A solution has pH = 4. What is the concentration of H⁺ ions?

The correct answer is A: 1 × 10⁻⁴ M. pH = -log[H⁺], so [H⁺] = 10⁻ᵖᴴ = 10⁻⁴ = 1 × 10⁻⁴ M.

A solution contains 342 g of sucrose (M = 342 g/mol) dissolved in 1000 mL of water. The molarity of the solution is:

The correct answer is A: 1.0 M. Moles of sucrose = 342/342 = 1 mol. Molarity = 1 mol/1 L = 1.0 M

A solution containing 0.5 mol of a non-volatile, non-electrolyte solute in 1 L of water shows a freezing point of -0.93°C. What is the cryoscopic constant (Kf) of water? (Tf of pure water = 0°C)

The correct answer is B: 1.86 K·kg/mol. ΔTf = Kf × m, where m = molality = 0.5 mol/1 kg (approximately). ΔTf = 0.93°C, so Kf = 0.93/0.5 = 1.86 K·kg/mol.

Which colligative property depends on the nature of solute as well as its concentration?

The correct answer is A: Osmotic pressure. Osmotic pressure depends on solute nature because it involves membrane interactions. Other colligative properties depend only on number of solute particles

At 273 K, 1 mole of an ideal gas occupies 22.4 L. What will be its volume at 546 K and same pressure?

The correct answer is B: 44.8 L. Using Charles's Law: V₁/T₁ = V₂/T₂ → V₂ = V₁ × (T₂/T₁) = 22.4 × (546/273) = 44.8 L

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NEET Chemistry

Chemistry questions for NEET UG — Physical, Organic, Inorganic Chemistry.

31 Q 1 Topics Take Mock Test

Difficulty: All Easy Medium Hard 31–31 of 31

Topics in NEET Chemistry

All Physical Chemistry 88

Q.31 Easy Physical Chemistry

Which of the following is the correct expression for the equilibrium constant (Kc) for the reaction: N₂(g) + 3H₂(g) ⇌ 2NH₃(g)?

A Kc = [NH₃]²/([N₂][H₂]³)

B Kc = [N₂][H₂]³/[NH₃]²

C Kc = [NH₃]/([N₂][H₂])

D Kc = [N₂] + [H₂]/[NH₃]

Correct Answer: A. Kc = [NH₃]²/([N₂][H₂]³)

EXPLANATION

The equilibrium constant expression follows the law of mass action where Kc = [products]^coefficients/[reactants]^coefficients. For this reaction, Kc = [NH₃]²/([N₂][H₂]³).

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