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# Solution Stoichiometry

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Sections
Solutions
Solubility and Intermolecular Forces
Solutions: Mass Percent
Percent Concentrations
Molarity
Osmolarity
Parts per Million (ppm)
Solubility: Temperature Effect
Intro to Henry's Law
Henry's Law Calculations
Dilutions
Solution Stoichiometry
Electrolytes (Simplified)
Equivalents
Molality
The Colligative Properties
Boiling Point Elevation
Freezing Point Depression
Osmosis
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).