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3 Apr 2020
Consider the reaction
CaSO4(s) Ca2+(aq) + SO42-(aq)
At 25 °C, the equilibrium constant is Kc = 2.4 × 10–5 for this reaction. (a) If excess CaSO4(s) is mixed with water at 25 °C to produce a saturated solution of CaSO4, what are the equilibrium concentrations of Ca2+ and SO42-? (b) If the resulting solution has a volume of 1.4 L, what is the minimum mass of CaSO4(s) needed to achieve equilibrium?
The equilibrium concentrations of Ca2+ and SO42- are 4.9×10–3 M.
b) The minimum mass of CaSO4(s) needed to achieve equilibrium corresponds to the molarity equal to the equilibrium solubility of Ca2+ and SO42– ions. We need to add at least
Consider the reaction
CaSO4(s) Ca2+(aq) + SO42-(aq)
At 25 °C, the equilibrium constant is Kc = 2.4 × 10–5 for this reaction. (a) If excess CaSO4(s) is mixed with water at 25 °C to produce a saturated solution of CaSO4, what are the equilibrium concentrations of Ca2+ and SO42-? (b) If the resulting solution has a volume of 1.4 L, what is the minimum mass of CaSO4(s) needed to achieve equilibrium?
The equilibrium concentrations of Ca2+ and SO42- are 4.9×10–3 M.
b) The minimum mass of CaSO4(s) needed to achieve equilibrium corresponds to the molarity equal to the equilibrium solubility of Ca2+ and SO42– ions. We need to add at least
Nelly StrackeLv2
25 May 2020