You have a solid 7.00 gram mixture of sodium nitrate and silver nitrate. You add distilled water to dissolve the solids. Now you have aqueous solutions of sodium nitrate and silver nitrate. Next you add excess sodium chloride which results in a precipitate forming. You collect and dry the precipitate that forms and it has a mass of 2.54 grams. Write a balanced net ionic equation for the reaction that occurred. Determine the percent silver nitrate in the original mixture by mass assuming 95.9% actual yield.
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Calculate the molarity of each of the following solutions. part a) 0.12 mol of lino3 in 5.5 l of solution part b) 60.7 g c2h6o in 2.48 l of solution part c) 14.2 mg ki in 100 ml of solution
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You have a solid 7.00 gram mixture of sodium nitrate and silver nitrate. You add distilled water to...
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