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Grade 11 Chemistry: formula sheet

The mole, balancing and stoichiometry, reactions, solutions, gases, water and pH · 31 formulas · metric edition 1

Download the PDF: 2 pagesThe full study guide: modules, problems, answer key
Module 1 · The Mole
Chemistry 11-1 Moles from Mass (n = m/M)
n=mMn = \frac{m}{M}
Converts a measured mass into an amount of substance by dividing by the molar mass.
Chemistry 11-2 Particles from Moles (Avogadro's Number)
N=n NAN = n\,N_A
Converts an amount in moles into an actual particle count using the Avogadro constant NA =…
Chemistry 11-3 Percent Composition of an Element
%X=a MXMcompound×100%\%X = \frac{a\,M_X}{M_{\text{compound}}} \times 100\%
Gives the mass percent an element contributes to a compound from the formula subscript and molar…
Module 2 · Balancing & Stoichiometry
Chemistry 11-4 Mole Ratio from a Balanced Equation
nB=nA ban_B = n_A \, \frac{b}{a}
Converts moles of one substance in a balanced equation into moles of another using the ratio of…
Chemistry 11-5 Mass-to-Mass Stoichiometry
mB=mAMA⋅ba⋅MBm_B = \frac{m_A}{M_A} \cdot \frac{b}{a} \cdot M_B
Gives the mass of one substance produced or consumed from the mass of another, routing through…
Chemistry 11-6 Gas Volume at STP
V=n VmV = n\,V_m
Converts between moles of an ideal gas and its volume at STP using the molar volume Vm = 22.414…
Chemistry 11-7 Theoretical Yield from the Limiting Reactant
nP=p min⁡ ⁣(nAa,  nBb)n_P = p \, \min\!\left(\frac{n_A}{a},\; \frac{n_B}{b}\right)
Gives the most product two reactants can make: divide each reactant's moles by its coefficient, and…
Chemistry 11-8 Excess Reagent Remaining
nexcess=nB−ba nAn_{\text{excess}} = n_B - \frac{b}{a} \, n_A
Gives how much of the reactant in excess is left unreacted once the limiting reagent A has been…
Module 3 · Reactions by the Numbers
Chemistry 11-9 Percent Yield
% yield=mactualmtheoretical×100%\%\,\text{yield} = \frac{m_{\text{actual}}}{m_{\text{theoretical}}} \times 100\%
Compares the mass actually isolated from a reaction to the maximum mass stoichiometry predicts.
Chemistry 11-10 Heat of Reaction
q=nΔHq = n \Delta H
Scales a reaction's molar enthalpy change by the amount reacted to give the total heat released or…
Module 4 · Solutions & Dilution
Chemistry 11-11 Molarity (C = n/V)
C=nVC = \frac{n}{V}
Defines molar concentration as moles of solute per volume of solution.
Chemistry 11-12 Mass Percent of a Solution
c=msolutemsolution×100%c = \frac{m_{\text{solute}}}{m_{\text{solution}}} \times 100\%
Expresses a solution's concentration as the solute's share of the total solution mass in percent.
Chemistry 11-13 Ion Concentration from Dissociation
cion=ν Cc_{\text{ion}} = \nu \, C
Gives the concentration of one ion in a solution of a soluble ionic compound: the compound's…
Chemistry 11-14 Dilution Equation (C1V1 = C2V2)
C1V1=C2V2C_1 V_1 = C_2 V_2
States that concentration times volume is conserved when a solution is diluted, since the moles of…
Module 5 · Gases
Chemistry 11-15 Ideal Gas Law
PV=nRTP V = n R T
Relates pressure, volume, amount, and temperature of a gas.
Chemistry 11-16 Boyle's Law
P1V1=P2V2P_1 V_1 = P_2 V_2
At constant temperature, pressure times volume stays constant for a fixed amount of gas.
Chemistry 11-17 Charles's Law
V1T1=V2T2\frac{V_1}{T_1} = \frac{V_2}{T_2}
At constant pressure, gas volume is directly proportional to absolute temperature.
Chemistry 11-18 Gay-Lussac's Law
P1T1=P2T2\frac{P_1}{T_1} = \frac{P_2}{T_2}
At constant volume, gas pressure is directly proportional to absolute temperature.
Chemistry 11-19 Combined Gas Law
P1V1T1=P2V2T2\frac{P_1 V_1}{T_1} = \frac{P_2 V_2}{T_2}
For a fixed amount of gas, pressure times volume over absolute temperature stays constant between…
Chemistry 11-20 Gas Density from Molar Mass
ρ=PMRT\rho = \frac{PM}{RT}
Gives an ideal gas's density from its molar mass, pressure, and absolute temperature using R =…
Module 6 · Water by the Numbers
Chemistry 11-21 Nutrient ppm from Fertiliser Weight
c=m fVc = \frac{m \, f}{V}
The concentration of a single nutrient element delivered to a reservoir, from the weight of…
Chemistry 11-22 TDS Estimated from Conductivity (TDS = k × EC)
TDS=k×EC\mathrm{TDS} = k \times \mathrm{EC}
Estimates total dissolved solids in mg/L from a conductivity reading in µS/cm using an empirical…
Chemistry 11-23 Total Hardness as CaCO₃
TH=2.497 Ca+4.118 Mg\mathrm{TH} = 2.497\,\mathrm{Ca} + 4.118\,\mathrm{Mg}
Converts a lab report's calcium and magnesium ion results into a single total hardness expressed as…
Chemistry 11-24 Grains per Gallon ↔ ppm Hardness
H=17.118 GH = 17.118\,G
Converts water hardness between grains per US gallon and mg/L as CaCO₃ using the exact 17.118 mg/L…
Chemistry 11-25 Ion Concentration as CaCO₃ Equivalent
CCaCO3=Cion×50.04EWC_{\mathrm{CaCO_3}} = C_{\mathrm{ion}} \times \frac{50.04}{\mathrm{EW}}
Restates any ion's concentration in the trade's common currency of CaCO₃ by scaling with the ratio…
Chemistry 11-26 Equivalent Weight from Molar Mass and Valence
EW=Mz\mathrm{EW} = \frac{M}{z}
Gives the gram-equivalent weight of an ion or compound as its molar mass divided by the number of…
Chemistry 11-27 Chlorine Dose, Demand and Residual
D=Cdemand+CresD = C_{\text{demand}} + C_{\text{res}}
The fundamental chlorination balance: the dose applied equals the chlorine consumed by the water's…
Chemistry 11-28 Chemical Feed Rate (lb/day = mg/L × MGD × 8.34)
m˙=C Q\dot m = C \, Q
Converts a target chemical dose and a plant flow into a mass feed rate, the classic pounds-per-day…
Module 7 · Acids, Bases & pH
Chemistry 11-29 pH from Hydrogen Ion Concentration
pH=−log⁡10 [H+]\mathrm{pH} = -\log_{10}\,[\mathrm{H^+}]
Expresses acidity as the negative base-10 logarithm of the hydrogen ion concentration in mol/L.
Chemistry 11-30 pH and pOH Relation
pH+pOH=14\mathrm{pH} + \mathrm{pOH} = 14
Links the acidity and basicity scales of any aqueous solution at 25 °C, where pKw = 14.
Chemistry 11-31 Titration: Concentration of an Unknown
Ca=n CbVbVaC_a = \frac{n\,C_b V_b}{V_a}
Finds an analyte's concentration from the titre volume, titrant concentration, and the reaction's…