SELINA Solutions for Class 9 Chemistry Chapter 3 - Water

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Chapter 3 - Water Exercise Ex. 3(A)

Question 1

Water exists in all three states. Discuss.

Solution 1

In the free state, water occurs in the solid, liquid and gaseous states.

  1. Solid state: A large amount of fresh water is found in the form of snow or ice.
  2. Liquid state: Most of the water present in oceans and found in streams, rivers, lakes, ponds and springs on land is water in the liquid state.
  3. Gaseous state: Water vapour present in the air is in the gaseous state. Water vapour condenses in the sky to form clouds. Mist and fog are also examples of water in the gaseous form.
Question 2

Why is water considered a compound?

Solution 2

Water is considered a compound because it is made of two elements hydrogen and oxygen combined in the ratio 1:8 by mass.

Mass ratio of elements H2O

 H : O, 2 × 1 : 16 × 1 = 1 : 8

(Atomic mass of H = 1, O = 16)

Components of water cannot be separated by physical methods but can be separated by electrolysis of water. 

Question 3
  1. Why does temperature in Mumbai and Chennai not fall as low as it does in Delhi?
  2. Give the properties of water responsible for controlling the temperature of our body.
Solution 3

a) The temperature in Mumbai and Chennai do not fall as low as in Delhi because these cities are situated in the coastal areas. Due to high specific heat capacity, the presence of a large amount of water is able to modify the climate of the nearby land areas making them warmer in winter and cooler in summer. So, the temperature does not fall as low as it does in Delhi.

b) Our body is almost 65% of water, and it has the property of specific heat. Due to high specific heat capacity, the presence of a large amount of water is able to modify the climate of the body and control the temperature of our body, which is warm in winter and cool in summer.

Question 4

'Water is the universal solvent'. Comment.

Solution 4

Water dissolves many substances forming an aqueous solution. It can dissolve solids, liquids and gases. When a solid dissolves in water, the solid is the solute, the water is the solvent and the resultant liquid is the solution. So, it is said that water is a universal solvent. In other words, water can dissolve nearly every substance. 

Question 5

What causes the violence associated with torrential rain?

Solution 5

The sudden release of the latent heat of condensation causes the violence associated with torrential rain. 

Question 6
  1. Which property of water enables it to modify the climate?
  2. Density of water varies with temperature. What are its consequences?
  3. What is the effect of impurities present in the water on the melting point and boiling point of water?
Solution 6
  1. Due to the high specific heat capacity, the presence of a large amount of water is able to modify the climate.

 

  1. The property of anomalous expansion of water enables marine life to exist in the colder regions of the world, because even when water freezes on the top, it is still liquid below the ice layer, as the density of water is greater than that of ice.

 

  1. The boiling point of water increases due to the presence of dissolved impurities.

The freezing point of water decreases due to the presence of dissolved impurities.

 

Question 7

How do fishes and aquatic animals survive when the pond gets covered with thick ice?

Solution 7

Water has an unusual physical property. When cooled, it first contracts in volume, as do other liquids, but at 4°C (maximum density), it starts expanding, and continues to do so till the temperature reaches 0°C, the point at which it freezes into ice.

The property of anomalous expansion of water enables marine life to exist in the colder regions of the world, because even when the water freezes on the surface, it is still liquid below the ice layer.

  

Formation of ice on the water surface of a pond 

 

Question 8

The properties of water are different from the properties of the elements of which it is formed. Discuss.

Solution 8

Properties of water are different from the properties of elements from which it is formed.

Property

Water

Elements - Oxygen and Hydrogen

Nature

It is a clear, colourless, odourless, tasteless and transparent liquid.

These are colourless, odourless, tasteless and non-poisonous gases.

Solubility

It can dissolve many substances and is called a universal solvent.

Oxygen and hydrogen are slightly soluble in water.

Density

Pure water has maximum density at 4°C.

Oxygen is heavier than air, and hydrogen is the lightest of all the known gases.

 

Question 9

How is aquatic life benefited by the fact that water has maximum density at 4oC?

Solution 9

The property of anomalous expansion of water enables aquatic life to exist because water freezes on the surface of the water body, but it is still liquid below the ice layer. 

Question 10

What are the observations and conclusions when tap water is boiled and evaporated? 

Solution 10

When tap water is boiled and evaporated:

Observations:

 A number of concentric rings of solid matter are seen on the watch glass after evaporation of tap water.

Conclusion:

 Tap water contains dissolved salts, minerals and impurities.

Question 11

What is the importance of dissolved salts in water?

Solution 11

Importance of dissolved salts in water:

  • Dissolved salts provide specific taste to water.
  • Dissolved salts act as micronutrients for the growth and development of living beings.
Question 12

State the importance of the suitability of CO2 and O2 in water.

Solution 12

They add taste to water for drinking purposes.

Question 13

How is air dissolved in water different from ordinary air?

Solution 13

Oxygen is more soluble in water than nitrogen. Air dissolved in water contains a higher percentage of oxygen (30-35%). Oxygen is only 21% in ordinary air. In this way, air dissolved in water is different from ordinary air. 

Question 14

Explain what you understand from the following diagram:

  

Solution 14
  1. When a solid changes into a liquid, it absorbs heat equal to the latent heat of fusion. When a liquid changes into a solid, it loses heat equal to the latent heat of solidification.
  2. When a liquid changes into a gas, it absorbs heat equal to the latent heat of vaporisation. When a gas condenses into a liquid, it loses heat equal to the latent heat of condensation.
Question 15

Explain why:

  1. Boiled or distilled water tastes flat.
  2. Ice at zero degrees centigrade has greater cooling effect than water at 0oC.
  3. Burns caused by steam are more severe than burns caused by boiling water.
  4. Rivers and lakes do not freeze easily?
  5. Air dissolved in water contains a higher proportion of oxygen.
  6. If distilled water is kept in a sealed bottle for a long time, it leaves etchings on the surface of the glass.
  7. Rain water does not leave behind concentric rings when boiled.
Solution 15
  1. Boiled water tastes flat because it does not contain dissolved matter such as air, carbon dioxide and other minerals.

 

  1. Ice at 0°C gives more cooling effect than water at 0°C because at 0°C ice absorbs 336 J per gram of energy to melt to 0°C water.

 

  1. Burns caused by steam are more severe than burns caused by boiling water because of high specific latent heat of condensation. 2268 J/g of heat is released when 1 g of steam condenses to form 1 gm of water.
  2. Due to the high specific latent heat of solidification of water, rivers and lakes do not freeze easily.

 

  1. Air dissolved in water contains a higher percentage of oxygen because the solubility of oxygen in water is more than that of oxygen in air.

 

  1. If distilled water is kept in a sealed bottle for a long time, it etches the surface of glass because substances which are apparently insoluble in water actually dissolve in minute traces in water.

 

  1. Rain water does not leave concentric rings when boiled because rain water does not contain dissolved solids.

Chapter 3 - Water Exercise Ex. 3(B)

Question 1

Explain the terms:

  1. Solution
  2. Solute
  3. Solvent
Solution 1
  1. Solution: A solution is a homogeneous mixture of two or more substances, the components of which cannot be seen separately.
  2. Solute: A solute is the substance which dissolves in a solvent to form a solution.
  3. Solvent: A solvent is the medium in which a solute dissolves.

 Solution = Solute + Solvent

 

Question 2

Explain why a hot saturated solution of potassium nitrate forms crystals as it cools.

Solution 2

Solubility of nitrates decreases with a fall in temperature. Thus, when a hot saturated solution of potassium nitrate cools, it forms crystals as it separates from the solution. 

Question 3

Give three factors which affect the solubility of a solid solute in a solvent.

Solution 3

Three factors on which the solubility of a solid depend:

  1. Temperature
  2. Nature of the solid
  3. Nature of the solvent
Question 4

(a) If you are given some copper sulphate crystals, how would you proceed to prepare its saturated solution at room temperature?


(b) How can you show that your solution is really saturated?

Solution 4
  1. Take 100 g of distilled water in a beaker. Add to this one gram of copper sulphate crystals.
  2. Stir this mixture with the help of a glass rod and dissolve the copper sulphate crystals. Similarly, go on dissolving more copper sulphate (1 gram at a time) with constant and vigorous stirring. A stage is reached when no more copper sulphate dissolves. It is called a saturated solution at this temperature.
Question 5
  1. Define (i) Henry's law and (ii) Crystallisation.
  2. State the different methods of crystallisation.
Solution 5
  1.  
    1. Henry's law: At any given temperature, the mass of a gas dissolved in a fixed volume of a liquid or solution is directly proportional to the pressure on the surface of a liquid.
    2. Crystallisation: It is the process by which crystals of a substance separate out on cooling its hot saturated solution.

 

  1. In the laboratory, crystals may be obtained by the following methods: 
    1. By cooling a hot saturated solution gently
    2. By cooling a fused mass
    3. By sublimation
    4. By slowly evaporating a saturated solution
Question 6

What would you observe when crystals of copper (II) sulphate and iron (II) sulphate are separately heated in two test tubes?

Solution 6

Action of heat on copper (II) sulphate crystals

When copper (II) sulphate crystals are heated in a hard glass test tube, the following observations are observed:

  

Action of heat on copper (II) sulphate 

 

  1. The crystals are converted to a powdery substance.
  2. The crystals lose their blue coloration on further heating.
  3. Steaming vapours are produced inside the tube which condense near the mouth of the tube to form a colourless liquid.
  4. On further heating, steam escapes from the mouth of the tube and water gets collected in a beaker placed under the mouth of the tube.
  5. On further heating, the residue changes to a white powder and steam stops coming out.

CuSO4.5H2O   CuSO4 + 5H2O

 

 

Action of heat on iron (II) sulphate

When iron (II) sulphate is heated in a test tube, the following is observed:

  1. The crystals crumble to a white powder and a large amount of steam and gas are given out.
  2. On strong heating, a brown residue of ferric oxide (Fe2O3) is produced and a mixture of SO2 and SO3 is given off.

FeSO4.7H2O   FeSO4 + 7H2O

 

2FeSO4   Fe2O3 + SO2  + SO3

 

Question 7

Give the names and formulae of two substances in each case:

  1. Hydrated substance
  2. Anhydrous substance
  3. Liquid drying agent
  4. A basic drying agent
Solution 7
  1.  

 i. Washing soda crystals: Na2CO3.10H2O

 ii. Blue vitriol: CuSO4.5 H2O

  1.  

 i. Table salt: NaCl

 ii. Nitre: KNO3

  1. Sulphuric acid: H2SO4
  2. Quick lime: CaO
Question 8

What is the effect of temperature on solubility of KNO3 and CaSO4 in water?

Solution 8

Solubility of potassium nitrate (KNO3) in water increases with an increase in temperature.

Solubility of calcium sulphate (CaSO4) in water decreases with an increase in temperature. 

Question 9

Solubility of NaCl at 40oC is 36.5 g. What is meant by this statement?

Solution 9

Solubility of NaCl at 40°C is 36.5 g means that 36.5 g of NaCl dissolves in 100 g of water at a temperature of 40°C. 

Question 10

Which test will you carry out to find out if a given solution is saturated or unsaturated or supersaturated?

Solution 10
  1. A solution in which more of a solute can be dissolved at a given temperature is an unsaturated solution.
  2. A solution in which no more solute can be dissolved at a given temperature is a saturated solution at that temperature.
  3. A solution in which some solute separates on cooling slightly is a super saturated solution.
Question 11

What is the effect of pressure on solubility of gases? Explain with an example.

Solution 11

With an increase in pressure, the solubility of a gas in water increases.

With an increase in temperature, the solubility of a gas in water decreases.

For example, the solubility of carbon dioxide in water under normal atmospheric pressure is low, but when the water surface is subjected to higher pressure, a lot more of CO2 gas gets dissolved in it.

Similarly, in case of soda water, on opening the bottle, the dissolved gas rapidly bubbles out because the pressure on the surface of the water suddenly decreases. 

Question 12

State the term:

  1. A solution where solvent is a liquid other than water.
  2. When a substance absorbs moisture on exposure to moist air and dissolves in the absorbed water and turned to solution.
  3. A substance which contains water of crystallisation.
  4. When a substance absorbs moisture from the atmosphere but does not form a solution.
  5. When a compound loses its water of crystallisation on exposure to dry air.
  6. The substance that can remove hydrogen and oxygen atoms in the ratio of 2:1(in the form of water) from the compound.
Solution 12
  1. Non-aqueous solution
  2. Deliquescence
  3. Hydrated substance
  4. Hygroscopy
  5. Efflorescence
  6. Dehydrating agent
Question 13

Explain why:

  1. Water is an excellent liquid to use in cooling systems.
  2. A solution is always clear and transparent.
  3. Lakes and rivers do not suddenly freeze in the winters.
  4. The solute cannot be separated from a solution by filtration.
  5. Fused CaCl2 or conc. H2SO4 is used in a desiccator.
  6. Effervescence is seen on opening a bottle of soda water.
  7. Table salts become sticky on exposure to humid air during the rainy season.
Solution 13
  1. Water is an excellent liquid to use in cooling systems because of its high specific heat.

 

  1. A water-soluble solid disappears in a solution where the solvent is water, and water has the property of being clear and transparent. So, the solution is also clear and transparent.

 

  1. Lakes and rivers do not freeze suddenly in winters because of the high specific latent heat of solidification, i.e. the amount of heat released when 1 g of water solidifies to form 1 g of ice at 0°C. It is about 336 J/g or 80 cal/g.

 

  1. The component which dissolves in a solvent is known as a solute. So, it cannot be separated from a solution by filtration. However, filtration is used when the solute is insoluble in the solution.

 

  1. Fused CaCl2 or concentrated H2SO4 is deliquescent in nature, i.e. it absorbs moisture, and hence, these are used in desiccators as drying agents.

 

  1. Carbon dioxide is dissolved in soda water under pressure. On opening the bottle, the pressure on the surface of water suddenly decreases; therefore, the solubility of CO2 in water decreases and the gas rapidly bubbles out.

 

  1. Table salt becomes sticky on exposure during the rainy season, because it generally contains a small percentage of magnesium chloride and calcium chloride as impurities. These impurities absorb moisture from the monsoon air due to their deliquescent nature, and thus, table salt become sticky.
Question 14

Normally, solubility of crystalline solid increases with temperature. Does it increase uniformly in all cases? Name a substance whose solubility:

  1. Increases rapidly with temperature.
  2. Increases gradually with temperature.
  3. Increases slightly with temperature.
  4. Initially increases then decreases with rise in temperature.
Solution 14
  1. Potassium nitrate
  2. Potassium chloride
  3. Sodium chloride
  4. Calcium sulphate
Question 15

What are drying or desiccating agents? Give examples.

Solution 15

These are substances which can readily absorb moisture from other substances without chemically reacting with them.

Examples:

Phosphorous pentoxide (P2O5), quick lime (CaO) 

Question 16

Complete the following table:

Common Name

Chemical Name

Formula

Acid, base or salt

Efflorescent,

hygroscopic or deliquescent substance

Solid caustic potash

 

 

 

 

Quick lime

 

 

 

 

Oil of vitriol

 

 

 

 

Washing soda

 

 

 

 

Solid caustic soda

 

 

 

 

Blue vitriol

 

 

 

 

 

Solution 16

 

 

Common Name

Chemical Name

Formula

Acid, base or salt

Efflorescent,

hygroscopic or deliquescent substance

Solid caustic potash

Potassium hydroxide

KOH

Base

Deliquescent substance

Quick lime

Calcium oxide

CaO 

Base

Hygroscopic substance

Oil of vitriol

Sulphuric acid

H2SO4

Acid

Hygroscopic substance

Washing soda

Hydrated sodium carbonate

Na2CO3.10H2O

Salt

Efflorescent substance

Solid caustic soda

Sodium hydroxide

NaOH

Base

Deliquescent substance

Blue vitriol

 Copper sulphate

 CuSO4

 Salt

 Efflorescent substance

 

Question 17

In which of the following substances will there be

  1. Increase in mass
  2. Decrease in mass
  3. No change in mass when they are exposed to air?

 

  1. Sodium chloride
  2. Iron
  3. Conc. sulphuric acid
  4. Table salt
  5. Sodium carbonate crystals
Solution 17
  1. Increase in mass: Iron and conc. sulphuric acid
  2. Decrease in mass: Sodium carbonate crystals
  3. No change in mass: Sodium chloride
Question 18

State the methods by which hydrated salts can be made anhydrous.

Solution 18

Hydrated salts can be converted to anhydrous substances by heating and also when exposed to dry air.

Example:

Glauber's salt becomes powdery anhydrous sodium sulphate when exposed to dry air.

 

Chapter 3 - Water Exercise Ex. 3(C)

Question 1

What is the composition of water? In what volume its elements combine?

Solution 1

The composition of water is 2 atoms of hydrogen with 1 atom of oxygen (H2O).

By number of atoms, they combine in the ratio 2:1.

Question 2

What is the use of solubility of oxygen and carbon dioxide in water?

Solution 2

Air dissolved in water is biologically very important.

 Oxygen dissolved in water is used by marine life like fish for respiration, and thus, marine life is sustained.

 Aquatic plants make use of dissolved carbon dioxide in photosynthesis to prepare food.

 Carbon dioxide dissolved in water reacts with calcium carbonate to form calcium bicarbonate.

Marine organisms such as oysters and snails extract calcium carbonate from calcium bicarbonate to build their shells.

Question 3

Hot saturated solution of sodium nitrate forms crystals as it cools. Why?

Solution 3

Solubility of sodium nitrate decreases with a fall in temperature. Thus, when a hot saturated solution of sodium nitrate cools, it forms crystals as it separates from the solution. 

Question 4

What are hydrous substances? Explain with examples.

Solution 4

Substances which contain water molecules along with salt are hydrated substances.

Examples: Sodium carbonate decahydrate: Na2CO3.10H2O

 Copper sulphate pentahydrate: CuSO4.5H2O

Question 5

Name three methods[CM1]  by which hydrous substances can be made anhydrous.

Solution 5

Methods by which hydrous substances can be made anhydrous:

  • By heating
  • Exposure to dry air
Question 6

What is the importance of dissolved impurities in water?

Solution 6

The dissolved impurities in water are salts and minerals.

  • Dissolved salts provide specific taste to water.
  • Salts and minerals are essential for growth and development.
  • They supply the essential minerals needed by our body.
Question 7

State two ways by which a saturated solution can be changed to unsaturated solution.

Solution 7
  • On heating, a saturated solution becomes unsaturated and more solute can be dissolved in the solution.
  • By adding more solvent, a saturated solution can be made unsaturated.
Question 8

What do you understand by

  1. Soft water
  2. Hard water
  3. Temporary hard water
  4. Permanent hard water
Solution 8
  1. Water is said to be soft when the water containing sodium salts easily gives lather with soap.
  2. Water is said to be hard when it does not readily form lather with soap.
  3. Water which contains only hydrogen carbonates of calcium and magnesium is called temporary hard water.
  4. Water containing sulphates and chlorides of magnesium and calcium is called permanent hard water.
Question 9

What are the causes for

  1. Temporary hardness
  2. Permanent hardness
Solution 9
  1. The presence of hydrogen carbonates of calcium and magnesium makes water temporarily hard.
  2. The presence of sulphates and chlorides of magnesium and calcium makes water permanently hard.
Question 10

What are the advantages of (i) soft water and (ii) hard water?

Solution 10
  1. Advantages of soft water:
    • When the water is soft, you use much less soap and fewer cleaning products. Your budget will reflect your savings.
    • Plumbing will last longer. Soft water is low in mineral content and therefore does not leave deposits in the pipes.
    • Clothes last longer and remain bright longer if they are washed in soft water.
  1. Advantages of hard water:
    • Water free from dissolved salts has a very flat taste. The presence of salts in hard water makes it tasty. So, hard water is used in making beverages and wines.
    • Calcium and magnesium salts present in small amounts in hard water are essential for bone and teeth development.
    • Hard water checks the poisoning of water by lead pipes. When these pipes are used for carrying water, some lead salts dissolve in water to make it poisonous. Calcium sulphate present in hard water forms insoluble lead sulphate in the form of a layer inside the lead pipe and this checks lead poisoning.

 

Question 11

What are stalgmites and stalactites? How are they formed?

Solution 11

In some limestone caves, conical pillar-like objects hang from the roof and some rise from the floor. These are formed by water containing dissolved calcium hydrogen carbonate continuously dropping from the cracks in the rocks. Release of pressure results in the conversion of some hydrogen carbonate to calcium carbonate.

Ca(HCO3)2  CaCO3 + CO2 + H2O

This calcium carbonate little by little and slowly deposit on both roof and floor of the cave.

The conical pillar which grows downwards from the roof is called stalactite and the one which grows upward from the floor of the cave is called stalagmite.

These meet after a time. In a year, some grow less than even a centimetre, but some may be as tall as 100 cm.

CaCO3 + CO2 + H2O Ca(HCO3)2

MgCO3 + CO2 + H2O Mg(HCO3)2

If the water flows over beds of gypsum (CaSO4.2H2O), a little bit of gypsum gets dissolved in water and makes it hard.

Question 12

Name the substance which makes water (i) temporarily hard and (ii) permanently hard.

Solution 12
  1. Hydrogen carbonates of calcium and magnesium
  2. Sulphates and chlorides of magnesium and calcium
Question 13

Give equations to show what happens when temporary hard water is

  1. Boiled
  2. Treated with slaked lime
Solution 13
  1. Ca(HCO3)2   CaCO3 + H2O + CO2

Mg(HCO3)2   MgCO3 + H2O + CO2

  1. Ca(HCO3)2 + Ca(OH)2   2CaCO3 + 2H2O  

Mg(HCO3)2+ Ca(OH)2   MgCO3 + 2H2O  

 

Question 14

State the disadvantages of using hard water.

Solution 14
  • It is more difficult to form lather with soap.
  • Scum may form in a reaction with soap, wasting the soap.
  • Carbonates of calcium and magnesium form inside kettles. This wastes energy whenever you boil a kettle.
  • Hot water pipes 'fur up'. Carbonates of calcium and magnesium start to coat the inside of pipes which can eventually get blocked.
Question 15

What is soap? For what is it used?

Solution 15

Soap is chemically a sodium salt of stearic acid (an organic acid with the formula C17H35COOH) and has the formula C17H35COONa.

Soap is used for washing purposes.

Question 16

What is the advantage of a detergent over soap?

Solution 16

Detergents are more soluble in water than soap and are unaffected by the hardness of water as their calcium salts are soluble in water.

Question 17

Why does the hardness of water render it unfit for use in a (i) boiler and (ii) for washing purposes.

Solution 17
  1. Steam is usually made in boilers which are made of a number of narrow copper tubes surrounded by fire. As the cold water enters these tubes, it is immediately changed into steam, while the dissolved solids incapable of changing into vapour deposit on the inner walls of the tubes. This goes on and makes the bore of the tubes narrower. The result is that less water flows through the tubes at one time and less steam is produced. When the bore of the tube becomes very narrow, the pressure of the steam increases so much that at times the boiler bursts.
  2. If hard water is used, calcium and magnesium ions of the water combine with the negative ions of the soap to form a slimy precipitate of insoluble calcium and magnesium usually called soap curd (scum).

Formation of soap curd will go on as long as calcium and magnesium ions are present. Till then, no soap lather will be formed and cleaning of clothes or body will not be possible. Moreover, these precipitates are difficult to wash from fabrics and sometimes form rusty spots if iron salts are present in water.

Question 18

Explain with equation, what is noticed when permanent hard water is treated with

  1. Slaked time
  2. Washing soda
Solution 18
  1. Slaked lime

Ca(HCO3)2 + Ca(OH)2  2CaCO3 + 2H2O  

Mg(HCO3)2+ Ca(OH)2   MgCO3 + CaCO3 + 2H2O  

Lime is first thoroughly mixed with water in a tank and then fed into another tank containing hard water. Revolving paddles thoroughly mix the two solutions. Most of the calcium carbonate settles down. If there is any solid left over, it is removed by a filter. This is known as Clarke's process.

  1. Washing soda

When washing soda or soda ash is added to hard water, the corresponding insoluble carbonates settle down and can be removed by filtration.

Ca(HCO3)2 + Na2CO3  CaCO3 + 2NaHCO3 

Mg(HCO3)2+ Na2CO3  MgCO3 + 2NaHCO3

Question 19

Explain the permutit method for softening hard water.

Solution 19

Permutit is an artificial zeolite. Chemically, it is hydrated sodium aluminium orthosilicate with the formula Na2Al2Si2O8.XH2O. For the sake of convenience, let us give it the formula Na2P.

  

A tall cylinder is loosely filled with lumps of permutit. When hard water containing calcium and magnesium ions percolates through these lumps, ions exchange. Sodium permutit is slowly changed into calcium and magnesium permutit, and the water becomes soft with the removal of calcium and magnesium ions.

When no longer active, permutit is regenerated by running a concentrated solution of brine over it and removing calcium chloride formed by repeated washing.

CaP + 2NaCl Na2P + CaI2