For the chemical reaction that occurs when the precipitate forms, write a balanced, net-ionic equation for the reaction, and explain why the reaction is best represented by a net-ionic equation. Explain the purpose of drying and weighing the filter paper with the precipitate three times. In the filtrate solution, is [K+] greater than, less than, or equal to [NO3−] ? Justify your answer. Calculate the number of moles of precipitate that is produced in the experiment. Calculate the mass percent of I− in the tablet. In another trial, the student dissolves a tablet in 55.0 mL of water instead of 50.0 mL of water. Predict whether the experimentally determined mass percent of I− will be greater than, less than, or equal to the amount calculated in part (e). Justify your answer. A student in another lab also wants to determine the I− content of a KI tablet but does not have access to Pb(NO3)2 . However, the student does have access to 0.20 M AgNO3 , which reacts with I−(aq) to produce AgI(s). The value of Ksp for AgI is 8.5 x 10−17. Will the substitution of AgNO3 for Pb(NO3)2result in the precipitation of the I− ion from solution? Justify your answer. The student only has access to one KI tablet and a balance that can measure to the nearest 0.01 g. Will the student be able to determine the mass of AgI produced to three significant figures? Justify your answer.
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For the
chemical reaction that occurs when the precipitate forms,-
write a balanced, net-ionic equation for the reaction, and
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explain why the reaction is best represented by a net-ionic equation.
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Explain the purpose of drying and weighing the filter paper with the precipitate three times.
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In the filtrate solution, is [K+] greater than, less than, or equal to [NO3−] ? Justify your answer.
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Calculate the number of moles of precipitate that is produced in the experiment.
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Calculate the mass percent of I− in the tablet.
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In another trial, the student dissolves a tablet in 55.0 mL of water instead of 50.0 mL of water. Predict whether the experimentally determined mass percent of I− will be greater than, less than, or equal to the amount calculated in part (e). Justify your answer.
-
A student in another lab also wants to determine the I− content of a KI tablet but does not have access to Pb(NO3)2 . However, the student does have access to 0.20 M AgNO3 , which reacts with I−(aq) to produce AgI(s). The value of Ksp for AgI is 8.5 x 10−17.
-
Will the substitution of AgNO3 for Pb(NO3)2result in the precipitation of the I− ion from solution? Justify your answer.
-
The student only has access to one KI tablet and a balance that can measure to the nearest 0.01 g. Will the student be able to determine the mass of AgI produced to three significant figures? Justify your answer.
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