Скачать или смотреть Acid base salt class 10th English Hindi medium

This video provides an overview of acids, bases, and salts, along with their properties, identification methods, and common example

Acids (0:18)
Definition and properties: Sour in taste (0:21), turn blue litmus red (0:51), and have a pH less than 7 (0:53). They produce H+ ions in water (2:20).
Reaction with metals: Acids react with metals to produce hydrogen gas (1:19).
Examples: Hydrochloric acid (HCl), sulfuric acid (H2SO4), and acetic acid (1:01).

Bases (2:35)
Definition and properties: Bitter in taste (2:40), turn red litmus blue (2:55), and have a pH greater than 7 (2:57). They produce OH- ions in water (3:05).
Examples: Sodium hydroxide (NaOH) and potassium hydroxide (KOH) (3:26).

Salts (3:39)
Definition: Compounds formed from the reaction of an acid and a base (3:45), known as a neutralization reaction (4:54).
Properties: Ionic compounds (4:22) and soluble in water (4:59). They have high boiling and melting points (4:33).
Example: Sodium chloride (NaCl) (4:06).

Indicators (5:07)
Purpose: Substances used to determine if a substance is acidic or basic by changing color or odor (5:09, 6:40).
Types:
Natural indicators: Obtained from nature, such as litmus (6:00) (extracted from lichens) and turmeric (6:07).
Synthetic indicators: Man-made in labs, including methyl orange (6:32) and phenolphthalein (6:34).
Olfactory indicators: Change odor in acidic or basic mediums, such as onion and cloves (7:22).
Specific indicator reactions:
Litmus: Acid turns blue litmus red (8:07), base turns red litmus blue (8:23).
Phenolphthalein: Colorless in acid (8:35), pink in base (8:46).
Methyl orange: Red in acid (8:53), yellow in base (9:01).

pH Scale (9:06)
Purpose: Measures the strength (9:35) of an acid or base (9:41).
Range: 0 to 14 (9:53).
Values:
7: Neutral (10:14) (e.g., water (11:31)).
Less than 7: Acidic (10:19). The lower the pH, the stronger the acid (11:00).
Greater than 7: Basic (10:29). The higher the pH, the stronger the base (11:17).
Examples of pH values: Battery acid (pH 0), gastric juice (pH 1), lemon (pH 2), apple (pH 3), tomato (pH 4), black coffee (pH 5), water (pH 7) (12:06).

Important Compounds for Board Exams (13:08)
Sodium Hydroxide (Caustic Soda) - NaOH (13:26)
Preparation: Chlor-alkali process (13:34) involving electrolysis of brine (NaCl + H2O) (13:49).
Uses: Soap and detergent manufacturing, paper industry, textile industry (14:40, 15:49).
Bleaching Powder (Calcium Hypochlorite / Calcium Oxychloride) - CaOCl2 (16:29)
Preparation: Reacting chlorine gas with slaked lime (Ca(OH)2) (17:20).
Uses: Cleaning clothes (especially white), disinfectant (18:01), oxidizing agent (18:31).
Plaster of Paris (POP) - CaSO4 · ½H2O (19:21)
Preparation: Heating gypsum (CaSO4 · 2H2O) at 100°C or 373 K (19:58).
Uses: Setting fractured bones (20:51), making statues and decorative items (21:11), fireproofing (21:35).
Baking Soda (Sodium Bicarbonate / Sodium Hydrogen Carbonate) - NaHCO3 (23:52)
Preparation: Reacting brine, ammonia, and carbon dioxide (24:31).
Uses: Baking (25:16), cleaning (25:31), antacid (25:36), fire extinguishers (26:42).
Washing Soda (Sodium Carbonate Decahydrate) - Na2CO3 · 10H2O (29:54)
Preparation: Heating baking soda to form sodium carbonate, then recrystallizing with water (27:26).
Uses: Softening hard water (28:27), cleaning agent (28:46), glass, soap, and paper industries (28:55).