2. A concentration cell was prepared at 25 C; one cell compartment contained 0.070 M Pb(C2H3O2)2(aq)...
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2. A concentration cell was prepared at 25 °C; one cell compartment contained 0.070 M Pb(C2H3O2)2(aq) and was connected by a salt bridge to a compartment containing Pb¹2(aq) in saturated 0.050 M Na2SO4(aq). The measured voltage is 0.205 V. a. Write the Ksp expression for PbSO4. b. Use the Nerst Equation to solve the value of Q in the concentration cell. c. From the value of Q and the known [Pb 2]high, solve the diluted equilibrium [Pb+2]low. Note: [Pb 2]low is the equilibrium concentration. d. Using the value of diluted [Pb+2]eq and the saturated [SO4 2] determine Ksp. 2. A concentration cell was prepared at 25 °C; one cell compartment contained 0.070 M Pb(C2H3O2)2(aq) and was connected by a salt bridge to a compartment containing Pb¹2(aq) in saturated 0.050 M Na2SO4(aq). The measured voltage is 0.205 V. a. Write the Ksp expression for PbSO4. b. Use the Nerst Equation to solve the value of Q in the concentration cell. c. From the value of Q and the known [Pb 2]high, solve the diluted equilibrium [Pb+2]low. Note: [Pb 2]low is the equilibrium concentration. d. Using the value of diluted [Pb+2]eq and the saturated [SO4 2] determine Ksp.
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a The solubility product constant Ksp expression for the leadII sulfate PbSO4 is given by the equili... View the full answer
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