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25 July, 04:08

An industrial chemist studying bleaching and sterilizing prepares a hypochlorite buffer using 0.350 M HClO and 0.350 M NaClO. (Ka for HClO = 2.9 * 10-8) Find the pH of 1.00 L of the solution after 0.030 mol of NaOH has been added.

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  1. 25 July, 07:29
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    pH = 7.45

    Explanation:

    This is a buffer solution and we can solve it by using the Henderson-Hasselbalch equation:

    pH = pKa + log ((A⁻) / (HA))

    Here we will first have to calculate the A⁻ formed in the 1. 0 L solution which is formed by the reaction of HClO with the strong base NaOH and add it to the original mol of NaClO

    mol NaClO = mole NaCLO originally present in the 1L of M solution + 0.030 mol produced in the reaction of HCLO with NaOH

    0.350 mol +.030 mol = 0.380 mol

    New concentrations:

    HClO = 0. 350 mol-0.030 mol = 0.320 M (have to sustract the 0.030 mol reacted with NaOH)

    NaClO = 0.380 mol / 1 L = 0.380 M

    Now we have all the values required and we can plug them into the equation

    pH = - log (2.9 x 10^-8) + log (0.380/.320) = 7.45
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