B: Calcium Iodate, Added Calcium lon Concentration of Sodium Thiosulfate Solutio

Question

B: Calcium Iodate, Added Calcium lon Concentration of Sodium Thiosulfate Solution (M Volume of Calcium lodate Solution and CaCl, (mL) 10.00 Final Volume. Thiosulfate Solution (mL) Initial Volume, Thiosulfate Solution (mL) Volume of Thiosulfate Solution Added (mL) Moles Sodium Thiosulfate Used Moles lodate Equilibrium Concentration of Iodate Ion (M Equilibrium Concentration of Calcium Ion M Molar Solubility of Calcium Iodate 910o2 12 M Na, S,O Trial #1 Trial #2 Tri 10.00 4 035 (added Ca2 ion source) Average Molar Solubility of Calcium lodate (added Ca2 ion source) Standard deviation for Molar Solubility (added Ca?") % RSD Show calculations for Trial #1 on last page.

Explanation / Answer

Note: the value of added concentration of calcium salt as a common ion is not given. It assume that the concentration is S mole/lit for calcium ion as added common ion.

due to addition of common ion the equilibrium will shifted to the left hand side of the reaction. now this extra S mole/lit Ca2+ ion will bind 2S mole of iodate ion to shift the reaction left side.

now, the final concentration of iodate will be = 0.007 mole - 2S mole

now the total volume will also change, before addition of common ion ion the volume is 10 ml

after addition of V mlvolume of common ion, total volume will be = (10 + v) ml = (10 + v) *10-3 L

hence, final [iodate] = 0.007 mole - 2S mole / (10 + v) *10-3 L = y M

[Ca2+] = y/2 M

therefore, molar solubility of calcium iodate is y/2 M

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