Find the ionic strength

a) A solution of 0.00499 M FeSO3

b) A solution of 0.00128 M CuCl2

c) A solution of 0.000736 M HCl and 0.000474 M La(NO3)3

d) 0.00040 M La(IO3)3 Assume complete dissociation at this low concentration and no hydrolysis reaction to form LaOH2 .

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Casey DurganLv2

31 Dec 2019

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THIS IS A FOUR PART QUESTION. HELP NEEDED. THANK YOU VERY MUCH.

a) Using the solubility of Ca(IO3) 2 that you determined in pure water, calculate the value of K sp using only concentrations, that is assuming that all activity coefficients are 1.0. Use 3 sig figs. Solubility of Ca(IO3)2 in Water: 0.00828 mols/L

b) Using the solubility of Ca(IO3)2 that you determined in 0.01M KIO3 as a solvent (the answer from part a), calculate the value of Ksp using only concentrations, that is assuming that all activity coefficients are 1.0. Solubility of Ca(IO3)2 = 0.00327

c) The next few questions will incorporate activity effects into the calculation of Ksp for Ca(IO3)2 using your data from the saturated solution of Ca(IO3)2 in pure water.To do so, we must first know the ionic strength of the solutions. Use your value of the solubility of Ca(IO3)2 in pure water to calculate the ionic strength of that solution.

d) Using the value of the ionic strength of a saturated solution of Ca(IO3)2 in pure water, use TABLE I under the solubility product experiment from the laboratory manual, and enter the activity coefficient for Ca2+ ions listed there at the ionic strength closest to that of the saturated solution of Ca(IO3)2 in pure water. If your ionic strength happens to lie exactly between two values in TABLE I, then use the activity coefficient for the higher ionic strength.