NCERT Solutions for Class 10 Science Chapter 1 Activity 1.2

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NCERT Solutions for Class 10 Science Chapter 1 Activity 1.2

Welcome to this comprehensive guide where we explore the NCERT Solutions for Class 10 Science Chapter 1 Activity 1.2. This activity is a fundamental experiment in understanding chemical reactions and equations, specifically focusing on double displacement reactions. In this detailed solution, we will walk through the complete procedure, observations, chemical equations, and scientific explanations to help you master this important concept from the ncert solutions for class 10 science curriculum.

Understanding the Activity 🧐

The NCERT Solutions for Class 10 Science Chapter 1 Activity 1.2 demonstrates one of the most visually striking chemical reactions you'll encounter in your Class 10 Science journey. This activity involves mixing two aqueous solutions – lead nitrate and potassium iodide – to observe a beautiful double displacement reaction. The core scientific principle here is understanding how ions in solution can exchange partners to form new compounds, particularly when one of those compounds is insoluble and forms a precipitate.

Think of this reaction like a dance where partners swap! Lead ions (\(\ce{Pb^{2+}}\)) initially paired with nitrate ions (\(\ce{NO3-}\)) decide to partner with iodide ions (\(\ce{I-}\)), while potassium ions (\(\ce{K+}\)) pair up with nitrate ions. The result? A brand new compound – lead iodide – that's so insoluble it immediately falls out of solution as a bright yellow solid!

📋 Activity 1.2: Procedure and Observation

Aim: To observe the reaction between lead nitrate solution and potassium iodide solution and identify the type of chemical reaction.

Materials Required 🧪

  • Lead nitrate solution (\(\ce{Pb(NO3)2}\)) – approximately 5 mL
  • Potassium iodide solution (\(\ce{KI}\)) – approximately 5 mL
  • Test tube
  • Test tube holder
  • Dropper or pipette
⚠️ Safety Precautions: Lead nitrate is toxic. Avoid direct contact with skin and eyes. Always wear safety goggles and gloves. Perform this experiment under teacher supervision in a well-ventilated laboratory. Wash hands thoroughly after the activity.

Step-by-Step Procedure 📝

Step 1: Take a clean, dry test tube and add approximately 5 mL of lead nitrate solution (\(\ce{Pb(NO3)2}\)) into it. The solution should be clear and colorless.
Step 2: Using a dropper or pipette, carefully add approximately 5 mL of potassium iodide solution (\(\ce{KI}\)) to the test tube containing lead nitrate solution. The potassium iodide solution is also clear and colorless initially.
Step 3: Observe the reaction immediately. Note any color changes, formation of precipitate, or other visible changes in the test tube.
Step 4: Allow the test tube to stand for a few minutes and observe if the precipitate settles at the bottom.

Observation 👁️

What do you observe?

When potassium iodide solution is added to lead nitrate solution, the following observation is made:

✅ A bright yellow precipitate forms immediately in the test tube.
✅ The yellow precipitate is lead iodide (\(\ce{PbI2}\)).
✅ The precipitate gradually settles at the bottom of the test tube.
✅ The solution above the precipitate (called the supernatant) remains colorless and contains dissolved potassium nitrate (\(\ce{KNO3}\)).

Chemical Equation and Explanation 🔬

The NCERT Solutions for Class 10 Science Chapter 1 Activity 1.2 beautifully demonstrates a double displacement reaction. Let's break down the chemistry step by step:

Word Equation:

Lead nitrate + Potassium iodide → Lead iodide + Potassium nitrate

Balanced Chemical Equation:

\[\ce{Pb(NO3)2(aq) + 2KI(aq) -> PbI2(s) + 2KNO3(aq)}\]

Detailed Explanation:

1. Reactants:

  • Lead nitrate (\(\ce{Pb(NO3)2}\)) – This compound dissociates in water to form lead ions (\(\ce{Pb^{2+}}\)) and nitrate ions (\(\ce{NO3-}\)).
  • Potassium iodide (\(\ce{KI}\)) – This compound dissociates in water to form potassium ions (\(\ce{K+}\)) and iodide ions (\(\ce{I-}\)).

2. The Reaction Process:

When these two solutions are mixed, the ions are free to move and interact. According to the principles of double displacement reactions, the positive ions (cations) exchange their negative ion partners (anions):

  • \(\ce{Pb^{2+}}\) ions from lead nitrate combine with \(\ce{I-}\) ions from potassium iodide
  • \(\ce{K+}\) ions from potassium iodide combine with \(\ce{NO3-}\) ions from lead nitrate

3. Products:

  • Lead iodide (\(\ce{PbI2}\)) – This is insoluble in water and appears as a bright yellow precipitate. The (s) notation indicates it's in solid state.
  • Potassium nitrate (\(\ce{KNO3}\)) – This is soluble in water and remains dissolved in the solution. The (aq) notation indicates it's in aqueous state.

4. Why Does a Precipitate Form?

The key to understanding this reaction lies in solubility rules. While lead nitrate, potassium iodide, and potassium nitrate are all soluble in water, lead iodide is highly insoluble. When \(\ce{Pb^{2+}}\) and \(\ce{I-}\) ions meet, they immediately form solid \(\ce{PbI2}\) crystals that cannot remain dissolved. This solid separates from the solution as a precipitate.

Type of Reaction 🎯

The reaction observed in NCERT Solutions for Class 10 Science Chapter 1 Activity 1.2 is classified as:

🔹 Double Displacement Reaction (or Double Decomposition Reaction)

In a double displacement reaction, two compounds exchange their ions or radicals to form two new compounds. The general form is:

\[\ce{AB + CD -> AD + CB}\]

In our case:

  • \(\ce{A = Pb^{2+}}\) (lead ion)
  • \(\ce{B = NO3-}\) (nitrate ion)
  • \(\ce{C = K+}\) (potassium ion)
  • \(\ce{D = I-}\) (iodide ion)

The ions swap partners: \(\ce{Pb^{2+}}\) pairs with \(\ce{I-}\) to form \(\ce{PbI2}\), and \(\ce{K+}\) pairs with \(\ce{NO3-}\) to form \(\ce{KNO3}\).

🔹 Precipitation Reaction

This reaction is also a precipitation reaction because one of the products (\(\ce{PbI2}\)) is insoluble and forms a precipitate (solid particles suspended in the liquid that eventually settle down).

A precipitation reaction occurs when two soluble salts react to form an insoluble salt that separates from the solution as a solid.

Ionic Equation Representation 📊

For a deeper understanding, let's look at the ionic equation for this reaction:

Complete Ionic Equation:

\[\ce{Pb^{2+}(aq) + 2NO3^{-}(aq) + 2K^{+}(aq) + 2I^{-}(aq) -> PbI2(s) + 2K^{+}(aq) + 2NO3^{-}(aq)}\]

Net Ionic Equation:

If we remove the spectator ions (ions that don't participate in the reaction – \(\ce{K+}\) and \(\ce{NO3-}\)), we get:

\[\ce{Pb^{2+}(aq) + 2I^{-}(aq) -> PbI2(s)}\]

This net ionic equation shows that the actual reaction is between lead ions and iodide ions to form lead iodide precipitate.

Why is This Reaction Important? 💡

Understanding the NCERT Solutions for Class 10 Science Chapter 1 Activity 1.2 is crucial because:

  1. Visual Learning: The bright yellow precipitate makes this reaction easy to observe and remember, helping you understand abstract chemical concepts through concrete visual evidence.
  2. Understanding Ion Exchange: This activity demonstrates how ions in solution can move freely and combine to form new compounds based on their chemical properties.
  3. Solubility Concepts: You learn about solubility rules – why some compounds dissolve in water while others don't.
  4. Predicting Reactions: Once you understand double displacement reactions, you can predict the products of similar reactions between other ionic compounds.
  5. Real-World Applications: Precipitation reactions are used in:
    • Water treatment to remove unwanted ions
    • Qualitative analysis to identify unknown substances
    • Manufacturing of certain chemicals and pigments
    • Medical diagnostics
💡 Fun Fact: Lead iodide (\(\ce{PbI2}\)) is not just any yellow precipitate – it has a beautiful golden-yellow color that has been used historically as a pigment in art! However, due to lead's toxicity, it's no longer commonly used. The precipitate you see in this experiment demonstrates the same stunning color that artists once valued. Additionally, if you heat lead iodide, it turns red, and when it cools down, it returns to yellow – a reversible color change!

Conclusion and Key Principles ✅

The NCERT Solutions for Class 10 Science Chapter 1 Activity 1.2 provides an excellent hands-on demonstration of double displacement reactions and precipitation reactions. Through this simple yet powerful experiment, you've learned how lead nitrate reacts with potassium iodide to produce a bright yellow precipitate of lead iodide and a solution of potassium nitrate.

The key takeaway from this activity is understanding that in a double displacement reaction, ions exchange partners to form new compounds. When one of these new compounds is insoluble, it forms a precipitate – a solid that separates from the solution. This fundamental concept appears throughout chemistry and is essential for understanding more complex reactions you'll encounter in higher classes.

Remember, the ncert solutions for class 10 science are designed to build your conceptual understanding through practical activities like Activity 1.2, making chemistry not just a subject to memorize, but a fascinating science to explore and understand!

📌 Key Points to Remember:

  • Reactants: Lead nitrate (\(\ce{Pb(NO3)2}\)) and Potassium iodide (\(\ce{KI}\)) – both are colorless solutions
  • Products: Lead iodide (\(\ce{PbI2}\)) – yellow precipitate, and Potassium nitrate (\(\ce{KNO3}\)) – colorless solution
  • Balanced Equation: \(\ce{Pb(NO3)2(aq) + 2KI(aq) -> PbI2(s) + 2KNO3(aq)})
  • Type of Reaction: Double displacement reaction and Precipitation reaction
  • Observation: Bright yellow precipitate of lead iodide forms immediately
  • Reason for Precipitate: Lead iodide is insoluble in water
  • State Symbols: (aq) = aqueous (dissolved in water), (s) = solid (precipitate)
  • Safety: Lead compounds are toxic – handle with care and follow safety precautions
  • Spectator Ions: \ce K + \ceK+ and \ce N O 3 − \ceNO3− ions don't participate in the actual reaction
  • Net Ionic Equation: \ce P b 2 + ( a q ) + 2 I − ( a q ) − > P b I 2 ( s ) \cePb 2+ (aq)+2I − (aq)−>PbI2(s)

Frequently Asked Questions (FAQ) ❓

What is Activity 1.2 in Class 10 Science Chapter 1?

Activity 1.2 is a practical experiment from NCERT Class 10 Science Chapter 1 (Chemical Reactions and Equations) where students mix lead nitrate solution with potassium iodide solution to observe a double displacement reaction. The reaction produces a bright yellow precipitate of lead iodide (\(\ce{PbI2}\)) and demonstrates how ions exchange partners to form new compounds. This activity helps students understand precipitation reactions and chemical equation balancing through visual observation.

What is observed when lead nitrate reacts with potassium iodide?

When lead nitrate solution (\(\ce{Pb(NO3)2}\)) is mixed with potassium iodide solution (\(\ce{KI}\)), a bright yellow precipitate forms immediately. This yellow solid is lead iodide (\(\ce{PbI2}\)), which is insoluble in water. The precipitate gradually settles at the bottom of the test tube, while the solution above (supernatant) remains colorless and contains dissolved potassium nitrate (\(\ce{KNO3}\)). The reaction is instantaneous and visually striking, making it an excellent demonstration of chemical change.

What is the chemical equation for Activity 1.2?

The balanced chemical equation for Activity 1.2 is:

Word Equation: Lead nitrate + Potassium iodide → Lead iodide + Potassium nitrate

Chemical Equation: \(\ce{Pb(NO3)2(aq) + 2KI(aq) -> PbI2(s) + 2KNO3(aq)}\)

Here, (aq) indicates aqueous state (dissolved in water) and (s) indicates solid state (precipitate). Note that 2 molecules of potassium iodide are needed to balance the equation because lead has a +2 charge and needs two iodide ions (each with -1 charge) to form neutral lead iodide.

What type of reaction is Activity 1.2?

Activity 1.2 demonstrates two types of reactions simultaneously:

1. Double Displacement Reaction: Two compounds exchange their ions to form two new compounds. The general form is \(\ce{AB + CD -> AD + CB}\). In this case, lead ions (\(\ce{Pb^{2+}}\)) swap partners with potassium ions (\(\ce{K+}\)).

2. Precipitation Reaction: A reaction where an insoluble solid (precipitate) forms when two solutions are mixed. Lead iodide (\(\ce{PbI2}\)) is insoluble and precipitates out as a yellow solid.

Both classifications are correct and describe different aspects of the same reaction.

Why does a yellow precipitate form in Activity 1.2?

The yellow precipitate forms because lead iodide (\(\ce{PbI2}\)) is highly insoluble in water. When lead ions (\(\ce{Pb^{2+}}\)) from lead nitrate meet iodide ions (\(\ce{I-}\)) from potassium iodide in solution, they immediately combine to form \(\ce{PbI2}\). According to solubility rules, most iodides are soluble except for those of lead, silver, and mercury. Since lead iodide cannot dissolve in water, it separates from the solution as solid yellow crystals – the precipitate we observe. The yellow color is a characteristic property of lead iodide compound.

What safety precautions should be taken during Activity 1.2?

Important Safety Precautions:
⚠️ Lead nitrate is toxic – avoid direct contact with skin, eyes, and mouth
⚠️ Always wear safety goggles and gloves during the experiment
⚠️ Perform the activity in a well-ventilated laboratory under teacher supervision
⚠️ Do not inhale fumes or dust from lead compounds
⚠️ Wash hands thoroughly with soap and water after completing the activity
⚠️ Dispose of chemicals properly according to school guidelines – do not pour down the sink
⚠️ Clean up any spills immediately
⚠️ Never taste or eat anything in the laboratory

What is a double displacement reaction?

A double displacement reaction (also called double decomposition or metathesis reaction) is a type of chemical reaction where two compounds exchange their positive and negative ions to form two entirely new compounds. The general form is:

\(\ce{AB + CD -> AD + CB}\)

Where A and C are typically positive ions (cations), and B and D are negative ions (anions). In Activity 1.2, \(\ce{Pb(NO3)2}\) and \(\ce{KI}\) exchange ions: lead (\(\ce{Pb^{2+}}\)) combines with iodide (\(\ce{I-}\)) to form \(\ce{PbI2}\), while potassium (\(\ce{K+}\)) combines with nitrate (\(\ce{NO3-}\)) to form \(\ce{KNO3}\). These reactions often occur in aqueous solutions and may produce a precipitate, gas, or water.

Can we use other solutions instead of lead nitrate in Activity 1.2?

Yes! Many other combinations can demonstrate double displacement and precipitation reactions:

1. Silver nitrate + Sodium chloride: \(\ce{AgNO3 + NaCl -> AgCl(s) + NaNO3}\) – Forms white precipitate of silver chloride

2. Barium chloride + Sodium sulphate: \(\ce{BaCl2 + Na2SO4 -> BaSO4(s) + 2NaCl}\) – Forms white precipitate of barium sulphate

3. Calcium chloride + Sodium carbonate: \(\ce{CaCl2 + Na2CO3 -> CaCO3(s) + 2NaCl}\) – Forms white precipitate of calcium carbonate

4. Copper sulphate + Sodium hydroxide: \(\ce{CuSO4 + 2NaOH -> Cu(OH)2(s) + Na2SO4}\) – Forms blue precipitate of copper hydroxide

Each combination produces different colored precipitates, making them excellent for demonstrating chemical reactions!

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💬 Common Questions

Here are frequently asked questions by students about Activity 1.2:

  • What happens when lead nitrate solution is mixed with potassium iodide solution?
  • Why does a yellow precipitate form in Activity 1.2?
  • What is the balanced chemical equation for the reaction between lead nitrate and potassium iodide?
  • Is Activity 1.2 a double displacement reaction or precipitation reaction?
  • What are the products formed in Activity 1.2 of Class 10 Science?
  • How do you write the ionic equation for lead nitrate and potassium iodide reaction?
  • What is the color of lead iodide precipitate?
  • Why is lead iodide insoluble in water?
  • What safety precautions should be taken while performing Activity 1.2?
  • Can we reverse the reaction in Activity 1.2?
  • What are spectator ions in Activity 1.2?
  • How do you balance the equation for lead nitrate and potassium iodide?
  • What is the difference between double displacement and precipitation reaction?
  • Give examples of other precipitation reactions similar to Activity 1.2
  • What is the net ionic equation for Activity 1.2 reaction?

Additional Insights and Extended Learning 📚

Understanding Solubility Rules 💧

The formation of precipitate in Activity 1.2 is governed by solubility rules. These are general guidelines that help predict whether a compound will dissolve in water or form a precipitate:

Ion/Compound Type Solubility Rule Important Exceptions
Nitrates (\(\ce{NO3-}\)) All nitrates are soluble No exceptions
Chlorides, Bromides, Iodides Most are soluble Insoluble: \(\ce{AgCl}\), \(\ce{PbCl2}\), \(\ce{Hg2Cl2}\), \(\ce{PbI2}\)
Sulphates (\(\ce{SO4^{2-}}\)) Most are soluble Insoluble: \(\ce{BaSO4}\), \(\ce{PbSO4}\), \(\ce{CaSO4}\)
Carbonates (\(\ce{CO3^{2-}}\)) Most are insoluble Soluble: \(\ce{Na2CO3}\), \(\ce{K2CO3}\), \(\ce{(NH4)2CO3}\)
Hydroxides (\(\ce{OH-}\)) Most are insoluble Soluble: \(\ce{NaOH}\), \(\ce{KOH}\), \(\ce{Ba(OH)2}\)

In Activity 1.2, lead iodide (\(\ce{PbI2}\)) falls into the exception category for iodides – it's one of the few iodides that is insoluble in water, which is why it forms a precipitate.

Real-World Applications of Precipitation Reactions 🌍

The type of reaction you observed in NCERT Solutions for Class 10 Science Chapter 1 Activity 1.2 has numerous practical applications:

1. Water Purification: Precipitation reactions are used to remove harmful ions from water. For example, adding lime (\(\ce{Ca(OH)2}\)) to hard water precipitates out calcium and magnesium compounds, softening the water.

2. Qualitative Analysis: In chemistry laboratories, precipitation reactions help identify unknown substances. Different ions produce characteristic colored precipitates that help chemists determine what's in a sample.

3. Medical Diagnostics: Some medical tests use precipitation reactions. For example, detecting proteins in urine or identifying blood types involves precipitation reactions.

4. Industrial Manufacturing: Many industrial processes use precipitation to purify products or remove unwanted impurities. For instance, in the production of certain chemicals and pharmaceuticals.

5. Environmental Monitoring: Precipitation reactions help detect and measure pollutants in water samples, such as heavy metals like lead, mercury, and cadmium.

6. Photography: Traditional photography used silver halide precipitation reactions. Silver bromide (\(\ce{AgBr}\)), which is light-sensitive, was used in photographic films.

Comparison with Other Activities in Chapter 1 📊

Activity 1.2 is part of a series of activities in Chapter 1 that demonstrate different types of chemical reactions:

Activity 1.1: Burning of magnesium ribbon – demonstrates combination reaction and oxidation

Activity 1.2: Lead nitrate + Potassium iodide – demonstrates double displacement and precipitation reaction

Activity 1.3: Heating of ferrous sulphate – demonstrates decomposition reaction

Activity 1.4: Iron nail in copper sulphate solution – demonstrates displacement reaction

Each activity builds your understanding of different reaction types, and together they provide a comprehensive foundation for studying chemical reactions in the ncert solutions for class 10 science curriculum.

💡 Did You Know? The reaction in Activity 1.2 is so reliable and produces such a distinctive yellow precipitate that it's sometimes used as a qualitative test for the presence of lead ions (\(\ce{Pb^{2+}}\)) in solution! If you add potassium iodide to an unknown solution and get a bright yellow precipitate, you can be fairly confident that lead ions are present. This is called a "confirmatory test" for lead in analytical chemistry.

Troubleshooting Common Issues ⚠️

If the precipitate doesn't form or is not clearly visible:

  • Check concentration: Solutions might be too dilute. Use freshly prepared solutions with appropriate concentrations.
  • Verify chemicals: Ensure you're using the correct chemicals – lead nitrate and potassium iodide, not other compounds.
  • Mix thoroughly: Gently shake or stir the test tube to ensure proper mixing of the solutions.
  • Allow time: Although the reaction is instantaneous, sometimes it takes a few seconds for the precipitate to become clearly visible.
  • Use clean glassware: Contaminated test tubes might interfere with the reaction.
  • Check expiry: Old or degraded chemicals might not react properly.

Practice Questions for Better Understanding 📝

To master the concepts from Activity 1.2, try answering these questions:

  1. Write the balanced chemical equation for the reaction between lead nitrate and potassium iodide, including state symbols.
  2. Identify the type of reaction observed in Activity 1.2 and explain why it is classified as such.
  3. What is a precipitate? Why does lead iodide form a precipitate while potassium nitrate remains in solution?
  4. Write the net ionic equation for the reaction in Activity 1.2. Which ions are spectator ions?
  5. If you have 10 mL of 0.1 M lead nitrate solution, how much 0.1 M potassium iodide solution would you need to completely react with it? (Hint: Use the balanced equation)
  6. Predict what would happen if you mixed silver nitrate solution with sodium chloride solution. Write the equation and identify the precipitate.
  7. Explain the difference between a double displacement reaction and a single displacement reaction with examples.
  8. Why is it important to use aqueous solutions in Activity 1.2? What would happen if you mixed solid lead nitrate with solid potassium iodide?

Practicing these questions will deepen your understanding of the concepts demonstrated in Activity 1.2 and prepare you well for examinations!

Connection to Other Chemistry Concepts 🔗

The NCERT Solutions for Class 10 Science Chapter 1 Activity 1.2 connects to several important chemistry concepts you'll encounter throughout your studies:

1. Ionic Bonding: The formation of lead iodide demonstrates how ionic compounds form through the transfer of electrons and electrostatic attraction between oppositely charged ions.

2. Chemical Equilibrium: Although not immediately apparent, the precipitation reaction reaches an equilibrium between the dissolved ions and the solid precipitate. This concept becomes important in higher classes.

3. Stoichiometry: The balanced equation shows the exact ratio in which reactants combine (1:2 ratio of lead nitrate to potassium iodide), which is fundamental to quantitative chemistry.

4. Solubility Product (Ksp): In Class 11 and 12, you'll learn that the solubility of compounds like lead iodide can be expressed mathematically using the solubility product constant.

5. Qualitative Analysis: This activity introduces you to the concept of using chemical reactions to identify substances, which is the basis of analytical chemistry.

6. Environmental Chemistry: Understanding precipitation reactions helps in comprehending how pollutants can be removed from water or how minerals precipitate in natural water bodies.

Final Summary and Exam Tips 🎓

🎯 Exam-Focused Key Points:

  • Always write state symbols in chemical equations: (aq) for aqueous, (s) for solid, (l) for liquid, (g) for gas
  • Balance equations correctly: Remember that 2 moles of \(\ce{KI}\) are needed for 1 mole of \(\ce{Pb(NO3)2}\)
  • Identify reaction types: Activity 1.2 is BOTH a double displacement AND a precipitation reaction
  • Describe observations clearly: "Bright yellow precipitate of lead iodide forms" is better than just "yellow color appears"
  • Explain the science: Don't just state what happens – explain WHY it happens (solubility rules, ion exchange, etc.)
  • Know the colors: Lead iodide = yellow, Silver chloride = white, Copper hydroxide = blue, etc.
  • Safety matters: Always mention safety precautions when describing practical activities
  • Connect to real life: Being able to give practical applications shows deeper understanding
🌟 Exam Success Tip: When writing about Activity 1.2 in exams, structure your answer in this order: (1) Aim of the activity, (2) Procedure, (3) Observation, (4) Chemical equation with balancing, (5) Type of reaction with explanation, (6) Conclusion. This logical flow ensures you cover all aspects and score maximum marks!

Congratulations! 🎉 You've now mastered the NCERT Solutions for Class 10 Science Chapter 1 Activity 1.2. This comprehensive understanding will serve as a strong foundation for your chemistry studies. Keep practicing, stay curious, and remember – chemistry is all around us, making our world colorful and fascinating, just like that bright yellow precipitate!

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