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Chemistry Chapters

9th Class Chapter 6 Chemistry Long Questions

Dear students, prepare for chemistry class 9th chapter 6 long questions. These important long questions are carefully added to get you best preparation for your 9th class chemistry ch. 6 exams.
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Question: 1
Q no<gwmw class="ginger-module-highlighter-mistake-type-6" id="gwmw-15859222153259317715906">:</gwmw>5<gwmw class="ginger-module-highlighter-mistake-type-6" id="gwmw-15859222153252428860884">(</gwmw>A) Write <gwmw class="ginger-module-highlighter-mistake-type-3" id="gwmw-15859222153252481436200">difference</gwmw> types of solutions with examples.
Answer: 1
1-21
Solute Solvent Examples
1-Gas Gas Air, mixture of H2 and He in weather ballons.
2-Gas Liquid Oxygen in water, CO in water
3- Gas Solid Hydrogen adsorbed on palladium.
4- Liquid Gas Mist, fog, liquid air
5- liquid Liquid Alchol in water, benzene
6- liquid Solid Butter chese
7- Liquid Gas Dust particles or smoke
8- Solid liquid Sugar in water
9- Solid solid Mettal alloys, opals
Question: 2
Q no: 5 (B) Write a note Super saturate solution.
Answer: 2
2-21
That solution that is more concentrated than a saturated solutions are heated, They develop further capacity to dissolve more solute Such Solutions contain greater amount of solute than is required to form a saturated solution and they become more concentrated.
Supersaturated solutions are not stable . Therefore an easy way to get a supersaturated solution is to prepare a saturate solution at high temperature where access solute crystallizes out and leaves behind a saturated solution.
Question: 3
Q no<gwmw class="ginger-module-highlighter-mistake-type-6" id="gwmw-15859236834860969730462">:</gwmw>6<gwmw class="ginger-module-highlighter-mistake-type-6" id="gwmw-15859236834867217993456">(</gwmw>A) What is meant by solubility name factors effect solubility and explain any one <gwmw class="ginger-module-highlighter-mistake-type-3" id="gwmw-15859236834866852611385">factors</gwmw>.
Answer: 3
3-21
Solubility:
It is defined as the number of grams of the solute dissolved in loogof a solvent t prepare a saturated solution at a particular temperature.
Factors affect solubility:
1- The general principle of solubility is, like dissolve like
(a) The ionic and polar substance are solute in polar substance are solute in polar solvents . Ionic Solids and polar Covalent compounds are Soluble in water eg, Kcl ,Na2 Co3etc
(b) Non polar covalent are not soluble in polar solvents. Non-polar covalent compounds are not soluble in water such as ether, benzene and petard are insoluble in water.
2- Solute - solvent interaction
3- Temperature

Question: 4
Q no: 6 (B) Write down properties of colloids.?
Answer: 4
4-21
1- The particles are large consisting of many atoms, ions or molecules .
2- A colloid appears to be a homogenous but actually it is a heterogeneous mixture. Hence, they are not true solution. Particles do not settle down for a long time, therefore, colloids are quite stable.
3- Particles are large but can't be seen with naked eye
4- Although particles are big nut they can pass through a filter paper
5- particles scatter the path of light rays thus emitting the beam light.
Question: 5
Q no: 7<gwmw class="ginger-module-highlighter-mistake-type-6" id="gwmw-15859246868562353796437">(</gwmw>A) When we dissolved 20g of NaCl in400 cm³ of solution, what will be its <gwmw class="ginger-module-highlighter-mistake-type-1" id="gwmw-15859246901499620468600">molarity</gwmw>?
Answer: 5
5-21
Mass of NaCl = 20g
Volume of solution = 400cm³
Volume of solution in dm³ = 400cm³/1000cm³
Molar mass of NaCl = 23+35.5
=58.5g mol-¹
Required:
Molarity of solution =?
Solution:
Molarity = Mass of solute/molar mass of solute x volume of solution
=20g/58.5x 0.4
=29/23.4
= 0.85M
Question: 6
Question no: 7<gwmw class="ginger-module-highlighter-mistake-type-6" id="gwmw-15859252591573923013881">(</gwmw>B) Comparison of the Characteristics of solution, colloid and suspension.
Answer: 6
6-21
Solution;
1- There are the particles that exist in their simplest form
2- particles dissolve uniformly throughout and from a homogeneous mixture
3- Particles are so small that they can't be seen with naked eye.

Colloid:
1- The particles are large consisting of many atoms, ions or molecules.
2- Particles are large but can,t be seen with naked eye.
Although particles are big but they can pass through a filter paper.
Suspension:
1- The particles are of largest size. They are larger than 10-6cm in diameter
2- particles are big enough to be seen with naked eye.
Solute particles cannot pass through filter paper
Question: 7
Define solution. Describe its components with suitable examples
Answer: 7
7-21
Definition; " a solution is a homogenous mixture of two or more substances".
Or
" a homogenous mixture of two or more substances is called a solution".
Example: gas-gas solution: air: solution of different gases
solid-solid solution: brass: solid solution of Zn and Cu
liquid-liquid solution: salt or sugar dissolved in water
Question: 8
Describe some important characteristics of a solution
Answer: 8
8-21
Characteristics of a solution: a true solution must have the following characteristics.
  1. A solution must be homogeneous mixture.
  2. It shows the properties of its components
  3. The boundaries of the components cant be distinguished i.e. a solution exist in one phase
  4. Solutions have variable composition
  5. The solute particles will not settle down
  6. A true solution is transparent , through it may be colored
  7. The solution as whole must be electrically neutral
  8. the solute and solvent may be separated by physical means
  9. Example: air, soft drinks, alloys, sea water etc
  10. Solutions are found in three physical states depending upon the physical state of solvent e.g.
  • Alloy is a solid solution
  • Sea water is liquid solution
  • Air is a gaseous solution
Question: 9
What is meant by aqueous solution? distinguish between dilute and concentrated solution.
Answer: 9
9-21
Aqueous solution:
Definition: " the solution which is formed by dissolving a substance in water is called an aqueous solution". It is the solution in which solvent is water.
Examples:
  • Sugar in water
  • Table salt in water
  • CuSO4 in water
  • Alcohol in water
Question: 10
Briefly describe the saturated solution , unsaturated solution and supersaturated solution with suitable examples.<div>Or</div><div>Describe the various type of solution which based on " the extent of solute solubility".</div>
Answer: 10
10-21
  • Saturated solution:
Definition: " a solution containing maximum amount of solute at a given temperature is called saturated solution".
Or
" a solution in which non more quantity of the solute can be dissolved at room temperature is called saturated solution".
On the particle level; a saturated solution is the one, in which un-dissolved solute is in equilibrium with dissolved solute.
Question: 11
Give different types of solution according to the nature of solute and solvent.
Answer: 11
11-21
Definition: " solution are the homogeneous mixture of two or more components".
Generally , solution are found in three physical state depending upon the physical state of solvent.
So the solvent as well as solute may exist as gas, liquid or solid.
Depending upon the nature of solute and solvent nine different types of solutions may form.
Question: 12
Define molarity? explain it in detial.
Answer: 12
12-21
Molarity: " it is a concentration unit defined as number of moles of solute dissolved in one dm3 of solution".
Question: 13
Differentiate dilute solution and concentrated solution.
Answer: 13
13-21
Dilute solution; the solution are classified as dilute or concentrated on the bases of relative amount of solute present in them. Dilute solutions are those which contain relatively small amount of dissolved solute in the solution.
Question: 14
Difference between suspension and colloid?
Answer: 14
14-21
Colloid:
  1. The particles are large consisting of many atoms ions or molecules
  2. Particles are large but cant be seen with naked eye
  3. Although particles are big but they can pass through a filter paper
  4. Particles scatter the path of light i.e. exhibit the tyndall effect
Question: 15
Explain percentage in three different ways
Answer: 15
15-21
Percentage: percentage unit of concentration refers to be percentage of solute preset in a solution. The percentage of solute can be expressed by mass or by volume.
Question: 16
Explain solubility and its factors.
Answer: 16
16-21
Solubility: solubility is defined as the number of grams of the solute dissolved in 100g of solvent to prepare a saturated solution at a particular temperature
Factors:
  • The general principle of solubility is , like dissolve like.
  • The polar substances are soluble in polar solvents, ionic solids and polar covalent compounds are soluble in water. e.g. KCl, Na2CO3, CuSO4 , sugar and alcohol are soluble in water.
  • Non-polar substances are not soluble in polar solvents. Non-polar covalent compounds are not soluble in water such as ether , benzene are insoluble in water.
  • Non-polar covalent substances are soluble in non-polar solvent( mostly organic solvents). Grease, paint , naphthalene are soluble in ether or carbon tetrachloride etc.
  • solute solvent interaction
  • Temperature
Question: 17
Write down the effect of temperature on solubility
Answer: 17
17-21
Effect of temperature on solubility: temperature has major effect on the solubility of most of the substances . Generally, it seems that solubility increase with the increase of temperatures but it is not always true. When a solution is formed by adding a salt in solvent, there are different possibilities with reference to effect of temperature on solubility these possibilities are discussed here
Question: 18
Write down the effect of temperature on solubility
Answer: 18
18-21
Effect of temperature on solubility: temperature has major effect on the solubility of most of the substances . Generally, it seems that solubility increase with the increase of temperatures but it is not always true. When a solution is formed by adding a salt in solvent, there are different possibilities with reference to effect of temperature on solubility these possibilities are discussed here
Question: 19
Define solutions, colloids and suspensions and explain with examples.
Answer: 19
19-21
Solution: solutions are the homogeneous mixtures of tow or more than two components.
Each component is mixed in such a way that their individual identity is not visible.
Example: the simplest example is that of a drop of ink mixed in water. This is an example of true solution.
Question: 20
Give comparison between solution, colloids and suspensions.
Answer: 20
20-21
Comparison of solution , colloids and suspension:
Solution:
  1. Particles dissolve uniformly throughout and from a homogenous mixture
  2. Particles are too small to see with naked eye less than 1 nanometer =0.000000001m) or 10-8cm diameter
  3. Solute particles will pass through a filter paper and a semi permeable membrane ; cannot be separated except through distillation
  4. Particles are so small that they cannot scatter the rays of light, thus do not show Tyndall effect
  5. Homogenous mixture
Question: 21
Explain dilution of solution
Answer: 21
21-21
Dilution of solution: dilute molar solution is prepared from a concentrated solution of known molarity as explained below: suppose we want to prepare 100cm3 of 0.0 M solution from given 0.1 m solution of potassium permanganate .First 0.1M solution is prepared by dissolving 15.8 g of potassium permanganate in 1dm3 of solution. Then 0.01 M solution is prepared.
Concentration solution of KMnO4 has dense purple color. Take 10cm3 of this solution with the help of a graduated pipette and put in a measuring flask of 100cm3 . Add water up to the mark present at the neck of the flask. Now it is 0.01 molar solution of KMnO4.