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Redox and electrochemistry — Question 87

Original QCE Vault practice · 6 marks

Q87 · Practice questionComplex unfamiliar6 marks

QUESTION 87 (6 marks)

50.0 mL of 0.100 mol L⁻¹ AgNO₃ is mixed with 50.0 mL of 0.100 mol L⁻¹ NaCl at 25∘C. AgCl precipitates. For AgCl, Ksp=1.8×10−10. After equilibrium, the liquid is completely separated from the solid. Use F=96485 Cmol−1.

a) Calculate the equilibrium silver-ion concentration in the liquid. [2 marks]

b) Calculate the theoretical charge needed to reduce all dissolved Ag⁺ in the 100.0 mL liquid to Ag, assuming no competing reaction. [3 marks]

c) Explain why leaving the AgCl solid in contact with the liquid would invalidate this calculation as a prediction of total available silver. [1 marks]

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