Chemistry Reference Tables
Source-cited data for general chemistry, from SI units to nuclear half-lives, with interactive charts for curves and diagrams.
22 of 22 tables
Fundamentals
Compounds & Naming
Common Ions
Reference table of common monatomic and polyatomic ions with their charges and formulas. Essential for writing chemical formulas and naming compounds.
→Ion Naming Patterns
The systematic per-/ate/-ite/hypo- naming pattern for oxyanions, organized by element series. Master this pattern to name the common oxyanion families from their formulas.
→Reactivity
Bonding
Organic Chemistry
Acids & Bases
Strong Acids & Bases
The seven strong acids and eight strong bases that ionize completely in water. Essential for pH calculations and acid-base reaction predictions.
→Indicators
The common acid-base indicators with their pKa values, color-change intervals, and acid/base colors. Choose an indicator whose full transition interval lies inside the steep region of the titration curve.
→Titration Curves
Explore four classic titration curves: strong acid + strong base, weak acid + strong base, weak base + strong acid, and strong base + strong acid. Each uses 25.00 mL of 0.100 M analyte and 0.100 M titrant. Read the pH at any volume and compare eight indicator transition ranges.
→Equilibrium
Ka / Kb Constants
Acid-ionization (Ka) and base-ionization (Kb) constants at 25 °C for the weak acids, weak bases, and conjugate pairs used throughout the acid-base, buffer, hydrolysis, and titration topics. Use Ka × Kb = Kw = 1.0 × 10⁻¹⁴ to convert between a conjugate pair.
→Ksp Values
Solubility product constants (Ksp) at 25 °C for 100 sparingly soluble ionic compounds, grouped by metal, each with its dissolution equilibrium. Use Ksp with the dissolution stoichiometry to compute molar solubility, predict precipitation with Q vs Ksp, and analyze common-ion and complex-ion effects.
→Kf Values
Formation (stability) constants Kf at 25 °C for common complex ions, each with its formation equilibrium. Large Kf values explain why complexation dissolves sparingly soluble salts: couple the dissolution with the formation equilibrium (K = Ksp × Kf) to compute solubility in the presence of a complexing agent.
→Solutions
Solubility Rules
Quick-reference solubility rules for predicting whether ionic compounds dissolve in water. Essential for precipitation reactions and net ionic equations.
→Kb / Kf (molal)
Molal boiling-point-elevation (Kb) and freezing-point-depression (Kf) constants for common solvents. Use ΔTb = i·Kb·m and ΔTf = i·Kf·m, where m is the molality of the solution and i is the van 't Hoff factor.
→Solubility Curves
Interactive solubility curves for nine common salts in water (g of solute per 100 g of H₂O, 0 to 100 °C). Click or tap anywhere on a curve to read the solubility at that temperature. Points below a curve are unsaturated, on the curve saturated, and above it supersaturated.
→Thermodynamics
Kinetics
Electrochemistry
Coordination Chemistry
Gases & Liquids
Water Vapor Pressure
Vapor pressure of liquid water from 0 °C to 100 °C in torr, kPa, and atm. Needed whenever a gas is collected over water: subtract the water vapor pressure from the total pressure (Dalton's law, P_gas = P_total − P_H₂O) before applying the ideal gas law.
→Phase Diagrams
Interactive pressure-temperature phase diagrams for water and carbon dioxide. Click or tap anywhere to identify the phase at that temperature and pressure; points on a curve read as the two-phase equilibrium, and the triple and critical points announce themselves. Vapor curves are Clausius-Clapeyron fits through measured reference points; fusion lines are anchored linear fits.
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