One hundred mL of 0.00075 M sodium sulfate, Na2SO4, and 50.0mL of 0.15 M barium

Question

One hundred mL of 0.00075 M sodium sulfate, Na2SO4, and 50.0mL of 0.15 M barium chloride, BaCl2, solutions are mixed.    a. Write the molecular and net ionicequation for the reaction that occurs in the resultingsolution.    b. Determine the molarity of eachsolute at the instant of mixing.    c. Determine the concentration of eachion in the solution.    d. Will a precipitate form? Justify you answer. Ksp for BaSO4 is 1.1*10^-10. One hundred mL of 0.00075 M sodium sulfate, Na2SO4, and 50.0mL of 0.15 M barium chloride, BaCl2, solutions are mixed.    a. Write the molecular and net ionicequation for the reaction that occurs in the resultingsolution.    b. Determine the molarity of eachsolute at the instant of mixing.    c. Determine the concentration of eachion in the solution.    d. Will a precipitate form? Justify you answer. Ksp for BaSO4 is 1.1*10^-10.

Explanation / Answer

a) SO42- + Ba2+ ->BaSO4 Net ionic equation b) moles of Na2SO4 = 0.00075 mol/L*100 mL*(1L/1000 mL) = 7.5e-5moles moles of BaCl2 = 0.15 mol/L *(50 mL)*(1L/1000mL) = 7.5 e-3moles total vol = 100 mL + 50 mL = 0.15 L [Na2SO4] = 7.5e-5moles /0.15 L = 5e-4 M [BaCl2] = 7.5e-3 moles/0.15 L = 5e-2 M c) [Na+] = 2*5e-4 = 1e-3 M [SO42-] = 5e-4 M [Ba2+] = 5e-2 [Cl-] = 1e-1 M d) Q = [Ba2+][SO42-] = [5e-2][5e-4 ] = 2.5e-5 KsP Ksp)

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