Clutch Prep is now a part of Pearson
All Chapters
Ch.1 Matter and Measurements
Ch.2 Atoms and the Periodic Table
Ch.3 Ionic Compounds
Ch.4 Molecular Compounds
Ch.5 Classification & Balancing of Chemical Reactions
Ch.6 Chemical Reactions & Quantities
Ch.7 Energy, Rate and Equilibrium
Ch.8 Gases, Liquids and Solids
Ch.9 Solutions
Ch.10 Acids and Bases
Ch.11 Nuclear Chemistry
BONUS: Lab Techniques and Procedures
BONUS: Mathematical Operations and Functions
Solubility and Intermolecular Forces
Solutions: Mass Percent
Percent Concentrations
Parts per Million (ppm)
Solubility: Temperature Effect
Intro to Henry's Law
Henry's Law Calculations
Solution Stoichiometry
Electrolytes (Simplified)
The Colligative Properties
Boiling Point Elevation
Freezing Point Depression
Osmotic Pressure

Solution Stoichiometry deals with stoichiometric calculations in solutions that involve volume and molarity.

Solution Stoichiometry

Concept #1: Solution Stoichiometry

Use the solution stoichiometric chart when dealing with calculations involving molarity and/or volume. 

Example #1: How many moles of hydrogen gas were produced when 38.74 mL of 0.275 M H2O reacts with excess sodium?

Practice: How many milliliters of 0.325 M HCl are needed to react with 16.2 g of magnesium metal? 

2 HCl (aq) + Mg (s) → MgCl2 + H2 (g)

Practice: What is the molar concentration of a hydrobromic acid solution if it takes 34.12 mL of HBr to completely neutralize 82.56 mL of 0.156 M Ca(OH)­2

2 HBr (aq) + Ca(OH)2 (aq)  → CaBr2 (aq) + 2 H2O (l)

Practice: Consider the following balanced chemical equation: 

H2O+ 2 MnO4 + 3 SO32-  → 2 MnO2 + 3 SO42-+ 2 OH

How many grams of MnO2 (MW: 86.94 g/mol) will be created when 25.0 mL of 0.120 M MnO4 (MW: 118.90 g/mol) reacts with 32.0 mL of 0.140 M SO32- (MW: 80.07 g/mol).