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Concentration of a weak acid or base from its dissociation constant and degree of dissociation

The same question, asked 6 times: 4 May 2023 S1*, 9 May 2023 S1*, 13 May 2024 S2*, 19 Apr 2026 S1*, 19 Apr 2026 S2*, 14 May 2026 S2. Every wording below, oldest first.

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  1. Question 1

    4 May 2023 S1

    92
    Calculate the concentration of weak monobasic acid if its degree of dissociation and dissociation constant are 5.0×10−45.0\times10^{-4} and 5.0×10−95.0\times10^{-9} respectively.

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  2. Question 2

    9 May 2023 S1

    92
    Dissociation constant and degree of dissociation of weak acid are 1.8×10−51.8\times10^{-5} and 0.03 respectively. What will be the concentration of solution of weak acid?

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  3. Question 3

    13 May 2024 S2

    55
    What is the molar concentration of acetic acid if value of it's dissociation constant is 1.8×10−51.8\times10^{-5} and degree of dissociation is 0.02?

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  4. Question 4

    19 Apr 2026 S1

    11
    A weak base is 1.3%1.3\% dissociated in its aqueous solution. If KbK_b for weak base is 1.69×10−51.69 \times 10^{-5} at 298298 K. Find the concentration of aqueous solution of weak base.

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  5. Question 5

    19 Apr 2026 S2

    12
    Calculate the molar concentration of weak monobasic acid if Ka=1.8×10−5K_a = 1.8 \times 10^{-5} and degree of dissociation is 0.010.01 ?

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  6. Question 6

    14 May 2026 S2

    10
    Calculate the amount of acetic acid in one liter of its solution if the degree of dissociation is 1.3%1.3\% [Ka=1.8×10−5][K_a = 1.8 \times 10^{-5}]

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