Grade 11 Chemistry — formula sheet

The mole, reactions, solutions, gases, water and pH · 26 formulas · metric edition 1

Moles from Mass (n = m/M)

n = \frac{m}{M}

Particles from Moles (Avogadro's Number)

N = n\,N_A

Percent Composition of an Element

\%X = \frac{a\,M_X}{M_{\text{compound}}} \times 100\%

Percent Yield

\%\,\text{yield} = \frac{m_{\text{actual}}}{m_{\text{theoretical}}} \times 100\%

Heat of Reaction

q = n \Delta H

Molarity (C = n/V)

C = \frac{n}{V}

Mass Percent of a Solution

c = \frac{m_{\text{solute}}}{m_{\text{solution}}} \times 100\%

Dilution Equation (C1V1 = C2V2)

C_1 V_1 = C_2 V_2

Ideal Gas Law

P V = n R T

Boyle's Law

P_1 V_1 = P_2 V_2

Charles's Law

\frac{V_1}{T_1} = \frac{V_2}{T_2}

Gay-Lussac's Law

\frac{P_1}{T_1} = \frac{P_2}{T_2}

Combined Gas Law

\frac{P_1 V_1}{T_1} = \frac{P_2 V_2}{T_2}

Gas Volume at STP

V = n\,V_m

Gas Density from Molar Mass

\rho = \frac{PM}{RT}

Nutrient ppm from Fertiliser Weight

c = \frac{m \, f}{V}

TDS Estimated from Conductivity (TDS = k × EC)

\mathrm{TDS} = k \times \mathrm{EC}

Total Hardness as CaCO₃

\mathrm{TH} = 2.497\,\mathrm{Ca} + 4.118\,\mathrm{Mg}

Grains per Gallon ↔ ppm Hardness

H = 17.118\,G

Ion Concentration as CaCO₃ Equivalent

C_{\mathrm{CaCO_3}} = C_{\mathrm{ion}} \times \frac{50.04}{\mathrm{EW}}

Equivalent Weight from Molar Mass and Valence

\mathrm{EW} = \frac{M}{z}

Chlorine Dose, Demand and Residual

D = C_{\text{demand}} + C_{\text{res}}

Chemical Feed Rate (lb/day = mg/L × MGD × 8.34)

\dot m = C \, Q

pH from Hydrogen Ion Concentration

\mathrm{pH} = -\log_{10}\,[\mathrm{H^+}]

pH and pOH Relation

\mathrm{pH} + \mathrm{pOH} = 14

Titration: Concentration of an Unknown

C_a = \frac{n\,C_b V_b}{V_a}