Barium hydroxide powder is stirred in water. Then the excess barium hydroxide is removed by centrifugation. The kip of barium hydroxide is 5x10^-3(5E-3)

A. What is the equilibrium barium ion concentration in the solution

B. What is the equilibrium pH of the solution?

C. If 1 liter of the solution of the above solution is treated with Sodium phosphate to precipitate all of the barium (Ksp of Ba3(PO4)2 is 3x10â23) how many grams of barium phosphate would be recovered?

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Casey DurganLv2

15 Feb 2019

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please show work and help thanks

A---Which of the following solutions of strong electrolytes contains the largest total number of ions? Show your calculations and explain your reasoning.

100.0 mL of 0.100 M sodium hydroxide

50.00 mL of 0.200 M barium chloride

75.0 mL of 0.150 M sodium phosphate

B--35.0 mL of lead(II) nitrate solution reacts with excess sodium iodide solution to yield 0.628 g of precipitate.

--Write a balanced equation for this reaction, and identify the precipitate. Indicate states of matter with parentheses and (aq) or (s).
--How many moles of precipitate formed?
--How many moles of lead nitrate were in the original solution?
--What is the concentration of the lead nitrate solution in grams per mL?

C---A gas mixture, with a total pressure of 300.0 torr, consists of equal masses of Ne (atomic weight 20.18) and Ar (atomic weight 39.95). What is the partial pressure of Ar, in torr?

jadegrasshopper512

22) Given the following hydroxides and their solubility productconstants, which would be the most soluble in 1.0 L of water?

A) Magnesium hydroxide; Ksp=1.2x10-11

B) Iron(II) hydroxide;Ksp=1.6x10-14

C) Zinc hydroxide;Ksp=1.8x10-14

D) Copper (II) hydroxide; Ksp=2.2x10-20

E) Calcium Hydroxide; Ksp=8.0x10-6

23) Consider the equilibrium of AgCl(s) in water: AgCl(s) ??Ag+Cl- What is the effect of adding 6.5x10-3 M AgNO3?

a) The concentration will AgCl(s) will increase

b) The concentration will AgCl(s) will decrease

c) AgNO3 will precipitate

d) Silver dichloride precipitates

e) The AgNO3 has no effect on the solubility of AgCl

29) The Ksp of Mg(OH)2 is 3.6x10-4. At what pH will 0.2 M Mg+2solution begin to show precipitation? 1.4, 2.8, 10.7, 11.2,12.6

27) The solubility product for calcium phosphate is Ksp=1.36 x10-26. What is the molar solubility of calcium phosphate?1.3X10-26M, 1.5x10-7M, 2.6x10-6M, 4.6x10-6M,6.6x10-6M Show work, explain or no points