My own custom emoji , You can also use !

🔬 My Chemistry Emoji Symbols

💧

H₂O

Water

Used in every reaction!

🎈

H₂

Hydrogen Gas

Explosive – pop test

🌫️

CO₂

Carbon Dioxide

Extinguishes fire

🧪

HCl

Hydrochloric Acid

Strong acid in labs

☣️

H₂SO₄

Sulfuric Acid

Corrosive oxidizer

🍬

C₆H₁₂O₆

Glucose

Sugar in respiration

⚙️

Zn

Zinc

Metal in acid tests

🧲

Fe

Iron

Used in rusting demo

🪨

CaCO₃

Calcium Carbonate

In limestone/chalk

Different reactions of acid

🧪 Reactions of Acids with Other Substances

Acids are powerful chemical substances that show different types of reactions depending on what they interact with. In this article, we explore the reactions of acids with bases, metals, non-metals, carbonates, and bicarbonates in a simple and interactive way.

1️⃣ Acid + Base → Salt + Water

🧬 This is called a Neutralization Reaction

When an acid reacts with a base, it forms salt and water. This reaction is known as neutralization and it helps in reducing the effect of both acid and base.

HCl + NaOH → NaCl + H₂O

✔️ This is an exothermic reaction (heat is released).

2️⃣ Acid + Metal → Salt + Hydrogen Gas

🧪 Formation of Hydrogen Gas

Acids react with reactive metals like zinc, magnesium, and iron to form salt and release hydrogen gas.

Zn + 2HCl → ZnCl₂ + H₂↑

⚠️ You’ll often see bubbles (effervescence) due to gas release.

3️⃣ Acid + Non-Metal Oxide → No Reaction

🚫 No Chemical Change Occurs

Acids do not react with non-metal oxides like carbon dioxide (CO₂), as both are acidic in nature.

CO₂ + HCl → ❌ No Reaction

🔍 Non-metal oxides are acidic, hence no acid-acid reaction occurs.

4️⃣ Acid + Carbonate → Salt + Water + Carbon Dioxide

🎈 Fizzing Due to CO₂ Formation

Acids react with carbonates like calcium carbonate (chalk) to form salt, water, and carbon dioxide gas.

CaCO₃ + 2HCl → CaCl₂ + H₂O + CO₂↑

🫧 You can observe fizzing or bubbles due to carbon dioxide release.

5️⃣ Acid + Bicarbonate → Salt + Water + Carbon Dioxide

🧁 Common in Baking Soda Reactions

Acids react with bicarbonates like sodium bicarbonate (baking soda) to form salt, water, and CO₂.

NaHCO₃ + HCl → NaCl + H₂O + CO₂↑

🎉 This reaction is commonly used in baking for leavening.

Potassium Permanganate: Uses, Properties, Reactions & Safety

Potassium Permanganate (KMnO₄)

Potassium permanganate (KMnO₄) is a dark purple crystalline compound widely used in chemistry and industry as a strong oxidizing agent. It is soluble in water and produces a pink or purple solution. Due to its powerful oxidation properties, it is used in water treatment, disinfection, and organic synthesis.

• Color: Deep purple or dark violet crystals
• Solubility: Soluble in water, producing purple solutions
• Melting Point: Decomposes at 240°C
• Odor: Odorless
• Molar Mass: 158.03 g/mol

KMnO₄ is a strong oxidizing agent. In acidic conditions, it gets reduced from Mn⁷⁺ to Mn²⁺:

2 KMnO₄ + 3 H₂SO₄ → 2 MnSO₄ + K₂SO₄ + 3 H₂O + 5 [O]

In alkaline or neutral medium, it forms MnO₂ (manganese dioxide):

2 KMnO₄ + H₂O → 2 MnO₂ + 2 KOH + 3 [O]

• Water purification: Removes iron, manganese, and odors.
• Medical use: Antiseptic for wounds and fungal infections.
• Organic chemistry: Used in oxidation reactions.
• Textile industry: Bleaching and dyeing agent.
• Waste treatment: Removes hydrogen sulfide and other pollutants.

• KMnO₄ is a strong oxidizer; avoid contact with organic matter or reducing agents.
• It can cause skin and eye irritation; always wear gloves and goggles.
• Store in a cool, dry place away from combustible materials.
• In case of ingestion or inhalation, seek immediate medical help.

Did you know? In the 19th century, potassium permanganate was used as a cure for snakebites and as a disinfectant in hospitals. Its deep purple color also made it popular in experiments and demonstrations in school labs.

Molar concept

Concept of Mole in Chemistry

The mole is one of the most fundamental concepts in chemistry. It bridges the gap between the atomic scale and the real-world scale. When chemists deal with atoms, molecules, or ions, their sizes are too small to be counted individually in a practical sense. That’s where the mole comes into play.

Definition of Mole

A mole is defined as the amount of substance that contains exactly 6.022 × 10²³ particles (atoms, molecules, ions, etc.). This number is called Avogadro's number.

"One mole of a substance is the quantity that contains as many elementary units as there are atoms in 12 grams of carbon-12."

Why Do We Use Mole?

Atoms and molecules are incredibly tiny. A single drop of water contains over a billion billion molecules. Using moles allows scientists to count these minuscule particles in manageable quantities. It is a counting unit just like:

• 1 dozen = 12 items
• 1 gross = 144 items
• 1 mole = 6.022 × 10²³ particles

📌 Remember: The mole is not the mass or volume — it is a number of particles.

Avogadro's Number

Avogadro's number (6.022 × 10²³) is a huge quantity, but it allows accurate conversions between mass, number of particles, and volume. This number is constant for all substances.

Mass and the Mole

To relate the mole to the mass of a substance, we use the molar mass, which is the mass of one mole of a substance. The molar mass of a substance in grams is numerically equal to its atomic or molecular mass in atomic mass units (amu).

Moles = Mass (g) / Molar Mass (g/mol)

🧪 Example: If you have 18 grams of water (H₂O), how many moles is that?
Molar Mass of H₂O = 18 g/mol
Moles = 18 / 18 = 1 mole

Volume and the Mole

For gases, the mole is also related to volume. At Standard Temperature and Pressure (STP: 0°C and 1 atm), one mole of any gas occupies 22.4 L.

🧪 Example: 2 moles of oxygen gas will occupy = 2 × 22.4 = 44.8 L at STP.

Mole and Number of Particles

To calculate the number of atoms, molecules, or ions from moles, multiply the given moles by Avogadro’s number.

Particles = Moles × 6.022 × 10²³

Applications of the Mole Concept

• Determining chemical formulas
• Balancing chemical equations
• Calculating theoretical yields
• Analyzing gases in stoichiometry

Without the mole, chemistry would be like doing math without numbers.

Conclusion

The concept of the mole is essential in chemistry as it provides a bridge between the atomic and macroscopic worlds. Whether it's measuring reactants, calculating yields, or analyzing molecular formulas, the mole serves as the cornerstone of quantitative chemistry. A strong grasp of the mole concept enables better understanding of all chemical calculations and laboratory experiments.

💡 Tip: Always check the units: grams, liters, or particles — and apply the correct mole formula.