NEET Equilibrium — Set 11

Question 1

The ionic product of water at 298 K is $ 1.0 \times 10^{-14} $. What is the pH of pure water at this temperature?

Accepted Answer

$ K_w = [\ce{H+}][\ce{OH-}] = 1.0 \times 10^{-14} $. In pure water, $ [\ce{H+}] = [\ce{OH-}] = \sqrt{1.0 \times 10^{-14}} = 1.0 \times 10^{-7} $, so $ \text{pH} = -\log(1.0 \times 10^{-7}) = 7 $.

Question 2

Which species is a Lewis acid?

Accepted Answer

$ \ce{Fe^{3+}} $ can accept an electron pair due to its vacant orbitals.

Question 3

The solubility product of $ \ce{AgCl} $ is $ 1.8 \times 10^{-10} $. What is the solubility of $ \ce{AgCl} $ in pure water in mol/L?

Accepted Answer

$ K_{sp} = [\ce{Ag+}][\ce{Cl-}] = S^2 = 1.8 \times 10^{-10} $, so $ S = \sqrt{1.8 \times 10^{-10}} = 1.34 \times 10^{-5} \, \text{mol/L} $.

NEET Chemistry: Equilibrium — Practice Set 11

Q1. The ionic product of water at 298 K is \( 1.0 \times 10^{-14} \). What is the pH of pure water at this temperature?

Q2. Which species is a Lewis acid?

Q3. The solubility product of \( \ce{AgCl} \) is \( 1.8 \times 10^{-10} \). What is the solubility of \( \ce{AgCl} \) in pure water in mol/L?

Q4. A weak acid \( \ce{HY} \) has \( K_a = 1.6 \times 10^{-7} \). What is the pH of a 0.02 M solution of \( \ce{HY} \)?

Q5. What is the pH of a solution with \( [\ce{OH-}] = 5.0 \times 10^{-3} \, \text{M} \)?

Q6. For \( \ce{2A(g) + B(g) <=> 3C(g)} \), \( K_p = 2 \) at 700 K. If \( P_{\ce{A}} = 1 \, \text{atm} \), \( P_{\ce{B}} = 0.5 \, \text{atm} \) initially, what is \( P_{\ce{C}} \) at equilibrium?

Q7. The \( K_{sp} \) of \( \ce{CaF2} \) is \( 3.9 \times 10^{-11} \). What is \( [\ce{Ca^{2+}}] \) in a saturated solution with 0.02 M \( \ce{NaF} \)?

Q8. For \( \ce{2AB(g) <=> A2(g) + B2(g)} \), \( K_p = 0.25 \) at 600 K. If the initial pressure of \( \ce{AB} \) is 4 atm, what is \( P_{\ce{A2}} \) at equilibrium?

Q9. The \( K_{sp} \) of \( \ce{CaCO3} \) is \( 3.8 \times 10^{-9} \). What is \( [\ce{Ca^{2+}}] \) in a saturated solution with 0.02 M \( \ce{Na2CO3} \)?

Q10. For \( \ce{PbSO4(s) <=> Pb^{2+}(aq) + SO4^{2-}(aq)} \), \( K_{sp} = 1.6 \times 10^{-8} \). In a 0.02 M \( \ce{Na2SO4} \) solution, what is \( [\ce{Pb^{2+}}] \) at equilibrium?