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17 Nov 2019
Assume that the molarity of the NaOH solution used to titrate the saturated solution was actually higher than reported. Would the calculated KHT solubility be incorrectly high or low? Briefly explain. Assume that the filter paper had a small hole in it, allowing some solid KHT to get into the saturated solution filtrate. If some of the solid were included in the portion of solution titrated with NaOH solution, what effect would the solid have on the calculated KHT solubility? Briefly explain. An experiment was performed to determine the K_sp of Ca(OH)_2. A solution containing 2.00 times 10^-2 M Ca(NO_3)_2 was saturated with Ca(OH)_2 and filtered. Two samples of the saturated solution were titrated with 5.021 times 10^-2 M HCl, in order to determine the OH^- ion concentration in the saturated solution. In doing this problem, note that 1 mol of HCl reacts with 1 mol of OH^- ions. This relationship is the basis for the determination of the OH^- ton concentration: 1 mol Ca^2+ ions are produced for every 2 mols of OH^- ions produced. The data resulting from this experiment are shown in Table 2. Table 2 Student data used to determine the K_sp of Ca(OH)_2
Assume that the molarity of the NaOH solution used to titrate the saturated solution was actually higher than reported. Would the calculated KHT solubility be incorrectly high or low? Briefly explain. Assume that the filter paper had a small hole in it, allowing some solid KHT to get into the saturated solution filtrate. If some of the solid were included in the portion of solution titrated with NaOH solution, what effect would the solid have on the calculated KHT solubility? Briefly explain. An experiment was performed to determine the K_sp of Ca(OH)_2. A solution containing 2.00 times 10^-2 M Ca(NO_3)_2 was saturated with Ca(OH)_2 and filtered. Two samples of the saturated solution were titrated with 5.021 times 10^-2 M HCl, in order to determine the OH^- ion concentration in the saturated solution. In doing this problem, note that 1 mol of HCl reacts with 1 mol of OH^- ions. This relationship is the basis for the determination of the OH^- ton concentration: 1 mol Ca^2+ ions are produced for every 2 mols of OH^- ions produced. The data resulting from this experiment are shown in Table 2. Table 2 Student data used to determine the K_sp of Ca(OH)_2
Hubert KochLv2
29 Aug 2019