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Acid Base and Salt - Class notes, Class 10, CBSE, NCERT
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Page 1 10TH CHEMISTRY NOTES 1. Acids: Acids are sour in taste, turn blue litmus red and give H3O+ ion (hydronium ions in solution. e.g. HCl, H2SO4, HNO3 etc 2. Bases: Bases are bitter in taste, have soapy touch, turns red litmus blue and give hydroxide ions (OH-) in solution. Example – NaOH, KOH etc 3. Salts: - A salt is a compound which is formed by neutralization reaction between an acid and base. For example, sodium chloride is formed by reaction between hydrochloric acid and sodium hydroxide. Acid + base ? ? Salt + water HCl+NaOH ? NaCl+H2O 4. Indicators - Indicators are substances which indicate the acidic or basic nature of the solution by their colour change. The colour of some acid-base indicators in acidic and basic medium are given below INDICATORS COLOUR IN ACIDIC COLOUR IN BASIC MEDIUM MEDIUM 1. Litmus Solution Red Blue 2. Methyl Orange Pink Orange 3. Phenolphthalein Colourless Pink 4. Methyl Red Yellow Red 5 Chemical properties of acids (i) Acids react with active metals to give hydrogen gas. Zn + H2SO4 ? ? ZnSO4 + H2 (ii) Acids react with metal carbonate and metals hydrogen carbonate to give carbon dioxide. NaHCO3+HCl ? ? NaCl + H2O+CO2 (iii) Acids react with bases to give salt and water. This reaction is called neutralization reaction. NaOH +HCl ? ? NaCl + H2O+CO2 (iv) Acids react with metals oxides to give salt and water. Page 1 Page 2 10TH CHEMISTRY NOTES 1. Acids: Acids are sour in taste, turn blue litmus red and give H3O+ ion (hydronium ions in solution. e.g. HCl, H2SO4, HNO3 etc 2. Bases: Bases are bitter in taste, have soapy touch, turns red litmus blue and give hydroxide ions (OH-) in solution. Example – NaOH, KOH etc 3. Salts: - A salt is a compound which is formed by neutralization reaction between an acid and base. For example, sodium chloride is formed by reaction between hydrochloric acid and sodium hydroxide. Acid + base ? ? Salt + water HCl+NaOH ? NaCl+H2O 4. Indicators - Indicators are substances which indicate the acidic or basic nature of the solution by their colour change. The colour of some acid-base indicators in acidic and basic medium are given below INDICATORS COLOUR IN ACIDIC COLOUR IN BASIC MEDIUM MEDIUM 1. Litmus Solution Red Blue 2. Methyl Orange Pink Orange 3. Phenolphthalein Colourless Pink 4. Methyl Red Yellow Red 5 Chemical properties of acids (i) Acids react with active metals to give hydrogen gas. Zn + H2SO4 ? ? ZnSO4 + H2 (ii) Acids react with metal carbonate and metals hydrogen carbonate to give carbon dioxide. NaHCO3+HCl ? ? NaCl + H2O+CO2 (iii) Acids react with bases to give salt and water. This reaction is called neutralization reaction. NaOH +HCl ? ? NaCl + H2O+CO2 (iv) Acids react with metals oxides to give salt and water. Page 1 10TH CHEMISTRY NOTES CuO + H2SO4 ? ? CuSO4 + H2O 6 Chemical properties of Bases- 1. Reaction with Metals – Certain metals such as Zinc, Aluminum, Tin react with Alkali solutions on heating and hydrogen gas is evolved 2NaOH + Zn ? Na2ZnO2 + H2 2. Reaction with acids – Bases react with acids to form salt and water. KOH + HCl ? KCl + H2O 3. Reaction with Non – metallic oxides – Non - metallic oxides are generally acidic in nature. They react with bases to form salt and water. 2NaOH + CO2 ? Na2CO3 + H2O 7. Strong and Weak Acids An acid which completely dissociates into ions in aqueous solution is called strong acid such as HCl, H2SO4, and HNO3 etc. Weak acids are those which are weakly dissociated in its aqueous solution such as CH3COOH, H2CO3, and HCN etc. ] 8. Strong and Weak Bases A base such as NaOH or KOH which is completely dissociated in aqueous solution is called a strong base. On the other hand a base which is weakly dissociated such as NH4 OH in its aqueous solution is called a weak base. 9. pH Scale The concentration of hydrogen ions in solution is expressed in terms of pH. The pH of a solution is defined as the negative logarithm of hydrogen ion concentration in moles per litre. pH =-log [H+] pH =-log [H3O+] where [H+] or [H3O+] represents concentrations of hydrogen ions in solution. For water or neutral solutions, pH =7 Page 2 Page 3 10TH CHEMISTRY NOTES 1. Acids: Acids are sour in taste, turn blue litmus red and give H3O+ ion (hydronium ions in solution. e.g. HCl, H2SO4, HNO3 etc 2. Bases: Bases are bitter in taste, have soapy touch, turns red litmus blue and give hydroxide ions (OH-) in solution. Example – NaOH, KOH etc 3. Salts: - A salt is a compound which is formed by neutralization reaction between an acid and base. For example, sodium chloride is formed by reaction between hydrochloric acid and sodium hydroxide. Acid + base ? ? Salt + water HCl+NaOH ? NaCl+H2O 4. Indicators - Indicators are substances which indicate the acidic or basic nature of the solution by their colour change. The colour of some acid-base indicators in acidic and basic medium are given below INDICATORS COLOUR IN ACIDIC COLOUR IN BASIC MEDIUM MEDIUM 1. Litmus Solution Red Blue 2. Methyl Orange Pink Orange 3. Phenolphthalein Colourless Pink 4. Methyl Red Yellow Red 5 Chemical properties of acids (i) Acids react with active metals to give hydrogen gas. Zn + H2SO4 ? ? ZnSO4 + H2 (ii) Acids react with metal carbonate and metals hydrogen carbonate to give carbon dioxide. NaHCO3+HCl ? ? NaCl + H2O+CO2 (iii) Acids react with bases to give salt and water. This reaction is called neutralization reaction. NaOH +HCl ? ? NaCl + H2O+CO2 (iv) Acids react with metals oxides to give salt and water. Page 1 10TH CHEMISTRY NOTES CuO + H2SO4 ? ? CuSO4 + H2O 6 Chemical properties of Bases- 1. Reaction with Metals – Certain metals such as Zinc, Aluminum, Tin react with Alkali solutions on heating and hydrogen gas is evolved 2NaOH + Zn ? Na2ZnO2 + H2 2. Reaction with acids – Bases react with acids to form salt and water. KOH + HCl ? KCl + H2O 3. Reaction with Non – metallic oxides – Non - metallic oxides are generally acidic in nature. They react with bases to form salt and water. 2NaOH + CO2 ? Na2CO3 + H2O 7. Strong and Weak Acids An acid which completely dissociates into ions in aqueous solution is called strong acid such as HCl, H2SO4, and HNO3 etc. Weak acids are those which are weakly dissociated in its aqueous solution such as CH3COOH, H2CO3, and HCN etc. ] 8. Strong and Weak Bases A base such as NaOH or KOH which is completely dissociated in aqueous solution is called a strong base. On the other hand a base which is weakly dissociated such as NH4 OH in its aqueous solution is called a weak base. 9. pH Scale The concentration of hydrogen ions in solution is expressed in terms of pH. The pH of a solution is defined as the negative logarithm of hydrogen ion concentration in moles per litre. pH =-log [H+] pH =-log [H3O+] where [H+] or [H3O+] represents concentrations of hydrogen ions in solution. For water or neutral solutions, pH =7 Page 2 10TH CHEMISTRY NOTES For acidic solutions, pH< 7 For basic solutions, pH > 7 10. pH of Salts (a) pH of salts of strong acid – strong base such as NaCl=7 (b) pH of salts of strong acid – weak base such as CuSO4 is <7 (c) pH of salts of weak acid – and strong base such as CH3COONa >7 11. Some Important Chemical Compounds (a) Common Salt (NaCl) Sodium chloride is known as common salt .Its main source is sea water. It also exists in the form of rocks and sodium chloride obtained from rocks is called rock salt. Common salt is an important component of our food. It is also used for preparing sodium hydroxide, baking soda, washing soda etc. (b) Sodium Hydroxide or Caustic Soda (NaOH) Sodium hydroxide is prepared by passing electricity through an aqueous solution of sodium chloride (also known as brine). 2NaCl (aq) + 2H2O (l) 2NaOH (aq) + Cl2 (g) + H2 (g) This process is known as chlor -alkali process due to the formation of chlorine and sodium hydroxide (an alkali) as the products. Properties – 1. It is a white translucent solid. 2. It is readily soluble in water to give a strongly alkaline solution. 3. Crystals of sodium hydroxide are deliquescent. (c) Bleaching Powder (CaOCl2) Page 3 Page 4 10TH CHEMISTRY NOTES 1. Acids: Acids are sour in taste, turn blue litmus red and give H3O+ ion (hydronium ions in solution. e.g. HCl, H2SO4, HNO3 etc 2. Bases: Bases are bitter in taste, have soapy touch, turns red litmus blue and give hydroxide ions (OH-) in solution. Example – NaOH, KOH etc 3. Salts: - A salt is a compound which is formed by neutralization reaction between an acid and base. For example, sodium chloride is formed by reaction between hydrochloric acid and sodium hydroxide. Acid + base ? ? Salt + water HCl+NaOH ? NaCl+H2O 4. Indicators - Indicators are substances which indicate the acidic or basic nature of the solution by their colour change. The colour of some acid-base indicators in acidic and basic medium are given below INDICATORS COLOUR IN ACIDIC COLOUR IN BASIC MEDIUM MEDIUM 1. Litmus Solution Red Blue 2. Methyl Orange Pink Orange 3. Phenolphthalein Colourless Pink 4. Methyl Red Yellow Red 5 Chemical properties of acids (i) Acids react with active metals to give hydrogen gas. Zn + H2SO4 ? ? ZnSO4 + H2 (ii) Acids react with metal carbonate and metals hydrogen carbonate to give carbon dioxide. NaHCO3+HCl ? ? NaCl + H2O+CO2 (iii) Acids react with bases to give salt and water. This reaction is called neutralization reaction. NaOH +HCl ? ? NaCl + H2O+CO2 (iv) Acids react with metals oxides to give salt and water. Page 1 10TH CHEMISTRY NOTES CuO + H2SO4 ? ? CuSO4 + H2O 6 Chemical properties of Bases- 1. Reaction with Metals – Certain metals such as Zinc, Aluminum, Tin react with Alkali solutions on heating and hydrogen gas is evolved 2NaOH + Zn ? Na2ZnO2 + H2 2. Reaction with acids – Bases react with acids to form salt and water. KOH + HCl ? KCl + H2O 3. Reaction with Non – metallic oxides – Non - metallic oxides are generally acidic in nature. They react with bases to form salt and water. 2NaOH + CO2 ? Na2CO3 + H2O 7. Strong and Weak Acids An acid which completely dissociates into ions in aqueous solution is called strong acid such as HCl, H2SO4, and HNO3 etc. Weak acids are those which are weakly dissociated in its aqueous solution such as CH3COOH, H2CO3, and HCN etc. ] 8. Strong and Weak Bases A base such as NaOH or KOH which is completely dissociated in aqueous solution is called a strong base. On the other hand a base which is weakly dissociated such as NH4 OH in its aqueous solution is called a weak base. 9. pH Scale The concentration of hydrogen ions in solution is expressed in terms of pH. The pH of a solution is defined as the negative logarithm of hydrogen ion concentration in moles per litre. pH =-log [H+] pH =-log [H3O+] where [H+] or [H3O+] represents concentrations of hydrogen ions in solution. For water or neutral solutions, pH =7 Page 2 10TH CHEMISTRY NOTES For acidic solutions, pH< 7 For basic solutions, pH > 7 10. pH of Salts (a) pH of salts of strong acid – strong base such as NaCl=7 (b) pH of salts of strong acid – weak base such as CuSO4 is <7 (c) pH of salts of weak acid – and strong base such as CH3COONa >7 11. Some Important Chemical Compounds (a) Common Salt (NaCl) Sodium chloride is known as common salt .Its main source is sea water. It also exists in the form of rocks and sodium chloride obtained from rocks is called rock salt. Common salt is an important component of our food. It is also used for preparing sodium hydroxide, baking soda, washing soda etc. (b) Sodium Hydroxide or Caustic Soda (NaOH) Sodium hydroxide is prepared by passing electricity through an aqueous solution of sodium chloride (also known as brine). 2NaCl (aq) + 2H2O (l) 2NaOH (aq) + Cl2 (g) + H2 (g) This process is known as chlor -alkali process due to the formation of chlorine and sodium hydroxide (an alkali) as the products. Properties – 1. It is a white translucent solid. 2. It is readily soluble in water to give a strongly alkaline solution. 3. Crystals of sodium hydroxide are deliquescent. (c) Bleaching Powder (CaOCl2) Page 3 10TH CHEMISTRY NOTES Its chemical name is calcium oxychloride .It is prepared by passing chlorine gas through dry slaked lime. Ca (OH) 2 + Cl2 CaOCl2 + H2O Slaked lime Bleaching powder Uses- 1. For bleaching cotton and linen in textile industry. 2. For bleaching wood pulp in paper industry. 3. For disinfecting drinking water. (d) Baking soda (NaHCO3) Its chemical name is sodium hydrogen carbonate .It is prepared by passing CO2 gas through brine solution saturated with ammonia. NaCl + H2O + CO2 + NH3 -------------------- ? NH4Cl + NaHCO3 Ammonium chloride Sodium Hydrogen carbonate The precipitated sodium hydrogen carbonate is filtered off. Properties – 1. It is a white crystalline solid, sparingly soluble in water at room temperature. 2. Its aqueous solution is weakly alkaline due to hydrolysis. 3. On heating, it decomposes to give sodium carbonate and carbon dioxide. 2NaHCO3 Na2 CO3 + H2O + CO2 4. It reacts with acids to give CO2 gas. NaHCO3 + HCl NaCl + H2O + CO2 Uses- 1. It is used as a component of baking powder. In addition to sodium hydrogen carbonate baking soda contains tartaric acid. 2. It is used in soda- acid fire extinguisher. Page 4 Page 5 10TH CHEMISTRY NOTES 1. Acids: Acids are sour in taste, turn blue litmus red and give H3O+ ion (hydronium ions in solution. e.g. HCl, H2SO4, HNO3 etc 2. Bases: Bases are bitter in taste, have soapy touch, turns red litmus blue and give hydroxide ions (OH-) in solution. Example – NaOH, KOH etc 3. Salts: - A salt is a compound which is formed by neutralization reaction between an acid and base. For example, sodium chloride is formed by reaction between hydrochloric acid and sodium hydroxide. Acid + base ? ? Salt + water HCl+NaOH ? NaCl+H2O 4. Indicators - Indicators are substances which indicate the acidic or basic nature of the solution by their colour change. The colour of some acid-base indicators in acidic and basic medium are given below INDICATORS COLOUR IN ACIDIC COLOUR IN BASIC MEDIUM MEDIUM 1. Litmus Solution Red Blue 2. Methyl Orange Pink Orange 3. Phenolphthalein Colourless Pink 4. Methyl Red Yellow Red 5 Chemical properties of acids (i) Acids react with active metals to give hydrogen gas. Zn + H2SO4 ? ? ZnSO4 + H2 (ii) Acids react with metal carbonate and metals hydrogen carbonate to give carbon dioxide. NaHCO3+HCl ? ? NaCl + H2O+CO2 (iii) Acids react with bases to give salt and water. This reaction is called neutralization reaction. NaOH +HCl ? ? NaCl + H2O+CO2 (iv) Acids react with metals oxides to give salt and water. Page 1 10TH CHEMISTRY NOTES CuO + H2SO4 ? ? CuSO4 + H2O 6 Chemical properties of Bases- 1. Reaction with Metals – Certain metals such as Zinc, Aluminum, Tin react with Alkali solutions on heating and hydrogen gas is evolved 2NaOH + Zn ? Na2ZnO2 + H2 2. Reaction with acids – Bases react with acids to form salt and water. KOH + HCl ? KCl + H2O 3. Reaction with Non – metallic oxides – Non - metallic oxides are generally acidic in nature. They react with bases to form salt and water. 2NaOH + CO2 ? Na2CO3 + H2O 7. Strong and Weak Acids An acid which completely dissociates into ions in aqueous solution is called strong acid such as HCl, H2SO4, and HNO3 etc. Weak acids are those which are weakly dissociated in its aqueous solution such as CH3COOH, H2CO3, and HCN etc. ] 8. Strong and Weak Bases A base such as NaOH or KOH which is completely dissociated in aqueous solution is called a strong base. On the other hand a base which is weakly dissociated such as NH4 OH in its aqueous solution is called a weak base. 9. pH Scale The concentration of hydrogen ions in solution is expressed in terms of pH. The pH of a solution is defined as the negative logarithm of hydrogen ion concentration in moles per litre. pH =-log [H+] pH =-log [H3O+] where [H+] or [H3O+] represents concentrations of hydrogen ions in solution. For water or neutral solutions, pH =7 Page 2 10TH CHEMISTRY NOTES For acidic solutions, pH< 7 For basic solutions, pH > 7 10. pH of Salts (a) pH of salts of strong acid – strong base such as NaCl=7 (b) pH of salts of strong acid – weak base such as CuSO4 is <7 (c) pH of salts of weak acid – and strong base such as CH3COONa >7 11. Some Important Chemical Compounds (a) Common Salt (NaCl) Sodium chloride is known as common salt .Its main source is sea water. It also exists in the form of rocks and sodium chloride obtained from rocks is called rock salt. Common salt is an important component of our food. It is also used for preparing sodium hydroxide, baking soda, washing soda etc. (b) Sodium Hydroxide or Caustic Soda (NaOH) Sodium hydroxide is prepared by passing electricity through an aqueous solution of sodium chloride (also known as brine). 2NaCl (aq) + 2H2O (l) 2NaOH (aq) + Cl2 (g) + H2 (g) This process is known as chlor -alkali process due to the formation of chlorine and sodium hydroxide (an alkali) as the products. Properties – 1. It is a white translucent solid. 2. It is readily soluble in water to give a strongly alkaline solution. 3. Crystals of sodium hydroxide are deliquescent. (c) Bleaching Powder (CaOCl2) Page 3 10TH CHEMISTRY NOTES Its chemical name is calcium oxychloride .It is prepared by passing chlorine gas through dry slaked lime. Ca (OH) 2 + Cl2 CaOCl2 + H2O Slaked lime Bleaching powder Uses- 1. For bleaching cotton and linen in textile industry. 2. For bleaching wood pulp in paper industry. 3. For disinfecting drinking water. (d) Baking soda (NaHCO3) Its chemical name is sodium hydrogen carbonate .It is prepared by passing CO2 gas through brine solution saturated with ammonia. NaCl + H2O + CO2 + NH3 -------------------- ? NH4Cl + NaHCO3 Ammonium chloride Sodium Hydrogen carbonate The precipitated sodium hydrogen carbonate is filtered off. Properties – 1. It is a white crystalline solid, sparingly soluble in water at room temperature. 2. Its aqueous solution is weakly alkaline due to hydrolysis. 3. On heating, it decomposes to give sodium carbonate and carbon dioxide. 2NaHCO3 Na2 CO3 + H2O + CO2 4. It reacts with acids to give CO2 gas. NaHCO3 + HCl NaCl + H2O + CO2 Uses- 1. It is used as a component of baking powder. In addition to sodium hydrogen carbonate baking soda contains tartaric acid. 2. It is used in soda- acid fire extinguisher. Page 4 10TH CHEMISTRY NOTES 3. It acts as mild antiseptic and antacid. (e) Washing soda (Na2 CO3 .10 H2O) Its chemical name is sodium carbonate decahydrate. It is obtained by heating baking soda in turn is obtained by passing CO2 gas through sodium chloride solution saturated with ammonia . NaCl + H2O + CO2 + NH3 ----------------------- ? NH4Cl + NaHCO3 2 NaHCO3 ---------- ?------------------- ? ? Na2 CO3 + H2O + CO2 Sodium hydrogen carbonate Sodium Carbonate Recrystallisation of sodium carbonates gives washing soda. Na2 CO3 + 10 H2O Na2 CO3 .10 H2O Uses- 1. It is used in glass, soap and paper industries. 2. It is used for removing permanent hardness of water. 3. It can be used as a cleaning agent for domestic purposes. (f)Plaster of Paris (CaSO4 ..1/2 H2O) Its chemical name is calcium sulphate hemihydrate. It is obtained by heating Gypsum upto 373 K. CaSO4 .2H2O ----------- ?----------- ? ? CaSO4 ..1/2 H2O + 11/2 H2O Gypsum Plaster of Paris On treatment with water it is again converted into gypsum and sets as a hard mass. CaSO4 ..1/2 H2O + 11/2 H2O ------------------- ? ? CaSO4 .2H2O Plaster of Paris Gypsum Uses – 1. It is used by Doctors for setting fractured bones. 2. It is used for making statues, models and other decorative materials. Page 5Read More
FAQs on Acid Base and Salt - Class notes, Class 10, CBSE, NCERT
| 1. What are acids and bases? |  |
Ans. Acids are substances that release hydrogen ions (H+) when dissolved in water, while bases are substances that release hydroxide ions (OH-) when dissolved in water. Acids have a sour taste and can corrode metals, while bases have a bitter taste and a slippery feel.
| 2. How do acids and bases react with each other? | |
Ans. When an acid and a base react with each other, they undergo a neutralization reaction. During this reaction, the hydrogen ions from the acid combine with the hydroxide ions from the base to form water. Additionally, a salt is formed as a byproduct of the reaction.
| 3. What is a salt? | |
Ans. A salt is a compound formed when the hydrogen ions from an acid are replaced by metal or ammonium ions. Salts are electrically neutral and are composed of positive and negative ions. They can be either soluble or insoluble in water and have a variety of uses, including as food preservatives, fertilizers, and in the production of chemicals.
| 4. How can we differentiate between acids and bases? | |
Ans. There are several ways to differentiate between acids and bases. One way is to use indicators, which are substances that change color in the presence of acids or bases. For example, litmus paper turns red in the presence of an acid and blue in the presence of a base. Another way is to test the conductivity of a solution using a conductivity tester. Acids are generally good conductors of electricity, while bases are poor conductors.
| 5. What are the common examples of acids, bases, and salts? | |
Ans. Some common examples of acids include vinegar (acetic acid), lemon juice (citric acid), and hydrochloric acid. Examples of bases include baking soda (sodium bicarbonate), ammonia, and sodium hydroxide. Common salts include table salt (sodium chloride), Epsom salt (magnesium sulfate), and baking powder (a mixture of a salt and an acid).
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