1.

    100 mL of a buffer solution contains 0.1 M NH4_4OH and 0.1 M NH4_4Cl. If Kb_b for NH4_4OH is 1.8 x 10−5^{-5}, what is the pH change when 0.01 moles of HCl are added?

    A

    -4.28

    B

    -0.56

    C

    +4.74

    D

    +0.88

    Question Tags
    📚 Subject:Chemistry
    📑 Chapter:Chemical Equilibrium
    🎯Topic:Buffer Solutions
    🎓 Ncert Level:Application
    🎯Difficulty :Hard
    ⚡ Time Required :3 mins
    🔄Ncert Concepts :Buffer Solutions, Henderson-Hasselbalch Equation, pH calculations, basic buffers

    Related Questions

    1.

    A buffer solution contains 0.2 M formic acid (HCOOH) and 0.3 M sodium formate (HCOONa). The KaK_a of formic acid is 1.8imes10−41.8 imes 10^{-4}. What is the pH of this buffer solution?

    A

    3.52

    B

    3.74

    C

    3.92

    D

    4.11

    Question Tags
    📚 Subject:Chemistry
    📑 Chapter:Chemical Equilibrium
    🎯Topic:Buffer Solutions
    🎓 Ncert Level:Application
    🎯Difficulty :Medium
    ⚡ Time Required :2 mins
    🔄Ncert Concepts :Buffer Solutions, Henderson-Hasselbalch Equation, pH Calculation

    2.

    Which of the following is an example of a buffer solution?

    A

    A mixture of hydrochloric acid and sodium chloride

    B

    A mixture of acetic acid and sodium acetate

    C

    A solution of sodium hydroxide

    D

    A solution of nitric acid

    Question Tags
    📚 Subject:Chemistry
    📑 Chapter:Chemical Equilibrium
    🎯Topic:Buffer Solutions
    🎓 Ncert Level:Understanding
    🎯Difficulty :Easy
    ⚡ Time Required :1 mins
    🔄Ncert Concepts :Buffer Solutions, Acids and Bases

    3.

    A buffer mixture of acetic acid and potassium acetate has pH=5.24.{\rm{pH}} = 5.24. The ratio of [CH3COO−]/[CH3COOH]\left[ {{\rm{C}}{{\rm{H}}_3}{\rm{CO}}{{\rm{O}}^ - }} \right]/\left[ {{\rm{C}}{{\rm{H}}_3}{\rm{COOH}}} \right] in this buffer is, (pKa=4.74):\left( {{\rm{p}}{K_a} = 4.74} \right):

    A

    3:13:1

    B

    1:31:3

    C

    1:11:1

    D

    1:21:2

    Question Tags
    📚 Subject:Chemistry
    📑 Chapter:Chemical Equilibrium
    🎯Topic:Buffer Solutions
    🎓 Ncert Level:Application
    🎯Difficulty :Easy
    ⚡ Time Required :2 mins
    🔄Ncert Concepts :buffer solutions, Henderson-Hasselbalch equation, pH, pKa

    4.

    Buffer solutions have constant acidity and alkalinity because:

    A

    They have large excess of H+{{\rm{H}}^ + } or OH−{\rm{O}}{{\rm{H}}^ - } ions

    B

    They have fixed value of pH

    C

    These give unionised acid or base on reaction with added acid or alkali

    D

    Acids and alkalies in these solutions are shielded from attack by other ions

    Question Tags
    📚 Subject:Chemistry
    📑 Chapter:Chemical Equilibrium
    🎯Topic:Buffer Solutions
    🎓 Ncert Level:Understanding
    🎯Difficulty :Easy
    ⚡ Time Required :2 mins
    🔄Ncert Concepts :buffer solutions, chemical equilibrium, Le Chatelier's principle

    5.

    In a buffer solution consisting of a weak acid and its conjugate base, the ratio of concentration of conjugate base to acid is increased tenfold; then the pH of the solution will:

    A

    Increase by one

    B

    Increase tenfold

    C

    Decrease by one

    D

    Decrease tenfold

    Question Tags
    📚 Subject:Chemistry
    📑 Chapter:Chemical Equilibrium
    🎯Topic:Buffer Solutions
    🎓 Ncert Level:Application
    🎯Difficulty :Easy
    ⚡ Time Required :2 mins
    🔄Ncert Concepts :Buffer solutions, Henderson-Hasselbalch equation, pH

    6.

    1  M  NaCl{\rm{1}}\;{\rm{M}}\;{\rm{NaCl}} and 1  M  HCl{\rm{1}}\;{\rm{M}}\;{\rm{HCl}} are present in an aqueous solution. The solution is

    A

    Not a buffer solution with pH < 7

    B

    Not a buffer solution with pH > 7

    C

    A buffer solution with pH < 7

    D

    A buffer solution with pH > 7

    Question Tags
    📚 Subject:Chemistry
    📑 Chapter:Chemical Equilibrium
    🎯Topic:Buffer Solutions
    🎓 Ncert Level:Understanding
    🎯Difficulty :Easy
    ⚡ Time Required :2 mins
    🔄Ncert Concepts :buffer solutions, pH, strong acids, salts

    7.

    Adding a small amount of strong acid to a buffer solution will primarily:

    A

    Increase the pH significantly

    B

    Decrease the pH significantly

    C

    React with the conjugate base

    D

    Have no effect on the pH

    Question Tags
    📚 Subject:Chemistry
    📑 Chapter:Chemical Equilibrium
    🎯Topic:Buffer Solutions
    🎓 Ncert Level:Application
    🎯Difficulty :Medium
    ⚡ Time Required :1 mins
    🔄Ncert Concepts :Buffer Solutions, Acid-Base Reactions

    8.

    Which will make basic buffer?

    A

    50 mL of 0.1 M NaOH + 25 mL of 0.1 MCH3COOH{\rm{50}}\,{\rm{mL}}\,{\rm{of}}\,{\rm{0}}{\rm{.1}}\,{\rm{M}}\,{\rm{NaOH}}\,{\rm{ + }}\,{\rm{25}}\,{\rm{mL}}\,{\rm{of}}\,{\rm{0}}{\rm{.1}}\,{\rm{M C}}{{\rm{H}}_{\rm{3}}}{\rm{COOH}}

    B

    100 mL of 0.1 M CH3COOH +  100 mL of 0.1 M NaOH{\rm{100}}\,{\rm{mL}}\,{\rm{of}}\,0.{\rm{1}}\,{\rm{M}}\,{\rm{C}}{{\rm{H}}_3}{\rm{COOH}}\,{\rm{ + }}\,\,10{\rm{0}}\,{\rm{mL}}\,{\rm{of}}\,0.1\,{\rm{M}}\,{\rm{NaOH}}

    C

    100 mL of 0.1 M HCL + 200 mL of 0.1 M NH4OH{\rm{100}}\,{\rm{mL}}\,{\rm{of}}\,0.1\,{\rm{M}}\,{\rm{HCL}}\,{\rm{ + }}\,20{\rm{0}}\,{\rm{mL}}\,{\rm{of}}\,0.{\rm{1}}\,{\rm{M}}\,{\rm{N}}{{\rm{H}}_4}{\rm{OH}}

    D

    100 mL of 0.1 M HCL + 100 mL of 0.1 M NaOH{\rm{100}}\,{\rm{mL}}\,{\rm{of}}\,0.{\rm{1}}\,{\rm{M}}\,{\rm{HCL}}\,{\rm{ + }}\,10{\rm{0}}\,{\rm{mL}}\,{\rm{of}}\,0.1\,{\rm{M}}\,{\rm{NaOH}}

    Question Tags
    📚 Subject:Chemistry
    📑 Chapter:Chemical Equilibrium
    🎯Topic:Buffer Solutions
    🎓 Ncert Level:Analyzing
    🎯Difficulty :Easy
    ⚡ Time Required :3 mins
    🔄Ncert Concepts :Buffer solutions, Weak acid/base, Neutralization reaction

    9.

    50  mL50\;mL of 2  N2\;N acetic mixed with 10  mL10\;mL of 1  N1\;N sodium acetate solution will have an approximate pH{\rm{pH}} of (Ka=10−5):\left( {{K_a} = {{10}^{ - 5}}} \right):

    A

    4

    B

    5

    C

    6

    D

    7

    Question Tags
    📚 Subject:Chemistry
    📑 Chapter:Chemical Equilibrium
    🎯Topic:Buffer Solutions
    🎓 Ncert Level:Application
    🎯Difficulty :Medium
    ⚡ Time Required :3 mins
    🔄Ncert Concepts :Acid-Base Chemistry, Henderson-Hasselbalch Equation, Normality, Molarity

    10.

    Which will make basic buffer?

    A

    50 mL of 0.1 M NaOH + 25 mL of 0.1 MCH3COOH{\rm{50}}\,{\rm{mL}}\,{\rm{of}}\,{\rm{0}}{\rm{.1}}\,{\rm{M}}\,{\rm{NaOH}}\,{\rm{ + }}\,{\rm{25}}\,{\rm{mL}}\,{\rm{of}}\,{\rm{0}}{\rm{.1}}\,{\rm{M C}}{{\rm{H}}_{\rm{3}}}{\rm{COOH}}

    B

    100 mL of 0.1 M CH3COOH +  100 mL of 0.1 M NaOH{\rm{100}}\,{\rm{mL}}\,{\rm{of}}\,0.{\rm{1}}\,{\rm{M}}\,{\rm{C}}{{\rm{H}}_3}{\rm{COOH}}\,{\rm{ + }}\,\,10{\rm{0}}\,{\rm{mL}}\,{\rm{of}}\,0.1\,{\rm{M}}\,{\rm{NaOH}}

    C

    100 mL of 0.1 M HCL + 200 mL of 0.1 M NH4OH{\rm{100}}\,{\rm{mL}}\,{\rm{of}}\,0.1\,{\rm{M}}\,{\rm{HCL}}\,{\rm{ + }}\,20{\rm{0}}\,{\rm{mL}}\,{\rm{of}}\,0.{\rm{1}}\,{\rm{M}}\,{\rm{N}}{{\rm{H}}_4}{\rm{OH}}

    D

    100 mL of 0.1 M HCL + 100 mL of 0.1 M NaOH{\rm{100}}\,{\rm{mL}}\,{\rm{of}}\,0.{\rm{1}}\,{\rm{M}}\,{\rm{HCL}}\,{\rm{ + }}\,10{\rm{0}}\,{\rm{mL}}\,{\rm{of}}\,0.1\,{\rm{M}}\,{\rm{NaOH}}

    Question Tags
    📚 Subject:Chemistry
    📑 Chapter:Chemical Equilibrium
    🎯Topic:Buffer Solutions
    🎓 Ncert Level:Analyzing
    🎯Difficulty :Easy
    ⚡ Time Required :3 mins
    🔄Ncert Concepts :buffer solutions, weak base, strong acid, stoichiometry, neutralization

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