How Do I Solve It?
This page contains links to guides to solving many of the the types of quantitative problems found in Chemistry 116. If you don't know where to start, try the links with the same name as the chapter the problem comes from.
Sections
| Chemical Equilibrium | Electrochemistry |
| Kinetics | Nuclear Chemistry |
| Solutions | Thermodynamics |
- Writing Equilibrium Expressions
- Techniques for Solving Equilibrium Problems
- Solving Perfect Squares
- Solving Higher Order Equations containing x3, x4, ...
- Using the Quadratic Equation
- The Method of Successive Approximations
- Common Asumptions in Solving Equilibrium Problems
- Making an "ICE" Chart-An Aid in Solving Equilibrium Problems
- Calculating Equilibrium Constants
- Calculating K from known equilibrium amounts of each species
- Calculating K from initial amounts of each species and known equilibrium amount of one of the species
- Calculating K from known initial amounts of each species and the known change in amount of one of the species
- Converting Between Kc and Kp
- Calculating K for a Reaction Using Known K's for Other Reactions
- Reaction Written Backwards
- Reaction Coefficients Multiplied by a Number
- Combining Two or More Equations Algebraically
- Calculations Incorporating Two or More of these Algebraic Manipulations
- Calculating the Reaction Quotient, Q
- Determining Equilibrium Quantities from Initial Quantities and Known K
- Types of Equilibrium Systems
- Weak Acids, Ka
- What is a weak acid?
- Calculating Ka
- Calculating equilibrium concentraions in an aqueous solution of a weak acid
- Weak Bases, Kb
- What is a weak base?
- Calculating Kb
- Calculating equilibrium concentraions in an aqueous solution of a weak base
- The Auto-Ionization of Water, Kw
- Finding pH, pOH, pKa, and pKb
- Calculating pH
- Calculating hydronium ion concentration from known pH
- Calculating pOH
- Calculating hydroxide ion concentration from known pOH
- The relationship between pH and pOH
- Calculating pKa
- Calculating Ka from pKa
- Calculating pKb
- Calculating Kb from pKb
- Salt Solutions
- Buffer Systems
- Solubility Product Constants, Ksp
- Electrochemical Cell Potentials
- Equilibrium Constants and Free Energy Changes for Electrochemical Cells
- Determining equilibrium constants
- Determining standard state free energy changes
- Determining nonstandard state free energy changes
- Electrolysis
- Determining Reaction Rates
- Rate Laws and Order of a Reaction
- Determining Rate Laws from Rate versus Concentration Data (Differential Rate Laws)
- Determining Rate Laws from Graphs of Concentration versus Time (Integrated Rate Laws)
- Using Integrated Rate Laws
- How long does it take to react?
- What concentration remains after a given time?
- What was the initial concentration?
- Half Life
- Nuclear Binding Energy
- Determining the mass defect
- Converting mass defect into energy
- Expressing nuclear binding energy as energy per mole of atoms or as energy per nucleon
- Determining the Energy of a Nuclear Reaction
- Kinetics of Radioactive Decay
- Calculations using the first order rate equation: r = k[N]
- Calculations using the first order rate equation: ln(N/No) = -kt
- Determining the amount of radioisotope remaining after time "t"
- Determining the initial amount of a radioisotope at the beginning of time "t"
- Determining the rate constant
- Determining and using the half-life of a radioisotope
- Determining the age of an artefact using carbon-14 dating
- Concentrations
- Colligative Properties
- Determining Molar Mass (Molecular Weight) from Colligative Properties
- Calorimetry
- Expansion Work
- Internal Energy, Heat, and Work
- Enthalpy Changes
- Entropy Changes
- Four Ways to Determine Free Energy Changes
- From Free Energies of Formation
- From Enthalpy Changes and Entropy Changes
- From Equilibrium Constants
- From Cell Potentials
- Free Energy Changes under Non-standard State Conditions
- Calculating an Equilibrium Constant from a Free Energy Change
- Calculating a Cell Potential from a Free Energy Change
- Determination of Thermodynamic Properties from Changes in an Equilibrium Constant with Temperature
