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A conjugate acid-base pair consists of two species that differ by one proton (H⁺). The acid donates a proton, and the base accepts it. Example: NH3 + H2O ⇔ NH4+ + OH¯ In the reaction. NH3 and NH4+ , form a conjugate pair, as do H2O and OH¯. Related Questions: Define and give examples of Arrhenius … Read more
Because BF₃ can accept an electron pair from a donor, which is the characteristic behavior of a Lewis acid. Related Questions: Why H⁺ ion acts as a Lewis acid? Define and give examples of Arrhenius acids? Define a conjugate acid-base pair. What is the role of indicators in acid-base titrations? What is meant by the … Read more
According to the Bronsted-Lowry theory, a base is a proton acceptor. NH₃ can accept a proton (H⁺), thus it acts as a base. Related Questions: CHEMICAL EQUILIBRIUM Define chemical equilibrium with example What is meant by chemical equilibrium? Differentiate between reversible and irreversible reactions? State Le-Chatelier’s principle. What is the significance of the equilibrium … Read more
Reason: A Lewis acid is an electron pair acceptor. The H⁺ ion has no electrons and can accept an electron pair, making it a Lewis acid. Related Questions: Why BF₃ acts as a Lewis acid? Define and give examples of Arrhenius acids? Define a conjugate acid-base pair. What is the role of indicators in acid-base … Read more
Definition: An Arrhenius acid is a substance that dissociates in water to release ions. Examples: HCl, H₂SO₄, HNO₃ Related Questions: Why H⁺ ion acts as a Lewis acid? Why BF₃ acts as a Lewis acid? Define a conjugate acid-base pair. What is the role of indicators in acid-base titrations? What is meant by the neutralization … Read more
The equation for the self-ionization of water: 2H2O⇔H3O+ + OH¯ H2O⇔H+ + OH¯ Related Questions: ACIDS, BASES AND SALTS Define chemical equilibrium with example What is meant by chemical equilibrium? What is the effect of decreasing pressure on a gaseous equilibrium system? What is dynamic equilibrium? How does temperature affect the equilibrium constant? Define and … Read more
Related Questions: CHEMICAL EQUILIBRIUM Define chemical equilibrium with example What is meant by chemical equilibrium? Differentiate between reversible and irreversible reactions? State Le-Chatelier’s principle. What is the significance of the equilibrium constant (Kc)? Why does a catalyst not affect the position of equilibrium? What happens to the equilibrium position if the concentration of a reactant … Read more
Aspect Reversible reaction Irreversible reaction Definition A reversible reaction occurs in both forward and reverse directions. An irreversible reaction occurs in one direction only. Equilibrium It achieves a state of dynamic equilibrium where the rate of the forward reaction equals the rate of the reverse reaction. No equilibrium is established in such reactions. Completion … Read more
Role of Catalyst: A catalyst speeds up both the forward and reverse reactions equally. It lowers the activation energy for both reactions, allowing equilibrium to be reached more quickly. Effect on Equilibrium Position: A catalyst does not change the position of equilibrium or the value of the equilibrium constant (Kc). It only reduces the time … Read more
Applications: 1. Haber Process (Ammonia Production): To increase ammonia production: Increase pressure (favors fewer gas molecules). Decrease temperature (favors the exothermic reaction). Remove ammonia as it forms (shifts equilibrium to the right). 2. Contact Process (Sulfuric Acid Production): High pressure and low temperature favor the formation of sulfuric acid . 3. Production of Methanol: High … Read more