A chemist mixes 100.0 mL of 0.020 M AgNO3 with 100.0 mL of 0.020 M NaCl. At 25 °C, Ksp for AgCl is 1.8×10−10; at 60 °C, Ksp is 9.0×10−10. Assume that the total volume is the sum of the individual volumes.
(a) Calculate the value of the ionic product Q for AgCl immediately after the solutions are mixed at 25 °C.
(b) Using the value of Q from part (a) and the 25 °C Ksp, predict whether AgCl precipitates at 25 °C. Explain your reasoning briefly.
(c) The mixture is then heated to 60 °C with no change in volume or composition. Using the 60 °C Ksp, predict whether the amount of solid AgCl present will increase, decrease, or remain unchanged upon heating. Justify your answer quantitatively.
(d) Write the net ionic equation for any precipitation or dissolution process that occurs during heating.