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Calculate the concentration of H(3)O^(+)...

Calculate the concentration of `H_(3)O^(+)` ions in a mixture of 0.02 M acetic acid and 0.2 M sodium acetate. Given that the ionization constant `(K_(a))` for acetic acid is `1.8xx10^(-5)`.

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AI Generated Solution

To calculate the concentration of \( H_3O^+ \) ions in a mixture of 0.02 M acetic acid and 0.2 M sodium acetate, we can use the Henderson-Hasselbalch equation, which is applicable for buffer solutions. ### Step-by-Step Solution: 1. **Identify the Components**: - Acetic acid (\( CH_3COOH \)) is a weak acid. - Sodium acetate (\( CH_3COONa \)) is the salt of the weak acid and provides the conjugate base (\( CH_3COO^- \)). ...
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Calculate the concentration of H_3O^+ ions in a mixture of 0.02 M acetic acid and 0.1 M sodium acetate. K_alpha for acetic acid is 1.8 xx 10^(-5) .

What would be the pH of 0.1 molar sodium acetate solution, given that the dissociation constant of acetic acid is 1.8xx10^(-5) .

Knowledge Check

  • A buffer solution contains 0.1 M of acetic acid and 0.1 M of sodium acetate. What will be its pH, it pK_(a) of acetic acid is 4.75

    A
    `4.00`
    B
    4.75
    C
    `5.00`
    D
    5.25

  • At 298 K a 0.1 M CH_(3)COOH solution is 1.34% ionized. The ionization constant K_(a) for acetic acid will be

    A
    `1.82 xx 10^(-5)`
    B
    `18.2 xx 10^(-5)`
    C
    `0.182 xx 10^(-5)`
    D
    None of these

    • Similar Questions

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    Calculate the pH of a buffer which is 0.1 M in acetic acid and 0.15 M in sodium acetate. Given that the ionization constants of acetic acid is 1.75xx10^(-5) . Also calculate the change in pH of the buffer if to 1 litre of the buffer (i) 1 cc of 1 M NaOH are added (ii) 1 cc of 1 M HCl are added. Assume that the change in volume is negligible. What will be the buffer index of the above buffer ?

    Calculate t the H^(+) ion concentration in 0.10 M acetic acid solution. Given that the dissociation constant of acetic acid in water is 1.8xx10^(-5)

    Calculate the H^(+) ion concentration in 0.10 M acetic acid solution. Given that the dissociation constant of acetic acid in water is 1.8xx10^(-5) .

    Calculate the percent ionization of 0.10M acetic acid (K_a=1.8xx10^(-5)) .

    Calculate the H^+ ion concentration in 0.10 M acetic acid solution- Given that the dissociation constant of acetic acid in water is 1.8 xx 10^(-6) .

    Calculate the hydrogen ion concentration ( "in mol"//dm^3 ) in a solution containing 0.04 mole of acetic acid and 0.05 mole of sodium acetate in 500 mL of solution.Dissociation constant for acetic acid is 1.75xx10^(-6) Report your answer after multiplying by 2xx10^(6)

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