Barium sulfate has a Ksp value=9.1*10^-11. if 500 mL of water containing 1 g of

Question

Barium sulfate has a Ksp value=9.1*10^-11. if 500 mL of water containing 1 g of barium nitrate (FW=199.33) is combined with 500 mL of water contaning 1 g of sodium sulfate(FW=142.03) will there be any precipitate?

A) Barium sulfate will precipitate.

B) There will be no precipitate

C) Impossible to tell

D) Sodium nitrate will precipitate

(3 pts) hich of the following equilibria in aqueous solutions do not do not take place solutions olve the water molecule as a product B. solubility A. acid-base D. All of them involve water as a C. complexation product or reactant. when dilute nitric is added to (2 pts) The solubility of silver chloride B. decreases A. increases D. first increases, then decreases C. first decreases, then increases E. does not change (3 pts) Which of the following substances has the greatest solubility in water? Ba(IO3)2, K 1.5 x 10 B. PbF2, Ksp 3.6 x 10 D. Cucl, K 1.9 x 10 C. srsoa, Ksp 3.2 x 10 E. cds, KS 1.0 x 10 24

Explanation / Answer

total volume = 500 mL + 500 mL = 1 L

mol of Ba(NO3)2 = mass/molar mass

= 1 g / 199.33 g/mol

=5.017*10^-3 mol

[Ba(NO3)2] = mol of Ba(NO3)2 / volume in L

= 5.017*10^-3 mol / 1 L

= 5.017*10^-3 M

So,

[Ba2+] = 5.017*10^-3 M

mol of Na2SO4 = mass/molar mass

= 1 g / 142.03 g/mol

=7.041*10^-3 mol

Na2SO4 = mol of Na2SO4 / volume in L

= 7.041*10^-3 mol / 1 L

= 7.041*10^-3 M

So,

[SO42-] = 7.041*10^-3 M

BaSO4   <—> Ba2+   +   SO42-

Qsp = [Ba2+] [SO42-]

= (5.017*10^-3)*(7.041*10^-3)

= 3.53*10^-5

This is more than Ksp

So, precipitation will take place

Answer: A) Barium sulfate will precipitate.

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