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31 March, 13:17

If 25 mls of 0.01 M NaOH is added to 75 mls of 0.005 HCl, what is the resulting pH

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  1. 31 March, 16:32
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    pH of the resulting solution will be 2.9.

    Explanation:

    25 ml of 0.01 M NaOH contains = 25 * 0.01 = 0.25 milli moles

    75 ml of 0.005 M HCl contains = 75 * 0.005 = 0.375 milli moles

    (0.375 - 0.25) = 0.125 milli moles

    0.125 milli moles of each NaOH and HCl may neutralize each other and so the final solution may contain 0.125 milli moles of HCl.

    In 1 L or 1000 ml of the solution, the quantity of HCl present is 0.125 * 10 = 1.25 milli moles

    It can be converted to moles by dividing milli moles by 1000, we will get,

    0.00125 moles

    So the concentration of Hydrogen ions, [H⁺] = 0.00125 M

    pH = - log₁₀[H⁺]

    = - log₁₀[0.00125]

    = 2.9

    So pH of the resulting solution will be 2.9.
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