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Problem 1. Calcium carbonate [CaCO3] is used as a water softener and for corrosion control. Assume the following reversible reaction occurs in water: CaCO3(s)Ca2++CO32 The

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Problem 1. Calcium carbonate [CaCO3] is used as a water softener and for corrosion control. Assume the following reversible reaction occurs in water: CaCO3(s)Ca2++CO32 The solubility product for this reaction is 108.305. (Recall that for solid dissolution/precipitation reactions, the equilibrium constant is called the solubility product, Ksp.) If 50.0mg of CO32 and 50.0mg of Ca2+ are currently present in 1L of water, what will be the final (equilibrium) concentration of Ca2+ ? Give your answer in mg/L

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