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Calculate the pH of 1.0 xx 10^(-3) M s...

Calculate the pH of ` 1.0 xx 10^(-3)` M sodium phenolate `NaOC_(6)H_(5) K_(a) ` for `C_(6)H_(5)OH` is `1 xx 10^(-10)`

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To calculate the pH of a 1.0 x 10^(-3) M sodium phenolate solution, we will follow these steps: ### Step 1: Understand the dissociation of sodium phenolate Sodium phenolate (NaOC₆H₅) dissociates in water to form phenolate ions (C₆H₅O⁻) and sodium ions (Na⁺). The phenolate ion can react with water to produce phenol (C₆H₅OH) and hydroxide ions (OH⁻): \[ \text{C}_6\text{H}_5\text{O}^- + \text{H}_2\text{O} \rightleftharpoons \text{C}_6\text{H}_5\text{OH} + \text{OH}^- \] ### Step 2: Calculate Kb using Kw and Ka ...
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What is the pH of a 0.10 M C_(6)H_(5)O^(-) solution? The K_(a) of C_(6)H_(5)OH is 1.0xx10^(-10)

Calculate the pH of 0.01M solution of AICI_(3), (K_(a) of [AI(H_(2)O)_(6)]^(3+) is 1.4xx10^(-5))

Knowledge Check

  • The pH of 1 xx 10^(-3) M H_(2)O_(2) solution (K_(a)=2.2 xx 10^(-12)) is

    A
    `approx 3`
    B
    slightly less than 7
    C
    slightly greater than 7
    D
    `=7`

  • What is the pH of a 0.200 M solution of C_6H_5COONa ? (The K_a of C_6H_5COOH is 6.4xx10^(-5) )

    A
    5.25
    B
    `5.40`
    C
    `8.60`
    D
    `8.75`

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