10th class Science Salts a neutral substance

In chemistry, salts are ionic compounds that can result from the neutralization reaction of an acid and a base according to Arrhenius concept.

 They are composed of cations (positively charged ions) and anions (negatively charged ions) so that the product is electrically neutral (without a net charge).

These component ions can be inorganic such as chloride (Cl−), as well as organic such as acetate (CH3COO−) and monatomic ions such as fluoride (F−) as well as polyatomic ions such as sulfate (SO42−).

Classification of salts: Salts are classified as follows.

(i) Normal salt - The salt which does not contain any ionizable or replaceable hydrogen atom in its molecule is called a normal salt. It is produced by complete replacement of all the obtainable hydrogen ions by metallic or ammonium ions e.g. NaCl, K2SO4 .

NaOH + HCl → NaCl + H2O ; 2 KOH + H2SO4 → K2SO4 + 2 H2O

(ii) Acid salts - The salt which contains one or more replaceable hydrogen ions in its molecule is called an acid salt. It is produced by the partial replacement of the obtainable hydrogen ions by metallic or ammonium ions. Acid salts ionise in water giving hydronium ions ( H3O) +. e.g. Na2HPO4 , KHSO4

2 NaOH + H3PO4 → Na2HPO4 + 2 H2O ; KOH + H2SO4 → KHSO4 + H2O

An acid salt can react with a base to form a normal salt.

(iii) Basic salts – The salt which contains one or more replaceable hydroxide ions in its molecule is called a basic salt. It is produced by the partial replacement of the obtainable hydroxide ions by acidic radicals. Basic salts ionize in water to give OH – ions. e.g. Mg(OH)Cl, Pb(OH) NO3

Mg(OH)2 + HCl → Mg(OH) Cl + H2O ; Pb(OH)2 + HNO3 → Pb(OH)NO3 + H2O

A basic salt can react with an acid to form a normal salt.

(iv) Mixed salt – A salt which contains more than one acidic or basic radicals, other than hydrogen or hydroxyl ion, in its molecule is called a mixed salt. e.g. Ca(OCl) Cl, NaKSO4 . Mixed salts are prepared by different methods.

Ca(OH)2 + Cl2 → Ca(OCl) Cl + H2O ; NaOH + KOH + H2SO4 → NaKSO4 + 2 H2O

(v) Double salt - A salt which is formed by the combination of two simple salts is called a double salt. Such a salt is formed when the two salts are slowly crystallized together from a mixture of their saturated salt solution. e.g. saturated solutions of KCl and

MgCl2 on crystallization form a double salt KCl,MgCl2,6H2O. Similarly, saturated solutions of FeSO4 and (NH4)2SO4 on crystallization form a double salt FeSO4 (NH4)2SO4. 6 H2O.

KCl + MgCl2. 6 H2O --- H2O ----→ KCl. MgCl2. 6 H2O

FeSO4 7 H2O + (NH4)2SO4 --- H2O-------→ FeSO4. (NH4)2SO4 . 6 H2O

(vi) Complex salt - The salt which contains a simple ion and a complex ion is called a complex salt. It is formed by the combination of two simple salts under proper experimental conditions. Examples of complex salts include [Co(NH3)6] Cl3 , K4 [Fe(CN)6].

CoCl3 + 6 NH3 → [Co(NH3)6] Cl3 ; Fe(CN)2 + 4 KCN → K4 [Fe(CN)6]

This salt dissociates in water to give a simple ion and a complex ion. The ion which contains both metallic and non-metallic ions together which do not dissociate in water is called a complex ion.

[Co(NH3)6] Cl3 → [Co(NH3)6] 3 + + 3 Cl - ; K4 [Fe(CN)6] → 4 K+ + [Fe(CN)6] 4 –

In aqueous medium, only the simple ion gives its characteristic tests.

Acidic salts and basic salts are defined in an alternative way also.

1) Basic salts - Salts that hydrolyze to produce hydroxide ions when dissolved in water are called basic salts . These salts react with water to produce alkalinity in the solution.

Such salts are prepared by the reaction between a strong base and a weak acid. For example, sodium carbonate is a salt of strong base NaOH and weak acid H2CO3 . This salt hydrolyses in water to produce OH – ions. Hence though it does not contain OH – ion, sodium carbonate is a basic salt.

Na2CO3 + 2 H2O → 2 Na+ + 2 OH - + H2CO3

Other examples of such salts include KCN, CH3COONa, Na3PO4 .

2) Acidic salts - Salts that hydrolyze to produce H + ions when dissolved in water are called acidic salts. These salts react with water to produce acidity in the solution. Such salts are made by the reaction between a strong acid and weak base.

For example, ammonium chloride is a salt of strong acid HCl and a weak base NH4OH. This salt hydrolyzes in water to produce H + ions . Hence though it does not contain H + ion, ammonium chloride is an acidic salt.

NH4Cl + H2O → NH4OH + H + + Cl –

Other examples of such salts include FeCl3 , Al2(SO4)3, NH4NO3 .

3) Neutral salts – Salts that do not hydrolyze when dissolved in water are called neutral salts. All normal salts are neutral salts. Such salts are made by the reaction between a strong acid and a strong base. For example, sodium chloride is a salt of strong base NaOH and strong acid HCl. On dissolution in water, the base and acid fully ionize and produce equal number of H + and OH – ions. Hence this salt solution is neither acidic nor basic i.e. it is neutral.

NaOH + HCl → Na+ + OH - + H + + Cl –

Other examples of such salts include KCl , K2SO4, NaNO3 .

Uses of salts Many salts find use in day to day life.

1) Potassium permanganate and potash alum are used to purify water.

2) Magnesium sulphate ( Epsom salt ) is used in purgatives.

3) Baking soda is used in cooking so also as a mild antacid.

4) Common salt is added to add taste to our food.

5) Plaster of paris is used for making statues and for false ceiling.

6) Ammonium sulphate, ammonium nitrate and some phosphates are used as fertilizers.

7) Silver bromide is used in photography.

8) Calcium carbonate is used in making chalk powder.

Typical properties of some water soluble salts

(i) Water of crystallization - 

Several salts contain definite amount of water molecules loosely combined in their structure. This chemically combined water present in the salt accounts for the crystalline nature of the salt. Hence this water is called ‘water of crystallization’. Salts containing water of crystallization are called hydrated salts. The examples of hydrated salts include FeSO4. 7 H2O, CuSO4. 5 H2O, Na2CO3. 10 H2O.

(ii) Efflorescence - 

Certain hydrated crystals, when exposed to the atmosphere at ordinary temperature, lose their water of crystallization and are transformed into a powder. Such substances are called efflorescent substances and the property is called efflorescence. Effloresce is maximum when the temperature is high and the atmosphere is dry. The examples of efflorescent substances include Na2SO4. 10H2O, MgSO4.7 H2O.

(iii) Deliquescence - 

Certain substances, when exposed to the atmosphere at ordinary temperature, absorb moisture from the atmosphere or air . They become moist, lose their crystalline form and ultimately dissolve in the absorbed water forming a saturated solution. Such substances are called deliquescent substances and the property is called deliquescence. Deliquescence is maximum when temperature is low and atmosphere is humid. The examples of deliquescent substances include CaCl2. 6 H2O, Cu(NO3)2. 3 H2O, MgCl2.6 H2O.

(iv) Hygroscopy -

Certain substances, when exposed to the atmosphere at ordinary temperature, absorb moisture from the atmosphere without dissolving in it . Such substances are called hygroscopic substances and the property is called hygroscopy. Hygroscopic substances are generally anhydrous solids or liquids. They are used as drying agents for drying gases. The examples of hygroscopic substances include CaCl2, CaO, Silica gel, Ethyl alcohol.

SSIGNMENT :TERM-1(2012-2013) X - Chemistry

CHEMISTRY : CHEMICAL REACTIONS AND EQUATIONS

CHEMISTRY CHAPTER: ACIDS AND BASES

CHEMISTRY:CHAPTER: METALS AND NON- METALS

ASSIGNMENT:FIRST TERM(2012-2013)X -Physics

Physics: Magnetic effects of currents assignments

Physics : Class X Chapter: ELECTRICITY Assignment

MCQ: Fill in the blanks: Acid base and salt d salt

MCQ	Fill in the blanks:  Acid base and salt d salt
1.	The substances whose aqueous solution change the blue litmus to red ------------------Acids
2.	The substances having a tendency to lose one or more protons are called: ------------   Acids
3.	The substances which donate the pair of electrons for bond formation, are known as:-------     Base
4.	When equivalent quantities of acid and base are mixed, salt and water are formed, the reaction is termed as:----------- Neutralization
5.	The acids which contain one acidic hydrogen are called:-------- Mono-protic
6.	The number of acidic hydrogen atoms present in a molecule of an acid is called: ----  Basicity
7.	The number of replaceable [OH] ions present in a molecule of base, is called: ---    Acidity
8.	An acid that produces large number of (H) ions in aqueous solution is called: ---------Strong acid
9.	An ionic compound, that is formed when an acid neutralizes a base, is called:------ Salt
10.	SaIts that formed by the reaction of strong acid with weak base are:----Acidic
11.	Alums are example of  ---------salt:               Double salts
12.	The formula of Washing Soda is                                                  Na₂CO₃ 6H₂O
13.	Acids are the substances which give H+ ions aqueous solution, is the concept of:   Arrhenius
14.	Arrehenius theory of acid-base is not applicable in:     non — aqueous solution
15.	According to the Arrhenius concept, the strength of acid or base is based on their:   -------- a. rates of ionization          b. rates of dissociation
16	According to Bronsted — Lowry concept, a base is a substance which acts as:      a proton acceptor(NH₃)

X : 10th Acid Base and Salt:Solved Edugain questions

Q. 1.  What happens if sodium hydroxide is added to cupper  ammonium sulphate solution and what is the inference?

Answer:  When sodium hydroxide is added to cupper  ammonium sulphate solution, no blue precipitate of Cu(OH)₂ is seen, which is normally observed for Cu²⁺ ion. Hence it is an example of a complex salt.

Q 2. When lead dioxide reacts with concentrated HCl and produces a salt and water, the reaction is not called a neutral reaction why?

Answer:  For a reaction to be called a neutral reaction the products should be only salt and water. But in the above reaction, Cl₂ gas is also liberated.

Q 3.Define a base and acid in terms of proton.

Answer:  A base is a proton acceptor and an acid is a proton donor.

Q 4. Answer these: 
 1) Name the anions that can be detected in the laboratory using dilute HCl or dilute H₂SO₄ and give the ionic equation common to both reactions.  
2) Which property of the acid is indicated?

Answer:  

Carbonate and Bicarbonate Ions      2H⁺  + CO₃^{2-  ........>}   H₂O + CO₂ ­


Q 5.   1) What do you observe when concentrated H₂SO₄ is added slowly to blue CuSO₄ crystals in a test tube and why? 

2) Is these any other way of observing the above result?

Answer:  1) The blue crystals turn to white amorphous anhydrous powder. Hence concentrated H₂SO₄ acts as a dehydrating agent, removing the water of crystallization molecules from CuSO₄.5H₂O crystals. 

Q6: Name two crystalline salts that do not have water of crystallization.

Answer:  The chlorides of K, Na and Pb and the nitrates of K, Na, Pb, Ag, [NH₄⁺] do not have water of crystallization.

Q 7. Why do acids not show acidic behavior in the absence of water?

Ans: Acids do not show acidic behaviour in absence of water because the dissociation of hydrogen ions from an acid occurs in presence of water only. It is hydrogen ions that are responsible for the acidic behaviour.  

Q 8. How is NH₄OH used as a laboratory reagent?

Answer:  NH₄OH is used to detect cations in their salt solutions by precipitating their hydroxides whose colour and solubility in excess NH₄OH, identifies them. 

Q 9. Name four gases that can be prepared in the laboratory using dilute H₂SO₄. Show how they can be prepared?

Answer:  The four gases are:
 1) H₂ gas            2) CO₂ gas         3) SO₂ gas       4) H₂S gas 

Their respective methods of preparations are: 

2) Any carbonate salt and dilute H₂SO₄ gives CO₂ gas.

3) Any sulphite salt and dilute H₂SO₄ gives SO₂ gas. 
4) Any sulphide salt and dilute H₂SO₄ gives H₂S gas.

Q 10. While diluting concentrated H₂SO₄, what care must be taken and why?

Answer:  While diluting concentrated H₂SO₄ never add water to concentrated acid; instead, add concentrated H₂SO₄ slowly with stirring to the volume of water. As this reaction is highly exothermic the heat produced will splash the acid and may cause burns.

Q 11. What is the cause of tooth decay?

Answer:  The bacteria present in the mouth act on sugar and food particles remaining in the mouth after eating to produce acids. The acid produced lowers the pH in the mouth to 5.5 and begins to attack the hard enamel and corrode it resulting in tooth decay.

Q 12. Plaster of Paris should be stored in a moisture-proof container. Explain why?

Answer:  Plaster of Paris (POP) or calcium sulphate with half a molecule of water per molecule of the salt (hemi-hydrate) is a hygroscopic substance. Should it absorb a little water from the surroundings, it evolves heat and quickly sets to a hard porous mass hence it should be stored in a moisture-proof container to keep it dry

Q.13 A milkman adds a very small amount of baking soda to fresh milk.

(a) Why does he shift the pH of the fresh milk from 6 to slightly alkaline?

(b) Why does this milk take a long time to set as curd?  

Ans: 
 (a) By adding small amount of baking soda, the milkman shifts the pH of the fresh milk from 6 to slightly alkaline so that he can keep it for longer time as the milk in alkaline condition, does not set curd easily.

(b) Since, this milk is slightly basic than the usual milk, acids produced due to bacterial actions in it are neutralized by the base. Therefore, it takes longer time to set as curd.    

Q.14.Give two important uses of washing soda and baking soda.

Ans: Uses of Washing Soda:

1. Sodium carbonate (washing soda) is used in glass, soap, and paper industries.

2. It is used in the manufacture of sodium compounds such as Borax.

Uses of Baking Soda:

1. Sodium hydrogen carbonate is also ingredient in antacids. Being alkaline, it neutralizes excess acid in the stomach and provides relief.2. It is also used in soda-acid fire extinguishers.

3. It is used as baking powder in confectionery items like cake, pastry etc.  

Q. 15. What will happen if a solution of sodium hydrocarbonate is heated? Give the equation of the reaction involved.

Ans. When a solution of sodium hydrocarbonate (sodium hydrogencarbonate) is heated, sodium carbonate and water are formed with the evolution of carbon dioxide gas.

2NaHCO₃    +        heat                  →    Na₂CO₃      +   H₂ O  + CO₂

Q. 16. Equal lengths of magnesium ribbons are taken in test tubes A and B. Hydrochloric acid (HCl) is added to test tube A, while acetic acid (CH₃COOH) is added to test tube B. In which test tube will the fizzing occur more vigorously and why?

Ans: The fizzing will occur strongly in test tube A, in which hydrochloric acid (HCl) is added. This is because HCl is a stronger acid than CH₃COOH and therefore produces hydrogen gas at a faster speed due to which fizzing occurs.

Q17. Plaster of Paris should be stored in a moisture-proof container. Explain why?

Ans. Plaster of Paris (POP) should be stored in a moisture-proof container because Plaster of Paris, a powdery mass, absorbs water (moisture) to form a hard solid known as gypsum.

Ca SO₄ . ½ H₂ O     +   1¹/₂ H₂ O     →   Ca SO₄ . 2 H₂O

Q 18 :Why should curd and sour substances not be kept in brass and copper vessels?

Ans:  Curd and other sour substances contain acids. Therefore, when they are kept in brass and copper vessels, the metal reacts with the acid to liberate hydrogen gas and harmful products, thereby spoiling the food.

Q19. Which gas is usually liberated when an acid reacts with a metal? Illustrate with an example. How will you test for the presence of this gas?

Ans: Hydrogen gas is usually liberated when an acid reacts with a metal.

Take few pieces of zinc granules and add 5 ml of dilute H₂SO₄. Shake it and pass the gas produced into a soap solution. The bubbles of the soap solution are formed. These soap bubbles contain hydrogen gas.                 
2H₂SO₄            +     Zn      →  Zn (SO₄)₂   +  2H₂  

We can test the evolved hydrogen gas by its burning with a pop sound when a candle is brought near the soap bubbles.

Q 20: Metal compound A reacts with dilute hydrochloric acid to produce effervescence. The gas evolved extinguishes a burning candle. Write a balanced chemical equation for the reaction if one of the compounds formed is calcium chloride.

  Ans:     CaCO₃  (s)   +    HCI(aq)    →   CaCI₂(aq) + CO₂   + H₂ O (I)

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10th SA-1-Acid Base and Salt Trend Setter Question Paper

1: Which gas is usually liberated when an acid reacts with a metal? Illustrate with an example. How will you test for the presence of this gas?

Ans: Hydrogen gas is usually liberated when an acid reacts with a metal.fig 2.1 page 19  

Take few pieces of zinc granules and add 5 ml of dilute H₂SO₄. Shake it and pass the gas produced into a soap solution. The bubbles of the soap solution are formed. These soap bubbles contain hydrogen gas.                 

2H₂SO₄    +     Zn   →  Zn(SO₄)₂   +  2H₂  

We can test the evolved hydrogen gas by its burning with a pop sound when a candle is brought near the soap bubbles.

2: Metal compound A reacts with dilute hydrochloric acid to produce effervescence. The gas evolved extinguishes a burning candle. Write a balanced chemical equation for the reaction if one of the compounds formed is calcium chloride.

             CaCO₃  (s)   +    HCI(aq)    →   

CaCI₂(aq) + CO₂   + H₂ O (I)

3 : Why do HCl, HNO₃, etc., show acidic characters in aqueous solutions while solutions of compounds like alcohol and glucose do not show acidic character?

Ans: The dissociation of HCl or HNO₃ to form hydrogen ions always occurs in the presence of water. Hydrogen ions (H⁺) combine with H₂O to form hydronium ions (H₃O⁺).     

HCI -------->   H⁺  +  CI ^–      H⁺     +     H₂ O -->   H₃ O⁺

Although aqueous solutions of glucose and alcohol contain hydrogen, these cannot dissociate in water to form hydrogen ions. Hence, they do not show acidic character.

4  Why does an aqueous solution of an acid conduct electricity?

Ans.:   Acids dissociate in aqueous solutions to form ions. These ions are responsible for conduction of electricity.

5.   Why does dry HCl gas not change the colour of the dry litmus paper?

Ans. : Colour of the litmus paper is changed by the hydrogen ions. Dry HCl gas does not contain H⁺ ions. It is only in the aqueous solution that an acid dissociates to give ions. Since in this case, neither HCl is in the aqueous form nor the litmus paper is wet, therefore, the colour of the litmus paper does not change.

6. While diluting an acid, why is it recommended that the acid should be added to water and not water to the acid?

Ans.:  Since the process of dissolving an acid in water is exothermic, it is always recommended that acid should be added to water. If it is done the other way, then it is possible that because of the large amount of heat generated, the mixture splashes out and causes burns

7: How is the concentration of hydronium ions (H₃O⁺) affected when a solution of an acid is diluted?

Ans. : When an acid is diluted, the concentration of hydronium ions (H₃O⁺) per unit volume decreases. This means that the strength of the acid decreases.

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Salt - The Spice of Life

Salt - The Spice of Life: For every meal there is one thing people generally reach for before they even take a bite – the salt shaker. Salt is one of the oldest spices used and is a key component to humans, animals, and plants.

Its flavor is unique and versatile, salt has been a staple throughout time. Enhancing almost every dish, salt is added to breads, meats, fruits and vegetables to sauces and desserts.

Additionally, salt aids foods in a variety of ways like:

Preservation – helps protect against microorganisms, bacteria through dehydration and preventing growth of bacteria, which slows or prevents spoilage.

Texture Aid – in bread making, allows the dough to rise by giving helping the gluten hold more water and carbon dioxide. In meats it improves tenderness and in cheeses it aids in consistency of the cheese and the hardness of the rind.

Binder – in processed meats it helps retain water which reduces the loss of meat when cooking.

Color Developer – in ham, bacon, and other processed meats it helps obtain the desired color. It also helps create a golden crust for breads.

Fermentation Control – slows and controls the fermentation process in:

Pickling

Cheese production Sauerkraut production Summer sausage production

Acid Bases And Salts clas 10th :Test paper for examination

Chapter 2. Acids, Base and Salts

1. What is the chemical name of washing soda?
2. When sodium hydrogen carbonate is added to water, the hydrogen ion concentration decreases. What is the nature of the solution? Acidic or basic?
3. Write the chemical name and formula of bleaching powder.

4. A milkman adds a very small amount of baking soda to fresh milk.

(a) Why does he shift the pH of the fresh milk from 6 to slightly alkaline?

(b) Why does this milk take a long time to set as curd?

5. Plaster of Paris should be stored in a moisture proof container. Explain why?

6. What is a neutralization reaction? Give two examples.

7. Explain how pH change in the river water can endanger the lives of aquatic animals like fish.

8. What happens when  (i) plaster of Paris is heated to 473 K? (ii) Plaster of Paris is mixed with water?

9. Which gas is usually liberated when an acid reacts with a metal? Illustrate with an example. How will you 

test for the presence of this gas?

10. Explain the pH change as the cause of tooth decay. How can tooth decay caused by pH change be 

prevented?

11. Name the raw material used for the preparation of plaster of Paris. Write an equation to show the 

reaction between Plaster of Paris and water. What will happen if heating is not controlled while preparing 

plaster of Paris?

12. (i) Why are acids not stored in meal containers? Containers made from which material are safe to store 

acids.

(ii) Explain why dry hydrochloric acid not conducts electricity but its aqueous solution conducts electricity.

(iii) Why are commercial samples of bleaching powder not completely soluble in water?

                                                                 Or

Write one activity to show the reaction of acids with metal carbonates/bicarbonates salts.

13. (i) What is a salt?

(ii) Why aqueous solution of sodium carbonate is basic in nature?

(iii)Why is an aqueous solution of ammonium chloride acidic in nature?

14.(a) What is acid rain? How does it affect our aquatic life?

(b)What happens during a bee sting? What is its remedy?

(c)Two solutions X and Y are tested with universal indicator. Solution X turns orange whereas solution Y 

turns red. Which of the solution is a stronger acid?

15. (i) Write the chemical names and formula of bleaching powder.

(ii) Why does bleaching powder smell of chlorine when exposed to air?

(iii) Write chemical equation to represent the action of dilute hydrochloric acid on bleaching powder. 
Solution

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