Molar mass of CaSO4,
MM = 1*MM(Ca) + 1*MM(S) + 4*MM(O)
= 1*40.08 + 1*32.07 + 4*16.0
= 136.15 g/mol
Molar mass of CaSO4= 136.15 g/mol
s = 0.209 g/100 mL
= 0.209 g / 0.100 L
= 2.09 g/L
To covert it to mol/L, divide it by molar mass
s = 2.09 g/L / 136.15 g/mol
s = 1.535*10^-2 mol/L
At equilibrium:
CaSO4 <----> Ca2+ + SO42-
s s
Ksp = [Ca2+][SO42-]
Ksp = (s)*(s)
Ksp = 1(s)^2
Ksp = 1(1.535*10^-2)^2
Ksp = 2.356*10^-4
Answer: 2.36*10^-4
Be sure to answer all parts. The solubility of calcium sulfate at 30°C is 0.209 g/100 mL solution. Calculate its Ksp. K...
I found that the molar solubility of Calcium Sulfate is 0.00490 if its Ksp is 2.40x10^-5. But I do not really know how to find the solubility of CaSO4 (136.2 g/mol) in g/mL. Could someone also explain the different parts of this problem as well please? (solubility, molar solubility, and Ksp) Much thanks :) -5.9x107 Find the molar solubility (mol/L) of calcium sulfate if its Ksp = 2:40 Casoy, 7 Cacaq) + soucans K[x][y] 8 52.40xions =x² chong x= .00490...
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