Question

A) The Ksp of BaCO3 is 5.0 x 10-9. What is the soliubility of barium carbonate...

A) The Ksp of BaCO3 is 5.0 x 10-9. What is the soliubility of barium carbonate in a solution that contains 1.56 M of Na2CO3?

B) At a ceratin temperature ths solubility of Ca3(PO4)2 is 1.43 x 10-6M. What is the Ksp at this temperature?

Express your answer in scientific notation.

Homework Answers

Answer #1

A )

[CO3-2] = 1.56 M

BaCO3 ----------------------> Ba+2 + CO3-2

S S ------------> in absence common ion

S S + 1.56------------> in absence common ion

S 1.56   

Ksp = [Ba+2][CO3-2]

5.0 x 10^-9 = (S) x 1.56

S = 3.20 x 10^-9 M

solubility = 3.20 x 10^-9 M

B)

Solubility = S = 1.43 x 10^-6

Ca3(PO4)2 --------------------> 3 Ca+2 + 2 PO4-3

3S 2S

Ksp = [Ca+2]^3 [PO4-3]^2

Ksp = (3S)^2 (2S)^3

Ksp = 108 S^5

Ksp = 108 x (1.43 x 10^-6)^5

Ksp = 6.46 x 10^-28

Know the answer?
Your Answer:

Post as a guest

Your Name:

What's your source?

Earn Coins

Coins can be redeemed for fabulous gifts.

Not the answer you're looking for?
Ask your own homework help question
Similar Questions
The Ksp for BaCO3 is 1.6 x 10-9 . A)Write a chemical equation for the equilibrium...
The Ksp for BaCO3 is 1.6 x 10-9 . A)Write a chemical equation for the equilibrium of BaCO3 (s) with its ions. B) When 20.0 mL of a 0.10 M Ba(NO3)2 is added to 50.0 mL of a 0.10 M Na2CO3 calculate the reaction quotient and determine if a precipitate will form? C) For the same reaction, predict the direction the system once it gets to equilibrium will shift when acid is added to the system.
The Ksp for BaCO3 is 1.6 x 10-9 . A)Write a chemical equation for the equilibrium...
The Ksp for BaCO3 is 1.6 x 10-9 . A)Write a chemical equation for the equilibrium of BaCO3 (s) with its ions. B) When 20.0 mL of a 0.10 M Ba(NO3)2 is added to 50.0 mL of a 0.10 M Na2CO3 calculate the reaction quotient and determine if a precipitate will form? C) For the same reaction, predict the direction the system once it gets to equilibrium will shift when acid is added to the system.
What is the molar solubility BaCO3 in pure water? (Ksp = 5.1*10-9) Answer = 7.1 *...
What is the molar solubility BaCO3 in pure water? (Ksp = 5.1*10-9) Answer = 7.1 * 10-5M
The solubility-product constants, Ksp, at 25 ∘C for two compounds [iron(II) carbonate, FeCO3, and cadmium(II) carbonate,...
The solubility-product constants, Ksp, at 25 ∘C for two compounds [iron(II) carbonate, FeCO3, and cadmium(II) carbonate, CdCO3] are given by the table Part A A solution of Na2CO3 is added dropwise to a solution that contains 1.04×10−2M Fe2+ and 1.50×10−2M Cd2+. What concentration of CO32− is need to initiate precipitation? Neglect any volume changes during the addition. Express the molar concentration numerically. Part B In the solution from Part A, what will the concentration of CO32− be when Fe2+ begins...
a. The Ksp for Ag2SO3 = 1.50 X 10-14. What is the molar solubility of Ag2SO3...
a. The Ksp for Ag2SO3 = 1.50 X 10-14. What is the molar solubility of Ag2SO3 in a 5 M solution of lithium sulfite? b.The Ksp for Mg3(PO4)2 = 1.04 X 10-24. What is the molar solubility of Mg3(PO4)2 in a 1.40 M solution of sodium phosphate? c.If the Ksp for Y(OH)3 = 1.00 X 10-22, what is the molar solubility of Y(OH)3 in a buffer solution composed of 1.60M trimethylamine (= (CH3)3N) (Kb = 6.5 X 10-5) and 1.40M...
Which of the following has the greatest molar solubility? Ca3(PO4)2 Ksp = 1.0 x 10-26 CaF2...
Which of the following has the greatest molar solubility? Ca3(PO4)2 Ksp = 1.0 x 10-26 CaF2 Ksp = 3.4 x 10-11 CaCO3 Ksp = 3.9 x 10-9 CaC2O4 Ksp = 2.3 x 10-9 CaSO4 Ksp = 2.4 x 10-5
1)At 25 oC the solubility of silver iodide is 8.94 x 10-9 mol/L. Calculate the value...
1)At 25 oC the solubility of silver iodide is 8.94 x 10-9 mol/L. Calculate the value of Ksp at this temperature. Give your answer in scientific notation to 2 SIGNIFICANT FIGURES (even though this is strictly incorrect) 2)The Ksp of Al(OH)3 is 1.0 x 10-33. What is the solubility of Al(OH)3 in 0.0000010 M Al(NO3)3? Give your answer using scientific notation and to 2 significant figures (i.e., one decimal place).
The Ksp of barium fluoride is 1.00 x 10–6. The Ksp of calcium fluoride is 3.90...
The Ksp of barium fluoride is 1.00 x 10–6. The Ksp of calcium fluoride is 3.90 x 10–11. An aqueous solution of sodium fluoride is slowly added to a water sample that contains barium ion (4.50×10-2M ) and calcium ion (3.75×10-2M ). What is the remaining concentration of the first ion to precipitate when the second ion begins to precipitate?
The Ksp of barium fluoride is 1.00 x 10^–6. The Ksp of calcium fluoride is 3.90...
The Ksp of barium fluoride is 1.00 x 10^–6. The Ksp of calcium fluoride is 3.90 x 10^–11. An aqueous solution of sodium fluoride is slowly added to a water sample that contains barium ion (3.95×10^-2M ) and calcium ion (4.65×10^-2M ). What is the remaining concentration of the first ion to precipitate when the second ion begins to precipitate?_____M
The Ksp of barium fluoride is 1.00 x 10–6. The Ksp of calcium fluoride is 3.90...
The Ksp of barium fluoride is 1.00 x 10–6. The Ksp of calcium fluoride is 3.90 x 10–11. An aqueous solution of sodium fluoride is slowly added to a water sample that contains barium ion (4.45×10-2M ) and calcium ion (5.50×10-2M ). What is the remaining concentration of the first ion to precipitate when the second ion begins to precipitate?
ADVERTISEMENT
Need Online Homework Help?

Get Answers For Free
Most questions answered within 1 hours.

Ask a Question
ADVERTISEMENT