Question

Pre-Lab for Determination of Solubility Product Constant 1. Write the solubility product constant (Ksp) for the following reaction as a function of the concentrations of the products: Ca(103) (s) Ca²+ (aq) + 210,- (aq) 2. Ca(IO3)2 will ionize in water to produce 10, ions. The 10, ions will react with KI. Write the reaction for this reaction. 3. We will be using starch as an indicator. Why? 4. In this experiment, we will first produce Izby mixing calcium iodate with excess amount of KI. Based on the following reactions, how many moles of I will be produced if we started with 6 moles of calcium iodate and excess amount of KI? Ca(103)2 (s) Calt (aq) + 210,- (aq) 10,- (aq) + 51" (aq) + 6H(aq) 312 (aq) + 3H20 (1) 5. In this experiment, we will titrate I, with Na S203 (sodium thiosulfate). The reaction is provided below. If we needed 22.5 mL of 0.15 M Na S2O3 to reach the endpoint, how many moles of I were present in the solution? (Must show all calculation steps.) 12 (aq) + 25,0,?- (aq) 21" (aq) + 5.0,- (aq) 6. How many moles of Ca(103)2 are needed to produce the amount of I, in Problem #5? 7. The solubility product constant (Ksp) for calcium iodate is 6.47 x 10" The molar mass of calcium iodate is 389.88 g/mol. 175.4 g of calcium iodate is added to 1 liter of water. What would be the concentrations of Ca and IO;at equilibrium? Would this solution form a precipitate? Is the solution unsaturated, saturated, or supersaturated when it reaches equilibrium? (Must show all calculation steps.)

Answer 1

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