jee main chemistry important questions | Solutions jee main questions FREE

Q 1 :

If a substance ‘A’ dissolves in solution of a mixture of ‘B’ and ‘C’ with their respective number of moles as $n_{A}, n_{B}$ and $n_{C}$ . Mole fraction of C in the solution is [2024]

$\frac{n_{C}}{n_{A} \times n_{B} \times n_{C}}$
$\frac{n_{C}}{n_{A} + n_{B} + n_{C}}$
$\frac{n_{C}}{n_{A} - n_{B} - n_{C}}$
$\frac{n_{B}}{n_{A} + n_{B}}$

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(2)

Mole fraction of any substance = $\frac{Moles of that substance}{Total number of moles}$

Q 2 :

The Molarity (M) of an aqueous solution containing 5.85 g of NaCl in 500 mL water is:
(Given: Molar Mass Na : 23 and Cl : 35.5 g ${mol}^{- 1}$ ) [2024]

0.2
20
4
2

1

2

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4

(1)

Assuming volume of solution same as volume of water,

$V_{solution} = 500 mL = 0.5 L$

$n_{solute} = \frac{W_{solute}}{M_{solute}} = \frac{5.85 g}{58.5 {g mol}^{- 1}} = 0.1 mol$

$M = \frac{n_{solute}}{V_{solution} (in L)} = \frac{0.1 mol}{0.5 L} = 0.2 M$

Q 3 :

The density of ‘x’ M solution (‘x’ molar) of NaOH is 1.12 g ${mL}^{- 1}$ , while in molality, the concentration of the solution is 3 m (3 molal). Then x is (Given: Molar mass of NaOH is 40 g/mol) [2024]

3.8
3.5
2.8
3.0

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(4)

$molality = \frac{1000 \times Molarity}{1000 \times density - Molarity \times M_{solute}}$

$3 = \frac{1000 x}{1000 \times 1.12 - x \times 40}$

$3360 - 120 x = 1000 x$

$1120 x = 3360$

$x = 3$

Q 4 :

Molality (m) of 3 M aqueous solution of NaCl is:
(Given: Density of solution = 1.25 g ${mL}^{- 1}$ , Molar mass in g ${mol}^{- 1}$ : Na - 23, Cl - 35.5) [2024]

2.90 m
2.79 m
1.90 m
3.85 m

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(2)

3M aqueous NaCl means:

3 mol NaCl in 1000 mL solution

$3 \times 58.5 g = 175.5 g NaCl in 1.25 {g mL}^{- 1} \times 1000 mL - 1250 g solution$

$3 mol NaCl in (1250 - 175.5) g = 1074.5 g = 1.074 kg solution$

$m = \frac{n_{solute}}{V_{solvent} (in kg)} = \frac{3}{1.0745} m = 2.79 m$

Q 5 :

Volume of 3 M NaOH (formula weight 40 g ${mol}^{- 1}$ ) which can be prepared from 84 g of NaOH is ______ $\times 10^{- 1}$ ${dm}^{3}$ . [2024]

(7)

$Moles of NaOH (n_{NaOH}) = \frac{Given mass}{Molar mass} = \frac{84 g}{40 {g mol}^{- 1}} = 2.1 mol$

$Molarity of NaOH \times Volume of NaOH in L = Moles of NaOH$

$3 {mol L}^{- 1} \times Volume of NaOH in L = 2.1 mol$

$Volume of NaOH in L = 0.7 L or 0.7 {dm}^{3} = 7 \times 10^{- 1} {dm}^{3}$

Q 6 :

A solution of $H_{2} {SO}_{4}$ is 31.4% $H_{2} {SO}_{4}$ by mass and has a density of 1.25 g/mL. The molarity of the $H_{2} {SO}_{4}$ solution is _____ M (nearest integer)

[Given molar mass of $H_{2} {SO}_{4}$ = 98 g ${mol}^{- 1}$ ] [2024]

(4)

$31.4 % H_{2} {SO}_{4} by mass means:$

$31.4 {gm H}_{2} {SO}_{4} in 100gm solution$

$\Rightarrow \frac{31.4}{98} mol = 0.32 {mol H}_{2} {SO}_{4} in \frac{100 g}{1.25 {g mL}^{- 1}}$

$= 80 mL solution$

$Molarity = \frac{n_{solute}}{V_{solution} (in mL)} \times 1000 = \frac{0.32}{80} \times 1000 M = 4 M$

Q 7 :

Molality of 0.8 M $H_{2} {SO}_{4}$ solution (density 1.06 g ${cm}^{- 3}$ ) is ______ $\times 10^{- 3}$ m. [2024]

(815)

$m = \frac{M \times 1000}{d \times 1000 - M \times M_{solute}} = \frac{0.8 \times 1000}{1.06 \times 1000 - 0.8 \times 98} m$

$= 815 \times 10^{- 3} m$

Q 8 :

The mass of sodium acetate ( ${CH}_{3} COONa$ ) required to prepare 250 mL of 0.35 M aqueous solution is _____ g.
(Molar mass of ${CH}_{3} COONa$ is 82.02 g ${mol}^{- 1}$ ) [2024]

(7)

$Volume of solution (V) = 250 mL = 0.25 L .$

${Moles of CH}_{3} COONa (n)$

$= Molarity \times volume = 0.35 \frac{mol}{L} \times 0.25 L = 0.0875 mol$

${Mass of CH}_{3} COONa$

$= n \times molar mass = 0.0875 mol \times 82.02 \frac{g}{mol} = 7.177 g$

Q 9 :

The molarity of 1 L orthophosphoric acid ( $H_{3} {PO}_{4}$ ) having 70% purity by weight (specific gravity 1.54 g ${cm}^{- 3}$ ) is ______ M.
(Molar mass of $H_{3} {PO}_{4}$ = 98 g ${mol}^{- 1}$ ) [2024]

(11)

$70% w/w H_{3} {PO}_{4} solution means:$

$70 g H_{3} {PO}_{4} in 100 g solution$

$\Rightarrow \frac{70}{98} mol H_{3} {PO}_{4} in \frac{100}{1.54} mL solution$

$M = \frac{n_{solute}}{V_{solution} (in mL)} \times 1000$

$M = \frac{70 / 98}{100 / 1.54} \times 1000 M = \frac{70 \times 1.54 \times 1000}{98 \times 100} M = 11 M$

Q 10 :

Molality of an aqueous solution of urea is 4.44 m. Mole fraction of urea in solution is $x \times 10^{- 3}$ . Value of $x$ is _____ (integer answer) [2024]

(74)

$m = \frac{x_{solute} \times 1000}{x_{solvent} \times M_{solvent}}$

$4.44 = \frac{x_{urea} \times 1000}{x_{water} \times 18}$

$\frac{x_{urea}}{x_{water}} = \frac{79.92}{1000}$

$x_{urea} = \frac{79.92}{79.92 + 1000} = 74 \times 10^{- 3}$

Q 11 :

A solution is prepared by adding 1 mole ethyl alcohol in 9 mole water. The mass percent of solute in the solution is ______ (Integer Answer)

(Given: Molar mass in g ${mol}^{- 1}$ Ethyl alcohol : 46, water : 18) [2024]

(22)

$W_{C_{2} H_{5} O H} = n_{C_{2} H_{5} O H} \times M_{C_{2} H_{5} O H} = 1 mol \times 46 {g mol}^{- 1} = 46 g$

$W_{H_{2} O} = n_{H_{2} O} \times M_{H_{2} O} = 9 mol \times 18 {g mol}^{- 1} = 162 g$

$Mass percent of solute = \frac{W_{solute}}{W_{solution}} \times 100$

$= \frac{W_{C_{2} H_{5} O H}}{W_{H_{2} O} + W_{C_{2} H_{5} O H}} \times 100$

$= \frac{46}{162 + 46} \times 100 = 22.11 % \approx 22 %$

Q 12 :

Molarity (M) of an aqueous solution containing $x$ g of anhyd. ${CuSO}_{4}$ in 500 mL solution at 32°C is $2 \times 10^{- 1}$ M. Its molality will be _____ $\times 10^{- 3}$ m. (nearest integer).

[Given density of the solution = 1.25 g/mL] [2024]

(164)

$W_{solution} = d_{solution} \times V_{solution} = 1.25 \frac{g}{mL} \times 500 mL = 625 g$

$n_{solute} = {Molarity}_{solution} \times V_{solution} = 2 \times 10^{- 1} M \times 0.5 L = 0.1 mol$

$W_{solute} = n_{solute} \times molar mass of solute = 0.1 mol \times 159.5 {gmol}^{- 1} = 15.95 g$

$W_{solvent} = W_{solution} - W_{solute} = 625 g - 15.95 g = 609.05 g$

$m = \frac{n_{solute} \times 1000}{W_{solvent} (in g)} = \frac{0.1 \times 1000}{609.05} m = 0.1642 m = 164 \times 10^{- 3} m$

Q 13 :

The quantity which changes with temperature is: [2024]

Molarity
Mass percentage
Molality
Mole fraction

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(1)

Q 14 :

‘x’ g of NaCl is added to water in a beaker with a lid. The temperature of the system is raised from 1°C to 25°C. Which out of the following plots, is best suited for the change in the molarity (M) of the solution with respect to temperature?

[Consider the solubility of NaCl remains unchanged over the temperature range] [2025]

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(2)

Density of water is maximum at 4°C. This is because from 0°C to 4°C, hydrogen bonds break and molecules come closer. After 4°C volume increases due to thermal expansion. Thus from 1°C to 4°C, volume of solution decreases and hence molarity increases. Heating the solution beyond 4°C increases its volume hence the molarity decreases.

Q 15 :

10 mL of 2 M NaOH solution is added to 20 mL of 1 M HCl solution kept in a beaker. Now, 10 mL of this mixture is poured into a volumetric flask of 100 mL containing 2 moles of HCl and made the volume upto the mark with distilled water. The solution in this flask is : [2025]

0.2 M NaCl solution
20 M HCl solution
10 M HCl solution
Neutral solution

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(2)

Final solution contains 2 mol HCl in 100 mL of solution (0.1 L solution). So concentration of final solution is $\frac{n_{HCl}}{V_{solution} (in L)} = \frac{2}{0.1} M = 20 M$

Q 16 :

20 mL of 2 M NaOH solution is added to 400 mL of 0.5 M NaOH solution. The final concentration of the solution is ______ $\times 10^{- 2}$ M. (Nearest integer) [2025]

(57)

$Final concentration = \frac{M_{1} V_{1} + M_{2} V_{2}}{V_{1} + V_{2}}$

$= \frac{2 \times 20 + 0.5 \times 400}{20 + 400} M$

$= \frac{240}{420} M = 0.571 M = 57.1 \times 10^{- 2} M$

Q 17 :

Fortification of food with iron is done using ${FeSO}_{4} . 7 H_{2} O$ . The mass in grams of the ${FeSO}_{4} . 7 H_{2} O$ required to achieve 12 ppm of iron in 150 kg of wheat is _____ (Nearest integer)

[Given: Molar mass of Fe, S and O respectively are 56, 32 and 16 g ${mol}^{- 1}$ ] [2025]

(9)

$ppm = \frac{w_{iron}}{w_{wheat}} \times 10^{6}$

$12 = \frac{w_{iron}}{150} \times 10^{6}$

$w_{iron} = \frac{12 \times 150}{10^{6}} kg = \frac{12 \times 150}{10^{6}} \times 1000 g = 1.8 g$

$Moles of iron = \frac{W_{iron}}{M_{iron}} = \frac{1.8}{56} mol$

${Moles of FeSO}_{4} . 7 H_{2} O = Moles of iron = \frac{1.8}{56} mol$

${Molar mass of FeSO}_{4} . 7 H_{2} O = 56 + 32 + 4 \times 16 + 7 \times 18 = 278 g/mol$

${Mass of FeSO}_{4} . 7 H_{2} O = {moles of FeSO}_{4} . 7 H_{2} O \times {molar mass of FeSO}_{4} . 7 H_{2} O$ $= \frac{1.8}{56} \times 278 g = 8.935 gm \approx 9 gm$

Q 18 :

Sea water, which can be considered as a 6 molar (6 M) solution of NaCl, has a density of 2 g ${mL}^{- 1}$ .

The concentration of dissolved oxygen ( $O_{2}$ ) in sea water is 5.8 ppm. Then the concentration of dissolved oxygen ( $O_{2}$ ) in sea water, is $x \times 10^{- 4}$ m.

x = _______. (Nearest integer)

Given: Molar mass of NaCl is 58.5 g ${mol}^{- 1}$

Molar mass of $O_{2}$ is 32 g ${mol}^{- 1}$ [2025]

(2)

$(i) 6M NaCl solution means 6 mol NaCl in 1000 mL solution$

$i.e. 6 mol NaCl in 1000 mL \times 2 {g mL}^{- 1} solution$

$i.e. 6 mol NaCl in 2000 g solution$

$i.e. 6 \times 58.5 g NaCl in 2000 g solution$

$i.e. 351 g NaCl in 2000 g water.$

${(ii) ppm of O}_{2} = \frac{W_{O_{2}}}{W_{solvent}} \times 10^{6}$

$5.8 = \frac{W_{O_{2}}}{2000} \times 10^{6}$

$W_{O_{2}} = \frac{5.8 \times 2000}{10^{6}} = 0.0116 g$

$(iii) Mass of solvent in 2000 g solution (W_{solvent})$

$= W_{solution} - W_{NaCl} - W_{O_{2}}$

$= 2000 - 351 - 0.0116 = 1648.9884 g$

$Molality of oxygen (m) = \frac{W_{O_{2}} \times 1000}{M_{O_{2}} \times W_{solvent}}$

$= \frac{0.0116 \times 1000}{32 \times 1648.9884} = 2.19 \times 10^{- 4}$

Q 19 :

What is the mass ratio of ethylene glycol ( $C_{2} H_{6} O_{2}$ , molar mass = 62 g/mol) required for making 500 g of 0.25 molal aqueous solution and 250 mL of 0.25 molal aqueous solution? [2023]

1 : 2
1 : 1
3 : 1
2 : 1

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(4)

$\frac{Millimoles of 1st case}{Millimoles of 2nd case} = \frac{500 \times 0.25}{250 \times 0.25} = \frac{2}{1} = 2 : 1$

Q 20 :

A solution is prepared by adding 2 g of “X” to 1 mole of water. Mass percent of “X” in the solution is [2023]

20%
5%
2%
10%

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(4)

$Mass % of A in solution = \frac{W_{A}}{S_{solution}} \times 100$

$= \frac{2}{20} \times 100 = 10 %$

Q 21 :

Given below are two statements: one is labelled as Assertion A and the other is labelled as Reason R

Assertion A: 3.1500 g of hydrated oxalic acid dissolved in water to make 250.0 mL solution will result in 0.1 M oxalic acid solution.

Reason R: Molar mass of hydrated oxalic acid is 126 g ${mol}^{- 1}$ .

In the light of the above statements, choose the correct answer from the options given below: [2023]

A is true but R is false
Both A and R are true and R is the correct explanation of A
A is false but R is true
Both A and R are true but R is not the correct explanation of A

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(2)

$Molarity (M) = \frac{wt}{M . wt} \times \frac{1000}{V (mL)}$

$= \frac{3.15}{126} \times \frac{1000}{250} = 0.1$

Reason is correct as it is used as a fact in the explanation of Assertion.

Q 22 :

The density of 3 M solution of NaCl is 1.0 g ${mL}^{- 1}$ . Molality of the solution is ______ $\times 10^{- 2}$ m. (Nearest Integer).

Given: Molar mass of Na and Cl is 23 and 35.5 g ${mol}^{- 1}$ respectively. [2023]

(364)

$Molality (m) = \frac{M \times 1000}{1000 \times d - M \times M_{solute}}$

$= (\frac{3 \times 1000}{1000 \times 1 - 3 \times 58.5})$

$= 3.6386 m$

$= 363.86 \times 10^{- 2} m = 364$

Q 23 :

A 300 mL bottle of soft drink has 0.2 M ${CO}_{2}$ dissolved in it. Assuming ${CO}_{2}$ behaves as an ideal gas, the volume of the dissolved ${CO}_{2}$ at STP is ______ mL. (Nearest Integer)

Given: At STP, molar volume of an ideal gas is 22.7 L ${mol}^{- 1}$ . [2023]

(1362)

${Number of moles of CO}_{2} = M \times V \times 10^{- 3}$

$= 0.2 \times 300 \times 10^{- 3} = 0.06 mole$

${Volume of CO}_{2} (at STP) = 0.06 \times 22.7$

$= 1.362 L = 1362 mL$

Q 24 :

20 mL of calcium hydroxide was consumed when it was reacted with 10 mL of unknown solution of $H_{2} {SO}_{4}$ . Also 20 mL standard solution of 0.5 M HCl containing 2 drops of phenolphthalein was titrated with calcium hydroxide, the mixture showed pink colour when burette displayed the value of 35.5 mL whereas the burette showed 25.5 mL initially.
The concentration of $H_{2} {SO}_{4}$ is ______ M. (Nearest integer) [2023]

(1)

(i) ${Ca(OH)}_{2} + 2 HCl \to {CaCl}_{2} + 2 H_{2} O$

Millimole $M_{1} \times 10 (2 \times M_{1}) 10$

Millimole of HCl = $(2 \times M_{1}) 10 = 0.5 \times 20$

$M_{{Ca(OH)}_{2}} of HCl = 0.5 M$

(ii) With $H_{2} {SO}_{4}$ ${⇒Ca(OH)}_{2} + H_{2} {SO}_{4} \to {CaSO}_{4} + 2 H_{2} O$

$0.5 \times 2 (M_{2} \times 10)$

$M_{2} \times 10 = 0.5 \times 20$

$M_{2} = 1$

${Molarity of H}_{2} {SO}_{4} = 1$

Q 25 :

The number of units, which are used to express concentration of solution from the following is ______. Mass percent, Mole fraction, Molarity, ppm, Molality [2023]

(5)

Mole fraction, molarity, molality, mass % and ppm describes the concentration of solution.

Q 26 :

A solution of sugar is obtained by mixing 200 g of its 25% solution and 500 g of its 40% solution (both by mass). The mass percentage of the resulting sugar solution is ______ (Nearest integer). [2023]

(36)

Total mass of sugar in mixture of 25% of 200 and 40% of 500 g

$Sugar in solution = 0.25 \times 200 + 0.40 \times 500$

$= 50 + 200 = 250 g$

$Total mass of solution = 200 + 500 = 700 g$

$Mass of sugar in solution = \frac{250}{700} \times 100 = 35.7 %$

$\approx 36 %$

Q 27 :

Assume a living cell with 0.9% $(ω / ω)$ of glucose solution (aqueous). This cell is immersed in another solution having equal mole fraction of glucose and water.

(Consider the data upto first decimal place only) The cell will : [2025]

shrink since solution is 0.5% $(ω / ω)$
shrink since solution is 0.45% $(ω / ω)$ as a result of association of glucose molecules (due to hydrogen bonding)
swell up since solution is 1% $(ω / ω)$
show no change in volume since solution is 0.9% $(ω / ω)$

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Topic Question Set

Q 1 :

If a substance ‘A’ dissolves in solution of a mixture of ‘B’ and ‘C’ with their respective number of moles as $n_{A}, n_{B}$ and $n_{C}$ . Mole fraction of C in the solution is [2024]

Q 2 :

The Molarity (M) of an aqueous solution containing 5.85 g of NaCl in 500 mL water is:
(Given: Molar Mass Na : 23 and Cl : 35.5 g ${mol}^{- 1}$ ) [2024]

Q 3 :

The density of ‘x’ M solution (‘x’ molar) of NaOH is 1.12 g ${mL}^{- 1}$ , while in molality, the concentration of the solution is 3 m (3 molal). Then x is (Given: Molar mass of NaOH is 40 g/mol) [2024]

Q 4 :

Molality (m) of 3 M aqueous solution of NaCl is:
(Given: Density of solution = 1.25 g ${mL}^{- 1}$ , Molar mass in g ${mol}^{- 1}$ : Na - 23, Cl - 35.5) [2024]

Q 5 :

Volume of 3 M NaOH (formula weight 40 g ${mol}^{- 1}$ ) which can be prepared from 84 g of NaOH is ______ $\times 10^{- 1}$ ${dm}^{3}$ . [2024]

Q 6 :

A solution of $H_{2} {SO}_{4}$ is 31.4% $H_{2} {SO}_{4}$ by mass and has a density of 1.25 g/mL. The molarity of the $H_{2} {SO}_{4}$ solution is _____ M (nearest integer)

[Given molar mass of $H_{2} {SO}_{4}$ = 98 g ${mol}^{- 1}$ ] [2024]

Q 7 :

Molality of 0.8 M $H_{2} {SO}_{4}$ solution (density 1.06 g ${cm}^{- 3}$ ) is ______ $\times 10^{- 3}$ m. [2024]

Q 8 :

The mass of sodium acetate ( ${CH}_{3} COONa$ ) required to prepare 250 mL of 0.35 M aqueous solution is _____ g.
(Molar mass of ${CH}_{3} COONa$ is 82.02 g ${mol}^{- 1}$ ) [2024]

Q 9 :

The molarity of 1 L orthophosphoric acid ( $H_{3} {PO}_{4}$ ) having 70% purity by weight (specific gravity 1.54 g ${cm}^{- 3}$ ) is ______ M.
(Molar mass of $H_{3} {PO}_{4}$ = 98 g ${mol}^{- 1}$ ) [2024]

Q 10 :

Molality of an aqueous solution of urea is 4.44 m. Mole fraction of urea in solution is $x \times 10^{- 3}$ . Value of $x$ is _____ (integer answer) [2024]

Q 11 :

A solution is prepared by adding 1 mole ethyl alcohol in 9 mole water. The mass percent of solute in the solution is ______ (Integer Answer)

(Given: Molar mass in g ${mol}^{- 1}$ Ethyl alcohol : 46, water : 18) [2024]

Q 12 :

Molarity (M) of an aqueous solution containing $x$ g of anhyd. ${CuSO}_{4}$ in 500 mL solution at 32°C is $2 \times 10^{- 1}$ M. Its molality will be _____ $\times 10^{- 3}$ m. (nearest integer).

[Given density of the solution = 1.25 g/mL] [2024]

Q 13 :

The quantity which changes with temperature is: [2024]

Q 15 :

10 mL of 2 M NaOH solution is added to 20 mL of 1 M HCl solution kept in a beaker. Now, 10 mL of this mixture is poured into a volumetric flask of 100 mL containing 2 moles of HCl and made the volume upto the mark with distilled water. The solution in this flask is : [2025]

Q 16 :

20 mL of 2 M NaOH solution is added to 400 mL of 0.5 M NaOH solution. The final concentration of the solution is ______ $\times 10^{- 2}$ M. (Nearest integer) [2025]

Q 19 :

What is the mass ratio of ethylene glycol ( $C_{2} H_{6} O_{2}$ , molar mass = 62 g/mol) required for making 500 g of 0.25 molal aqueous solution and 250 mL of 0.25 molal aqueous solution? [2023]

Q 20 :

A solution is prepared by adding 2 g of “X” to 1 mole of water. Mass percent of “X” in the solution is [2023]

Q 22 :

The density of 3 M solution of NaCl is 1.0 g ${mL}^{- 1}$ . Molality of the solution is ______ $\times 10^{- 2}$ m. (Nearest Integer).

Given: Molar mass of Na and Cl is 23 and 35.5 g ${mol}^{- 1}$ respectively. [2023]

Q 23 :

A 300 mL bottle of soft drink has 0.2 M ${CO}_{2}$ dissolved in it. Assuming ${CO}_{2}$ behaves as an ideal gas, the volume of the dissolved ${CO}_{2}$ at STP is ______ mL. (Nearest Integer)

Given: At STP, molar volume of an ideal gas is 22.7 L ${mol}^{- 1}$ . [2023]

Q 25 :

The number of units, which are used to express concentration of solution from the following is ______. Mass percent, Mole fraction, Molarity, ppm, Molality [2023]

Q 26 :

A solution of sugar is obtained by mixing 200 g of its 25% solution and 500 g of its 40% solution (both by mass). The mass percentage of the resulting sugar solution is ______ (Nearest integer). [2023]

Q 27 :

Assume a living cell with 0.9% $(ω / ω)$ of glucose solution (aqueous). This cell is immersed in another solution having equal mole fraction of glucose and water.

(Consider the data upto first decimal place only) The cell will : [2025]

(4)

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Topic Question Set

Q 1 : If a substance ‘A’ dissolves in solution of a mixture of ‘B’ and ‘C’ with their respective number of moles as nA,nB and nC. Mole fraction of C in the solution is [2024]

Q 2 : The Molarity (M) of an aqueous solution containing 5.85 g of NaCl in 500 mL water is: (Given: Molar Mass Na : 23 and Cl : 35.5 gmol-1) [2024]

Q 3 : The density of ‘x’ M solution (‘x’ molar) of NaOH is 1.12 g mL-1, while in molality, the concentration of the solution is 3 m (3 molal). Then x is (Given: Molar mass of NaOH is 40 g/mol) [2024]

Q 4 : Molality (m) of 3 M aqueous solution of NaCl is: (Given: Density of solution = 1.25 g mL-1, Molar mass in g mol-1: Na - 23, Cl - 35.5) [2024]

Q 5 : Volume of 3 M NaOH (formula weight 40 g mol-1) which can be prepared from 84 g of NaOH is ______ ×10-1 dm3. [2024]

Q 6 : A solution of H2SO4 is 31.4% H2SO4 by mass and has a density of 1.25 g/mL. The molarity of the H2SO4 solution is _____ M (nearest integer) [Given molar mass of H2SO4 = 98 g mol-1] [2024]

Q 7 : Molality of 0.8 M H2SO4 solution (density 1.06 g cm-3) is ______ ×10-3 m. [2024]

Q 8 : The mass of sodium acetate (CH3COONa) required to prepare 250 mL of 0.35 M aqueous solution is _____ g. (Molar mass of CH3COONa is 82.02 g mol-1) [2024]

Q 9 : The molarity of 1 L orthophosphoric acid (H3PO4) having 70% purity by weight (specific gravity 1.54 g cm-3) is ______ M. (Molar mass of H3PO4 = 98 g mol-1) [2024]

Q 10 : Molality of an aqueous solution of urea is 4.44 m. Mole fraction of urea in solution is x×10-3. Value of x is _____ (integer answer) [2024]

Q 11 : A solution is prepared by adding 1 mole ethyl alcohol in 9 mole water. The mass percent of solute in the solution is ______ (Integer Answer) (Given: Molar mass in g mol-1 Ethyl alcohol : 46, water : 18) [2024]

Q 12 : Molarity (M) of an aqueous solution containing x g of anhyd. CuSO4 in 500 mL solution at 32°C is 2×10-1 M. Its molality will be _____ ×10-3m. (nearest integer). [Given density of the solution = 1.25 g/mL] [2024]

Q 13 : The quantity which changes with temperature is: [2024]

Q 15 : 10 mL of 2 M NaOH solution is added to 20 mL of 1 M HCl solution kept in a beaker. Now, 10 mL of this mixture is poured into a volumetric flask of 100 mL containing 2 moles of HCl and made the volume upto the mark with distilled water. The solution in this flask is : [2025]

Q 16 : 20 mL of 2 M NaOH solution is added to 400 mL of 0.5 M NaOH solution. The final concentration of the solution is ______ ×10-2 M. (Nearest integer) [2025]

Q 17 : Fortification of food with iron is done using FeSO4.7H2O. The mass in grams of the FeSO4.7H2O required to achieve 12 ppm of iron in 150 kg of wheat is _____ (Nearest integer) [Given: Molar mass of Fe, S and O respectively are 56, 32 and 16 g mol-1] [2025]

Q 19 : What is the mass ratio of ethylene glycol (C2H6O2, molar mass = 62 g/mol) required for making 500 g of 0.25 molal aqueous solution and 250 mL of 0.25 molal aqueous solution? [2023]

Q 20 : A solution is prepared by adding 2 g of “X” to 1 mole of water. Mass percent of “X” in the solution is [2023]

Q 22 : The density of 3 M solution of NaCl is 1.0 g mL-1. Molality of the solution is ______ ×10-2 m. (Nearest Integer). Given: Molar mass of Na and Cl is 23 and 35.5 g mol-1 respectively. [2023]

Q 23 : A 300 mL bottle of soft drink has 0.2 M CO2 dissolved in it. Assuming CO2 behaves as an ideal gas, the volume of the dissolved CO2 at STP is ______ mL. (Nearest Integer) Given: At STP, molar volume of an ideal gas is 22.7 L mol-1. [2023]

Q 25 : The number of units, which are used to express concentration of solution from the following is ______. Mass percent, Mole fraction, Molarity, ppm, Molality [2023]

Q 26 : A solution of sugar is obtained by mixing 200 g of its 25% solution and 500 g of its 40% solution (both by mass). The mass percentage of the resulting sugar solution is ______ (Nearest integer). [2023]

Q 27 : Assume a living cell with 0.9% (ω/ω) of glucose solution (aqueous). This cell is immersed in another solution having equal mole fraction of glucose and water. (Consider the data upto first decimal place only) The cell will : [2025]

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Q 1 :

If a substance ‘A’ dissolves in solution of a mixture of ‘B’ and ‘C’ with their respective number of moles as $n_{A}, n_{B}$ and $n_{C}$ . Mole fraction of C in the solution is [2024]

Q 2 :

The Molarity (M) of an aqueous solution containing 5.85 g of NaCl in 500 mL water is:
(Given: Molar Mass Na : 23 and Cl : 35.5 g ${mol}^{- 1}$ ) [2024]

Q 3 :

The density of ‘x’ M solution (‘x’ molar) of NaOH is 1.12 g ${mL}^{- 1}$ , while in molality, the concentration of the solution is 3 m (3 molal). Then x is (Given: Molar mass of NaOH is 40 g/mol) [2024]

Q 4 :

Molality (m) of 3 M aqueous solution of NaCl is:
(Given: Density of solution = 1.25 g ${mL}^{- 1}$ , Molar mass in g ${mol}^{- 1}$ : Na - 23, Cl - 35.5) [2024]

Q 5 :

Volume of 3 M NaOH (formula weight 40 g ${mol}^{- 1}$ ) which can be prepared from 84 g of NaOH is ______ $\times 10^{- 1}$ ${dm}^{3}$ . [2024]

Q 6 :

A solution of $H_{2} {SO}_{4}$ is 31.4% $H_{2} {SO}_{4}$ by mass and has a density of 1.25 g/mL. The molarity of the $H_{2} {SO}_{4}$ solution is _____ M (nearest integer)

[Given molar mass of $H_{2} {SO}_{4}$ = 98 g ${mol}^{- 1}$ ] [2024]

Q 7 :

Molality of 0.8 M $H_{2} {SO}_{4}$ solution (density 1.06 g ${cm}^{- 3}$ ) is ______ $\times 10^{- 3}$ m. [2024]

Q 8 :

The mass of sodium acetate ( ${CH}_{3} COONa$ ) required to prepare 250 mL of 0.35 M aqueous solution is _____ g.
(Molar mass of ${CH}_{3} COONa$ is 82.02 g ${mol}^{- 1}$ ) [2024]

Q 9 :

The molarity of 1 L orthophosphoric acid ( $H_{3} {PO}_{4}$ ) having 70% purity by weight (specific gravity 1.54 g ${cm}^{- 3}$ ) is ______ M.
(Molar mass of $H_{3} {PO}_{4}$ = 98 g ${mol}^{- 1}$ ) [2024]

Q 10 :

Molality of an aqueous solution of urea is 4.44 m. Mole fraction of urea in solution is $x \times 10^{- 3}$ . Value of $x$ is _____ (integer answer) [2024]

Q 11 :

A solution is prepared by adding 1 mole ethyl alcohol in 9 mole water. The mass percent of solute in the solution is ______ (Integer Answer)

(Given: Molar mass in g ${mol}^{- 1}$ Ethyl alcohol : 46, water : 18) [2024]

Q 12 :

Molarity (M) of an aqueous solution containing $x$ g of anhyd. ${CuSO}_{4}$ in 500 mL solution at 32°C is $2 \times 10^{- 1}$ M. Its molality will be _____ $\times 10^{- 3}$ m. (nearest integer).

[Given density of the solution = 1.25 g/mL] [2024]

Q 13 :

The quantity which changes with temperature is: [2024]

Q 15 :

10 mL of 2 M NaOH solution is added to 20 mL of 1 M HCl solution kept in a beaker. Now, 10 mL of this mixture is poured into a volumetric flask of 100 mL containing 2 moles of HCl and made the volume upto the mark with distilled water. The solution in this flask is : [2025]

Q 16 :

20 mL of 2 M NaOH solution is added to 400 mL of 0.5 M NaOH solution. The final concentration of the solution is ______ $\times 10^{- 2}$ M. (Nearest integer) [2025]

Q 19 :

What is the mass ratio of ethylene glycol ( $C_{2} H_{6} O_{2}$ , molar mass = 62 g/mol) required for making 500 g of 0.25 molal aqueous solution and 250 mL of 0.25 molal aqueous solution? [2023]

Q 20 :

A solution is prepared by adding 2 g of “X” to 1 mole of water. Mass percent of “X” in the solution is [2023]

Q 22 :

The density of 3 M solution of NaCl is 1.0 g ${mL}^{- 1}$ . Molality of the solution is ______ $\times 10^{- 2}$ m. (Nearest Integer).

Given: Molar mass of Na and Cl is 23 and 35.5 g ${mol}^{- 1}$ respectively. [2023]

Q 23 :

A 300 mL bottle of soft drink has 0.2 M ${CO}_{2}$ dissolved in it. Assuming ${CO}_{2}$ behaves as an ideal gas, the volume of the dissolved ${CO}_{2}$ at STP is ______ mL. (Nearest Integer)

Given: At STP, molar volume of an ideal gas is 22.7 L ${mol}^{- 1}$ . [2023]

Q 25 :

The number of units, which are used to express concentration of solution from the following is ______. Mass percent, Mole fraction, Molarity, ppm, Molality [2023]

Q 26 :

A solution of sugar is obtained by mixing 200 g of its 25% solution and 500 g of its 40% solution (both by mass). The mass percentage of the resulting sugar solution is ______ (Nearest integer). [2023]

Q 27 :

Assume a living cell with 0.9% $(ω / ω)$ of glucose solution (aqueous). This cell is immersed in another solution having equal mole fraction of glucose and water.

(Consider the data upto first decimal place only) The cell will : [2025]