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Formula Sheet
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.
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.
Explore the fundamentals of chemical reactions, types, and balancing equations in this chapter, essential for understanding chemistry basics.
Explore the properties, reactions, and uses of metals and non-metals, understanding their role in daily life and industrial applications.
Explore the versatile world of carbon, its allotropes, and the vast array of compounds it forms, including hydrocarbons and their derivatives, in this comprehensive chapter.
Life Processes explores the essential functions that sustain living organisms, including nutrition, respiration, transportation, and excretion.
