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    Quantitative Chemistry Analysis

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    1) What is the pH of a solution prepared by adding 7.21 mL of 2.14 M NaOH to 1.00 g of hypochlorous acid (HOCl, FW - 52.46, pKa = 7.53), 1.00 g sodium hypochlorite (NaOCl, FW - 74.44) and diluting to 100.0 mL.

    2) What mass of solid citric acid (g) and how many milliliters of 0.500 M NaOH are needed to produce 100.0 mL of a buffer with a pH of 6.50 and a weak base concentration of 0.0250 M. The acidic form of citric acid has the general formula H3A(s), FW - 192.123, and pKa values of 3.128, 4.761, and 6.396. hide problem

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    Solution Summary

    This solution helps explore some quantitative analysis problems within the context of chemistry.

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