Ch.16 - Aqueous Equilibrium WorksheetSee all chapters
All Chapters
Ch.1 - Intro to General Chemistry
Ch.2 - Atoms & Elements
Ch.3 - Chemical Reactions
BONUS: Lab Techniques and Procedures
BONUS: Mathematical Operations and Functions
Ch.4 - Chemical Quantities & Aqueous Reactions
Ch.5 - Gases
Ch.6 - Thermochemistry
Ch.7 - Quantum Mechanics
Ch.8 - Periodic Properties of the Elements
Ch.9 - Bonding & Molecular Structure
Ch.10 - Molecular Shapes & Valence Bond Theory
Ch.11 - Liquids, Solids & Intermolecular Forces
Ch.12 - Solutions
Ch.13 - Chemical Kinetics
Ch.14 - Chemical Equilibrium
Ch.15 - Acid and Base Equilibrium
Ch.16 - Aqueous Equilibrium
Ch. 17 - Chemical Thermodynamics
Ch.18 - Electrochemistry
Ch.19 - Nuclear Chemistry
Ch.20 - Organic Chemistry
Ch.22 - Chemistry of the Nonmetals
Ch.23 - Transition Metals and Coordination Compounds

Solution: Consider these mixtures:I. 100. mL of 0.06 M Pb(NO3)2 and 50.0 mL of 0.03 M NaBrII. 100. mL of 0.08 M Pb(NO3)2 and 100.0 mL of 0.05 M NaBrThe Ksp of PbBr2 = 6.6 x 10-6.

Problem

Consider these mixtures:

I. 100. mL of 0.06 M Pb(NO3)2 and 50.0 mL of 0.03 M NaBr

II. 100. mL of 0.08 M Pb(NO3)2 and 100.0 mL of 0.05 M NaBr

The Ksp of PbBr2 = 6.6 x 10-6.

Solution

We are being asked to determine if a precipitate will form from for the given mixtures:


I. 100. mL of 0.06 M Pb(NO3)2 and 50.0 mL of 0.03 M NaBr

II. 100. mL of 0.08 M Pb(NO3)2 and 100.0 mL of 0.05 M NaBr


For this problem, follow these steps:

Step 1. Determine the molarity of each ion involved in the precipitate (Pb2+ and Br-) via dilution

Step 2.. Calculate for Q (reaction quotient) and determine if a precipitate will form.

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