This chapter focuses on the characteristics and behaviors of solutions, including their formation, composition, and properties.
Solutions – Formula & Equation Sheet
Essential formulas and equations from Chemistry - I, tailored for Class 12 in Chemistry.
This one-pager compiles key formulas and equations from the Solutions chapter of Chemistry - I. Ideal for exam prep, quick reference, and solving time-bound numerical problems accurately.
Key concepts & formulas
Essential formulas, key terms, and important concepts for quick reference and revision.
Formulas
Mass % of component = (Mass of component in solution / Total mass of solution) × 100
This formula expresses the concentration of a component in a solution as a percentage of its mass relative to the total mass of the solution.
Volume % of component = (Volume of component / Total volume of solution) × 100
This formula expresses the concentration of a liquid component in a solution as a percentage of its volume relative to the total volume.
Mass by Volume % (w/V) = (Mass of solute in g / Volume of solution in mL) × 100
This formula indicates the mass of solute per 100 mL of solution, ideal for pharmaceutical applications.
ppm = (Number of parts of component / Total number of parts in solution) × 10^6
Parts per million (ppm) expresses small concentrations, particularly used for pollutants.
Mole fraction (x) = (Number of moles of component) / (Total number of moles in solution)
This formula calculates the ratio of moles of a component to the total moles in a solution, crucial in gas mixture calculations.
Molarity (M) = (Moles of solute / Volume of solution in L)
Molarity defines the concentration of a solution in terms of solute amount per liter of solution.
Molality (m) = (Moles of solute / Mass of solvent in kg)
This formula measures concentration, independent of temperature, as moles of solute per kilogram of solvent.
Henry’s Law: p = K_H × x
Describes the solubility of a gas in a liquid; p is the partial pressure of the gas, K_H is the Henry’s law constant, and x is the mole fraction in the solution.
p_1 = x_1 * p_1^0
Raoult’s law shows that the partial vapor pressure of a component in a solution is equal to its mole fraction multiplied by its vapor pressure.
DT_b = K_b * m
Elevation of boiling point, where DT_b is the increase in boiling point, K_b is the boiling point elevation constant, and m is the molality.
DT_f = K_f * m
Depression of freezing point formula, where DT_f is the decrease in freezing point, K_f is the depression constant, and m is the molality.
Equations
p = CRT
This equation relates osmotic pressure (p) to concentration (C), gas constant (R), and temperature (T).
dT_f = K_f * m
Relates the freezing point depression (dT_f) to the molality (m) of the solution and the freezing point depression constant (K_f).
dT_b = K_b * m
Relates the change in boiling point (dT_b) to the molality (m) of the solution and the boiling point elevation constant (K_b).
Δp = (p^0 - p) / p^0 = x_2
Defines the relative lowering of vapor pressure concerning the mole fraction of solute in the solution.
p_1 + p_2 = p_{total}
States that the total vapor pressure above the solution is the sum of the partial pressures of each component.
i = normal molar mass / abnormal molar mass
The van't Hoff factor relates the expected number of particles in a solution to the actual number due to dissociation or association.
M_2 = (ΔT_f K_f 1000) / (w_2 w_1)
Calculates molar mass (M_2) of solute using the depression in freezing point (ΔT_f), cryoscopic constant (K_f), mass of solute (w_2), and mass of solvent (w_1).
P_{solution} = (n_2/V)*R*T
Defines osmotic pressure based on number of moles of solute (n_2), volume of solution (V), gas constant (R), and temperature (T).
M = (n_2/V)
Relates the number of moles (n_2) of solute to the volume of solution (V) for calculating molarity.
ΔP = K_H * p_g
Expresses the change in pressure concerning how much gas is dissolved in the liquid based on Henry's law.
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