I. Lead ions can be precipitated from aqueous solutions by the addition of aqueous iodide. Below is an unbalanced net ionic equation of the reaction: Pb2+ (aq) + I-1 (aq) → PbI2 (s) Lead iodide is virtually insoluble in water so that the reaction appears to go to completion. How many milliliters of 3.550 M HI(aq) must be added to a solution containing 45.0 g of Pb(NO3)2 (aq) to completely precipitate the lead?
I. Lead ions can be precipitated from aqueous solutions by the addition of aqueous iodide. Below is an unbalanced net ionic equation of the reaction: Pb2+ (aq) + I-1 (aq) → PbI2 (s) Lead iodide is virtually insoluble in water so that the reaction appears to go to completion. How many milliliters of 3.550 M HI(aq) must be added to a solution containing 45.0 g of Pb(NO3)2 (aq) to completely precipitate the lead?
Principles of Modern Chemistry
8th Edition
ISBN:9781305079113
Author:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler
Publisher:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler
Chapter15: Acid–base Equilibria
Section: Chapter Questions
Problem 98AP
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Show all work please.. answer both questions
I. Lead ions can be precipitated from aqueous solutions by the addition of aqueous iodide. Below is an unbalanced net ionic equation of the reaction:
Pb2+ (aq) + I-1 (aq) → PbI2 (s)
Lead iodide is virtually insoluble in water so that the reaction appears to go to completion. How many milliliters of 3.550 M HI(aq) must be added to a solution containing 45.0 g of Pb(NO3)2 (aq) to completely precipitate the lead?
II. Pure magnesium metal is often found as ribbons and can easily burn in the presence of oxygen. When 3.86 g of magnesium ribbon burns with 155ml of oxygen at 1.0 atm and 275 K , a bright, white light and a white, powdery product is formed, magnesium oxide. How many grams of excess reactant remain?
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