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4.5 Solution Stoichiometry

Chad's General Chemistry Videos

Course Menu

Chapter 1 – Matter and Measurement
- 1.1 Matter
- 1.2 Significant Figures
- 1.3 Units and Conversions
Chapter 2 – Atoms, Molecules, and Ions
- 2.1 Atomic Structure and Introduction to the Periodic Table
- 2.2 Naming Ionic Compounds
- 2.3 Naming Molecular Compounds
- 2.4 Naming Acids
Chapter 3 – Stoichiometry
- 3.1 Chemical Reactions & Chemical Equations
- 3.2 Calculations With Moles
- 3.3 Mass Percent and Empirical and Molecular Formulas
- 3.4 Limiting Reagent Calculations
Chapter 4 – Aqueous Reactions and Solution Stoichiometry
- 4.1 Solutions and Electrolytes
- 4.2 Double Displacement Reactions
- 4.3 Oxidation-Reduction Reactions
- 4.4 Molarity and Dilutions
- 4.5 Solution Stoichiometry
Chapter 5 – Thermochemistry
- 5.1 First Law of Thermodynamics and Enthalpy
- 5.2 Calorimetry
- 5.3 Hess’s Law and Enthalpies of Formation
Chapter 6 – Electronic Structure
- 6.1 Nature of Light and the Photoelectric Effect
- 6.2 Electronic Transitions (Absorption and Emission)
- 6.3 The de Broglie Relation and the Heisenberg Uncertainty Principle
- 6.4 Quantum Numbers and Atomic Orbitals
- 6.5 Electronic Configuration
Chapter 7 – Periodic Trends
- 7.1 Atomic Radius
- 7.2 Ionization Energy
- 7.3 Electron Affinity & Electronegativity
- 7.4 Properties of Elements & Compounds
Chapter 8 – Bonding and Lewis Structures
- 8.1 Ionic Bonding
- 8.2 Lewis Dot Structures
- 8.3 Bond Enthalpy
Chapter 9 – Molecular Geometry
- 9.1 VSEPR Theory and Molecular Geometry
- 9.2 Polarity
- 9.3 Hybridization
- 9.4 Sigma and Pi Bonds
- 9.5 Molecular Orbital Theory
Chapter 10 – Gases
- 10.1 Properties of Gases
- 10.2 Gas Laws Including the Ideal Gas Law
- 10.3 Additional Gas Laws
- 10.4 Real Gases & the Van der Waals Equation
Chapter 11 – Intermolecular Forces, Liquids, and Solids
- 11.1 Intermolecular Forces
- 11.2 Phase Diagrams
- 11.3 Structures of Solids
Chapter 13 – Solutions
- 13.1 Solution Formation and Solubility
- 13.2 Units of Concentration
- 13.3 Colligative Properties
Chapter 14 – Kinetics
- 14.1 Rate Expressions and the Rate of Reaction
- 14.2 Rate Laws
- 14.3 Reaction Mechanisms, Catalysts, and Reaction Coordinate Diagrams
- 14.4 Collision Theory and the Arrhenius Equation
- 14.5 Integrated Rate Laws
Chapter 15 – Equilibrium
- 15.1 Equilibrium and Equilibrium Constants
- 15.2 Le Chatelier’s Principle
- 15.3 Equilibrium Calculations (ICE Tables)
Chapter 16 – Acids and Bases
- 16.1 Introduction to Acids and Bases
- 16.2 Binary Acids, Oxoacids, and Polyprotic Acids
- 16.3 Introduction to the pH Scale and pH Calculations
- 16.4 pH Calculations for Strong Acids and Bases
- 16.5 pH Calculations for Weak Acids and Bases
- 16.6 Acidity and Basicity of Salts
Chapter 17 – Buffers, Titrations, and Solubility
- 17.1 Buffers
- 17.2 Titrations and Titration Curves
- 17.3 pH Calculations Involving Titrations
- 17.4 Solubility and Ksp
- 17.5 Common Ion Effect and Precipitation
- 17.6 pH Effects on Solubility
Chapter 18 – Thermodynamics
- 18.1 The Laws of Thermodynamics
- 18.2 Entropy
- 18.3 Gibbs Free Energy and the Relationship between ΔG, ΔH, & ΔS
- 18.4 ΔG, ΔH, ΔS, and Formation Reactions
- 18.5 Gibbs Free Energy and the Equilibrium Constant
Chapter 19 – Electrochemistry
- 19.1 How to Assign Oxidation Numbers
- 19.2 How to Balance Oxidation Reduction Reactions
- 19.3 Galvanic Cells
- 19.4 How to Calculate Standard Cell Potential
- 19.5 How to Calculate Nonstandard Cell Potential [Nernst Equation]
- 19.6 Cell Potential, Delta G, and the Equilibrium Constant
- 19.7 Electrolytic Cells
- 19.8 Electrolysis Calculations
Chapter 20 – Nuclear Chemistry
- 20.1 Introduction to Nuclear Chemistry
- 20.2 Balancing Nuclear Reactions
- 20.3 Spontaneous Routes of Nuclear Decay, Fission, & Fusion
- 20.4 Kinetics of Nuclear Decay
- 20.5 Energy of Nuclear Reactions and Nuclear Binding Energy
Chapter 21 – Coordination Chemistry
- 21.1 Introduction to Coordination Chemistry
- 21.2 Naming Complex Ions and Coordination Compounds
- 21.3 Isomers in Coordination Chemistry
- 21.4 Crystal Field Theory
- 21.5 Color & Paramagnetism of Coordination Compounds

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4.4 Molarity and Dilutions

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HCl(aq) + NaOH(aq) ➔ H₂O(l) + NaCl(aq)

What volume of 2.0M HCl would be required to neutralize 20.0g NaOH?

H₂SO₄(aq) + 2NaOH(aq) ➔ 2H₂O(l) + Na₂SO₄(aq)

What volume of 0.10 M H₂SO₄ is required to neutralize 0.50L of 0.40M NaOH?

4.4 Molarity and Dilutions

5.1 First Law of Thermodynamics...

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