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3 acid base titrations solved and explained

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.

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.