CHEM 6C Chapter Notes - Chapter 22: Ionic Compound, Reaction Quotient, Equilibrium Constant

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browngnu790

17 Apr 2016

School

UCSD

Department

Chemistry and Biochemistry

Course

CHEM 6C

Professor

Stacey Brydges

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22. 2 common ion efect: the solubility of an ionic solid decreases when a common ion is present in the soluion, ex: determine the solubility of agbro3 in 0. 10m nabro3 soluion. Present in the soluion, so the addiion of the ion shits equilibrium to the let towards the solid agbro3, decreasing its solubility. S = 5. 4 x 10-4m (the solubility in pure water is 7. 3 x 10-3m: common ion efect oten used in separaions in qualitaive analysis. 22. 3 formaion of complexes: the solubility of an ionic solid is increased by the formaion of a soluble complex ion, complex ion: a metal ion with small molecules or ions atached to it. Ex: ag+ + 2nh3 [ag(nh3)2]+ (complexaion reacion) To nh3: agbro3 + 2nh3 [ag(nh3)2]+ + bro3: add agbro3. By adding 2 reacions together, you muliply the k values to get a larger.

Related Questions

Determine the molar amounts of Pb+2 and Cl-

use the values of this handout

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.

If you need any other information, please let me know.

CHEM 6C Chapter Notes - Chapter 22: Ionic Compound, Reaction Quotient, Equilibrium Constant

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