Q1
An acidic buffer is typically prepared from:
📝 SolutionAn acidic buffer consists of a weak acid and the salt of its conjugate base, e.g. $CH_3COOH$ and $CH_3COONa$.
Q2
The common ion effect refers to the suppression of ionization of a weak electrolyte when:
📝 SolutionAdding a strong electrolyte with an ion common to a weak electrolyte shifts the weak electrolyte's equilibrium backward, suppressing its ionization (common ion effect).
Q3
Assertion (A): Increasing temperature shifts an exothermic equilibrium reaction backward.
Reason (R): Heat can be treated as a product in an exothermic reaction, and Le Chatelier's principle predicts the equilibrium shifts to consume the added heat.
Choose the correct option:
Reason (R): Heat can be treated as a product in an exothermic reaction, and Le Chatelier's principle predicts the equilibrium shifts to consume the added heat.
Choose the correct option:
📝 SolutionIn an exothermic reaction, heat is released as a product; raising temperature adds 'more product', so equilibrium shifts backward (towards reactants) to absorb the extra heat, exactly as R explains.
Q4
Assertion (A): A large value of the equilibrium constant $K$ indicates the reaction goes almost to completion.
Reason (R): A large $K$ means the equilibrium concentration of products is much greater than that of reactants.
Choose the correct option:
Reason (R): A large $K$ means the equilibrium concentration of products is much greater than that of reactants.
Choose the correct option:
📝 Solution$K$ is the ratio of product to reactant concentrations at equilibrium; a very large value means products dominate, so the reaction proceeds nearly to completion. R correctly explains A.
Q5
A catalyst affects a reaction at equilibrium by:
📝 SolutionA catalyst speeds up both forward and reverse reactions equally, so it helps the system reach equilibrium faster but does not change the position of equilibrium or the value of $K$.
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Class 11 · Chemistry
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