Acid Base and Salt solved Question Answer

 Question (1): Define the terms: Acid, alkali and salt.

 Answer:  An acid is a compound, which releases hydronium ions (H₃O⁺) as the only positive ions in solution. An alkali is a compound, which releases hydroxyl ions (OH^-) as the only negative ions in solution. A salt is one of the products of neutralization between an acid and a base; water being the only other product. OR A salt gives positive ions other than H⁺ ion and negative ions other than OH^- ion in solution.

Question (2): Identify the number of replaceable hydrogen ions (H⁺) in the following acids: HCl, CH₃COOH, H₂SO₄, H₃PO₄.

Answer:  HCl = 1    CH₃COOH = 1       H₂SO₄ = 2     H₃PO₄ = 3.

Question (3): What is a neutralization reaction?

Answer:  Neutralization is essentially a chemical reaction between H₃O⁺ ions of an acid with OH^- ions of the base, to give undissociated molecules of water.

Question (4): What are strong and weak acids? Give one example of each?

Answer:  A strong acid is one, which is almost completely dissociated in solution. Examples: Dilute nitric acid, dilute sulphuric acid and dilute hydrochloric acid. A weak acid is one, which is only partially ionized in solution (degree of dissociation is >30%). Examples: Acetic acid, carbonic acid and sulphurous acid.

Question (5): Why is acetic acid called a weak acid though there are 4 'H' atoms in the molecule?

Answer:  Acetic acid is called a monobasic acid because only one of the 4 'H' atoms of the acid is released as H⁺ ion in solution.

Question (6): How does a strong acid differ from a concentrated acid?

Answer:  The strength of an acid depends upon its dissociation power whereas concentration depends on water content in the acid.

Question (7): Name a salt of a strong acid HNO₃ and a weak base like NH₄OH. Represent the reaction that takes place.

Answer:  The salt that results due to the above reaction is Ammonium nitrate (NH₄NO₃). The reaction is represented as:  HNO₃         +             NH₄OH         --------à     NH₄NO₃    
                                          

Question (8):  1) Name a strong base and a weak base. 2) Name a hydrated salt.

Answer: 

1) A strong base is sodium hydroxide (NaOH) and a weak base is ammonium hydroxide (NH₄OH).
2) A hydrated salt is copper sulphate crystals (CuSO₄.5H₂O).

Question (9): Name the following:
1) Two non-hydrated crystalline salts  2) Two neutral salts  3) Two basic salts  4) Two acid salts

Answer:   1) Two non-hydrated crystalline salts are: sodium chloride (NaCl) and potassium nitrate (KnO₃)
2) Two neutral salts are: sodium chloride (NaCl) and sodium sulphate (Na₂SO₄)
3) Two basic salts are: basic copper carbonate (CuCO₃.Cu(OH)₂) and basic lead carbonate (PbCO₃.Pb(OH)₂)
4) Two acid salts are: sodium bicarbonate (NaHCO₃) and sodium phosphate (NaH₂PO₄)

Question (10): Name the salts of sulphuric acid.

Answer:  The salts of sulphuric acid are bisulphate and sulphate. Examples: NaHSO₄, KHSO₄ and Na₂SO₄.

Question (11): Define the term "pH"; what does" pH" stand for?

Answer:  The term "pH" is defined as the negative logarithm of H⁺ ion concentration of a given solution; the concentration being expressed as moles per litre. Mathematically pH = - log [H⁺] 'pH' stands for: Power of hydrogen ion concentration, 'p' for power and 'H' for H⁺ ion concentration.

Question (12): What is 'pH' scale? Explain briefly.

Answer:  The strength of an acid or a base is expressed in terms of hydronium ion concentration. This is expressed on a scale known as 'pH' scale. It is a 14 point scale; i.e., it has values ranging from 0 to 14, indicating the value of negative logs of H⁺ ion concentration of the solution. Some important benchmark values in the pH scale are: pH = 7 indicates neutral solutions e.g., aqueous solutions. pH > 7 to 14 indicates alkaline solutions and pH < 7 to 0 indicate acidic solutions

Question (13): What is the 'pH' of pure water and that of rain water? Explain the difference.

Answer:  The pH of pure water is seven. Rain water is slightly acidic because as rain drop fall, the carbon dioxide in the air dissolves with drops to form very weak carbonic acid. Accordingly, rain water has a pH that is slightly below 7.

Question (14): What is the pH of solution 'A' which liberates CO₂ gas with a carbonate salt? Give the reason?

Answer:  The pH of solution 'A' is lesser than 7. Carbonates salts react with acids (A) to liberate CO₂ gas.

Question (15): What is the pH of solution 'B' which liberates NH₃ gas with an ammonium salt? Give reason?

Answer:  The pH of solution 'B' is lesser than 7 because 'B' is an alkali as it liberates NH₃ gas. Question (16): How do you increase or decrease the pH of pure water? Answer:  By adding a few drops of alkali to pure water, it's pH increases; and by adding a few drops of an acid decreases the pH of pure water.

Question (17): What are indicators?

Answer:  Indicators are chemicals that show whether the given solution is acidic or basic, by the sudden change of color.

Question (18): Name the common acid-base indicators used in the laboratory with their color change.

Answer:  The three common indicators used in the laboratory are:

Indicator	Final colour
	Acid	Alkali
Litmus	Red	Blue
Methyl orange	Pink	Yellow
Phenolphthalein	Colourless	Deep pink

Question (19): What is a universal indicator? What is its advantage?

Answer:  A universal indicator is a mixed indicator of organic chemicals which not only shows whether the given solution is acidic or basic, but also shows the approximate pH values by giving a wide particular colour for a specific value of pH.

Question (20): What is the action of litmus on ferric chloride solution and why?

Answer:  An aqueous solution of FeCl₃ salt undergoes hydrolysis and releases H⁺ ions from the stronger acid HCl formed. Hence, the resulting solution is acidic and turns blue litmus turns red.

          Fecl₃    +   3 H₂O          ------------à     Fe (OH)₃    + 3 H Cl
                           HCl             --------------à   H⁺                 + Cl ^-

Question (21): What is the action of Na₂CO₃ solution on litmus and why?

 Answer:  In solution Na₂CO₃ salt undergoes hydrolysis and releases OH^- ions from the stronger alkali NaOH. Consequently, the resulting solution is basic and turns red litmus blue.

                      Na₂CO₃   +    2H₂O            ---------------------------à 2NaOH   + H₂CO₃

                     Na OH                              -----------------------------à Na⁺        +     OH^-

Question (22): What is the action of NaHSO₄ solution on litmus and why?

Answer:  Blue litmus turns red in NaHSO₄ solution due to the release of H⁺ ions along with Na⁺ ions. Thus, NaHSO₄ is an acid salt.

Question (23): Though NaHSO₄ solution releases H⁺ ions, why is it not called an acid?

Answer:  NaHSO₄ solution is not called an acid because an acid should release only H⁺ ions as positive ions and not any other positive ions. But NaHSO₄ is solution releases H⁺ ions as well as Na⁺ ions also as positive ion.

Question (24): Define the term ' normal salt ' with examples.

Answer:  A normal salt is produced when all the replaceable 'H' atoms of an acid are completely replaced by a metal or NH₄ group, during neutralization with a base. Examples: NaCl, K₂CO₃and (NH₄)₃PO₄.

Question (25): Define the term 'acid salt' with examples.

Answer:  An acid salt is formed when the available 'H' atoms of an acid are only partially replaced by a metal, during neutralization with a base, and hence there are still 'H' atoms present in the salt that are available for replacement.  Examples: NaHSO₄, NaHCO₃, Na₂HPO₄and NaH₂PO₄

Question (26): Define the term 'basic salt' with an example.

Answer:  A basic salt is formed by the incomplete neutralization of a base with an acid or partial replacement of hydroxyl radicals of a diacidic base or a triacidic base with an acid radical. Example: Zn(OH)Cl, Cu(OH)NO₃.

Question (27): Define a double salt. Give some examples.

Answer:  A double salt is formed between two simple salts by crystallization from a saturated solution of a mixture of the two. Examples  

K₂SO_4.Al₂(SO₄)₃.24H₂O ( potash Alum),

(NH₄)₂ Al₂(SO₄)₃.24H₂O (Ammonium Alum) 

 FeSO₄(NH₄)₂ SO₄.6H₂O (Mohr’s Salt)

Question (28): Define mixed salt giving some examples.

Answer:  Mixed salts contain more than one acid radical or basic radical other than H⁺ and OH^- ions.
Examples:  K⁺Ca²⁺PO^3- (Potassium calcium phosphate) , Na⁺K⁺SO₄^2- (Sodium potassium sulphate).

Ca²⁺(OCl)^-Cl^- [Bleaching powder (Calcium chloro hypochlorite)]


Question (29): Define complex salts with examples.

Answer:  Complex salts dissociate to give one simple ion and one complex ion in solution. Examples:

Na [Ag(CN)₂ ] (aq) ---------------------------    à Na⁺  +  [Ag(CN)₂ ]^-                 (complex Ions)

[Cu (NH₃)₄] SO₄                ----------------------à [ Cu (NH₃)₄ ]²⁺           + SO₄ ^2- (complex Ions)

Question (30): What happens if NaOH is added to ferrous ammonium sulphate solution and warmed? What is the inference?

Answer:  When NaOH is added to ferrous ammonium sulphate solution and warmed, both ferrous ion and ammonium ion separate and exhibit their individual properties. A green precipitate of Fe(OH)₂ is formed and the smell of NH₃ gas from (NH₄)⁺ ion is observed. Hence it is an example of the formation of a double salt.

Question (31): 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.

Question (32): 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.

Question (33): Define a base and acid in terms of proton.

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

Question (34):  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: 

1) The three anions that can be identified using dilute acids with their common ionic equations are:

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

Sulphate and Bi sulphate Ions     2H⁺  + SO₃^2-                        --------à    H₂O + SO₂ 
 ­
Sulphide Ion       2H⁺ (dil. Acid)  + S ^2-  (salt)   -------- >      H2S GasIdentified)

2) The property is that of releasing H⁺ ions by dilute HCl or dilute H₂SO₄ in solution i.e., the acidic property.

Question (37): a) What do you observe when concentrated H₂SO₄ is added slowly to blue CuSO₄ crystals in a test tube and why? 
b) Is these any other way of observing the above result?

Answer:  a) 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.


b) Another way of observing the above result is by gentle heating of blue crystals of CuSO₄.5H₂O directly in a test tube.

Question  (38) : 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.

Question (39): 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.  

Question (40): 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.
Examples of cations detected are Pb²⁺, Zn²⁺, Cu²⁺, Fe²⁺ and Fe³⁺.

Question (41):  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:
1) An active metal (above Pb) and dilute H₂SO₄ gives H₂ gas.

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.

Question (42): 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.

Question (43): 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.

 Question (44): 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.45  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.46: 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. 47. 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. 48. 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.

Q 49. 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

Question 50 :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.

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