हिंदी
CISCE(English Medium) ICSE Class 10
प्रश्न पत्र४०९
पाठ्यपुस्तक उत्तर४६०४८
MCQ ऑनलाइन अभ्यास परीक्षा७
महत्वपूर्ण प्रश्न एवं उत्तर६४९४
अवधारणा स्पष्टीकरण और वीडियो३५५
समय सारणी१९
पाठ्यक्रम

Classification of Salts

Advertisements

Topics

  • Experiment 
  • Classification of Salts

Experiment

1. Aim: To measure the pH of aqueous solutions of different salts and classify the salts based on their pH values.

2. Requirements: Sodium chloride (NaCl), ammonium chloride (NH₄Cl), sodium bicarbonate (NaHCO₃), distilled water, pH paper, beakers, weighing balance, measuring cylinder, and stirring rod.

3. Procedure

  • Weigh 1 gram each of sodium chloride, ammonium chloride, and sodium bicarbonate.
  • Dissolve each salt in 10 ml of distilled water in separate beakers to prepare aqueous solutions. Stir the solutions well using a stirring rod.
  • Use pH paper to measure the pH of each solution by dipping a strip into each solution and noting the pH value. Record the pH values and compare them.

4. Observations

  • Sodium chloride solution has a pH close to 7 (neutral salt).
  • Ammonium chloride solution has a pH less than 7 (acidic salt).
  • Sodium bicarbonate solution has a pH greater than 7 (basic salt).

5. Conclusion

  • Neutral Salt: Sodium chloride (NaCl) is neutral because it is formed from a strong acid (HCl) and a strong base (NaOH).
  • Acidic Salt: Ammonium chloride (NH₄Cl) is acidic as it is formed from a strong acid (HCl) and a weak base (NH₃).
  • Basic Salt: Sodium bicarbonate (NaHCO₃) is basic because it is formed from a weak acid (H₂CO₃) and a strong base (NaOH).

This experiment shows that the nature of a salt (neutral, acidic, or basic) depends on the strengths of the acid and base that reacted to form it.

Classification of Salts:

There are seven main types of salts in chemistry, categorised based on their formation and properties:

  1. Simple Salts: It is formed from the straightforward reaction between an acid and a base. For example, sodium chloride (NaCl) is formed from HCl (acid) and NaOH (base).
  2. Neutral Salts: These salts do not have replaceable protons or hydroxyl ions. They have a pH of 7, making them neither acidic nor basic. For example, sodium chloride (NaCl) and potassium chloride (KCl).
  3. Acidic Salts: It is formed by the reaction of a strong acid with a weak base. Incomplete neutralization of the acid results in salts with a pH below 7, exhibiting acidic properties. For example, ammonium sulphate ((NH₄)₂SO₄) and ammonium chloride (NH₄Cl).
  4. Basic Salts: It is formed by the reaction of a strong base with a weak acid. Incomplete neutralization of the base produces salts with a pH above 7, showing basic properties. For example, potassium cyanide (KCN) and zinc chloride hydroxide (Zn(OH)Cl).
  5. Double Salts: It contains more than one cation or anion in their structure. They are most stable in their solid form. For example, potash alum (KAl(SO₄)₂·12H₂O).
  6. Mixed Salts: It contains either two anions sharing a single cation or two cations sharing a single anion. Formed by the reaction of more than one acid or base. For example: Calcium disodium EDTA, sodium potassium carbonate.
  7. Complex Salts: It contains a central metal atom surrounded by neutral molecules and charged ions. Formed by the combination of ions and molecular compounds. For example, Tetra ammine cupric sulphate ([Cu(NH₃)₄]SO₄).
If you would like to contribute notes or other learning material, please submit them using the button below.
Advertisements
Share
Notifications

Englishहिंदीमराठी
Login
Create free account


      Forgot password?
Course
Use app×