This is a picture of the problems. SOLUTION STOICHIOMETRY - super fun - give it a try...remember, if you can determine how many moles are ina sample, you can use a molar ration - and do stoichiometry! So, with molarity - you can use the MOLARITYformula and determine how many moles are present in a given volume of a given molarity!!1. 50mL of a 0.6M Pb(NO,), is mixed with an excess of Nal solution. What mass of precipitate wouldexpect to collect from this reaction? How many moles of Nal were required to precipitate all of the Pb*2youions?2. If you have 50mL of .30 M K,PO, and 50mL of 1.0 M MgCl, how much of the precipitate will form fromthe reaction? (Hint: you need to find the limiting reagent first!)

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50mL of a 0.6M Pb(NO,), is mixed with an excess of Nal solution. What mass of precipitate would you expect to collect from this reaction? How many moles of Nal were required to precipitate all of the Pb*2 ions?

50mL of a 0.6M Pb(NO,), is mixed with an excess of Nal solution. What mass of precipitate would you expect to collect from this reaction? How many moles of Nal were required to precipitate all of the Pb*2 ions?

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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HO OH EtOEt cat H2SO4
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HO 1. LAH 2. H₂O* e.
could you space it out better with better labels?