# Chemistry 212

What is the solubility of RaSO4 in 0.1381M Na2SO4? Ksp = 4.3x10^-11?

1. 👍
2. 👎
3. 👁
1. RaSO4 ==> Ra^+2 + SO4^-2

Ksp = (Ra^+2)(SO4^-2).
If you let S = solubility RaSO4, then
Ra^+2 = S
SO4^-2 = S from RaSO4 and 0.1381 M in Na2SO4 so a total of (S + 0.1381)
Substitute those values into Ksp expression and solve for S.

1. 👍
2. 👎
2. Ksp = [Ra^+2][SO4^-2]
4.3x10^-11 = [x][x]
x=6.56x10^-6

6.56x10^-6 + .1381??

is that how im suppose to do it?

1. 👍
2. 👎
3. No.
4.3 x 10^-11 = (x)(x+0.1381)
solve for x.
NOTE:
If you solve the equation as I wrote it you will need to solve a quadratic. Those are usually easy to do with modern calculators; however, you CAN make a simplifying assumption. You make the assumption that x + 0.1381 = 0.1381 (that is, that x is so small in comparison to 0.1381 that when added it isn't different than 0.1381). The equation then would look like this.
4.3 x 10^-11 = (x)(0.1381) and solve for x. When you finish, then look at x+0.1381 and see how far it is from 0.1381. If x is so small that x+0.1381 is just 0.1381, then the assumption is ok. If not, the assumption is not ok and you must solve the quadratic. I ALWAYS make the assumption first and solve the easy equation, then check at the end and see if the assumption is ok.

1. 👍
2. 👎
4. thanks a bunch!

1. 👍
2. 👎

## Similar Questions

1. ### Chemistry

The Ksp of CaSO4 is 4.93× 10–5. Calculate the solubility (in g/L) of CaSO4(s) in 0.300 M Na2SO4(aq) at 25 °C

2. ### chemistry

do not understand this problem The Ksp of CaSO4 is 4.93× 10–5. Calculate the solubility (in g/L) of CaSO4(s) in 0.500 M Na2SO4(aq) at 25 °C.

3. ### chemistry

what is the solubility of barium sulfate in a solution containing 0.050 M sodium selfate? The Ksp value for barium sulfate is 1.1E-10. An insoluble salt with formula MX3 has a solubility product constant written in terms of

4. ### Chem 2

what is the solubility of silver carbonate in water in 25 degrees celcius if Ksp=8.4X10-12? i don't know what to do Write the equation. Ag2CO3(s) ==> 2Ag^+ + CO3^= Ksp = (Ag^+2)(CO3^=) Let x = solubility of Ag2CO3. At

1. ### Chemistry

Which of the following substances has the greatest solubility in water? A. Ca(OH)2, Ksp = 6.5 × 10-6 B. Ag2SO4, Ksp = 1.5 × 10-5 C. PbI2, Ksp = 7.9 × 10-9 D. Zn(IO3)2, Ksp = 3.9 × 10-6 E. BaF2, Ksp = 1.5 × 10-6

2. ### Chemistry

Determine the solubility of a sodium sulfate, Na2SO4, in grams per 100g of water, if 0.94 g of Na2SO4 is dissolved in 20 g of water to make a saturated solution.

3. ### chemistry

For which of the following mixtures will Ag2SO4(s) (Ksp=1.20E^-5)precipitate? More than one answer can be selected. a.) 150.0 mL of 0.10 M Na2SO4(aq) and 5.0 mL of 0.20 M AgNO3(aq) b.) 150.0 mL of 0.10 M Na2SO4(aq) and 5.0 mL of

4. ### Chemistry

Which of the following compounds has the greatest molar solubility? A) AgBr, Ksp= 5.4 x 10^13 B) Ba3(PO4)2, Ksp = 3.0 x 10^-23 C) Al(OH)3, Ksp = 1.9 x 10^-33 D) MgF2, Ksp = 7.4 x 10^-11 E) Pb(OH)2, Ksp = 1.2 x 10^-15 I know the

1. ### chemistry

Given the following solubility constants, which list arranges the solutes in order of increasing solubility? CaCO3: Ksp = 2.8 × 10-9 Ca(OH)2: Ksp = 5.5 × 10-6 CaSO4: Ksp = 9.1 × 10-6 CaF2: Ksp = 5.3 × 10-9 A. CaSO4 < Ca(OH)2 <

2. ### Chemistry

I might be overthinking this but my reference books, note and the internet don't have much on this topic. What is the relationship between the solubility product constant Ksp and temperature? A. They are directly proportional B.

3. ### chemistry

Calculate the solubility of AgCl in: Ksp = 1.6x10^-10 a) 100 ml of 4.00 x 10^-3 M Calcium chloride b) 100 ml of 4.00 x 10^-3 M Calcium Nitrate all i know is 1.6x10^-10=[Ag+][Cl-] which is 1.6x10^-10=x^2 x=1.3x10^-5, giving the M

4. ### chemistry

Calulate the molar solubility of Al(OH)3 in water. (Ksp = 3 x 10^-34) Al(OH)3(s) ==>Al^+3 + 3OH^- Ksp = (Al^+3)(OH^-)^3 = 3E-34 Let x = molar solubility of Al(OH)3 then x molar = (Al^+3) and 3x molar = (OH^-) Plug in to Ksp and