Determination of a solubility product constant lab Need help determining trail 1

Question

Determination of a solubility product constant lab Need help determining trail 1 calculations Please show work so I can understand B: Calcium Iodate, Added Calcium Ion Concentration of Sodium Thiosulfate Solution (M Volume of Calcium lodate Solution and Caci, (mlL) Final Volume, Thiosulfate Solution (mL) Initial Volume, Thiosulfate Solution (mL) Trial #1 Trial #2 Trial #3 10.00 10.00 21-22 Volume of Thiosulfate Solution Added (mL) Inu-1bLle ^ Moles Sodium Thiosulfate Used Moles Iodate Equilibrium Concentration of lodate Ion (M Equilibrium Concentration of Calcium Ion M Molar Solubility of Calcium lodate (added Ca 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

moles of thiosulfate = 0.02012 mole/lit * 0.02120 L = 0.00042 mole

as per standard reaction 1 mole of iodate reacts with 6 mole of thiosulfate

hence, mole of iodate = 0.00042/6 = 0.00070 mole

volume of solution = 10 ml = 0.01 L

[iodate[ = 0.00070 mole / 0.01 L = 0.07 M

standard reaction bewteen calcium ion and iodate ion shows that 2 mole iodate reacts with one mole of calcium.

hence, [calcium ion] = 0.035 M

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