5) The solubility of BaCO3 is 24 mg/L at room temperature. a. What is the molar solubility and the Ksp of barium carbonate? b. The carbonate ion can react with water as follows: CO3² (aq) + H₂O (1) HCO3 (aq) + OH(aq) Kb = 2.1 x 10-4 Write the reaction out from part a, add the two reactions together, and calculate the new K of the combined reaction. C. Using your K from part b, find the solubility of BaCO3 when the reaction in part b is also considered. Did the solubility increase or decrease from part a? Explain using Le Chatelier's Principle.
5) The solubility of BaCO3 is 24 mg/L at room temperature. a. What is the molar solubility and the Ksp of barium carbonate? b. The carbonate ion can react with water as follows: CO3² (aq) + H₂O (1) HCO3 (aq) + OH(aq) Kb = 2.1 x 10-4 Write the reaction out from part a, add the two reactions together, and calculate the new K of the combined reaction. C. Using your K from part b, find the solubility of BaCO3 when the reaction in part b is also considered. Did the solubility increase or decrease from part a? Explain using Le Chatelier's Principle.
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![5) The solubility of BaCO3 is 24 mg/L at room temperature.
a. What is the molar solubility and the Ksp of barium carbonate?
b. The carbonate ion can react with water as follows:
CO3² (aq) + H₂O (1)
HCO3 (aq) + OH- (aq)
Kb = 2.1 x 10-4
Write the reaction out from part a, add the two reactions together, and calculate the new K of the combined
reaction.
C. Using your K from part b, find the solubility of BaCO3 when the reaction in part b is also considered. Did the
solubility increase or decrease from part a? Explain using Le Chatelier's Principle.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F9b0e7686-0c0d-4eba-ac81-54e736b47f2f%2F473a0395-a731-4e67-8b67-52aa3210fdb1%2F64b8vmo_processed.jpeg&w=3840&q=75)
Transcribed Image Text:5) The solubility of BaCO3 is 24 mg/L at room temperature.
a. What is the molar solubility and the Ksp of barium carbonate?
b. The carbonate ion can react with water as follows:
CO3² (aq) + H₂O (1)
HCO3 (aq) + OH- (aq)
Kb = 2.1 x 10-4
Write the reaction out from part a, add the two reactions together, and calculate the new K of the combined
reaction.
C. Using your K from part b, find the solubility of BaCO3 when the reaction in part b is also considered. Did the
solubility increase or decrease from part a? Explain using Le Chatelier's Principle.
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