Explore the properties, reactions, and uses of acids, bases, and salts in everyday life and their importance in chemistry.
Acids, Bases and Salts – Formula & Equation Sheet
Essential formulas and equations from Science, tailored for Class X in Science.
This one-pager compiles key formulas and equations from the Acids, Bases and Salts chapter of Science. 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
pH = -log[H⁺]
pH measures the acidity or basicity of a solution. [H⁺] is the concentration of hydrogen ions in moles per liter. Lower pH values indicate higher acidity.
pOH = -log[OH⁻]
pOH measures the basicity of a solution. [OH⁻] is the concentration of hydroxide ions. Lower pOH values indicate higher basicity.
pH + pOH = 14
This relationship connects the pH and pOH of a solution at 25°C, showing that as acidity increases, basicity decreases, and vice versa.
Kw = [H⁺][OH⁻] = 1×10⁻¹⁴
Kw is the ionic product of water at 25°C, showing the equilibrium concentration of H⁺ and OH⁻ ions in water.
Molarity (M) = moles of solute / liters of solution
Molarity measures the concentration of a solution. Useful for calculating the strength of acids or bases in solution.
Normality (N) = Molarity (M) × n-factor
Normality is another concentration measure, where n-factor depends on the substance's reactivity. Important for titration calculations.
Dilution formula: M₁V₁ = M₂V₂
This formula calculates the new concentration (M₂) or volume (V₂) after dilution, where M₁ and V₁ are initial molarity and volume.
Heat of neutralization: ΔH = -57.1 kJ/mol
The heat released when one mole of water is formed from the neutralization of a strong acid and base. Demonstrates exothermic nature.
Buffer capacity
A measure of a buffer's ability to resist pH change upon addition of an acid or base. Depends on the concentration of the buffer components.
Henderson-Hasselbalch equation: pH = pKa + log([A⁻]/[HA])
Estimates the pH of a buffer solution, where [A⁻] is the conjugate base concentration and [HA] is the weak acid concentration.
Equations
Acid + Metal → Salt + Hydrogen gas
General reaction showing acids reacting with metals to produce salt and hydrogen gas. Example: Zn + 2HCl → ZnCl₂ + H₂.
Base + Metal → Salt + Hydrogen gas
Some bases react with metals to produce salt and hydrogen gas. Example: 2NaOH + Zn → Na₂ZnO₂ + H₂.
Acid + Metal carbonate → Salt + Water + CO₂
Reaction of acids with metal carbonates producing salt, water, and carbon dioxide. Example: CaCO₃ + 2HCl → CaCl₂ + H₂O + CO₂.
Acid + Metal hydrogencarbonate → Salt + Water + CO₂
Similar to metal carbonates, producing salt, water, and CO₂. Example: NaHCO₃ + HCl → NaCl + H₂O + CO₂.
Acid + Base → Salt + Water
Neutralization reaction. Example: HCl + NaOH → NaCl + H₂O.
Metal oxide + Acid → Salt + Water
Basic oxides react with acids to form salt and water. Example: CuO + 2HCl → CuCl₂ + H₂O.
Non-metal oxide + Base → Salt + Water
Acidic oxides react with bases to form salt and water. Example: CO₂ + 2NaOH → Na₂CO₃ + H₂O.
2NaCl + 2H₂O → 2NaOH + Cl₂ + H₂
Chlor-alkali process producing sodium hydroxide, chlorine, and hydrogen gas.
Ca(OH)₂ + Cl₂ → CaOCl₂ + H₂O
Production of bleaching powder from chlorine and dry slaked lime.
NaHCO₃ + H⁺ → CO₂ + H₂O + Sodium salt of acid
Reaction of baking soda with acids, releasing CO₂ gas, used in fire extinguishers and baking.
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