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quantitive analysis ch 7 solutions

# quantitive analysis ch 7 solutions - Argentometric...

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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. Ag + + Cl - ←→ AgCl Initial mmole 2.5 1.25 Change -1.25 -1.25 Equilibrium mmole 1.25 ____ Equilibrium concn 1.25mmole/50mL = 0.025 M Note: The amount of Ag + from the dissociation of AgCl can be considered negligible relative to excess Ag + at equilibrium. Hence, pAg = -log [Ag + ] pAg = -log 0.025 pAg = 1.6 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 Note: Since both Ca(IO3) 2 and Ba(IO3) 2 produce the same number of ions in solution, their Ksp can be directly used to compare their relative solubilities. The higher the Ksp, the greater is the solubility of the salt. Hence, Ba +2 is the ion that is more insoluble and Ca +2 is the ion that is more soluble.

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