Download App

Solutions Chemistry - Solutions

Rajasthan Board (RBSE) - STD 12 Science - Chemistry (Rajasthan - English Medium). 403 questions in this chapter.

Question types

Solutions question types

403 questions across 8 question groups — pick any mix to generate a Chemistry paper with step-by-step answer keys.

403
Questions
8
Question groups
5
Question types
Sample Questions

Solutions questions

One sample from each question group in this chapter. Select any group above to see the full set with answer keys.

Q 1M.C.Q (1 Marks)1 Mark
Which of the following statements is false?
  • ✓
    Two different solutions of sucrose of the same molality prepared in different solvents will have the same depression in the freezing point.
  • B
    The osmotic pressure of a solution is given by the equation  π = CRT  (where C is the molarity of the solution)
  • C
    Decreasing order of osmotic pressure for 0.01M aqueous solutions of barium chloride, potassium chloride, acetic acid and sucrose is  $\ce{BaCl2 > KCl > CH3COOH > Sucrose}$
     
  • D
    According to Raoult’s law the vapour pressure exerted by a volatile component of a solution is directly proportional to its mole fraction in the solution

Answer: A.

View full solution →
Q 3M.C.Q (1 Marks)1 Mark
Two beakers of capacity 500mL were taken. One of these beakers, labelled as “A”, was filled with 400mL water whereas the beaker labelled “B” was filled with 400mL of 2M solution of NaCl. At the same temperature both the beakers were placed in closed containers of same material and same capacity as shown in. At a given temperature, which of the following statement is correct about the vapour pressure of pure water and that of NaCl solution.
View full solution →
Q 6Assertion (A) & Reason (B) MCQ1 Mark
In these questions, a statement of assertion followed by a statement of reason is given. Choose the correct answer out of the following choices.
  1. Assertion and reason both are correct statements and reason is correct explanation for assertion.
  2. Assertion and reason both are correct statements but reason is not correct explanation for assertion.
  3. Assertion is correct statement but reason is wrong statement.
  4. Assertion is wrong statement but reason is correct statement.
Assertion: Osmotic pressure is a colligative property.
Reason: Osmotic pressure depends only on the number of particles dissolved in solution.
View full solution →
Q 7Assertion (A) & Reason (B) MCQ1 Mark
In these questions, a statement of assertion followed by a statement of reason is given.
Choose the correct answer out of the following choices.
Assertion: One molal aqueous solution of urea contains $60g$ of urea in $1 \ kg$ of water.
Reason: Solution containing one mole of solute in $1000g$ solvent is called one molal solution.
  • ✓
    Assertion and reason both are correct statements and reason is correct explanation for assertion.
  • B
    Assertion and reason both are correct statements but reason is not correct explanation for assertion.
  • C
    Assertion is correct statement but reason is wrong statement.
  • D
    Assertion is wrong statement but reason is correct statement.

Answer: A.

View full solution →
Q 8Assertion (A) & Reason (B) MCQ1 Mark
In these questions, a statement of assertion followed by a statement of reason is given. Choose the correct answer out of the following choices.
  1. Assertion and reason both are correct statements but the reason is the correct explanation for assertion.
  2. Assertion and reason both are correct statements but the reason is not a correct explanation for assertion.
  3. Assertion is a correct statement but the reason is a wrong statement.
  4. Assertion is a wrong statement but the reason is correct
Assertion: Molarity of a solution in liquid state changes with temperature.
Reason: The volume of a solution changes with change in temperature.
View full solution →
Q 9Assertion (A) & Reason (B) MCQ1 Mark
In these questions, a statement of assertion followed by a statement of reason is given. Choose the correct answer out of the following choices.
  1. Assertion and reason both are correct statements and reason is correct explanation for assertion.
  2. Assertion and reason both are correct statements but reason is not correct explanation for assertion.
  3. Assertion is correct statement but reason is wrong statement.
  4. Assertion is wrong statement but reason is correct statement.
Assertion: Sodium chloride used to clear snow on the roads.
Reason: Sodium chloride depresses the freezing point of water.
View full solution →
Q 10Assertion (A) & Reason (B) MCQ1 Mark
In these questions, a statement of assertion followed by a statement of reason is given. Choose the correct answer out of the following choices.
  1. Assertion and reason both are correct statements and reason is correct explanation for assertion.
  2. Assertion and reason both are correct statements but reason is not correct explanation for assertion.
  3. Assertion is correct statement but reason is wrong statement.
  4. Assertion is wrong statement but reason is correct statement.
Assertion: The boiling point of 200mL of 1M urea solution is less than that of 200mL of 2M glucose solution.
Reason: Elevation of boiling point is directly proportional to the number of species present in the solution.
View full solution →
Q 162 Marks Questions2 Marks
At absolute zero, an exothermic reaction is always spontaneous but at temperatures above absolute zero, we have to consider both enthalpy and entropy before we can predict spontaneity. Why?
View full solution →
Q 172 Marks Questions2 Marks
  1. Gas $(A)$ is more soluble in water than Gas $(B)$ at the same temperature. Which one of the two gases will have the higher value of $K_H ($Henry's constant$)$ and why?
  2. In non$-$ideal solution, what type of deviation shows the formation of maximum boiling azeotropes?
View full solution →
Q 182 Marks Questions2 Marks
  1. Why are aquatic species more comfortable in cold water than in warm water?
  2. What happens when we place the blood cell in saline water solution (hypertonic solution)? Give reason.
View full solution →
Q 202 Marks Questions2 Marks
Define the terms, ‘osmosis’ and ‘osmotic pressure’. What is the advantage of using osmotic pressure as compared to other colligative properties for the determination of molar masses of solutes in solutions?
View full solution →
Q 213 Marks Question3 Marks
  1. Urea forms an ideal solution in water. Determine the vapour pressure of anaqueous solution containing 10% by mass of urea at 40°C. (Vapour pressure of water at 40°C = 55.3 mm of Hg)
  2. Why is freezing point depression of 0.1 M sodium chloride solution nearly twice that of 0.1 M glucose solution?
View full solution →
Q 223 Marks Question3 Marks
Calculate the boiling point of solution when $4 g$ of $\ce{MgSO4}\ (M = 120 g\ mol^{-1})$ was dissolved in $100 g$ of water, assuming $\ce{MgSO4}$ undergoes complete ionization.
$(K_b$ for water $=0.52 K \ kg \ mol^{-1}).$
View full solution →
Q 233 Marks Question3 Marks
Vapour pressure of water at $20^oC$ is $17.5 \ mm \ Hg.$ Calculate the vapour pressure of water at $20^oC$ when $15 g$ of glucose $($Molar mass $=180 g \ mol^{-1})$ is dissolved in $150 g$ of water.
View full solution →
Q 243 Marks Question3 Marks
A solution prepared by dissolving 8.95mg of a gene fragment in 35.0mL. of water has an osmotic pressure of 0.335 torr at 25°C. Assuming that the gene fragment is a non-electrolyte, calculate its molar mass.
View full solution →
Q 253 Marks Question3 Marks
What mass of $\text{NaCl} ($molar mass $= 58.5\ g\ mol^{–1})$ must be dissolved in $65\ g$ of water to lower the freezing point by $7.50^\circ C$? The freezing point depression constant, $K_f,$ for water is $1.86\ K \ kg\  mol^{–1}.$ Assume van’t Hoff factor for $\text{NaCl}$ is $1.87.$
View full solution →
Q 26Case study (4 Marks)4 Marks
Read the passage given below and answer the following questions:
The solubility of gases increases with increase of pressure. William Henry made a systematic investigation of the solubility of a gas in a liquid. According to Henry's law "the mass of a gas dissolved per unit volume of the solvent at constant temperature is directly proportional to the pressure of the gas in equilibrium with the solution". Dalton during the same period also concluded independently that the solubility of a gas in a ti quid solution depends upon the partial pressure of the gas. If we use the mole fraction of gas in the solution as a measure of its solubility, then Henry's law can be modified as "the partial pressure of the gas in the vapour phase is directly proportional to the mole fraction of the gas in the solution"
The following questions are multiple choice questions. Choose the most appropriate answer:
  1. Henry's law constant for the solubility of methane in benzene at $298K$ is $4.27 \times 10^5\ mm\ Hg$. The solubility of methane in benzene at $298K$ under $760\ mm\ Hg$ is :
  1. $4.27 \times 10^{-5}$
  2. $1.78 \times 10^{-3}$
  3. $4.27 \times 10^{-3}$
  4. $1.78 \times 10^{-5}$
  1. The partial pressure of ethane over a saturated solution containing $6.56 \times 10^{-2}g$ of ethane is $I$ bar. If the solution contains $5.00 \times 10^{-2}g$ of ethane then what will be the partial pressure $($in bar$)$ of the gas?
  1. $0.762$
  2. $1.312$
  3. $3.81$
  4. $5.0$
  1. $K_H\ (K$ bar$)$ values for $\ce{Ar(g), CO2(g), HCHO(g)}$ and $\ce{CH4(g)}$ are $40.39, 1.67, 1.83 \times 10^{-5}$ and $0.413$ respectively. Arrange these gases in the order of their increasing solubility. Arrange these gases in the order of their increasing solubility.
  1. $\ce{HCHO < CH4 < CO2 < Ar}$
  2. $\ce{HCHO < CO2 < CH4 < Ar}$
  3. $\ce{Ar < CO2 < CH4 < HCHO}$
  4. $\ce{Ar < CH4 < CO2 < HCHO}$
  1. When a gas is bubbled through water at $298K,$ a very dilute solution of the gas is obtained. Henry's law constant for the gas at $298K$ is $150k$ bar. If the gas exerts a partial pressure of $2$ bar, the number of millimoles of the gas dissolved in $IL$ of water is :
  1. $0.55$
  2. $0.87$
  3. $0.37$
  4. $0.66$
  1. Which of the following statements is correct?
  1. $K_H$ increases with increase of temperature.
  2. $K_H$ decreases with increase of temperature.
  3. $K_H$ remains constant with increase of temperature.
  4. $K_H$ first increases then decreases, with increase of temperature.
View full solution →
Q 27Case study (4 Marks)4 Marks
Read the passage given below and answer the following questions:
The properties of the solutions which depend only on the number of solute particles but not on the nature of the solute are called colligative properties. Relative lowering in vapour pressure is also an example of colligative properties. For an experiment, sugar solution is prepared, for which lowering in vapour pressure was found to be 0.061 mm of Hg. (Vapour pressure of water at 20° C is 17.5 mm of Hg)
The following questions are multiple choice questions. Choose the most appropriate answer:
  1. Relative lowering of vapour pressure for the given solution is.
  1. 0.00348
  2. 0.061
  3. 0.122
  4. 1.75
  1. The vapour pressure (mm of Hg) of solution will be.
  1. 17.5
  2. 0.61
  3. 17.439
  4. 0.00348
  1. Mole fraction of sugar in the solution is.
  1. 0.00348
  2. 0.9965
  3. 0.061
  4. 1.75
  1. If weight of sugar taken is 5g in 108g of water, then molar mass of sugar will be.
  1. 358
  2. 120
  3. 240
  4. 400
  1. The vapour pressure (mm of Hg) of water at 293K when 25g of glucose is dissolved in 450g of water is.
  1. 17.2
  2. 17.4
  3. 17.120
  4. 17.02
View full solution →
Q 28Case study (4 Marks)4 Marks
Read the passage given below and answer the following questions: The phenomenon of the flow of solvent through a semipermeable membrane from pure solvent to the solution is called osmosis. Sometimes a pressure is applied to stop the process of osmosis, this is known as osmotic pressure. It is denoted by $\pi.$ Osmotic pressure is expressed as : $\pi=\text{CRT}$ Since, osmotic pressure depends upon the molar concentration of solution, therefore it is a colligative property. A statement of assertion followed by a statement of reason is given. Choose the correct answer out of the following choices.
  1. Assertion and reason both are correct statements and reason is correct explanation for assertion.
  2. Assertion and reason both are correct statements but reason is not correct explanation for assertion.
  3. Assertion is correct statement but reason is wrong statement.
  4. Assertion is wrong statement but reason is correct statement.
  1. Assertion: If red blood cells were removed from the body and placed in pure water, pressure inside the cells increases.
Reason: The concentration of salt content in the cells increases.
  1. Assertion: The osmotic pressure of a solution obtained by mixing 100mL of 3.4% solution of urea and 100mL of 1.6% solution of cane sugar at 293K is 7.46 bar.
Reason: The total osmotic pressure will be equal to the sum of partial osmotic pressures.
  1. Assertion: When a solution is separated from the pure solvent by a semipermeable membrane, the solvent molecules pass through it from pure solvent side to the solution side.
Reason: Diffusion of solvent occurs from a region of high concentration to a region of low concentration solution.
  1. Assertion: Two solutions having same osmotic pressure at a given temperature are called isotonic solutions.
Reason: Osmotic pressure is not a colligative property.
  1. Assertion: The preservation of meat by salting and fruits by adding sugar protects against bacterial action.
Reason: A bacterium on salted meat or candid fruit loses water due to osmosis shrivels and ultimately dies.
View full solution →
Q 29Case study (4 Marks)4 Marks
Read the passage given below and answer the following questions: If some solute is added to a solvent, the boiling point of solution increases. This is known as elevation in baiting point. $\Delta\text{T}_\text{b}=\text{K}_\text{b}\text{m}$ where$, K_b =$ Molal elevation constant, $\Delta\text{T}_\text{b}\propto\text{m}$ Hence, it is a colligative property, Also, $\text{K}_\text{b}=\frac{\text{MRT}^2_\text{b}}{\Delta\text{Vap}\text{H}\times1000}$ where$, M =$ Molar mass of solvent, $\Delta\text{vap} H =$ Enthalpy of vaporisation, Molar mass can also be calculated using elevation in boiling point. $\text{M}_\text{B}=\frac{\text{K}_\text{B}\times\text{W}_\text{B}\times1000}{\Delta\text{T}_\text{b}\times\text{W}_\text{A}}$
A statement of assertion followed by a statement of reason is given.
Choose the correct answer out of the following choices.
  1. Assertion and reason both are correct statements and reason is correct explanation for assertion.
  2. Assertion and reason both are correct statements but reason is not correct explanation for assertion.
  3. Assertion is correct statement but reason is wrong statement.
  4. Assertion is wrong statement but reason is correct statement.
  1. Assertion : In a pressure cooker, the water is brought to boil. The cooker is then removed from the stove. Now on removing the lid of pressure cooker, the water starts boiling again.
Reason : The impurities in water bring down its boiling point.
  1. Assertion : On dissolving $3.24g$ of sulphur in $40g$ of benzene, boiling point of solution get higher than that of benzene by $0.081K,$ then the formula of sulphur is $S_8.\ (K_b$ for benzene $= 2.53K \ kg\ mol^{-1})$
Reason : Molecular mass of sulphur comes out to be $253.$​​​​​​​
  1. Assertion : When sugar is added to water, boiling point of water increases.
Reason: When a non$-$volatile solute is added to a solvent, elevation in boiling point is observed.
  1. Assertion : Cooking time in pressure cookers is reduced.
Reason: Boiling point inside the pressure cooker in raised.
  1. Assertion : Elevation in boiling point of two isotonic solutions is same.
Reason : Boiling point depends upon the concentration of the solute.
View full solution →
Q 30Case study (4 Marks)4 Marks
Read the passage given below and answer the following questions
Few colligative properties are:
  1. Relative lowering of vapour pressure: depends only on molar concentration of solute $($mole fraction$)$ and independent of its nature.
  2. Depression in freezing point: it is proportional to the molal concentration of solution.
  3. Elevation of boiling point: it is proportional to the molal concentration of solute.
  4. Osmotic pressure: it is proportional to the molar concentration of solute
A solution of glucose is prepared with $0.052 g$ at glucose in $80.2 g$ of water.$(KJ = 1.86K \ \text{kg \ mol}^{-1}$ and $K_b = 5.2K \ \text{kg \ mol}^{-1})$
The following questions are multiple choice questions. Choose the most appropriate answer:
  1. Molality of the given solution is.
  1. $0.0052m$
  2. $0.0036m$
  3. $0.0006m$
  4. $1.29m$
  1. Boiling point for the solution will be.
  1. $373.05K$
  2. $373.15K$
  3. $373.02K$
  4. $373.02K$
  1. The depression in freezing point of solution will be.
  1. $0.0187K$
  2. $0.035K$
  3. $0.082K$
  4. $0.067K$
  1. Mole fraction of glucose in the given solution is.
  1. $6.28 \times 10^{-5}$
  2. $6.28 \times 10^{-4}$
  3. $0.00625$
  4. $0.00028$
  1. If same amount of sucrose $\ce{(C_{12} H_{22} O_{11})}$ is taken instead of glucose, then.
  1. Elevation in boiling point will be higher.
  2. Depression in freezing point will be higher.
  3. Depression in freezing point will be lower.
  4. Both $(a)$ and $(b).$
View full solution →
Q 315 Marks Questions5 Marks
  1. What type of deviation is shown by a mixture of ethanol and acetone? Give reason.
  2. A solution of glucose $($molar mass $= 180\ g\ mol^{–1})$ in water is labelled as $10\% ($by mass$).$ What would be the molality and molarity of the solution?
$($Density of solution $= 1.2\ g\ mL^{–1}).$
View full solution →
Q 325 Marks Questions5 Marks
  1. A $10\%$ solution $($by mass$)$ of sucrose in water has a freezing point of $269.15 K$. Calculate the freezing point of $10\%$ glucose in water if the freezing point of pure water is $273.15 K.$ Given:
$($Molar mass of sucrose $= 342\ g\ mol^{-1})$
$($Molar mass of glucose $= 180\ g\ mol^{-1})$
  1. Define the following terms:
  1. Molality $(m)$
  2. Abnormal molar mass
View full solution →
Q 335 Marks Questions5 Marks
  1. $30\ g$ of urea $(M = 60\ g\ mol^{-1})$ is dissolved in $846\ g$ of water. Calculate the vapour pressure of water for this solution if vapour pressure of pure water at $298\ K$ is $23.8\ mm\ Hg.$
  2. Write two differences between ideal solutions and non-ideal solutions.
View full solution →
Q 345 Marks Questions5 Marks
  1. Define the following terms:
  1. Molarity.
  2. Molal elevation constant$(Kb).$
  1. A solution containing $15\ g$ urea $($molar mass $= 60\ g\ mol^{–1})$ per litre of solution in water has the same osmotic pressure $($isotonic$)$ as a solution of glucose $($molar mass $= 180\ g\ mol^{–1})$ in water. Calculate the mass of glucose present in one litre of its solution.
View full solution →
Q 355 Marks Questions5 Marks
  1. State Raoult’s law for a solution containing volatile components.
 How does Raoult’s law become a special case of Henry’s law?
  1. $1.00\ g$ of a non-electrolyte solute dissolved in $50\ g$ of benzene lowered the freezing point of benzene by $0.40 K.$ Find the molar mass of the solute. $(K_f$ for benzene $= 5.12 \ kg\ mol^{-1}).$
View full solution →
Browse all question groups ↑

Generate a Solutions paper free

Pick question groups from the list above, set marks and difficulty, and export a branded PDF with step-by-step answer keys. First 3 chapters free — no signup.

Download App
Generate Paper FreeAll Chemistry chapters