Question:

What is the pH of the solution created by ?

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combining 12.60 mL of the 0.10 M NaOH(aq) with 8.00 mL of the 0.10 M HCl(aq)?

with 8.00 mL of the 0.10 M HC2H3O2(aq)?

What are the pH values if you take into account that the 8.00 mL of 0.10 M Acid was first diluted with 100 mL of water?

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  1. Moles NaOH = 0.01260 L x 0.10 = 0.001260

    Moles HCl = 0.0080 L x 0.10 = 0.00080

    Moles OH- in excess = 0.00046

    total volume = 0.0206 L

    [OH-] = 0.00046/ 0.0206 =0.0223 M

    pOH =1.65

    pH = 14 - 1.65 = 12.35

    If the acid is a weak acid this does not affect the pH because the concentation of H+ is in excess

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