Please calculate the Ksp for Ca(IO3)2 in each solution including an average calue and standard deviation.
You only need to answer #2 under calculations
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Procedure saturated solutions of calcium iodate in water and in 0.10 M calcium nitrate have been prepared well as standardized 0.05 M sodium thiosulfate solution. Make sure that you record the actual molarity of these solutions. This is found on the container label. Solubility Product of Ca(IO3)2 1. To a 250 mL Erlenmeyer flask, add approximately 2.0 g of KI and 50 mL of water. 2. Then pipet 10.00 ml of the saturated calcium iodate solution into the flask and add 100 mL of 1.0 M HCl Titrate the brown olution with standardized 0.05 M sodium thiosulfate to a light amber color. 3. 4. To the light ambr solution add 5 mL of prepared starch solution. Titrate the purple solution until it turns colurless. 5. Record the temerature of the solution. 6. Repeat the proedure two more times for a total of three trials. Common Ion ffect Duplicate the p cedure in "Solubility Product of Ca(IO3)2" (above) with 10.00 mL samples of the saturated solutin of calcium iodate prepared in 0.100 M calcium nitrate solution. Calculatin 1. Calculate he solubility of Ca(IO) in water and in 0.10 M Ca(NO3), solution. 2. of Ksp for Ca(IO3)2 in each solution including an average value and standard deviation 3. Using the average value of Ksp for Ca o,, in water determine the error from the value in the CRC. find Cod of Soluton in the Container moles of Todine to nd mones ot todene
