NEET Equilibrium — Set 17

Question 1

The solubility of $ \ce{Ag2CrO4} $ is $ 1.3 \times 10^{-4} \, \text{M} $. What is its $ K_{sp} $?

Accepted Answer

For $ \ce{Ag2CrO4 <=> 2Ag+ + CrO4^{2-}} $, $ [\ce{Ag+}] = 2S = 2.6 \times 10^{-4} $, $ [\ce{CrO4^{2-}}] = S = 1.3 \times 10^{-4} $. $ K_{sp} = (2.6 \times 10^{-4})^2 (1.3 \times 10^{-4}) = 8.79 \times 10^{-12} $.

Question 2

The $ K_{sp} $ of $ \ce{PbCl2} $ is $ 1.6 \times 10^{-5} $. What is its solubility in pure water in mol/L?

Accepted Answer

For $ \ce{PbCl2 <=> Pb^{2+} + 2Cl^-} $, $ K_{sp} = [\ce{Pb^{2+}}][\ce{Cl^-}]^2 = S (2S)^2 = 4S^3 = 1.6 \times 10^{-5} $. Solving, $ S^3 = 4 \times 10^{-6} $, $ S = (4 \times 10^{-6})^{1/3} \approx 1.6 \times 10^{-2} $.

Question 3

What is the conjugate base of $ \ce{HSO4-} $?

Accepted Answer

$ \ce{HSO4-} $ loses a proton ($ \ce{H+} $) to form $ \ce{SO4^{2-}} $, its conjugate base.

NEET Chemistry: Equilibrium — Practice Set 17

Q1. The solubility of \( \ce{Ag2CrO4} \) is \( 1.3 \times 10^{-4} \, \text{M} \). What is its \( K_{sp} \)?

Q2. The \( K_{sp} \) of \( \ce{PbCl2} \) is \( 1.6 \times 10^{-5} \). What is its solubility in pure water in mol/L?

Q3. What is the conjugate base of \( \ce{HSO4-} \)?

Q4. For \( \ce{X2(g) <=> 2X(g)} \), \( K_c = 0.25 \) at 500 K. If 0.4 mol \( \ce{X2} \) is in a 2 L vessel, what is the degree of dissociation at equilibrium?

Q5. A 0.01 M solution of \( \ce{KOH} \) is fully dissociated. What is its pH?

Q6. What is the effect of adding an inert gas at constant volume to the equilibrium \( \ce{2A(g) <=> B(g) + C(g)} \)?

Q7. The \( K_{sp} \) of \( \ce{AgBr} \) is \( 5.0 \times 10^{-13} \). What is \( [\ce{Ag+}] \) in a saturated solution with 0.05 M \( \ce{NaBr} \)?

Q8. Which species is a Lewis base?

Q9. The \( K_a \) of \( \ce{HSO4-} \) is \( 1.2 \times 10^{-2} \). What is the \( K_b \) of \( \ce{SO4^{2-}} \) at 298 K?

Q10. For \( \ce{CO2(g) <=> CO2(aq)} \), the equilibrium is governed by which law?