NameFormula
Acid Ionization ConstantK_a = \frac{{\left[ {H^ + } \right]\left[ {A^ - } \right]}}{{\left[ {HA} \right]}}
Base Ionization ConstantK_b = \frac{{\left[ {OH^ - } \right]\left[ {HB^ + } \right]}}{{\left[ B \right]}}
Ion Product Constant for Water\begin{array}{*{20}c} {K_w = \left[ {OH^ - } \right]\left[ {H^ + } \right] = K_a \times K_b } \\ {\begin{array}{*{20}c} { = 1.0 \times 10^{ - 14} } & {at} & {25^\circ C} \\ \end{array}} \\ \end{array}
pH DefinedpH = - \log \left[ {H^ + } \right]
pOH DefinedpOH = - \log \left[ {OH^ - } \right]
pH and pOH Relationship14 = pH + pOH
Buffer Design EquationpH \approx pK_a - \log \frac{{\left[ {HA} \right]_0 }}{{\left[ {A^ - } \right]_0 }}
pOH and Base Ionization Equilibrium Constant RelationshippOH = pK_b + \log \frac{{\left[ {HB^ + } \right]}}{{\left[ B \right]}}
pKa DefinitionpK_a = - \log K_a
pKb DefinitionpK_b = - \log K_b
Gas Pressure and Concentration RelationshipK_p = K_c \left( {RT} \right)^{\Delta n}
Ideal gas equationPV = nRT
Adibiatic changePV = k
Charles' Law\frac{V}{t} = k
Van der Waals equation\left( {P + \frac{{an^2 }}{{V^2 }}} \right)\left( {V - bn} \right) = nRT
Molar Heat Capacity at Constant PressureC_p = \frac{{\Delta H}}{{\Delta T}}
Partial Pressure of a Gas\begin{array}{*{20}c} {P_A = P_{total} X_A } \\ {\begin{array}{*{20}c} {where} & {X_A = \frac{{\begin{array}{*{20}c} {moles} & A \\ \end{array}}}{{\begin{array}{*{20}c} {total} & {moles} \\ \end{array}}}} \\ \end{array}} \\
Total Gas Pressure as Sum of Partial PressuresP_{total} = P_A + P_B + P_C + \ldots
Number of Molesn = \frac{m}{M}
Temperature in Kelvin from Degrees Celsius ConversionK = ^\circ C + 273
Combined Gas Law\frac{{P_1 V_1 }}{{n_1 T_1 }} = \frac{{P_2 V_2 }}{{n_2 T_2 }}
Density of a MaterialD = \frac{m}{V}
Root Mean Square Velocity of Gas Moleculesu_{rms} = \sqrt {\frac{{3kT}}{m}} = \sqrt {\frac{{3RT}}{M}}
Kinetic Energy per molecule\frac{{KE}}{{molecule}} = \frac{1}{2}m\upsilon ^2
Kinetic Energy per Mole\frac{{KE}}{{mole}} = \frac{3}{2}RTn
Graham's Law of Effusion\frac{{r_1 }}{{r_2 }} = \sqrt {\frac{{M_2 }}{{M_1 }}}
Molarity Defined\begin{array}{*{20}c} {molarity,} & {M = \frac{{\begin{array}{*{20}c} {moles} & {solute} \\ \end{array}}}{{\begin{array}{*{20}c} {liter} & {solution} \\ \end{array}}}} \\ \end{array}
Molality Defined\begin{array}{*{20}c} {molality,} & { = \frac{{\begin{array}{*{20}c} {moles} & {solute} \\ \end{array}}}{{\begin{array}{*{20}c} {kilogram} & {solvent} \\ \end{array}}}} \\ \end{array}
Freezing Point Depression\Delta T_f = iK_f \times molality
Boiling Point Elevation\Delta T_b = iK_b \times molality
Osmotic Pressure\pi = \frac{{nRT}}{V}i
van't Hoff equation\ln \left( {\frac{{K_2 }}{{K_1 }}} \right) = - \frac{{\Delta H^\circ }}{R}\left[ {\frac{1}{{T_2 }} - \frac{1}{{T_1 }}} \right]
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