WORKSHEET - 1 1.
Which of the following statement/s is/are true? a) A solution is a homogeneous mixture of one or more components. b) The major component of a solution is known as solvent. The minor minor component of a solution is known as solute. c) In syru syrup, p, sugar is the solute and w ater is the sol vent. d) In brine, salt is the solute and water is the solvent. 2. An example for a gas in liquid type of solution is a) So da wa te r b) milk milk c) Alloy Alloy d) Air 3. An example for a liquid in gas type of solution is a) So da wa te r b) milk milk c) Fog d) Smoke Smoke 4. (i) Which type of solution is milk? (ii) Name a solid - solid type solution. (iii) Which type of solution is smoke? (i) (ii) (iii) a) Liquid in solid Atmosphere Gas in liquid b) Liquid in gas Alloys Liquid in solid c) Liquid in liquid Rubber Solid in gas d) Gas in liqui liquid d Rubber Ru bber Li quid qu id in liq uid ui d
5.
Solution-A: A solution which can dissolve some more solute at a given temperature is known as an unsaturated solution. Solution-B: A solution which cannot dissolve any more solute at a given temperature is known as a saturated solution. Solution-C: A solution which has excess of solute dissolved in it than can be present in a saturated solution is known as a super saturated solution. Solution –A
a) c) d) 6.
7.
Saturated Saturated b) Unsaturated Unsaturated Super saturated Saturate Saturated d
Solution - B
Unsaturated Unsaturated Saturated Saturated Unsaturated Super Super saturate saturated d
Solution - C
Super saturated Super saturated Saturated Un sa tura tu ra te d
If a saturated solution is heated, it a) changes to unsaturated b) changes super saturated c) remains same d) till 50°C, changes to un saturated and then super saturated How can you obtain a saturated solution from an unsaturated solution? a) By heating b) By cooling c) By increasing the pressure d) By decreasing the pressure
8.
How can you obtain a saturated solution from a super saturated solution? a) By heating b) By cooling c) By disturbing d) By adding a crystal of the solute 9. What happens when some amount of solute is added to a saturated solution? a) changes to unsaturated b) changes super saturated c) remains same d) till 50°C, changes to un saturated and then super saturated 10. In which type of solution, a dynamic equilibrium exists between the solid solute and dissolved solute? a) Saturated b) Unsaturated c) Super saturated d) None 11. Match the following : Column - I Column - II a) Soda water i) gas in gas b) H2 in platinum ii) liquid in liquid c) Air iii) solid in solid d) fog iv) gas in solid e) milk v) gas in liquid f) cheese vi) solid in liquid g) smoke vii) solid in gas h) ink viii) liquid in solid i) alloy ix) liquid in gas 12. There are three types of solutions Solution - A :- The density of it increases on addition of some solute. Solution - B :- The density of it decreases on addition of some solute. Solution - C :- The density remains unchanged on addition of some solute. Identify which of the above three are saturated, unsaturated and supersaturated. Q No: 1 2 3 4 5 6 7 8 9 10 All a c c b a b c,d c a WORKSHEET - 2
1.
2.
3.
5g of a salt dissolved in 20g of water to form a saturated solution at 60 0C. Calculate the solubility of the salt at this temperature. a) 100 b) 75 c) 50 d) 50 When 100g of a saturated solution is evaporated at 50 0C, 50g of solid is left over. Find the solubility of the substance at 50 0C. a) 100 b) 200 c) 300 d) 400 A hot solution contains 5g of a substance in 15g of water, at 35 0C. What is the solubility of the substance at this temperature? a) 33.32 b) 66.66 c) 33.34 d) 16.67
4.
5.
6.
The solubility of salt at 30 0C is 50. Calculate the weight of water required to prepare a saturated solution containing 90g of salt. a) 360g b) 180g c) 90g d) 45g The solubility of a substance in water is 40. What is the maximum amount of solute required to prepare a saturated solution with 50g of water? a) 65g b) 50g c) 35g d) 20g Solubility of a substance in a solvent is ‘x’. What is the minimum weight of solution containing ‘y’ g of solute?
x(100 + y) gm y a) 7.
x(100+ y) gm x d)
100 × L K g b)
L K × 100 g d)
K 100 × L g c)
Solubility of a solute is 25. Minimum weight of solvent required to dissolve 10g of that solute is _________. a) 90g
9.
y(100 + x) gm y c)
Solubility of a substance in a solvent is K. What is the minimum weight of the solvent which can dissolve ‘L’ g of solute, to give a saturated solution? [L-II]
100 × K L g a) 8.
y(100+ x) gm x b)
b) 65g
c) 40g
d) 15g
Solubility of a solid at 30 0C is 30 and at 80 0C is 50. If a saturated solution is made with 50g of solvent at 80 0C and cooled to 30 0C, the weight of solute that comes out of the solution is _________. a) 30g
b) 20g
c) 10g
d) 5g
10. Solubility of the salt at 40 0C is 40. The least weight of water which dissolves 10 grams of substance is __________. a) 25g
b) 36g
c) 47g
d) 58g
11. 30 grams of saturated solution on evaporation gives a residue of 5 grams of solute. Solubility of solute is ____________. a) 40
b) 30
c) 20
d) 10
12. Solubility of a substance remains unchanged on heating or cooling. Plot its solubility curve.
a)
b) y t i l i b u l o S
c)
y t i l i b u l o S
Temperature
d)
y t i l i b u l o S
Temperature
y t i l i b u l o S
Temperature
Temperature
13. On cooling, solubility of a substance decreases. Identify its solubility curve.
c)
b)
a)
d)
14. (i)
Cooling favours the solubility of exothermic solutions. True or false? We know that solubility of exothermic solutions decreases on increase of temperature (heating). Therefore the given statement is true. (ii) Heating favours the solubility of endothermic solutions. True or false? We know that solubility increases with increase of temperature (heating). Therefore the given statement is true. (i) (ii) a) T F b) F T c) T T d) F F
Key to Worksheet - 2 Q.No.
1
2
3
4
5
6
7
8
9
10
Ans
d
a
c
b
d
b
b
c
b
a
Q.No.
11
12
13
14
Ans
c
a
c
c WORKSHEET - 3
1.
2.
3. 4.
5.
The graphs which indicate the effect of temperat ure on solubility of a solute are called solubility curves. a) Isothermic curves b) Isobaric curves c) solubility curve d) Isochoric curves The solutions that are formed by the absorptio n of heat from the surroundi ngs are known as a) Neutral solution b) Thermal solutions c) Exothermic solutions d) Endothermic solutions Which of the following forms endothermic solutions? a)NaNO 3 b) NaOH c) Na 2 CO 3 d) Na 2 SO 4 . The solutions that are formed by the evolution of heat to the surroundings are known as a) Neutral solution b) Thermal solutions c) Exothermic solutions d) Endothermic solutions Which of the following form exothermic solutions? a)NaNO 3 b) NaOH c) Na 2 CO 3 d) Na 2 SO 4
6.
7. 8. 9.
10.
11.
12. 13. 14. 15. 16. 17.
(i) What is the nature of solution, if lattice energy is greater than hydration energy? (ii) What is the nature of solution, if lattice energy is less than hydration energy? (i) (ii) a) Endothermic Endothermic b) Exothermic Exothermic c) Endothermic Exothermic d) Exothermic Endothermic Name some solutes whose solubility increases with increase in temperature. a)NaNO 3 b) KNO 3 c) KCl d) NH 4 Cl . Name some solutes whose solubility decreases with increase in temperature. a) NaOH b) Na 2 CO 3 c) Na 2 SO 4 d) All Name some solutes whose solubility fairy change or does not change with increase in temperature. a) NaOH b) Na 2 CO 3 c) NaCl d)Li2SO4 Solubility of a gas in liquid decreases with increase of temperatu re or decrease of pressure. This is called a) Boyle’s law b) Charles’ c) Henry’s law d)Dalton’s law of solutions Write the effect of temperature on the solubility of following solutions : Solute – A :- During its dissolution, it liberates heat to the surroundings. Solute – B :- During its dissolution, it absorbs heat from the surroundings. Solute – C :- During its dissolution, no heat exchange takes place with the surroundings. What are solubility curves and what is their utility ? State Henry's law. To what kind of gases it is applicable. What is the effect of temperature on the solubility of a gas in a liquid at constant pressure ? Solubility of a solid in a liquid decreases with increase of pressure. True / False. NaCl is soluble in water whereas naphthalene is not. Explain. Why ethyl alcohol, Glucose being non-polar dissolve in water ?
Key to Worksheet - 3 Q.No.
1
2
3
4
5
6
7
8
9
10
Ans
c
d
a
c
b, c, d
c
All
d
c, d
c
WORKSHEET - 4 1.
2.
3.
4.
5. 6.
7.
10 grams of NaOH is dissolved in 100 grams of water at 25°C to form a saturated solution. Find the solubility and weight percentage of the solution. Solubility Weight a) 10 9.09 b) 20 18.18 c) 9.09 10 d) 18.18 20 A research student has only 300 g of valuable solvent and wishes to m ake solution of 10% by weight from solute A. How many grams of ‘A’ is weighed out? a) 30g b) 33.33g c) 70g d) 66.66g A solution with weight percentage of sodium hydroxide of 6% is prepared by adding the following mass of water (in grams) to 200 grams of that solution with a weight percent of NaOH of 30% a) 300 g b) 500 g c) 800 g d) 1000 g If solubility of a solute is ‘S’, find its percentage by weight.
100S 100 + S 100S2 (100 + S)2 100S a) 100 + S b) 100S c) 100 + S d) If percentage by weight of a solute is its solubility, find the solubility of the solute. a) 25 b) 50 c) 75 d) 100 If 50 ml of a liquid solute is dissolved in 500 ml of liquid solvent, then find its % by volume (v/v). a) 6.06 b) 7.07 c) 8.08 d) 9.09 Calculate the volume of solvent required to prepare 20 % by volume (v/v) solution by using 70 ml of H 2SO4.
a) 280 ml b) 560 ml c) 1120 ml d) 2240 ml 8. 10 g of a solute is dissolved in 90 g of solvent. If the density of solution is 2g/m l , find the weight-volume percentage. a) 5 g/ml b) 10 g/ml c) 15 g/ml d) 20 g/ml 9. Find the following in 15% (w/v) of solution if the density of solution is 1.06 g/m l . a) Weight of solute b) Weight of solvent Weight of solute Weight of solvent a) 25 g 75 g b) 50 g 50 g c) 15 g 91 g d) 20 g 90 g 10. An aqueous solution of glucose is 10% (w/v). The volume in which 1 g mole of it is dissolved will be______. (Formula of glucose is C 6H12O6) a) 450 ml b) 900 ml c) 1800 ml d) 3600 ml 11. Calculate the mass percentage of K 2CO3 in a solution that is made by dissolving 15g of K2CO3 in 60g of H 2O. a) 10
b) 20
c) 30
d) 40
12. How many grams of NaCl have to be dissolved in 54.0g of H 2O to give a 10.0% weight solution? a) 3 g
b) 6 g
c) 9 g
d) 18 g
13. If the solubility of a solute in a solution is 50, find the percentage by weight of the solution. a) 33.33
b) 66.66
c) 25
d) 75
14. If 2.2 g of oxalic acid is dissolved in 500 ml of solution (density = 1.1 g/m l ), what is the weight percent of oxalic acid in solution? a) 0.1
b) 0.2
c) 0.3
d) 0.4
15. Calculate the masses of glucose and water required to prepare 180 g of 18% (w/w) glucose solution. Mass of water a)
b) c) d)
Mass of glucose
147.6 g 295.2 g 442.8 g 590.4 g
32.4 g 64.8 g 97.2 g 129.6 g
Key to Worksheet - 4 Q.No.
1
2
3
4
5
6
7
8
9
10
Ans
a
b
c
a
d
d
a
d
c
c
Q.No.
11
12
13
14
15
Ans
b
b
a
d
a
WORKSHEET - 5
1. 2. 3.
4. 5.
1.06 g of Na 2CO3 is present in 100 litres of solution. Find the molarity of the solution. a) 10 –2 M b) 10 –4 M c) 10 –1 M d) 10 –3 M Claculate the molarity of H 2O in pure water. a) 27.75 moles/lit b) 55.5 moles/lit c) 111 moles/lit d) 13.5moles/lit Mass of a solution is ‘m’ g. Its density is ‘d’ g/ml. Find molarity if the amount of solute present is ‘p’ g. [Molecular weight = W].
Pd mW Pb moles/lit moles/lit × 1000moles/lit mW Pb mW a) b) c) d) moles/lit Find the number of millimoles of KCl present in 3 litres of 2 molar solution. a) 6 × 103 b) 0.6 × 103 c) 6 × 102 d) 6 × 104 1.2 moles of CaCl 2 is dissolved in enough water to make 2 litres of solution. Calculate the concentration of each of ions present in that solution. a) 12 mole/lit b) 0.12 mole/lit c) 0.012 mole/lit d) 1.2 mole/lit
6.
7.
How many milligrams of barium and chloride ions are there in a millitre of 2M barium chloride, BaCl2 solution? (Atomic weight of Ba = 137.4 and Cl = 35.5) a) 14.2 mg b) 142 mg c) 71 mg d) 7.1 mg The number of sulphur atoms present in 100 ml of 0.1 M H 2SO4 is_________.
a) 1.505 × 1023 b) 15.05 × 1023 c) 15.05 × 1024 d) 1.05 × 1023 8. Find the number of molecules of NaOH present in 0.5 M, 500 ml solution. a) 6.023 × 1023 b) 6.023 × 1024 c) 6.023 × 1021 d) 6.023 × 1026 9. A concentrated acids is 38% pure by weight in aqueous solution. The density of the solution is 1.855 g/ml and molarity is 7.19 mol/litre. Identify the acid. a) 90 grams b) 94.03 grams c) 92 grams d) 98.03 grams 10. Calculate molarity of solution of H 2SO4 (density of solution is 2g/ml) containing 27% H2SO4 by weight. a) 42 M b) 04.2 M c) 5.5 M d) 55 M 11. The molarity of 4% (w/v) NaOH solution is___________ a) 2 M b) 0.2 M c) 1 M d) 0.1 M 12. Consider a solution of volume, V 1 whose molarity is M1, It is diluted by adding some amount of water. The molarity of the solution after addition of water is M 2(V2 > V1; M2 < M1). Calculate the volume or the amount of water added.
M M M M2 V1 1 − 1 V1 2 − 1 V2 V2 1 − 1 − 1 M M M M 1 1 2 2 a) b) c) d) 13. Calculate the final concentration of NaCl after 1.5 litres of 0.100M NaCl solution is diluted a) to 3.5 litres with water b) with 3.5 litres of water a) 0.214, 0.714 M b) 0.5M, 0.7 M c) 0.414 M, 0.614 M d) 0.0314 M, 0.414 M 14. Find the molarity of a mixed solution formed by adding 250 ml of 0.2M NaOH solution and 100 ml of 0.5M NaOH solution. a) 0.845 M b) 0.585 M c) 0.285 M d) 0.485 M 15. 250 ml of 6M HCl, 650 ml of 3 M HCl were mixed together. The volume of water to be added to make the solution 3 M is __________ml. a) 150 ml b) 200 ml c) 125 ml d) 250 ml Key to Worksheet - 5 Q.No.
1
2
3
4
5
6
7
8
9
10
Ans
b
b
c
a
d
b
c
a
d
c
Q.No.
11
12
13
14
15
Ans
c
a
a
c
d
WORKSHEET - 6 1.
The chloride of a metal (M) contains 65.5% of chlorine. 100ml of the vapour of the chloride of the metal at S.T.P. weighs 0.72g. The molecular formula of the metal chloride is: a) MCl c) MCl3 d) MCl4 b) MCl2
2.
The oxide of an element possesses the formula M 2O3. If the equivalent weight of the metal is 9, then the atomic weight of the metal will be: a) 9 b) 18 c) 27 d) none of these If m1 gram of a metal A displaces m 2 gram of another metal B from its salt solution and if the equivalent weights are E 1 and E2 respectively then, which of the following is true?
3.
a) E1 =
4.
5.
6.
7.
8.
m1 m2
×
E2 b) E1 =
m2 × E2 m1
c) E1 =
m1 × m2 E2
d) E1 =
m1 m2
×
E2
One gram of hydrogen is found to combine with 80 g of bromine. One gram of calcium (valency = 2) combines with 4 g of bromine. The equivalent weight of calcium is: a) 10 b) 20 c) 30 d) 40 1.520g of the hydroxide of a metal on ignition gave 0.995 g of oxide. The equivalent weight of metal is: a) 36.0 b) 27.0 c) 19.0 d) 9.0 One litre of hard water contains 12.00 mg Mg 2+. Milli-equivalents of washing soda required to remove its hardness is: a) 1 b) 2 c) 3 d) 4 A metal oxide has the formula Z 2O3. It can be reduced by hydrogen to give free metal and water. 0.1596 g of the metal oxide requires 6 mg of hydrogen for complete reduction. The atomic weight of the metal is: a) 27.9 b) 34.3 c) 49.8 d) 55.8
In the reaction 2Na2S2O3 + I2
→
Na2S4O6 + 2NaI.
The equivalent weight of Na 2S2O3 (mol. wt = M) is equal to:[At. wt. of iodine = 127] a) M b) M/2 c) M/3 d) M/4 9. If the equivalent weight of a trivalent metal is 32.7, the molecular weight of its chloride is: a) 68.2 b) 103.7 c) 204.6 d) 232.7 10. When a metal is burnt, its weight is increased by 24 percent. The equivalent weight of the metal will be: a) 20 b) 24 c) 33.3 d) 76 11. The specific heat of a metal is 0.11 and its equivalent weight is 18.61. Its exact atomic weight is: a) 58.2 b) 29.1 c) 55.83 d) 27.91 12. The vapour density of a volatile chloride of a metal is 95 and the specific heat of the metal is 0.13. The equivalent weight of the metal will be approximately: a) 6 b) 12 c) 18 d) 24
13. 0.84 g carbonate of a metal M gave on heating 0.40 g metal oxide. The specific heat of the metal is 0.25. The atomic weight of the metal would be: a) 12 b) 24 c) 36 d) 48 14. 1.5 g of a divalent metal displaced 4 g of copper (at. wt. = 64) from a solution of copper sulphate. The atomic weight of the metal is: a) 12 b) 24 c) 48 d) 56 15. 12g of an alkaline earth metal gave 14.8 g of its nitride. Atomic weight of that metal is: a) 20 b) 12 c) 40 d) 14.8 16. 3g of an oxide of a metal is converted to chloride completely and it yielded 5 g of chloride. The equivalent weight of the metal is: a) 33.25 b) 28.52 c) 20.32 d) 18.5 Q No:1 C
2 c
3 a
4 b
5 d
6 a
7 d
8 a
9 c
10 c
11 c
12 b
13 b
14 b
15 c
16 a
WORKSHEET - 7 1.
2.
3.
4.
5. 6.
7.
8.
What is the normality of solution containing 35g of KOH dissolved in sufficient water to make 400 ml solution? a) 1.56 N b) 2.34 N c) 3.02 N d) 4.54 N Calculate the normality of aqueous solution containing 31.5g of oxalic acid in 2.5 litres solutions. [Mol. wt. of oxalic acid = 126] a) 0.2 N b) 0.1 N c) 0.05 N d) 0.025 N Which amongst the following has the highest normality?] a) 8.0 g of KOH per 100 ml solution b) 6 g of NaOH per 100g of water c) 1 N H3PO4 d) 24.5 g of H2SO4 in 1 litre solution 0.1 N solution of a dibasic acid solution contains 6.3 g of the acid per 1000 ml or solution. Calculate the equivalent weight of the acid. a) 63 b) 54 c) 48 d) 36 Find the number of gram equivalents of solute present in 0.2 N, 250 ml solution. a) 0.25 b) 0.05 c) 0.025 d) 0.015 Calculate the number of milli equivalents of solute present in 1500 ml of 0.2 N aqueous urea solution. a) 400 b) 350 c) 300 d) 250 How many grams of KMnO4 would be required to prepare 2500 ml of 0.01 N solution, based on the following reaction? [Mol. wt of KMnO 4 = 158] a) 0.90 g b) 0.79 g c) 0.64 g d) 0.58 g How many grams of a dibasic acid (Mol. wt. = 200) should be present in 100 ml of its aqueous solution to give decinormal strength? a) 2 g b) 1 g c) 0.5 g d) 0.25 g
9.
How many milligrams of aluminium and chloride ions are present in a millilitre of 2N aluminium chloride, AlCl 3 solution?
A l +3 Cl – a) 9×103 mg 106.5×103 mg b) 18×103 mg 71×103 mg c) 18×103 mg 35.5×103 mg d) 27×103 mg 35.5×103 mg 10. Find the number of A l +3 and ions present in 500 ml of 0.5 N Al 2(SO4)3 solution. A l +3
SO4–2
a) 5.202×1022 7.227×1022 b) 4.818×1022 7.227×1022 c) 4.818×1022 5.230×1022 d) 2.324×1022 3.023×1022 11. How many number of nitrogen atoms are present in 100 ml of 0.1 N HNO 3? a) 12.044×1021 b) 6.023×1023 c) 6.023×1021 d) 3.011×1022 12. Find the number of molecules of Al(OH) 3 present in 0.5 N, 500 ml solution. a) 5.023×1022 b) 4.818×1022 c) 3.620×1022 d) 2.318×1022 13. If a solution of H 2SO4 contains 3.0115 × 10 23 atoms of sulphur in 500 ml of solution, find its normality? a) 2.5 N b) 2 N c) 1 N d) 0.5 N 14. What is the molarity of 2N Na 2SO4 solution? a) 2 M b) 1 M c) 0.5 M d) 0.25 M 15. Calculate the molarity and normality of a solution containing 0.5g of NaOH dissolved in 500 ml of the solution. a) 0.025 M, 0.025 N b) 0.025 M, 0.05 N c) 0.05 M, 0.075 N d) 0.025 M, 0.075 N 16. Express the concentration of a 5 percent phosphoric acid (w/v) solution having a density of 1.027 g/ml in terms of molarity and normality. Molarity Normality a) 0.712 M 3.12 N b) 0.635 M 2.34 N c) 0.524 M 1.57 N d) 0.460 M 0.85 N 17. The density of a solution containing 13% by mass of sulphuric acid is 1.09% g/ml. Calculate the molarity and normality of the solution. Molarity Normality a) 1.326 M 3.10 N b) 1.445 M 2.89 N c) 2.132 M 1.52 N d) 3.214 M 2.89 N
18. What percent by weight of NaOH is present in a 4N NaOH solution having density of 1.15 g/ml? a) 14.5 % b) 13.9% c) 12.2 % d) 1.6% Q No:1.a 2.a 3.c 4.a 5.b 6.c 7.b 8.b 9.b 10.b 11.c 12.b 13.b 14.b 15.a 16.c 17.b 18.b Worksheet - 8 1. How much MgCl 2 would be needed to make 250 ml of a solution having same concentrations of Cl– as the one containing 3.78 g of NaC l per 100 ml? 2.
3.
4.
5.
6.
7.
8.
a) 8.743 g b) 7.672 g c) 6.321 g d) 5.402 g Upon heating a litre of N/2 HC l solution, 2.675 g of Hydrogen chloride is lost and the volume of the solution shrinks to 750 ml. Calculate (i) The normality of the resultant solution, and (ii) The number of milli equivalents of HC l in 100 ml of the original solution. (i) (ii) a) 0.43 N 30 m.eq b) 0.51 N 40 m.eq c) 0.57 N 50 m.eq d) 0.63 N 60 m.eq How many millilitres of 0.2 N HC l solution will be required to react completely with 50 ml of 0.25 N NaOH? a) 38.6 ml b) 43.5 ml c) 58.2 ml d) 62.5 ml What is the strength in gram per litre of H 2SO4 solution of volume 12 ml of which neutralised with 15 ml of 0.1 N NaOH solution? a) 6.125 g/lit b) 5.435 g/lit c) 4.822 g/lit d) 3.684 g/lit Calculate the amount of KOH required to neutralise 15 Meq. of each of the following: a) HCl b) KHSO4 c) N2O5 d) CO2 a) 0.69 g b) 0.71 g c) 0.84 g d) 0.92 g A standard solution of NaOH contains 45g of NaOH in 800 ml of solution. During titration, 24.6 ml of the standard alkali solution is required to neutralise 36.4 ml of an unknown solution of sulphuric acid. i) Calculate the normality of the acid solution. ii) What weight of sulphuric acid is present in 250 ml of the acid solution? (i) (ii) a) 0.636 N 8.61 g b) 0.741 N 9.24 g c) 0.828 N 10.01 g d) 0.946 N 11.59 g How much volume (in m l ) of 0.2 N H 2SO4 can be made by diluting 20 m l of 0.5 N acid with water? a) 43 ml b) 50 ml c) 64 ml d) 70 ml Calculate the normality of the resulting solution made by adding 2 drops (0.1 ml) of 0.1 N H2SO4 in distilled water to make it 1 litre solution: a) 10 –3 N
b) 10 –4 N
c) 10 –5 N
d) 10 –6 N
9.
10.
11.
12.
13.
14.
–1 A piece of A l weighing 2.7 g is titrated with 75.0 ml of H 2SO4 (Density 1.18 g ml and 24.7% H2SO4 by weight). After the metal is completely dissolved, the solution is diluted to 400 ml. Calculate the molarity of free H 2SO4 in solution.
a) 6.15 g b) 7.15 g c) 8.15 g d) 9.15 g 200 ml of 0.1 M HCl and 150 ml of 0.3 M H 2SO4 solutions are mixed. Calculate the normality of the resulting mixture. a) 0.288 N b) 0.314 N c) 0.412 N d) 0.560 N Hydrochloric acid solutions A and B have concentration of 0.5 N and 0.1 N respectively. The volumes of solutions A and B required to make 2 litres of 0.2 N HC l are a) 0.5 litre of A + 1.5 litres of B b) 1.5 litres of A + 0.5 litre of B c) 1 litre of A + 1 litre of B d) 0.75 litre of A + 1.25 litres of B 100 m l of 0.2 M HC l and 200 ml of 0.15 M H 2SO4 are mixed. Calculate the proton concentration of the mixture. [Note : The proton concentration of resulting solution is equal to the normality of the resulting solution.] a) 0.267 N b) 0.314 N c) 0.483 N d) 0.512 N 100 ml of 0.2 N KOH solution is mixed with 100 ml of 0.1 M H 2SO4 solution. What is the normality of resulting solution? a) 3 N b) 2 N c) 1 N d) 0 N 100 ml of 0.2 N NaOH solution is mixed with 100 ml of 0.1 N HCl solution. What is the nature and normality of the resulting solution?
a) Acidic, 0.1 N b) Basic, 0.05 N c) Acidic, 0.025 N d) Basic, 0.20 N 15. What is the nature and normality of the resulting solution obtained by mixing? i) 100 ml of 0.1 N HCl and 50 ml of 0.25 N NaOH ii) 1 equivalent of 50 ml NaOH and 100 ml of 0.1 N HCl (i) (ii) a) Acidic, 0.0135 N Basic, 0.03 N b) Basic, 0.0149 N Acidic, 0.04 N c) Acidic, 0.0153 N Basic, 0.05 N d) Basic, 0.0167 N Acidic, 0.06 N Q No:1.b 2.c 3.d 4.a 5.c 6.d 7.b 8.c 9.b 10.b 11.a 12.a 13.d 15.d
14.b
WORKSHEET - 9 1.
2. 3.
Which one of the following is most concentrated solution among the following for the same solute? a) 1M b) 1m c) 1 N d) All have same strength 500 g of water and 0.46 g of ethanol are added to form a solution. Find its molality. a) 0.02 moles/kg b) 0.2 moles/kgc) 0.01 moles/kg d) 0.1 moles/kg 100 ml solution of Na 2CO3 is prepared by dissolving 8.653 g of salt in water. The density of the solution is 1.0816 g/ml. What is the molality of the solution? a) 0.9 moles/kg b) 0.41 moles/kg c) 0.82 moles/kg d) 0.4 moles/kg
4.
5.
6.
7.
8.
9.
The molality of 100 ml of solution of NaOH prepared by dissolving 0.4 g of it in water is 2 molal. Find the density of solution. a) 0.027 g/ml b) 0.0135 g/ml c) 0.108 g/ml d) 0.054 g/ml A solution of ethanol in water is 1.54 molal. How many grams of it are there in 2500 g of the solvent? (Mol. wt. of ethanol = 46). a) 177.1 g b) 88.5 g c) 35.42 g d) 24.27 g 2.45 g of H 2SO4 is used to prepare 0.1 molal aqueous solution. Calculate the amount of water. a) 250 g b) 125 g c) 62.5 g d) 31. 25 g Solubility of a substance is 100. If the molecular weight of the substa nce is 100, then, find its molality. a) 15 moles/kg b) 10 moles/kg c) 5 moles/kg d) 2.5 moles/kg The molality of a solution is ‘m’ moles/kg. If the solute is NaOH, how much amount of NaOH is present in 100 g of solvent? a) 1m g b) 2m g c) 4m g d) 8m g Calculate the molality of 10 percent (by weight) solution of Ca(NO 3)2.
a) 0.3385 mole/kg b) 0.677 mole/kg c) 0.169 mole/kg d) 1.3 mole/kg 10. What would be the molality of a solution made by mixing equal volumes of 30% by mass of H2SO4 (density 1.218 g cm –3) and 70% by mass of H 2SO4 (density 1.610 g cm –3)? a) 22.8 moles/kg b) 5.7 moles/kgc) 2.5 moles/kg d) 11.4 moles/kg 11. The molality of a solution containing sulphuric acid is 1.52 molal. Find its solubility and weight percentage. Solubility Weight percentage a) 29.997 16.586 b) 14.896 12.964 c) 7.4480 10.744 d) 3.7240 8.372 12. Calculate the molality of 1 litre solution of 93% (w/v) H 2SO4. The density of solution is 1.84 g/ml. a) 20.84 moles/kg b) 10.42 moles/kg c) 5.21 moles/kg d) 2.60 moles/kg 13. The molality of a solution of 90% (w/v) is 20.45, if the density of solution is 2 g/ml, the solute present in the solution is: a) H2SO4 b) Na 2CO3 c) HCl d) NaOH
14. The density of 3 M H 2SO4 solution is 1.84 g/ml. Find its molality. a) 3.88 moles/kg b) 2.60 moles/kg c) 1.94 moles/kg d) 0.97 mole/kg 15. The density of 3M solution of sodium thio sulphate (Na2S2O3) is 1.25 g/ml. Calculate the molality of Na + and ions respectively: Na + a) 7.731moles/kg 3.865 moles/kg b) 3.865 moles/kg 3.865 moles/kg c) 3.865 moles/kg 7.731moles/kg d) 1.9325 moles/kg 3.865 moles/kg
16. 8.0575 × 10 –2 kg of Glauber’s salt ( Na 2SO4.10H2O) is dissolved in water to obtain 1 litre of solution of density 1.0772 kg/m 3. Calculate its molarity and molality. Molarity Molality a) 0.125 mole/lit 1.5 moles/kg b) 0.5 mole/lit 1 mole/kg c) 1 mole/lit 0.5 mole/kg d) 0.25 mole/lit 0.25 mole/kg 17. ‘x’ g of solute is mixed with a solvent to get ‘y’ ml of solution. If molarity of the solution is ‘M’ and molality of solute is ‘m’, find the density of the solution.
mx + My my
y mxy + My
my mx + My
a) b) c) 18. A 1000 ml solution contains 410.3 g of H 2SO4 at 20°C. If 1.243 g/ml, finds its molarity and molality? Molarity Molality a) 5.028 moles/lit 4.187 moles/kg b) 2.09 moles/lit 2.40 moles/kg c) 2.40 moles/lit 2.09 moles/kg d) 4.187 moles/lit 5.028 moles/kg Q No:1 2 3 4 5 6 7 8 9 10 11 12 B a c d a a b c b d b b
My mx + My
d) the density of the solution is
13 d
14 c
15 a
16 d
17 18 a d
WORKSHEET - 10 1.
2.
3.
180 g of water is taken in a beaker and 196 g of H2SO4 is added to it. Find the mole fraction of H2SO4.
1 1 1 1 4 a) 3 b) c) 5 d) 6 A solution contains 25% water, 25% ethanol (C 2H5OH) and 50% acetic acid (CH 3COOH) by mass. Calculate the mole fraction of each component: Water Ethanol Acetic acid a) 0.414 0.097 0.489 b) 0.502 0.196 0.301 c) 0.502 0.169 0.329 d) 0.414 0.147 0.439 A gaseous mixture contains equal weights of nitrogen and ethylene (C2H4) at certain temperature and pressure. What is the ratio of the mole fractions of nitrogen and ethylene in the gas mixture? a) 1 : 4
4.
c) 1 : 2
d) 1 : 1
Mole fraction of NaCl in aqueous solution containing 5.85 g of it is 0.25. Find the number of molecules of water present in the solution. a) 2.769 ×1023
5.
b) 1 : 3
b) 1.806 ×1023
c) 0.956×1023
d) 0.365×1023
Mole fraction of urea is 0.25. Given solution contains 120 g of urea (Mol. wt = 60). The weight of water in the solution is _________. a) 108 g
b) 120 g
c) 148 g
d) 180 g
6.
The mole fraction of an acid of solubility 10 in its aqueous solution is 0.018. Calculate the molecular weight. a) 66
7.
b) 78
c) 84
d) 99
The solubility of C 6H6 is 15. If the solvent is carbon tetrachloride (CCl 4), find the mole fraction of solute and solvent. Solute a) 0.23
8.
0.77
b) 0.36
0.64
c) 0.42
0.58
d) 0.51
0.49
Calculate the mole fraction of ethanol and water in a sample of rectified spirit which contains 95 percent of ethanol by weight.(Gram mol. wt. of ethanol = 46) Ethanol a) 0.88
9.
Solvent
Water 0.12
b) 0.74
0.26
c) 0.63
0.37
d) 0.56
0.44
Molality of an aqueous solution is 0.45. Calculate the mole fraction of solute in that solution. a) 0.065
b) 0.008
c) 0.101
d) 1.20
10. Calculate the molality and mole fraction of the solute in aqueous solution containing 3.0 g of urea (mol. mass = 60) per 250 g of water. Molality a) 0.5 moles/kg
Mole fraction 0.00634
b) 0.4 moles/kg
0.00531
c) 0.3 moles/kg
0.00428
d) 0.2 moles/kg
0.00361
11. Molality of an aqueous solution of glucose (C6H12O6) is 0.12 moles/kg. What are the mole fractions of each component in the solution? C 6 H 12O 6 a) 0.002 b) 0.105 c) 0.214 d) 0.355
Water 0.998 0.895 0.786 0.645
12. 214.2 g of sugar syrup contains 34.2 g of sugar. Calculate. i) molality of the solution and Molality
Mole fraction
a) 0.55 moles/kg
ii) mole fraction of sugar in the syrup.
0.0099
b) 0.63 moles/kg
0.0084
c) 0.72 moles/kg
0.0073
d) 0.89 moles/kg
0.0056
Q No:1
2
3
4
5
6
7
8
9
10
11
12
D
b
d
b
a
d
a
a
b
d
a
a
WORKSHEET 11 1.
What is the volume (in ml) of 0.1 M potassium permanga nate solution is required to completely oxidize 100ml of 0.5M ferrous sulphate solution in acid medium? (Mol. wt. of KMnO 4 is 158) 2 KMnO4 + 10FeSO 4 + 8H2SO4 (5Fe2+ + + 8H+
2.
3.
4. 5.
→
5Fe2(SO4)3 + K2SO4 + 2MnSO4 + 8H2O
Mn2+ + 5Fe3+ + 4H2O)
a) 400 b) 300 c) 200 d) 100 500m l of a solution contains 12.6 grams of oxalic acid (mol. wt. = 126). 10ml of this solution is diluted to 100m l in a flask. What is the molarity of the resultant solution? a) 0.2 M b) 0.1 M c) 0.02 M d) 0.01 M An aqueous solution of glucose is 10%(w/v) in strength. The volume in which 1 gram mole of it is dissolved will be: a) 18 lt. b) 9 lt. c) 0.9 lt. d) 1.8 lt. The molality of 4% (w/w) NaOH solution is: a) 0.1 mole/kg b) 0.5 mole/kg c) 0.01 mole/kg d) 1.04 moles/kg The concentration of an aqueous solution of 0.01M CH 3OH solution is nearly equal to which of the following? a) 0.01% (w/v) CH3OH b) 0.01 m CH3OH c) 0.01 N CH3OH
6.
→
d) 0.99M H2O
Zn reacts with CuSO4 as follows: Zn + CuSO 4
→
ZnSO4 + Cu.
If excess of Zn is added to 100ml of 0.05M CuSO 4, the amount of copper formed will be: 7. 8.
9.
a) 0.6354 g b) 0.3175 g c) 0.177 g d) 6.354 g The mole fraction of water in 20% aqueous solution of H 2O2 is: a) 0.2 b) 0.4 c) 0.808 d) 0.117 If 20ml of 0.4M NaOH solution is completely neutralised by 40.0ml of a dibasic acid, the molarity of the acid solution is a) 0.1 M b) 0.2 M c) 0.3 M d) 0.4 M The weight of H2C2O4.2H2O required to prepare 500m l of 0.2N solution is:
a)1.26 g b) 6.3 g c) 1.575 g d) 3.15 g 10. The molarity of a solution containing 1 gram of NaOH in 250ml of the solution is: a) 0.1 M b) 0.2 M c) 0.05 M d) 0.15 M 11. The amount of anhydrous Na2CO3 present in 250ml of 0.25M solution is: a) 6.625 g
b) 8 g
c) 3.25 g
d) 1 .025 g
12. 3 grams of a substance of mol. wt. 30 is dissolved in 250 grams of H 2O. The molality of the solution is a) 1 m b) 0.4 m c) 0.3 m d) 0.2 m 13. The molecular weight of H 2SO4 is 98. The weight of acid present in 400ml of 0.125M solution is a) 2.45 g b) 3.92 g c) 4.9 g d) 9 g 14. 0.53 g of anhydrous sodium carbonate (M.W = 106) is dissolved in 100ml of solution. Molarity of that solution is a) 0.1 M b) 0.5 M c) 0.05 M d) 0.0 1 M 15. What volume of 0.8M solution contains 0.1 mole of the solute? a) 100 ml b) 125 ml c) 500 ml d) 62.5 ml 16. A molal solution is one that contains one mole of solute in: a) 1000 g of the solvent b) 199 ml of the solution c) one litre of the solvent d) 22.4 litres of the solution 17. 25 ml of 3 M HNO3 is mixed with 75ml of 4 M HNO 3. If the volumes are additive, the molarity of the final mixture would be a) 3.25 M b) 4.0 M c) 3.75 M d) 3.50 M 18. How many grams of NaOH will be needed to prepare 250ml of 0.1 M solution? a) 1 g b) 10 g c) 4 g d) 6 g 19. Molecular weight of tribasic acid is W. Its equivalent weight would be a) W/2 b) W/3 c) W d) 3W 20. What volume of 0.8M solution contains 0.4 moles of solute? a) 100 ml b) 125 ml c) 500 ml d) 6.25 ml 21. The molarity of 2N HC l is a) 2 M b) l M c) 0.5 M d) 3 M 22. In which mode of expression does the concentration of a solution remain independent of temperature? a) Molarity b) Normality c) Formality d) Molality 23. How much water is to be added to dilute 10 ml of 10N HCl to make it decinormal? a) 990 g b) 1010 g c) 100 g d) 1000 g 24. Equivalent weight of MnSO 4 is half of its molecular weight when it is converted to: a) Mn2O3
b) MnO2
c)
d)
25. A 0.6% (w/v) solution of urea (mol. wt. 60) would be isotonic with a) 0.1 M glucose b) 0.1 M KCl c) 0.6% (w/v) NaCl d) 0.6% (w/v) glucose Q No:1.d 2.c 3.d 4.d 5.c 6.b 7.c 8.a 9.b 10.a 11.a 12.b 13.c 15.b 16.a 17.c 18.a 19.b 20.c 21.a 22.d 23.a 24.b 25.a,b
14.c
