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| Chemistry 9th Chapter 6 Solutions Questions Bank |
Chemistry 9th Chapter 6 Solutions MCQs Questions Bank
Click the write option, green is correct and red color is wrong.
1. 1 ml is equal to :
2. 10% m/v sugar solution contains 10g of sugar in solution:
3. A 5 percent (w/w) sugar solution means that:
4. A solution containing maximum amount of solute at a given temperature is called _______ solution.
5. Air is an example of solution:
6. Brass and Bronze are considered as:
7. Brass is a solid solution of Zn and:
8. Brine is a _______ solution of common salt in water.
9. Concentrated solution of KMnO₄ has dense _____ colour.
10. Concentration is ratio of:
11. Example of aqueous solution is:
12. Example of liquid in liquid is:
13. Example of liquid-gas solution is:
14. Example of solid in solid solution is:
15. Example of true solution is:
16. Example of universal solvent is:
17. Grease, paints, naphthalene are soluble in:
18. Hydrogen absorbed in palladium is an example of solution:
19. If 10 cm³ of alcohol is dissolved in 100 g of water, it is called:
20. If the solute-solute forces are strong enough than those of solute-solvent forces. The solute:
21. In aqueous solution solvent is:
22. In soft drinks _______ is/are used as solute.
23. In soft drinks, CO₂ is:
24. Ionic solids and polar covalent compounds are soluble in:
25. Metal alloys are:
26. Mist is an example of solution:
27. Molarity is the number of moles of solute dissolved in:
28. Size of particles in true solution is:
29. Smoke in air is example of solution:
30. The component of solution which is present in large quantity is called:
31. The component of solution which is present in smaller quantity is called:
32. The components which are present in large quantity in a solution are called:
33. The compound soluble in water is/are:
34. The compound which is insoluble in water:
35. The example of solution of a solid solute in a solid solvent.
36. The formula of sodium thiosulphate is:
37. The liquid which evaporates completely, leaving no residue is a/an:
38. The minimum components of solution are:
39. The molarity of a solution is represented by:
40. The simplest way to distinguish between a solution and a pure liquid is:
41. The solubility of which salt decreases with the increase of temperature?
42. The solution of which salt are called brine?
43. The solution which is formed by dissolving a substance in water is called:
44. Tyndall effect is due to:
45. Tyndall effect is shown by:
46. Types of solutions are:
47. When a saturated solution is diluted it turns into:
48. When a saturated solution is diluted it turns into:
49. Which of the following compound is not soluble in water?
50. Which of the following is not a non-polar covalent compound?
51. Which of the following is soluble in carbon tetrachloride?
52. Which of the following is soluble in ether?
53. Which of the following is water soluble?
54. Which of the following shows Tyndall effect?
55. Which of the following solution contains more water?
56. Which one can easily dissolve in carbon tetrachloride?
57. Which one is a suspension?
58. Which one is example of colloid?
59. Which one of the following is a ‘liquid in solid’ solution?
60. Which one of the following is heterogeneous mixture?
61. Which one of the following is suspension?
62. Which one of the following solutions contains more water?
63. Which one of the following solutions has less water?
64. Which one of the following solutions is more dilute?
65. Which one of the following solvents is polar?
66. Which one of the following will show negligible effect of temperature on its solubility?
67. Which salt is used to prepare supersaturated solution?
Short Questions
1. State the general principle of solubility.
2. Classify the following into true solution and colloidal solution.
3. A saturated solution is in dynamic equilibrium stage. Justify.
4. A solution contains 50g of sugar dissolved in 450g of water. What is the concentration of this solution?
5. A supersaturated solution is unstable at room temperature. Comment.
6. Blood, starch solution, Glucose solution, toothpaste, copper sulphate solution, silver nitrate solution.
7. Brass and bronze cannot be separated by physical means, yet it is considered a mixture. Why?
8. Calculate molarity of a solution which is prepared by dissolving 28.4g of Na₂SO₄ in 400cm³ solution.
9. Calculate the concentration % (m/m) of a solution which contains 2.5 g of salt dissolved in 50 g of water.
10. Calculate the concentration v/v of solution, if we add 5 cm³ of acetone in water to prepare 90 cm³ of aqueous solution.
11. Can colloids be separated by filtration, if not why?
12. Dead sea is so rich with salts that it forms crystals when temperature lowers in the winter. Can you comment why is it named as "Dead Sea"?
13. Define a saturated solution and give example.
14. Define colloid.
15. Define dilute and concentrated solution.
16. Define Molarity. Write its formula.
17. Define percentage mass / mass (%m/m).
18. Define reduction in terms of loss or gain of oxygen or hydrogen. Give an example.
19. Define solubility.
20. Define solution and give an example.
21. Define supersaturated solution.
22. Define suspension.
23. Define unsaturated solution.
24. Differentiate between concentrated and dilute solution.
25. Differentiate between solute and solvent.
26. Distinguish between the following pairs as compound or solution:
27. Do the percentage calculations require the chemical formula of the solute?
28. How a 10% m/m sugar solution would be prepared?
29. How can you explain the solute-solvent interaction to prepare NaCl solution?
30. How can you justify that milk is a colloid?
31. How do we distinguish between solution and pure liquid?
32. How does nature of attractive forces of solute-solute and solvent-solvent affect the solubility?
33. How much NaOH is required to prepare 500cm³ of 0.4M solution?
34. How much water should be mixed with 18 cm³ of alcohol so as to obtain 18 % (v/v) alcohol solution?
35. How one molar solution is prepared?
36. How will you test whether given solution is colloidal solution or not?
37. Identify as colloids or suspensions from the following: Paints, milk, milk of magnesia, soap solution.
38. Justify with example that solubility of a salt increases with increase in temperature.
39. State the formula of molarity.
40. What are physical states of solutions?
41. What do you mean by volume/volume %?
42. What do you mean, like dissolves like? Explain with examples. / What is the general principle of solubility?
43. What is a saturated solution?
44. What is alloy? Give an example.
45. What is concentration of a solution?
46. What is difference between colloid and suspension?
47. What is meant by aqueous solution? Give example
48. What is meant by concentration?
49. What is meant by molarity? Give its formula.
50. What is meant by percentage unit of solution concentration?
51. What is percentage – mass / volume (%m/v)?
52. What is percentage volume by mass (%v/m)?
53. What is the difference between solute and solvent?
54. What is the difference between true solution and a colloidal solution?
55. What is the major difference between a solution and a mixture?
56. What is the reason for the difference between solutions, colloids and suspensions?
57. What is tyndall effect and on what factors it depends?
58. What will happen if the solute-solute forces are stronger than those of solute-solvent forces?
59. When solute-solute forces are weaker than those of solute-solvent forces? Will solution form?
60. Which of the following will scatter light and why?
61. Which one of the following solutions is more concentrated: one molar or three molar?
62. Why a solution is considered mixture?
63. Why do we stir paints thoroughly before using?
64. Why does solubility of Li₂SO₄ and Ce₂(SO₄)₃ decrease with the increase of temperature?
65. Why does suspension and solutions not show Tyndall effect while colloids do?
66. Why does the colloid show tyndall effect?
67. Why does the suspension not form a homogeneous mixture?
68. Why is iodine soluble in CCI₄ and not in water?
69. Why is the formula of solute necessary for calculation of the molarity of the solution?
70. Why test tube becomes cold when KNO₃ is dissolved in water?
71. Why water is called a universal solvent?
Long Questions
1. What is saturated solution and how it is prepared?
2. Differentiate between dilute and concentrated solutions with a common example.
3. Explain, how dilute solutions are prepared from concentrated solutions?
4. What is molarity and give its formula to prepare molar solution?
5. Explain the solute-solvent interaction for the preparation of solution.
6. What is general principle of solubility?
7. Discuss the effect of temperature on solubility.
8. Give the five characteristics of colloid.
9. Give at least five characteristics of suspension.
10. A solution contains 50 g of sugar dissolved in 450 g of water. What is concentration of this solution?
11. If 60 cm³ of alcohol is dissolved in 940 cm³ of water, what is concentration of this solution?
"12. How much salt will be required to prepare following solutions (atomic mass: K=39; Na=23; S=32; O=16 and H=1)
a. 250 cm³ of KOH solution of 0.5 M
b. 600 cm³ of NaN0 solution of 0.25 M
c. 800 cm of Na₂SO₄ solution of 1.0 M"
13. When we dissolve 20 g of NaCl in 400 cm³ of solution, what will be its molarity?
14. We desire to prepare 100 cm³ 0.4 M solution of MgCl₂ , how much MgCl₂ is needed?
15. 12 M H₂SO₄ solution is available in the laboratory. We need only 500cm of 0.1 M solution , how it will be prepared?
16. Compare characteristics of colloid and suspension.
17. Describe the properties of colloids.
18. What are the effects of temperature on solubility? Explain.
19. How solute solvent interaction affect the solubility?
20. Define solubility. Give the general principles of solubility.
21. When we dissolve 20g of NaCl in 400cm³ of solution, what will be its molarity?
22. Explain how dilute solutions are prepared from concentration solution?
23. What is molarity? Give its formula to prepare the molar solution.
24. Give any four characteristics of a solution.
25. What is meant by solution? Explain its types.
26. Write a note on dilute and concentration solution.
27. Define concentration. Explain four concentration units.
28. Define super saturated solution. Write method of its preparation.
29. Define saturated and super saturated solution and how they are prepared?