Acid-Base Theories - Arrhenius Bronsted-Lowry Lewis and Salts Hydrolysis

Acid-Base Theories - Arrhenius Bronsted-Lowry Lewis and Salts Hydrolysis

For the equilibrium 2NO(g) N₂(g) + O₂(g) , if Kc = 4 and initial concentration of NO is 0.4 M with no products, what is

Let [N₂] = [O₂] = x , [NO] = 0.4 - 2x . Kc = ([N₂][O₂]/[NO]²) = (x²/(0.4 - 2x)²) = 4 . Taking square root, (x/0.4 - 2x) = 2 , x = 0.8 - 4x , 5x = 0.8 , x = 0.16 M .

Ref: NCERT Class 11 Chemistry > Chapter 6: Equilibrium > Topic: Acid-Base Theories - Arrhenius Bronsted-Lowry Lewis and Salts Hydrolysis

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Acid-Base Theories - Arrhenius Bronsted-Lowry Lewis and Salts Hydrolysis

For the reaction X(g) + Y(g) 2Z(g) , if Kc = 25 and at equilibrium [Z] = 0.5 M , what is [X] if [Y] = 0.02 M ?

Kc = ([Z]²/[X][Y]) = 25 . Substituting, 25 = ((0.5)²/[X](0.02)) = (0.25/0.02 [X]) , 25 × 0.02 [X] = 0.25 , 0.5 [X] = 0.25 , [X] = 0.5 M .

Ref: NCERT Class 11 Chemistry > Chapter 6: Equilibrium > Topic: Acid-Base Theories - Arrhenius Bronsted-Lowry Lewis and Salts Hydrolysis

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Acid-Base Theories - Arrhenius Bronsted-Lowry Lewis and Salts Hydrolysis

A weak acid HY ( Ka = 1.0 × 10⁻⁴ ) is mixed with its salt NaY in a 2:1 molar ratio. If [HY] = 0.2 M , what is the pH?

[Y-] = 0.1 M , pKa = 4 , pH = pKa + log ([Y-]/[HY]) = 4 + log (0.1/0.2) = 4 + log 0.5 = 4 - 0.301 = 3.7 .

Ref: NCERT Class 11 Chemistry > Chapter 6: Equilibrium > Topic: Acid-Base Theories - Arrhenius Bronsted-Lowry Lewis and Salts Hydrolysis

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Acid-Base Theories - Arrhenius Bronsted-Lowry Lewis and Salts Hydrolysis

In the equilibrium N₂(g) + O₂(g) 2NO(g) , adding an inert gas at constant pressure will shift the equilibrium in which d

Adding an inert gas at constant pressure decreases the partial pressures of reactants and products. Since Δ n = 0 (2 mol reactants = 2 mol products), there is no shift.

Ref: NCERT Class 11 Chemistry > Chapter 6: Equilibrium > Topic: Acid-Base Theories - Arrhenius Bronsted-Lowry Lewis and Salts Hydrolysis

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Acid-Base Theories - Arrhenius Bronsted-Lowry Lewis and Salts Hydrolysis

For A(g) + B(g) 2C(g) , Kp = 0.5 at 300 K. If the total pressure at equilibrium is 4 atm and PA = PB , what is PC ?

Let PA = PB = x , PC = 4 - 2x , Kp = ((PC)²/PA PB) = ((4 - 2x)²/x²) = 0.5 , 4 - 2x = x sqrt0.5 , x ≈ 1.37 , PC = 1.26 atm .

Ref: NCERT Class 11 Chemistry > Chapter 6: Equilibrium > Topic: Acid-Base Theories - Arrhenius Bronsted-Lowry Lewis and Salts Hydrolysis

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Acid-Base Theories - Arrhenius Bronsted-Lowry Lewis and Salts Hydrolysis

A 0.01 M solution of KOH is fully dissociated. What is its pH?

For KOH , [OH-] = 0.01 M = 10⁻² , pOH = -log(10⁻²) = 2 , pH = 14 - 2 = 12 .

Ref: NCERT Class 11 Chemistry > Chapter 6: Equilibrium > Topic: Acid-Base Theories - Arrhenius Bronsted-Lowry Lewis and Salts Hydrolysis

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Acid-Base Theories - Arrhenius Bronsted-Lowry Lewis and Salts Hydrolysis

Which species is a Lewis base?

A Lewis base donates an electron pair. CN- has a lone pair and can donate it.

Ref: NCERT Class 11 Chemistry > Chapter 6: Equilibrium > Topic: Acid-Base Theories - Arrhenius Bronsted-Lowry Lewis and Salts Hydrolysis

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Acid-Base Theories - Arrhenius Bronsted-Lowry Lewis and Salts Hydrolysis

What is the conjugate base of HSO₄- ?

HSO₄- loses a proton ( H+ ) to form SO₄²⁻ , its conjugate base.

Ref: NCERT Class 11 Chemistry > Chapter 6: Equilibrium > Topic: Acid-Base Theories - Arrhenius Bronsted-Lowry Lewis and Salts Hydrolysis

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Acid-Base Theories - Arrhenius Bronsted-Lowry Lewis and Salts Hydrolysis

For the equilibrium CO(g) + H₂O(g) CO₂(g) + H₂(g) , if the initial concentrations of CO and H₂O are 0.2 M each and at eq

At equilibrium, [CO] = [H₂O] = 0.2 - 0.08 = 0.12 M , [CO₂] = [H₂] = 0.08 M . Thus, Kc = ([CO₂][H₂]/[CO][H₂O]) = ((0.08)²/(0.12)²) = (0.0064/0.0144) ≈ 0.444 .

Ref: NCERT Class 11 Chemistry > Chapter 6: Equilibrium > Topic: Acid-Base Theories - Arrhenius Bronsted-Lowry Lewis and Salts Hydrolysis

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Acid-Base Theories - Arrhenius Bronsted-Lowry Lewis and Salts Hydrolysis

For 2A(g) B(g) + C(g) , Kc = 0.04 at 300 K. If 0.8 mol A is in a 2 L vessel, what is [B] at equilibrium?

Initial: [A] = 0.4 M , [B] = [C] = 0 . Let x = [B] = [C] , [A] = 0.4 - 2x . Kc = ([B][C]/[A]²) = (x²/(0.4 - 2x)²) = 0.04 , (x/0.4 - 2x) = 0.2 , x = 0.08 - 0.4x , x ≈ 0.057 M .

Ref: NCERT Class 11 Chemistry > Chapter 6: Equilibrium > Topic: Acid-Base Theories - Arrhenius Bronsted-Lowry Lewis and Salts Hydrolysis

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Acid-Base Theories - Arrhenius Bronsted-Lowry Lewis and Salts Hydrolysis

A weak acid HX has Ka = 2.5 × 10⁻⁶ . What is the pH of a solution made by mixing 0.1 M HX and 0.05 M NaX ?

Using Henderson-Hasselbalch: pH = pKa + log ([X-]/[HX]) , pKa = -log(2.5 × 10⁻⁶) ≈ 5.6 , ([X-]/[HX]) = (0.05/0.1) = 0.5 , pH = 5.6 + log 0.5 = 5.6 - 0.301 = 5.3 .

Ref: NCERT Class 11 Chemistry > Chapter 6: Equilibrium > Topic: Acid-Base Theories - Arrhenius Bronsted-Lowry Lewis and Salts Hydrolysis

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Acid-Base Theories - Arrhenius Bronsted-Lowry Lewis and Salts Hydrolysis

For XY(s) X+(aq) + Y-(aq) , if Ksp = 9.0 × 10⁻⁶ , what is [X+] in mol/L?

Ksp = [X+][Y-] = S² = 9.0 × 10⁻⁶ , S = sqrt9.0 × 10⁻⁶ = 3.0 × 10⁻³ , so [X+] = 3.0 × 10⁻³ M .

Ref: NCERT Class 11 Chemistry > Chapter 6: Equilibrium > Topic: Acid-Base Theories - Arrhenius Bronsted-Lowry Lewis and Salts Hydrolysis

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