt of strong acid. It is never formed by mixing strong acid and strong base. The \(\mathrm{pH}\) of buffer solution remains constant but not always equal to 7.4.
AIIMS - 2017
CHXI07:EQUILIBRIUM
314504
Statement A : An aqueous solution of ammonium acetate can act as a buffer. Statement B : Acetic acid is a weak acid and \(\mathrm{NH}_{4} \mathrm{OH}\) is a weak base.
1 Statement A is correct but Statement B is incorrect.
2 Statement A is incorrect but Statement B is correct.
3 Both statements are correct.
4 Both Statements are incorrect.
Explanation:
An aqueous solution of ammonium acetate can act as a natural buffer as it resist changes in \(\mathrm {\mathrm{pH}}\) on dilution or an addition of small amount of acids or alkalies. Moreover, ammonium acetate is a salt of weak acid \(\mathrm {\left(\mathrm{CH}_{3} \mathrm{COOH}\right)}\) and weak base \(\mathrm {\left(\mathrm{NH}_{4} \mathrm{OH}\right)}\). So, the option (3) is correct.
314501
When 0.1 mole of an acid is added to 2 lit of a buffer solution, the \(\mathrm{pH}\) of the buffer decreases by 0.5. The buffer capacity of the solution is
1 0.6
2 0.4
3 0.2
4 0.1
Explanation:
Buffer capacity \(\rm {=\dfrac{\text { no.of moles of an acid added per lit solution }}{p H \text { change }}}\) 0.1 mole of an acid is added to \(\mathrm {2 \mathrm{~L}}\) of a buffer. \(\mathrm {1 \mathrm{~L}}\) of a buffer contains how many moles \(\mathrm {=\dfrac{1 \times 0.1}{2}=0.05}\) \(\mathrm {\mathrm{pH}}\) change \(\mathrm {=0.5}\) \(\mathrm {\therefore}\) Buffer capacity \(\mathrm {=\dfrac{0.05}{0.5}=0.1}\).
CHXI07:EQUILIBRIUM
314502
Buffer capacity of a buffer solution is \(x\), the volume of \({\text{1 M NaOH}}\) added to \(100 \mathrm{~mL}\) of this solution if the change of \(\mathrm{pH}\) by 1 is
1 \({\text{0}}{\text{.1x mL}}\)
2 \({\text{10x mL}}\)
3 \({\text{100x mL}}\)
4 \({\text{x mL}}\)
Explanation:
Moles of \(\mathrm {\mathrm{NaOH}}\) required for \(\mathrm {1 \mathrm{~L}}\) solution \(\mathrm {=}\) \(\mathrm {x}\) Moles of \(\mathrm {\mathrm{NaOH}}\) required for \(\mathrm {100 \mathrm{~mL}}\) of solution \(\mathrm {=0.1 x}\) Now, \(\mathrm {0.1 x=1 \times \mathrm{V}}\) and \(\mathrm {\mathrm{V}=100 x \mathrm{~mL}}\)
CHXI07:EQUILIBRIUM
314503
Assertion : Buffer solutions are composed of strong acids and strong bases. Reason : It maintains the \(\mathrm{pH}\) to a constant value of 7.4.
1 Both Assertion and Reason are correct and Reason is the correct explanation of the Assertion.
2 Both Assertion and Reason are correct but Reason is not the correct explanation of the Assertion.
3 Assertion is correct but Reason is incorrect.
4 Assertion is incorrect but reason is correct.
Explanation:
Both Assertion and Reason are false as buffer solutions are made by mixing weak acid with its salt of strong base or by mixing weak base with its salt of strong acid. It is never formed by mixing strong acid and strong base. The \(\mathrm{pH}\) of buffer solution remains constant but not always equal to 7.4.
AIIMS - 2017
CHXI07:EQUILIBRIUM
314504
Statement A : An aqueous solution of ammonium acetate can act as a buffer. Statement B : Acetic acid is a weak acid and \(\mathrm{NH}_{4} \mathrm{OH}\) is a weak base.
1 Statement A is correct but Statement B is incorrect.
2 Statement A is incorrect but Statement B is correct.
3 Both statements are correct.
4 Both Statements are incorrect.
Explanation:
An aqueous solution of ammonium acetate can act as a natural buffer as it resist changes in \(\mathrm {\mathrm{pH}}\) on dilution or an addition of small amount of acids or alkalies. Moreover, ammonium acetate is a salt of weak acid \(\mathrm {\left(\mathrm{CH}_{3} \mathrm{COOH}\right)}\) and weak base \(\mathrm {\left(\mathrm{NH}_{4} \mathrm{OH}\right)}\). So, the option (3) is correct.
314501
When 0.1 mole of an acid is added to 2 lit of a buffer solution, the \(\mathrm{pH}\) of the buffer decreases by 0.5. The buffer capacity of the solution is
1 0.6
2 0.4
3 0.2
4 0.1
Explanation:
Buffer capacity \(\rm {=\dfrac{\text { no.of moles of an acid added per lit solution }}{p H \text { change }}}\) 0.1 mole of an acid is added to \(\mathrm {2 \mathrm{~L}}\) of a buffer. \(\mathrm {1 \mathrm{~L}}\) of a buffer contains how many moles \(\mathrm {=\dfrac{1 \times 0.1}{2}=0.05}\) \(\mathrm {\mathrm{pH}}\) change \(\mathrm {=0.5}\) \(\mathrm {\therefore}\) Buffer capacity \(\mathrm {=\dfrac{0.05}{0.5}=0.1}\).
CHXI07:EQUILIBRIUM
314502
Buffer capacity of a buffer solution is \(x\), the volume of \({\text{1 M NaOH}}\) added to \(100 \mathrm{~mL}\) of this solution if the change of \(\mathrm{pH}\) by 1 is
1 \({\text{0}}{\text{.1x mL}}\)
2 \({\text{10x mL}}\)
3 \({\text{100x mL}}\)
4 \({\text{x mL}}\)
Explanation:
Moles of \(\mathrm {\mathrm{NaOH}}\) required for \(\mathrm {1 \mathrm{~L}}\) solution \(\mathrm {=}\) \(\mathrm {x}\) Moles of \(\mathrm {\mathrm{NaOH}}\) required for \(\mathrm {100 \mathrm{~mL}}\) of solution \(\mathrm {=0.1 x}\) Now, \(\mathrm {0.1 x=1 \times \mathrm{V}}\) and \(\mathrm {\mathrm{V}=100 x \mathrm{~mL}}\)
CHXI07:EQUILIBRIUM
314503
Assertion : Buffer solutions are composed of strong acids and strong bases. Reason : It maintains the \(\mathrm{pH}\) to a constant value of 7.4.
1 Both Assertion and Reason are correct and Reason is the correct explanation of the Assertion.
2 Both Assertion and Reason are correct but Reason is not the correct explanation of the Assertion.
3 Assertion is correct but Reason is incorrect.
4 Assertion is incorrect but reason is correct.
Explanation:
Both Assertion and Reason are false as buffer solutions are made by mixing weak acid with its salt of strong base or by mixing weak base with its salt of strong acid. It is never formed by mixing strong acid and strong base. The \(\mathrm{pH}\) of buffer solution remains constant but not always equal to 7.4.
AIIMS - 2017
CHXI07:EQUILIBRIUM
314504
Statement A : An aqueous solution of ammonium acetate can act as a buffer. Statement B : Acetic acid is a weak acid and \(\mathrm{NH}_{4} \mathrm{OH}\) is a weak base.
1 Statement A is correct but Statement B is incorrect.
2 Statement A is incorrect but Statement B is correct.
3 Both statements are correct.
4 Both Statements are incorrect.
Explanation:
An aqueous solution of ammonium acetate can act as a natural buffer as it resist changes in \(\mathrm {\mathrm{pH}}\) on dilution or an addition of small amount of acids or alkalies. Moreover, ammonium acetate is a salt of weak acid \(\mathrm {\left(\mathrm{CH}_{3} \mathrm{COOH}\right)}\) and weak base \(\mathrm {\left(\mathrm{NH}_{4} \mathrm{OH}\right)}\). So, the option (3) is correct.
314501
When 0.1 mole of an acid is added to 2 lit of a buffer solution, the \(\mathrm{pH}\) of the buffer decreases by 0.5. The buffer capacity of the solution is
1 0.6
2 0.4
3 0.2
4 0.1
Explanation:
Buffer capacity \(\rm {=\dfrac{\text { no.of moles of an acid added per lit solution }}{p H \text { change }}}\) 0.1 mole of an acid is added to \(\mathrm {2 \mathrm{~L}}\) of a buffer. \(\mathrm {1 \mathrm{~L}}\) of a buffer contains how many moles \(\mathrm {=\dfrac{1 \times 0.1}{2}=0.05}\) \(\mathrm {\mathrm{pH}}\) change \(\mathrm {=0.5}\) \(\mathrm {\therefore}\) Buffer capacity \(\mathrm {=\dfrac{0.05}{0.5}=0.1}\).
CHXI07:EQUILIBRIUM
314502
Buffer capacity of a buffer solution is \(x\), the volume of \({\text{1 M NaOH}}\) added to \(100 \mathrm{~mL}\) of this solution if the change of \(\mathrm{pH}\) by 1 is
1 \({\text{0}}{\text{.1x mL}}\)
2 \({\text{10x mL}}\)
3 \({\text{100x mL}}\)
4 \({\text{x mL}}\)
Explanation:
Moles of \(\mathrm {\mathrm{NaOH}}\) required for \(\mathrm {1 \mathrm{~L}}\) solution \(\mathrm {=}\) \(\mathrm {x}\) Moles of \(\mathrm {\mathrm{NaOH}}\) required for \(\mathrm {100 \mathrm{~mL}}\) of solution \(\mathrm {=0.1 x}\) Now, \(\mathrm {0.1 x=1 \times \mathrm{V}}\) and \(\mathrm {\mathrm{V}=100 x \mathrm{~mL}}\)
CHXI07:EQUILIBRIUM
314503
Assertion : Buffer solutions are composed of strong acids and strong bases. Reason : It maintains the \(\mathrm{pH}\) to a constant value of 7.4.
1 Both Assertion and Reason are correct and Reason is the correct explanation of the Assertion.
2 Both Assertion and Reason are correct but Reason is not the correct explanation of the Assertion.
3 Assertion is correct but Reason is incorrect.
4 Assertion is incorrect but reason is correct.
Explanation:
Both Assertion and Reason are false as buffer solutions are made by mixing weak acid with its salt of strong base or by mixing weak base with its salt of strong acid. It is never formed by mixing strong acid and strong base. The \(\mathrm{pH}\) of buffer solution remains constant but not always equal to 7.4.
AIIMS - 2017
CHXI07:EQUILIBRIUM
314504
Statement A : An aqueous solution of ammonium acetate can act as a buffer. Statement B : Acetic acid is a weak acid and \(\mathrm{NH}_{4} \mathrm{OH}\) is a weak base.
1 Statement A is correct but Statement B is incorrect.
2 Statement A is incorrect but Statement B is correct.
3 Both statements are correct.
4 Both Statements are incorrect.
Explanation:
An aqueous solution of ammonium acetate can act as a natural buffer as it resist changes in \(\mathrm {\mathrm{pH}}\) on dilution or an addition of small amount of acids or alkalies. Moreover, ammonium acetate is a salt of weak acid \(\mathrm {\left(\mathrm{CH}_{3} \mathrm{COOH}\right)}\) and weak base \(\mathrm {\left(\mathrm{NH}_{4} \mathrm{OH}\right)}\). So, the option (3) is correct.
