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Calculate the solubility of barium carbonate, BaCO3, in pure water. Ksp = 2.0 ✕ 10-9

a. 2.2 ✕ 10-5 M

b. 3.2 ✕ 10-5 M

c. 1.3 ✕ 10-3 M

d. 4.0 ✕ 10-18 M

e. 4.5 ✕ 10-5 M

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Rei Juez del Mundo
Rei Juez del MundoLv10
19 Nov 2020

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Related questions

Calculate the molar solubility of BaCrO4 (Ksp = 2.1 multiplied by 10-10) in each of the following.

(a) pure water

(b) 4.0 multiplied by 10-3 M Na2CrO4

1.Write equations representing the various ionic equilibriainvolved in the dissolution of barium carbonate in aceticacid.

========
2. Why test for ammonium on a sample of the originalmaterial?

======
3. In terms of ionic equilibria and solubility product theory,explain the dissolution of BaCrO4 in HCl.
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4. Which of the following metal carbonates is most watersoluble?

a) zinc carbonate (ZnCO3), Ksp = 1.2 x 10-10
b) calcium carbonate (CaCO3), Ksp = 5.0 x 10-9
c) barium carbonate (BaCO3), Ksp = 2.6 x 10-9
d) magnesium carbonate (MgCO3), Ksp = 6.8 x 10-6
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Calculate the molar solubility of barium fluoride in each of the following

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Part B 0.10 M Ba(NO3)2 S =

Part C 0.15 M NaF

Express all answers using three significant figures.

ksp=2.45×10−5.

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