Showing posts with label make chemistry better for you. Show all posts
Showing posts with label make chemistry better for you. Show all posts

Sunday, 29 June 2025

Temperature and Heat

 Temperature

Definition: The degree of hotness or coldness of a body or a place is called temperature.

Measurement: Temperature is measured using a thermometer.

Units: Celsius (°C), Fahrenheit (°F), and Kelvin (K) are common units of temperature.

Scales: Celsius scale and Fahrenheit scale are two commonly used temperature scales.

Fixed points: Melting point of ice (0°C or

32°F) and boiling point of water (100°C or 212°F) are used as fixed points to define the temperature scales.

Thermometers

Definition: A thermometer is a device used to measure temperature.

Fact: the first thermometer was invented by galeleo galilei in 1593.

Fact: The human body can perceive temperature difference, but it is not a reliable way to measure temperature accurately. 

Types:

Mercury thermometer: Uses mercury as the thermometric fluid.

Alcohol thermometer: Uses alcohol as the thermometric fluid.

Digital thermometer: Uses a thermistor or other electronic sensor to measure temperature.

Uses: Measuring body temperature, temperature of a substance, and ambient temperature.

Heat

Definition: Heat is a form of energy

that flows from a body at a higher temperature to a body at a lower temperature.

Measurement: Heat energy is measured in calories or joules (J).

Transfer: Heat can be transferred through conduction, convection, and radiation.

Fact:Metal are generally good conductor of heat, while non-metals are poor conductor. 

Modes of Heat Transfer

1. Conduction

Definition: Conduction is the transfer of heat energy through direct contact between particles.

Occurs in: Solids.

Examples: Heat transfer through a metal rod, cooking utensils.

Factors affecting conduction:

Thermal conductivity of the material, temperature difference, and cross-sectional area.

2. Convection

Definition: Convection is the transfer of heat energy through the movement of fluids.

Occurs in: Liquids and gases.

Examples: Sea breeze, land breeze, heating of water in a vessel.

Factors affecting convection: Density difference, temperature difference, and gravity.

Fact: convection current play a crucial role in shaping our climate & weather patterns. 

3. Radiation

Definition: Radiation is the transfer of

heat energy through electromagnetic waves.

Occurs in: Vacuum and medium.

Examples: Heat transfer from the sun, radiation from a fire.

Factors affecting radiation: Temperature, surface area, and emissivity.

Fact: Radiation is the fastest mode of heat transfer and can occur in a vacuum. 

Applications of Heat Transfer

Conduction: Cooking utensils, heat sinks, and thermal insulation.

Convection: Heating of buildings, sea breeze, land breeze, and ocean currents.

Radiation: Solar panels, heating of the Earth's surface, and thermal imaging.

Preventing Heat Loss

Insulation: Using materials that reduce heat transfer.

Thermos flask: A device that minimizes

heat loss through conduction, convection, and radiation.

Vacuum insulation: Using a vacuum to

reduce heat transfer through conduction and convection.

Practical Applications

Solar energy: Harnessing energy from the sun using solar panels.

Thermal insulation: Using materials to

reduce heat transfer in buildings and appliances.

Heat exchangers: Devices that transfer

heat energy from one fluid to another.

Fact;Thermoflascs use vacuum insulation to minimise heat transfer and keep liquids at a consistent temperature. 

Key Concepts

Heat flows from a body at a higher temperature to a body at a lower temperature.

Temperature is a measure of the degree of hotness or coldness of a body.

Different materials have different abilities to conduct heat.

Convection occurs in fluids due to density differences.

Radiation can occur in vacuum and medium.

Monday, 23 June 2025

Acid, base and salt

 Acids

Definition: Substances containing an acid (from Latin "acere" meaning sour)

Types: Mineral acids and organic acids

Mineral Acids

Examples: 

Hydrochloric acid (HCI),

sulphuric acid (H2SO4), and nitric acid (HNO3)

Uses: Laboratory, industrial applications

Properties: Strong, corrosive, and highly reactive towards metals

Organic Acids

Examples: Tartaric acid (grapes), acetic

acid (vinegar), formic acid (sting of ants and bees), malic acid (apples), citric acid (lemons and oranges), lactic acid (milk)

Properties: Weak, naturally occurring in animal and plant materials

Strong and Weak Acids

Strong acids: Highly corrosive, mineral

acids (e.g., hydrochloric acid, sulphuric acid, and nitric acid)

Weak acids: Less destructive, mostly organic acids (e.g., acetic acid)

Properties of Acids

Sour taste

Corrosive nature

Soluble in water

Can be dilute or concentrated

Uses of Acids

Hydrochloric acid (HCI):

Used in industries for heating applications

Cleaning sinks and sanitary ware

Sulphuric acid (H2SO4):

Used in car batteries

Manufacture of paints, drugs, dyes, and fertilizers

Nitric acid (HNO3):

Used by goldsmiths for cleaning gold and silver ornaments

Production of fertilizers

Acetic acid (CH3COOH):

Main ingredient of vinegar

Enhances flavor of food and acts as a preservative in pickles

Used as a cleansing agent

Acidic Environment and Microorganisms

Most microorganisms cannot live in an acidic environment.

Acidic environment can slow down or kill microorganisms.

This is why vinegar is used in many packaged food items like pickles, sauce, and ketchups.

Acid Rain

Acid rain is a major effect of air pollution.

Pollutants like sulphur dioxide and oxides of nitrogen react with atmospheric water and oxygen to form sulphuric acid and nitric acid.

Acid rain can damage plant and animal life, buildings, and monuments.

True or False Statements

1. Acids can be stored in metal containers: False (Acids are corrosive and can react with metals.)

2. Mineral acids are present in animal and plant materials: False (Mineral acids are produced from chemical substances, whereas organic acids are present in animal and plant materials.)

3. A dilute acid has more amount of water than a concentrated acid: True

4. Sulphuric acid is used for cleaning sinks and sanitary ware: False (Hydrochloric acid is used for cleaning sinks and sanitary ware.)

5. Nitric acid is used by goldsmiths for cleaning gold and silver ornaments: True

6. Hydrochloric acid is used to enhance the flavor of food and as a preservative in pickles: False (Acetic acid is used to enhance the flavor of food and as a preservative in pickles.)

Fill in the Blanks

1. Acids are sour to taste.

2. Apples contain malic acid, whereas spinach has oxalic acid.

3. Strong acids are highly corrosive.

4. Organic acids are weak acids.

5. Carbonic acid is present in fizzy drinks and soda water.

Bases

Definition: Substances containing a base are called basic substances.

Examples: Sodium hydroxide (NaOH), calcium hydroxide (Ca(OH)2)

Properties: Bitter taste, slippery feel, may or may not be soluble in water

Strong and Weak Bases

Strong bases: Highly corrosive, can burn skin (e.g., sodium hydroxide, potassium hydroxide)

Weak bases: Less corrosive (e.g., copper hydroxide, zinc hydroxide, ammonium hydroxide)

Uses of Bases

Calcium hydroxide (slaked lime):

Neutralizes acidity in soils

Used in whitewash and mortar

Used in Bordeaux mixture for protecting crops

Magnesium hydroxide (milk of magnesia):

Used as an antacid or laxative

Corrects excess acidity in the stomach

Sodium hydroxide (caustic soda):

Used in manufacture of paper and textiles

Used to unblock drains

Used in manufacture of soaps and detergents

Indicators

Definition: Substances that show a

change in color when brought in contact with acids and bases.

Examples: Litmus, phenolphthalein,

methyl orange

Types: Natural indicators (e.g., turmeric, red cabbage), universal indicators (e.g pH paper)

pH and Universal Indicators

pH: A measure of the strength of an acid or base, ranging from 1 to 14.

Universal indicator: A mixture of indicators that gives a different color for different pH values.

pH paper: A paper soaked in universal indicator solution.

A. Fill in the blanks

1. Strong acids are highly corrosive and can cause severe burns.

2. Bases are slippery to touch.

3. Sulphuric acid is used in the manufacture of paints, dyes, and drugs.

4. Sodium hydroxide is used to unblock drains.

5. Blue litmus changes to red in acids.

B. Choose the correct option

1. d. Sulphuric acid is called the "King of chemicals".

2. c. Acetic acid is present in vinegar.

3. a. Carbonic acid is a weak mineral acid.

4. b. Calamine lotion is used to neutralize bee stings.

5. c. Sugar cannot be used as an indicator.

6. d. Both Potash alum and Silver nitrate are salts.

7. b. Hydrochloric acid is used to remove deposits from the inside of boilers.

8. c. KOH is a strong base.

9. d. pH = 13 represents a strong alkali.

10. a. High melting point is a characteristic property of most salts.

Matching

1. CH3COOH - c. Acetic acid

2. AgNO3 a. Silver nitrate

3. NH4NO3 d. Ammonium nitrate

4. Ca(OH)2 - e. Calcium hydroxide

5. CaCO3 b. Calcium carbonate

Very Short Answer Type Questions

1. Alkalis

2. Indicator

3. pH paper

4. Neutral salt

5. Hydrated salts

Short Answer Type Questions

1. Properties of acids: Sour taste, corrosive nature

Properties of bases:

 Bitter taste, slippery feel

2. Acids or bases are added to soil to adjust its pH for optimal plant growth.

3. Neutralization reaction: A reaction between an acid and a base to form a salt and water. Example: HCI + NaOH NaCl + H2O

4. A hydrated salt can be converted into an anhydrous salt by heating it to remove the water of crystallization. Example: CuSO4.5H20 CuSO4 + 5H2O ←

Long Answer Type Questions

1. Natural indicators can be prepared from plant materials like flowers, roots, stems, and leaves. 

Examples:

Flower: Rose petals

Root: Beetroot

Stem: Turmeric

Leaf: Red cabbage

Red cabbage juice shows different colors in acidic, neutral, and basic mediums: deep red in acidic, purple in neutral, and green/yellow in basic.

2. a. Vinegar is used in packaged food items as a preservative.

b. Slaked lime is added to factory waste to neutralize acidic substances.

c. Magnesium hydroxide is used as an antacid to neutralize excess acid in the stomach.

d. Strong acids and bases should be handled carefully because they can cause severe burns and damage.

3. Water of crystallization: Water molecules present in the crystal structure of a salt. Example: CuSO4-5H2O (copper sulfate pentahydrate

Let's Observe

1. a. Food items: Not specified

b. Process: Not specified

c. Chemical used: Not specified

2. Acidic solution: Turns blue litmus

paper red

Basic solution: Turns red litmus paper blue

Let's Apply

1. Pickles and sauces are not packaged in metal containers because the preservative used (acidic substance) can react with the metal.

2. Hydrochloric acid in the stomach does not corrode the stomach lining because it is highly concentrated and the stomach lining has a protective mechanism.)

Let's Analyse and Evaluate

1. The sanitary ware cleaner likely contained an acidic substance that reacted with the marble flooring, causing discoloration.

2. The cleaner does not spoil sinks and sanitary ware because they are made of materials that can withstand acidic substances, but marble is more sensitive to acidic reactions.


Saturday, 14 June 2025

Chemicals and chemical changes.

Chemical Substances


Types of Chemical Substances

1. Pure Substances: Elements or compounds.

2. Mixtures: Combination of two or more substances not chemically combined.

Elements

1

. Definition: Substance made up of only one kind of atoms.

2.

Properties: Each element has its own distinct set of properties.

3. Examples: Silver, gold, aluminium, hydrogen, oxygen.

Compounds

1. Definition: Substance formed when

two or more elements combine chemically.

2. Properties: Properties of a compound differ from those of its constituent elements.

3. Examples

 Mixtures**


1 . Definition: Combination of two or

more substances not chemically combined.

2

. Properties: Retains properties of its components.

3. Examples: Air, mixture of iron filings and sulphur.

Chemical Symbols

1. Definition: Abbreviations used to represent elements.

2. Purpose: Simplifies writing and communication in chemistry.

Chemical Symbols and Atomicity


History of Chemical Symbols

1. Early Symbols: Pictorial symbols used by John Dalton.

2. Modern System: Developed by Jons Jacob Berzelius using letters of the English alphabet.

Features of Modern Chemical Symbols

1. First Letter: First letter of the element's name is used as its symbol.

2. Additional Letters: Second letter or distinct letter added when necessary.

3. Latin Names: Some symbols derived from Latin names (e.g., Au for Gold, Ag for Silver).

Examples of Chemical Symbols

1. Elements: H (Hydrogen), C (Carbon), O (Oxygen), N (Nitrogen).

2. Symbols from Latin Names: Na (Sodium), K (Potassium), Pb (Lead).

Chemical Formulae and Equations


Chemical Formulae

1. Definition: Representation of a molecule of a compound using chemical symbols of its constituent elements.

2. Examples: H2O (water), NaCl (common salt), CaCO3 (calcium carbonate).

Valency

1. Definition: Combining capacity of an atom of an element.

2. Examples: Hydrogen (1), Oxygen (2), Carbon (4).

Writing Chemical Formulae

1. Steps:

Write symbols of constituent elements.

Write valencies of elements.

Cross over valencies and write as subscripts.

Simplify formula if possible.

Atomicity


1

. Definition: Number of atoms present in one molecule of an element.

2. Types:

Monatomic: 1 atom (e.g., noble gases).

Diatomic: 2 atoms (e.g., oxygen, 02).

Tetratomic: 4 atoms (e.g.,

phosphorus, P4).

Chemical Equations

1 . Definition: Shorthand form of

representing a chemical reaction using symbols and formulae.

2. Components:

Reactants: Substances involved initially in the reaction.


Products: New substances formed in the reaction.

Writing Chemical Equations

1. Steps:

Identify reactants and products.

Write names of reactants on the left-hand side with a '+' sign between them.

Write names of products on the right-hand side with a '+' sign between them.

Use an arrow (→) to separate reactants from products.

Chemical Equations

Writing Chemical Equations

1. Steps:

Identify reactants and products.

Write names of reactants on the left-hand side with a '+' sign between them.

Write names of products on the right-hand side with a '+' sign between them.

Use an arrow (→) to separate reactants from products.

2. Example: Magnesium burns in oxygen to form magnesium oxide.

Word equation: magnesium + oxygen → magnesium oxide

Chemical equation: 2Mg + 02 → 2MgO

Balancing Chemical Equations

1. Definition: Ensuring the number of atoms of each element is equal on both sides of the equation.

2. Steps:

Count the number of atoms of each element on both sides.

Adjust coefficients to balance the equation.

Examples of Chemical Changes

1. Rusting of Iron: Iron reacts with

oxygen and moisture to form iron oxide (rust).

Chemical equation: 4Fe + 302 + 6H2O → 4Fe(OH)3

Importance of Chemical Equations

1. Representation: Chemical equations

represent chemical reactions in a concise and symbolic way.

2. Balancing: Balancing chemical equations ensures the law of conservation of mass is obeyed

Balancing Chemical Equations

1. Definition: Ensuring the number of atoms of each element is equal on both sides of the equation.

2. Steps:

Count the number of atoms of each element on both sides.

Adjust coefficients to balance the equation.

Examples of Chemical Changes

1. Rusting of Iron: Iron reacts with

oxygen and moisture to form iron oxide (rust).

Chemical equation: 4Fe + 302 + 6H2O → 4Fe(OH)3

Importance of Chemical Equations

1. Representation: Chemical equations

represent chemical reactions in a concise and symbolic way.

2. Balancing: Balancing chemical equations ensures the law of conservation of mass is obeyed.

Chemical Changes

Examples of Chemical Changes

1. Rusting of Iron: Iron reacts with

oxygen and moisture to form iron oxide (rust).

Conditions: Oxygen and water are essential for rusting.

Prevention: Oiling or galvanizing iron objects can prevent rusting.

2. Browning of Vegetables and Fruits:

Cut surfaces of vegetables and fruits turn brown due to reaction with atmospheric oxygen.

Prevention: Soaking cut vegetables and fruits in plain water can reduce browning.

3. Reaction between Vinegar and Baking Soda: Produces carbon dioxide gas.

Chemical equation: CH3COOH + NaHCO3 CH3COONa CO2 + H2O +

4. Reaction between Copper Sulphate Solution and Iron Nails: Iron displaces

copper from copper sulphate solution,

forming iron sulphate and copper.

Chemical equation: CuSO4 + Fe → FeSO4 + Cu

Characteristics of Chemical Changes

1. Permanent Change: Chemical

changes are often irreversible.

2. New Substances Formed: Chemical changes result in the formation of new substances with different properties

Physical and Chemical Changes

Physical Changes

1. Definition: Changes in which no new substances are formed.

2. Examples: Formation of ice from water, crystallization of common salt.

3. Characteristics: Properties such as color, shape, size, or physical form may change.

Chemical Changes

1. Definition: Changes in which new substances are formed.

2. Examples: Rusting of iron, reaction

between vinegar and baking soda, reaction between copper sulphate solution and iron nails.

3. Characteristics: Permanent change, new substances formed with different properties.

Crystallization

1. Definition: Process of obtaining crystals of a substance from its solution.

2. Example: Crystallization of common salt from seawater.

3. Steps:

Dissolve impure substance in water.

Filter the solution to remove insoluble impurities.

Allow the solution to cool and form crystals.

Examples of Chemical Reactions

1. Rusting of Iron: Iron reacts with

oxygen and moisture to form iron oxide (rust).

2. Reaction between Vinegar and Baking

Soda: Produces carbon dioxide gas.

3. Reaction between Copper Sulphate Solution and Iron Nails: Iron displaces copper from copper sulphate solution, forming iron sulphate and copper.



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