A soluble Iodide was dissolved in water. Then an excess of silver nitrate, AgNO3, was added to completely precipitate out all of the iodine ion as silver iodide, AgI. If 1.545 grams of soluble iodide gave 2.185 of silver iodide, then (a) How many moles of Iodine are in the original soluble iodide sample? (b) How many grams of Iodine are in the original soluble sample? (c) What is the percentage mass of Iodine in the original soluble iodide sample?
A soluble Iodide was dissolved in water. Then an excess of silver nitrate, AgNO3, was added to completely precipitate out all of the iodine ion as silver iodide, AgI. If 1.545 grams of soluble iodide gave 2.185 of silver iodide, then (a) How many moles of Iodine are in the original soluble iodide sample? (b) How many grams of Iodine are in the original soluble sample? (c) What is the percentage mass of Iodine in the original soluble iodide sample?
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Chapter4: Chemical Reactions
Section: Chapter Questions
Problem 4.84QP: A soluble iodide was dissolved in water. Then an excess of silver nitrate, AgNO3, was added to...
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A soluble Iodide was dissolved in water. Then an excess of silver nitrate, AgNO3, was added to completely precipitate out all of the iodine ion as silver iodide, AgI. If 1.545 grams of soluble iodide gave 2.185 of silver iodide, then
(a) How many moles of Iodine are in the original soluble iodide sample?
(b) How many grams of Iodine are in the original soluble sample?
(c) What is the percentage mass of Iodine in the original soluble iodide sample?
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