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3 March, 01:28

If 5.3g of the strong base NaOH is dissolved in water to form 1500 ml of solution what are the pH [H3O+] and [OH-]

I got up to OH=0.0883 but idk what to do after

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  1. 3 March, 03:46
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    NaOH is a strong base therefore it completely ionises to give out hydroxide ions.

    Number of moles of NaOH added - 5.3 g / 40 g/mol = 0.1325 mol

    molarity of NaOH - 0.1325 mol/1.5 L = 0.088 mol/L

    since NaOH - - > Na⁺ + OH⁻

    molarity of OH⁻ is 0.088 M

    we can calculate pOH value to find the pH value and then [H₃O⁺]

    pOH = - log (0.088 M)

    pOH = 1.05

    pH + pOH = 14

    Therefore pH = 14 - 1.05 = 12.95

    [H₃O⁺] = antilog (-pH)

    Therefore

    [H₃O⁺] = 1.12 x 10⁻¹³ M
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