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Suppose you wanted to find out how many milliliters of 1.0

Modern Chemistry: Student Edition 2012 | 1st Edition | ISBN: 9780547586632 | Authors: Jerry L. Sarquis, Mickey Sarquis ISBN: 9780547586632 214

Solution for problem 12.1.40 Chapter 12

Modern Chemistry: Student Edition 2012 | 1st Edition

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Modern Chemistry: Student Edition 2012 | 1st Edition | ISBN: 9780547586632 | Authors: Jerry L. Sarquis, Mickey Sarquis

Modern Chemistry: Student Edition 2012 | 1st Edition

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Problem 12.1.40

Suppose you wanted to find out how many milliliters of 1.0 M AgNO3 are needed to provide 169.9 g of pure AgNO3. a. What is the first step in solving the problem? b. What is the molar mass of AgNO3? c. How many milliliters of solution are needed? 2

Step-by-Step Solution:
Step 1 of 3

General Chemistry Week 9 Part Two Predicting When Precipitates Will Form  Write all of ions present in the reaction  Compare all possible combinations according to solubility rules Q: Will a precipitate form when aqueous solutions of Pb(NO3)2 A: Pb(NO3)2 (aq) + 2KI(aq)  PbI2 (s) + 2KNO3 (aq) Q: Will a precipitate form when aqueous solutions of Ca(NO3)2 and KI mix A: No, no reaction will occur Net Ionic Equations Balanced Equation: Pb(NO3)2 (aq) + 2KI(aq) ▯ PbI2 (s) + 2KNO3 (aq) Ionic Equation: Pb+2 (aq) + 2NO3­ (aq) + 2K+ (aq) + 2I­ (aq) PbI2 (s) + 2K+(aq0 + 2NO3­ (aq) Net Ionic Equation: Pb+2(aq) + 2I­(aq) PbI2(s)  Spectator ions are not included in the net ionic equation: not involved i

Step 2 of 3

Chapter 12, Problem 12.1.40 is Solved
Step 3 of 3

Textbook: Modern Chemistry: Student Edition 2012
Edition: 1
Author: Jerry L. Sarquis, Mickey Sarquis
ISBN: 9780547586632

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Suppose you wanted to find out how many milliliters of 1.0