Effect of Pressure on Solubility of Gases in Liquids

 Here’s a clear, CBSE Class 12–friendly explanation of the effect of pressure on the solubility of gases in liquids, including Henry’s Law — perfect for class presentations, revision notes, and board exam prep:

🧯 Effect of Pressure on Solubility of Gases in Liquids

📖 Key Concept:

Solubility of a gas in a liquid increases with an increase in pressure.

🔍 Why Does This Happen?

  • When the pressure above a liquid is increased, more gas molecules are forced into the liquid.

  • This increases the rate at which gas particles enter the solution, so more gas dissolves.

📌 A new equilibrium is established where more gas is dissolved.

📘 Henry’s Law – The Scientific Explanation

At constant temperature, the solubility of a gas in a liquid is directly proportional to the partial pressure of the gas above the liquid.

🧪 Formula:

p=KH⋅xp = K_H \cdot x

Where:

  • p = partial pressure of the gas

  • x = mole fraction of the gas in the solution

  • KH = Henry’s law constant (depends on nature of gas & temperature)

📌 Higher pressure (p) ⇒ Higher mole fraction (x) ⇒ More gas dissolves

🧠 Real-Life Examples:

  1. Soft Drinks – CO₂ is dissolved in soda under high pressure

  2. Scuba Diving – Under high pressure, more nitrogen dissolves in blood

  3. Canned Beer – Pressurized CO₂ keeps beer fizzy until the can is opened

📌 Summary Table:

Factor Effect on Gas Solubility in Liquid
↑ Pressure ↑ Solubility
↓ Pressure ↓ Solubility

📝 CBSE Exam Tip:

  • Define Henry’s Law clearly with the formula

  • Mention "increase in pressure increases gas solubility"

  • Add 1–2 applications like soda or diving for full marks

Would you like a diagram or animated slide to demonstrate this concept in class?

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