22Ebbing, Gammon. General Chemistry. Eleventh Edition. Cengage Learning.Is a precipitate expected to form when 50.0 mL of 0.0010 M BaCl2 isadded to 50.0 mL of 0.00010 M Na2SO4? The solubility product constantfor barium sulfate is 1.1×10−10. Assume that the total volume ofsolution, after mixing, equals the sum of volumes of separate solutions
Question
22Ebbing, Gammon. General Chemistry. Eleventh Edition. Cengage Learning.Is a precipitate expected to form when 50.0 mL of 0.0010 M BaCl2 isadded to 50.0 mL of 0.00010 M Na2SO4? The solubility product constantfor barium sulfate is 1.1×10−10. Assume that the total volume ofsolution, after mixing, equals the sum of volumes of separate solutions
Solution
To determine whether a precipitate will form when two solutions are mixed, we can compare the reaction quotient (Q) with the solubility product constant (Ksp).
The reaction for the formation of barium sulfate (BaSO4) from barium chloride (BaCl2) and sodium sulfate (Na2SO4) is:
Ba2+(aq) + SO4^2-(aq) ⇌ BaSO4(s)
The reaction quotient (Q) is given by the product of the concentrations of the ions in the solution. After mixing, the concentration of Ba2+ is (0.0010 M * 50.0 mL) / (50.0 mL + 50.0 mL) = 0.00050 M. Similarly, the concentration of SO4^2- is (0.00010 M * 50.0 mL) / (50.0 mL + 50.0 mL) = 0.000050 M.
So, Q = [Ba2+][SO4^2-] = (0.00050 M)(0.000050 M) = 2.5 x 10^-8.
The solubility product constant for barium sulfate is given as 1.1 x 10^-10. Since Q > Ksp, a precipitate is expected to form.
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