| Name | Formula |
|---|
| Acid Ionization Constant | \[K_a = \frac{{\left[ {H^ + } \right]\left[ {A^ - } \right]}}{{\left[ {HA} \right]}}\] |
| Base Ionization Constant | \[K_b = \frac{{\left[ {OH^ - } \right]\left[ {HB^ + } \right]}}{{\left[ B \right]}}\] |
| 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 Defined | \[pH = - \log \left[ {H^ + } \right]\] |
| pOH Defined | \[pOH = - \log \left[ {OH^ - } \right]\] |
| pH and pOH Relationship | \[14 = pH + pOH\] |
| Buffer Design Equation | \[pH \approx pK_a - \log \frac{{\left[ {HA} \right]_0 }}{{\left[ {A^ - } \right]_0 }}\] |
| pOH and Base Ionization Equilibrium Constant Relationship | \[pOH = pK_b + \log \frac{{\left[ {HB^ + } \right]}}{{\left[ B \right]}}\] |
| pKa Definition | \[pK_a = - \log K_a\] |
| pKb Definition | \[pK_b = - \log K_b\] |
| Gas Pressure and Concentration Relationship | \[K_p = K_c \left( {RT} \right)^{\Delta n}\] |
| Ideal gas equation | \[PV = nRT\] |
| Adibiatic change | \[PV = k\] |
| 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 Pressure | \[C_p = \frac{{\Delta H}}{{\Delta T}}\] |
| Partial Pressure of a Gas | \[\begin{array}{*{20}c}
{P_A = P_{total} X_A } \\
{\begin{array}{*{20}c}
{where} & {X_A = \frac{{\begin{array}{*{20}c}
{moles} & A \\
\end{array}}}{{\begin{array}{*{20}c}
{total} & {moles} \\
\end{array}}}} \\
\end{array}} \\
\end{array}\] |
| Total Gas Pressure as Sum of Partial Pressures | \[P_{total} = P_A + P_B + P_C + \ldots\] |
| Number of Moles | \[n = \frac{m}{M}\] |
| Temperature in Kelvin from Degrees Celsius Conversion | \[K = ^\circ C + 273\] |
| Combined Gas Law | \[\frac{{P_1 V_1 }}{{n_1 T_1 }} = \frac{{P_2 V_2 }}{{n_2 T_2 }}\] |
| Density of a Material | \[D = \frac{m}{V}\] |
| Root Mean Square Velocity of Gas Molecules | \[u_{rms} = \sqrt {\frac{{3kT}}{m}} = \sqrt {\frac{{3RT}}{M}}\] |
| 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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