NEET Chemistry Solutions Class 12 Questions

Calculate molarity of 63% w/w HNO₃ solution if density is 1.4 g/mL.

Which of the following aqueous solutions should have the highest boiling point?

The molar concentration of Cl⁻ ions in a solution obtained by mixing 300 mL of 0.3 M NaCl and 200 mL of 0.4 M BaCl₂ is

2.82 g of glucose is dissolved in 30 g of water. The mole fraction of glucose in the solution is

1 M, 2.5 litre NaOH solution is mixed with another 0.5 M, 3 litre NaOH solution. Then find out the molarity of resultant solution

The Henry's law constant for O₂ dissolved in water is 4.34 × 10⁴ atm at certain temperature. If the partial pressure of O₂ in a gas mixture that is in equilibrium with water is 0.434 atm, what is the mole fraction of O₂ in the solution?

Vapour pressure of benzene at 30°C is 121.8 mm. When 15 g of a non volatile solute is dissolved in 250 g of benzene, its vapour pressure decreased to 120.2 mm. The molecular weight of the solute (Mo. wt. of solvent = 78)

The mixture which shows positive deviation from Raoult's law is

Arrange the following aqueous solutions in the order of their increasing boiling points. (i) 10⁻⁴ M NaCl (ii) 10⁻⁴ M Urea (iii) 10⁻³ M MgCl₂ (iv) 10⁻² M NaCl

The elevation in boiling point of a solution of 9.43 g of MgCl₂ in 1 kg of water is (Kb = 0.52 K kg mol⁻¹, Molar mass of MgCl₂ = 94.3 g mol⁻¹)

Which of the following will have same value of van’t Hoff factor as that of K₄[Fe(CN)₆] ?

Match the column I with column II and mark the appropriate choice.

Which of the following will produce a buffer solution when mixed in equal volumes?

The mixture that forms maximum boiling azeotrope is

5 mL of 1 N HCl, 20 mL of N/2 H₂SO₄ and 30 mL of N/3 HNO₃ are mixed together and volume made to one litre. The normality of the resulting solution is

Which of the following pairs constitutes a buffer?

What will be the mole fraction of ethanol in a sample of spirit containing 85% ethanol by mass?

H₂S is a toxic gas used in qualitative analysis. If solubility of H₂S in water at STP is 0.195 m, what is the value of Kₕ?

Osmotic pressure of a solution containing 2g dissolved protein per 300 cm³ of solution is 20 mm of Hg at 27°C. The molecular mass of protein is :

If the concentration of glucose (C₆H₁₂O₆) in blood is 0.9 g L⁻¹, what will be the molarity of glucose in blood?

45 g of ethylene glycol (C₂H₆O₂) is mixed with 600 g of water. The freezing point of the solution is (Kf for water is 1.86 K kg mol⁻¹)

We have three aqueous solutions of NaCl labelled as 'A', 'B' and 'C' with concentrations 0.1 M, 0.01 M and 0.001 M, respectively. The value of van't Hoff factor for these solutions will be in the order

What are the conditions for an ideal solution which obeys Raoult's law over the entire range of concentration?

For 1 molal aqueous solution of the following compounds, which one will show the highest freezing point?

Identify the correct statements: (A) The molality of 2.5 g of ethanoic acid (Molar mass: 60 g mol⁻¹) in 75 g of benzene solution is 0.556 m. (B) The molarity of a solution containing 5 g of NaOH (molar mass: 40 g mol⁻¹) in 450 mL of solution is 0.278 M at 298 K. (C) Aquatic species are more comfortable in cold water. (D) The solubility of gas increases with decrease in pressure. (E) For a binary mixture of A and B, the number of moles of A and B are nₐ and nᵦ respectively. The mole fraction of B will be xᵦ = nᵦ / (nₐ + nᵦ). Choose the correct answer from the options given below:

Mixture of chloroform and acetone forms a solution with negative deviation from Raoult’s law due to:

Which of the following aqueous solution will exhibit highest boiling point?

5 moles of liquid X and 10 moles of liquid Y make a solution having a vapour pressure of 70 torr. The vapour pressures of pure X and Y are 63 torr and 78 torr respectively. Which of the following is true regarding the described solution?

The Henry’s law constant (KH) values of three gases (A, B, C) in water are 145, 2×10⁻⁵ and 35 kbar, respectively. The solubility of these gases in water follow the order:

The plot of osmotic pressure (Π) vs concentration (mol L⁻¹) for a solution gives a straight line with slope 25.73 L bar mol⁻¹. The temperature at which the osmotic pressure measurement is done is: (Use R = 0.083 L bar mol⁻¹ K⁻¹)

Given below are two statements: one is labelled as Assertion A and the other is labelled as Reason R: Assertion A: Helium is used to dilute oxygen in diving apparatus. Reasons R: Helium has high solubility in O2. In the light of the above statements, choose the correct answer from the options given below:

Which one is NOT correct mathematical equation for Dalton’s Law of partial pressure? Here p = total pressure of gaseous mixture

In one molal solution that contains 0.5 mole of a solute, there is

The following solutions were prepared by dissolving 10 g of glucose (C₆H₁₂O₆) in 250 ml of water (P₁), 10 g of urea (CH₄N₂O) in 250 ml of water (P₂) and 10 g of sucrose (C₁₂H₂₂O₁₁) in 250 ml of water (P₃). The right option for the decreasing order of osmotic pressure of these solutions is:

The correct option for the value of vapour pressure of a solution at 45°C with benzene to octane in molar ratio 3 : 2 is: [At 45°C vapour pressure of benzene is 280 mm Hg and that of octane is 420 mm Hg. Assume Ideal gas]

The mixture which shows positive deviation from Raoult’s law is :

The freezing point depression constant (Kf) of benzene is 5.12 K kg mol⁻¹. The freezing point depression for the solution of molality 0.078 m containing a non-electrolyte solute in benzene is (rounded off upto two decimal places) :

An alkene on ozonolysis gives methanal as one of the product. Its structure is:

For an ideal solution, the CORRECT option is ______.

The mixture that forms maximum boiling azeotrope is ______.

Which of the following is dependent on temperature?

If molarity of the dilute solutions is doubled, the value of molal depression constant (Kf) will be:

Which of the following statements about the composition of the vapour over an ideal 1 : 1 molar mixture of benzene and toluene is CORRECT? Assume that the temperature is constant at 25°C. (Given: Vapour pressure data at 25 °C, benzene = 12.8 kPa, toluene = 3.85 kPa)

At 100 °C, the vapour pressure of a solution of 6.5 g of a solute in 100 g water is 732 mm. If Kb = 0.52, the boiling point of this solution will be ______.

Which one of the following electrolytes has the same value of van't Hoff's factor (i) as that of Al₂(SO₄)₃ (if all are 100% ionised)?

Which one is NOT equal to zero for an ideal solution?

The boiling point of 0.2 mol kg⁻¹ solution of X in water is greater than equimolal solution of Y in water. Which one of the following statements is TRUE in this case?

Of the following 0.10 m aqueous solutions, which one will exhibit the largest freezing point depression?

Which condition is not satisfied by an ideal solution?