JEE Advanced Equilibrium Important Questions

The Joint Entrance Examination is held annually by one of the 7 IIT’s under the supervision of joint admission board, JAB. It is used to assess students on several subjects and the knowledge that they've acquired, and this exam is the only  prerequisite to get into any of the IIT colleges. JEE Advanced has an eligibility criterion which students must satisfy to appear for the same. Candidates should rank amongst the top scorers in the IIT JEE main paper and satisfy the marks criteria broken down for the paper to appear for the JEE advanced exam. The Jay East advanced exam is considered to be one of the toughest exams. A few tips to make sure you were fully prepared on your journey of the advanced exam are :

• Solve as many mock papers as you can.

• Following your own method of study.

• Managing time efficiently. Making sure you don't miss out on any questions. 

• Having an organized and attainable timetable and making realistic goals.

Topics of Equilibrium

1. Law of Mass Action:

In JEE Advanced Chemistry's "Chemical Equilibrium," you'll explore the law of mass action, understanding the role of concentrations in chemical reactions. Discover the significance of $(K_c)$ and $(K_p)$ – equilibrium constants that show how reactions balance. (Q), the reaction quotient, helps predict whether a system is at equilibrium. This chapter unveils the secrets of chemical balance in a way that's approachable and relevant for competitive exams.

2. Le Chatelier's Principle 

In JEE Advanced Chemistry's "Chemical Equilibrium," Le Chatelier's Principle is your guide. It explains how a system at equilibrium responds to changes in concentration, temperature, and pressure. Imagine it like a balancing act – if you tip the scales by adjusting these factors, the system adjusts itself to restore balance. It's a key concept in understanding how reactions behave and a crucial topic for excelling in your JEE Advanced studies.

3. Solubility Product and its Applications:

The solubility product tells you how much of a solid can dissolve in a liquid. This concept is crucial for understanding the equilibrium in solutions, and in JEE Advanced, it's like unlocking the secrets behind dissolving substances and predicting their behaviour.

4. Common Ion Effect:

The common ion effect is your backstage pass to understanding how ions impact solubility. Imagine a crowded concert – when a familiar face (common ion) joins, it affects the equilibrium, making some ions less likely to join the "musical" solution. It's a vital concept for predicting how substances interact in solutions, and mastering it in JEE Advanced gives you an edge in unraveling the complexities of chemical equilibrium.

5. PH and Buffer Solutions and Hydrolysis of Salts:

Picture pH as the 'mood' of a solution, indicating whether it's acidic or basic. Acids and bases, according to Bronsted and Lewis, are the key players in this chemical performance. And when salts undergo hydrolysis, it's like observing how substances react with water. Understanding these concepts not only unlocks the language of chemical equilibrium but also lays the foundation for mastering advanced chemistry in JEE.

Important Formulas of Chemical Equilibrium

1. Law of Chemical Equilibrium:

• $aA+bB\rightleftharpoons cC + dD$

• $Rate forward\propto [A]^{a} [B]^{b}$

• $Rate reverse \propto [C]^{c} [D]^{d}$

• At equilibrium: Rate forward = Rate reverse

2. Equilibrium Constant (K):

• $K_{c} = \frac{[C]^{c} [D]^{d}}{[A]^{a} [B]^{b}}$

• Equilibrium constant in terms of partial pressure: $K_{p} = K_{c}(RT)^{\Delta n}$

Where R is the universal gas constant, T is the temperature in Kelvin, and $\Delta$ n is the change in moles of gaseous reactants and products)

3. Reaction Quotient (Q):

• $Q_{c} = \frac{[C]^{c} [D]^{d}}{[A]^{a} [B]^{b}}$ (in terms of concentration)

• $Q_{p} = \frac{P_{C}^{c}P_{D}^{d}}{P_{A}^{a}P_{B}^{b}}$ (in terms of partial pressure)

4. Gibbs Free Energy (\Delta G):

• $\Delta G = \Delta H - T\Delta S$

• $\Delta G^{\circ} =$ RTln(K)(at equilibrium, Q = K)

5. Ionic Product of Water (Kw):

• $K_{w} = [H^{+}] [OH^{-}]$

• At $25^{\circ}C, Kw = 1.0 \times 10^{-14} mol^{2}/L^{2}$

6. Weak Acid and Base Ionization (Ka) (Kb):

• $K_{a} = \frac{[H^{+}] [A^{-}]}{[HA]}$ (for a weak acid)

• $Kb = \frac{[OH^{-}] [B^{+}]}{[BOH]}$ (for weak base)

• $K_{w} = K_{a} \times K_{b}$ (for a weak acid and its conjugate base or a weak base and its conjugate acid)

7. Thermodynamics of Equilibrium:

• $\Delta G = \Delta H - T\Delta S$

8. Salt Hydrolysis (Kh):

• $Kh = \frac{[H^{+}][A^{-}]}{[HA]}$ (for a salt of a weak acid and strong base)

• $Kh = \frac{[OH^{-}][B^{+}]}{[BOH]}$ (for a salt of a strong acid and weak base)