Question

Where am I messing up??

Answer 1

From the solubility data given, calculate the solubility products for the following compounds:
(a) SrF2, 7.3 x 10-2 g/L
(b) Ag3PO4, 6.7 x 10-3 g/L

Answer 2

For part a, cant you say7.3x10^-2 =4s^3??

Answer 3

@aaronq

Answer 4

you converted to the masses to moles?

Answer 5

By dividing by the molar mass?

Answer 6

yeah

Answer 7

7.3x10^-2/125.62=.000581
Now divide by 4 and take cubed root of ans?

Answer 8

no, i think they're asking you for the solubility product constant.

so Ksp=\(4(0.000581)^3\)

Answer 9

OHH! So solubility =s and molar solubility =Ksp?

Answer 10

yeaah

Answer 11

Thanks! Never ran into a problem like that before.

Answer 12

no problem! i think thats what they're asking for, you should double check though

Answer 13

Ok. I know usually you make the ICE table to determine the factor (like 4s^3).

Answer 14

yeah, you would, but you can always assume it's that when you have a \(XY_2\) compound