Chemical and Ionic Equilibrium Practice Questions
JEE · Chemistry · 1166 free MCQs with instant results and detailed explanations.
1166
Total
273
Easy
487
Medium
406
Hard
Start Practicing Chemical and Ionic Equilibrium
Take a timed quiz or customize your practice session
Topics in Chemical and Ionic Equilibrium
Law of Mass Action
152
Le Chatelier
111
Solubility Product
134
Common Ion Effect
112
Kc and Kp
142
Le Chatelier's Principle
134
Ionic Equilibrium
130
pH
109
Buffer Solutions
142
Sample Questions from Chemical and Ionic Equilibrium
Here are 10 sample questions. Start a quiz to get randomized questions with scoring.
Q1
Easy
According to the law of mass action, the rate of a reaction is directly proportional to what?
A.
the concentration of reactants
B.
the concentration of products
C.
the temperature of the reactants
D.
the surface area of the reactants
Show Answer & Explanation
Correct Answer: A
The law of mass action states that the rate of a reaction is proportional to the product of the concentrations of the reactants raised to their respective stoichiometric coefficients.
Q2
Easy
If the equilibrium constant (K) of a reaction at a given temperature is 4, what can be inferred about the concentrations of products and reactants?
A.
Products are favored at equilibrium
B.
Reactants are favored at equilibrium
C.
Reactants and products are equal at equilibrium
D.
The reaction does not reach equilibrium
Show Answer & Explanation
Correct Answer: A
A K value greater than 1 indicates that at equilibrium, the concentration of products is greater than that of reactants, meaning products are favored.
Q3
Easy
For a reaction represented as A + B ⇌ C + D, if the concentration of A is doubled, what happens to the equilibrium position?
A.
Shifts to the right
B.
Shifts to the left
C.
Remains unchanged
D.
Becomes spontaneous
Show Answer & Explanation
Correct Answer: A
According to Le Chatelier's principle, increasing the concentration of a reactant (A) will shift the equilibrium position to the right to produce more products (C and D).
Q4
Medium
Consider the equilibrium reaction 2A(g) ⇌ B(g) + C(g). If the equilibrium constant Kc is 2 at a certain temperature, what is the reaction quotient Qc when the concentrations are [A] = 1 M, [B] = 0.5 M, [C] = 0.5 M?
A.
1
B.
0.5
C.
2
D.
0.25
Show Answer & Explanation
Correct Answer: D
To find Qc, use the formula Qc = [B][C]/[A]^2. Plugging in the values gives Qc = (0.5)(0.5)/(1^2) = 0.25.
Q5
Medium
For the reaction N2(g) + 3H2(g) ⇌ 2NH3(g), if the initial concentrations are [N2] = 1 M, [H2] = 3 M, what will be the concentration of NH3 at equilibrium if Kc = 4?
A.
0.5 M
B.
1 M
C.
2 M
D.
0.25 M
Show Answer & Explanation
Correct Answer: C
Using the ICE table and Kc expression, after setting up the reaction we find that NH3 will reach 2 M at equilibrium.
Q6
Medium
In the equilibrium 2SO2(g) + O2(g) ⇌ 2SO3(g), if the concentration of SO3 is initially 0.5 M and the equilibrium constant Kc is 0.25, what is the initial concentration of SO2?
A.
0.5 M
B.
1 M
C.
2 M
D.
0.25 M
Show Answer & Explanation
Correct Answer: B
Rearranging the Kc expression for the reaction and substituting the known concentration of SO3 allows us to find the initial concentration of SO2.
Q7
Medium
Which of the following statements regarding the Law of Mass Action is correct?
A.
The equilibrium constant changes with concentration.
B.
Kc is always greater than Kp.
C.
Kc is temperature dependent.
D.
The reaction quotient is constant.
Show Answer & Explanation
Correct Answer: C
The Law of Mass Action states that Kc varies with temperature, while the reaction quotient Q changes with concentration.
Q8
Hard
In a saturated solution of AgCl, if the concentration of Ag+ is 1.0 × 10^-5 mol/L, what is the solubility product (Ksp) of AgCl?
A.
1 × 10^-10
B.
1 × 10^-20
C.
1 × 10^-15
D.
1 × 10^-30
Show Answer & Explanation
Correct Answer: A
For the dissociation AgCl ⇌ Ag+ + Cl-, Ksp = [Ag+][Cl-]. Given [Ag+] = 1 × 10^-5, [Cl-] = [Ag+] in a saturated solution, therefore Ksp = (1 × 10^-5)(1 × 10^-5) = 1 × 10^-10.
Q9
Hard
At equilibrium, the concentration of products is twice that of reactants in the reaction P ⇌ 2Q. What is the expression for the equilibrium constant Kc?
A.
Kc = [Q]^2/[P]
B.
Kc = [P]/[Q]^2
C.
Kc = 2[P]/[Q]
D.
Kc = [P]^2/[Q]
Show Answer & Explanation
Correct Answer: A
The equilibrium constant expression is derived from the coefficients of the balanced equation. Here, Kc = [Q]^2/[P] as per the stoichiometry of the equation.
Q10
Hard
The equilibrium constant Kc for the reaction 2A + B ⇌ C is 10. If the initial concentrations are [A] = 1 M, [B] = 2 M, and [C] = 0 M, what will be the concentration of C at equilibrium?
A.
0.5 M
B.
1 M
C.
2 M
D.
4 M
Show Answer & Explanation
Correct Answer: A
Set up the reaction table and apply the Kc expression. The reaction shifts toward products, and at equilibrium, the calculated concentration of C is 0.5 M.
Showing 10 of 1166 questions. Start a quiz to practice all questions with scoring and timer.
Practice All 1166 Questions →More Chemistry Chapters
Other JEE Subjects
Chemical and Ionic Equilibrium — JEE Chemistry Practice Questions Online
This page contains 1166 practice MCQs for the chapter Chemical and Ionic Equilibrium in JEE Chemistry. The questions are organized by difficulty — 273 easy, 487 medium, 406 hard — so you can choose the right level for your preparation.
Every question includes a detailed explanation to help you understand the concept, not just memorize answers. Take a timed quiz to simulate exam conditions, or practice at your own pace with no time limit. This chapter covers 9 topics, giving you comprehensive coverage of the entire chapter.