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    3 acid base titrations solved and explained

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    How many milliliters of 0.105 M HCl are needed to titrate each of the following solutions to the equivalence point:

    -- 45.0 mL of 0.0950 M NaOH
    -- 22.5 mL of 0.118 M NH3
    -- 125.0 mL of solution that contains 1.35g of NaOH per liter.

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    Solution Preview

    0.105M HCl means 0.105 moles of hydrochloric acid per liter of solution

    Other useful numbers: molar mass of HCl = 36.46 g/mol
    molar mass of NaOH = 39.9971 g/mol
    molar mass of NH3 = 17.0306 (though it exists in solution as NH4OH, which has a mol. mass of 35.046)

    Other useful facts: HCl is monoprotic, meaning it is an acid that donates only a single proton
    NaOH and NH3 are ...

    Solution Summary

    The question asks for how much of a certain concentration of acid is required to titrate to equivalence 3 different amounts of 3 different bases. The solution and full explanation are given.