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    Argentometric titrations

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    Argentometric titrations typically use a standard solution of silver ions to form a silver halide precipitate. Calculate the pAg+ value when 25.0 mL of 0.100 M AgNO3 is added to 25.0 mL of 0.0500 M chloride ion.

    A solution of NaIO3 was used to titrate 50.0 mL of a mixture containing 0.100 M Ca2+ and 0.100 M Ba2+. Calculate the concentration of the most insoluble ion when the most soluble ion begins to precipitate. Ksp for Ca(IO3)2 = 7.1 x 10-7 and Ksp for Ba(IO3)2 = 1.5 x 10-9

    A 0.05002 gram sample of methyl amine (CH3NH2: MW = 31.07 g/mol; Kb = 4.35 x 10-4) was mixed with 100.0 mL of HCl. Calculate the molar concentration of the acid if 5.55 mL of 0.1057 M KOH was needed to back-titrate the unreacted acid.

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    https://brainmass.com/chemistry/experimental-design-and-methods-in-chemistry/argentometric-titrations-281040

    Solution Summary

    This solution helps explore the concept of argentometric titrations within the context of chemistry.

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