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Chemistry of the Environment - Fertilisers (NPK)

Grade 11A LevelChemistry

Review the key concepts, formulae, and examples before starting your quiz.

🔑Concepts

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Plants require three essential elements for healthy growth: Nitrogen (NN), Phosphorus (PP), and Potassium (KK). These are often supplied via NPK fertilisers.

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Nitrogen (NN) is vital for the synthesis of proteins and chlorophyll, promoting healthy leaf and stem growth. Common sources include NH4NO3NH_{4}NO_{3} and (NH4)2SO4(NH_{4})_{2}SO_{4}.

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Phosphorus (PP) is essential for root development and energy transfer (ATP). It is often supplied as ammonium phosphate (NH4)3PO4(NH_{4})_{3}PO_{4} or calcium dihydrogenphosphate Ca(H2PO4)2Ca(H_{2}PO_{4})_{2}.

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Potassium (KK) helps in the regulation of water movement and enzyme activation, which is critical for flower and fruit production. It is typically supplied as KClKCl or K2SO4K_{2}SO_{4}.

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Ammonium salts are prepared by reacting ammonia (NH3NH_{3}) with an appropriate acid. For example, NH3+HNO3→NH4NO3NH_{3} + HNO_{3} \rightarrow NH_{4}NO_{3}.

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Ammonia displacement: If an alkali (like lime, Ca(OH)2Ca(OH)_{2}) is added to soil that has been treated with ammonium fertilisers, a reaction occurs that releases ammonia gas (NH3NH_{3}), leading to a loss of nitrogen from the soil: NH4+(aq)+OH−(aq)→NH3(g)+H2O(l)NH_{4}^{+}(aq) + OH^{-}(aq) \rightarrow NH_{3}(g) + H_{2}O(l).

📐Formulae

N2(g)+3H2(g)⇌2NH3(g)N_{2}(g) + 3H_{2}(g) \rightleftharpoons 2NH_{3}(g) (Haber Process for Ammonia)

NH3(aq)+HNO3(aq)→NH4NO3(aq)NH_{3}(aq) + HNO_{3}(aq) \rightarrow NH_{4}NO_{3}(aq) (Formation of Ammonium Nitrate)

2NH3(aq)+H2SO4(aq)→(NH4)2SO4(aq)2NH_{3}(aq) + H_{2}SO_{4}(aq) \rightarrow (NH_{4})_{2}SO_{4}(aq) (Formation of Ammonium Sulfate)

% of element=Total Ar of element in formulaMr of compound×100\% \text{ of element} = \frac{\text{Total } A_r \text{ of element in formula}}{M_r \text{ of compound}} \times 100

💡Examples

Problem 1:

Calculate the percentage by mass of nitrogen in ammonium nitrate, NH4NO3NH_{4}NO_{3}. Given ArA_r values: N=14,H=1,O=16N=14, H=1, O=16.

Solution:

  1. Calculate the MrM_r of NH4NO3NH_{4}NO_{3}: (2×14)+(4×1)+(3×16)=28+4+48=80(2 \times 14) + (4 \times 1) + (3 \times 16) = 28 + 4 + 48 = 80.
  2. Identify the mass of nitrogen: 2×14=282 \times 14 = 28.
  3. Calculate percentage: 2880×100=35%\frac{28}{80} \times 100 = 35\%.

Explanation:

To find the percentage composition, we divide the total relative atomic mass of the specific element by the total relative molecular mass of the entire compound.

Problem 2:

Explain why a farmer should not add calcium hydroxide (Ca(OH)2Ca(OH)_{2}) to a field immediately after applying ammonium sulfate ((NH4)2SO4(NH_{4})_{2}SO_{4}) fertiliser.

Solution:

A chemical reaction occurs between the ammonium salt and the base: (NH4)2SO4+Ca(OH)2→CaSO4+2H2O+2NH3(g)(NH_{4})_{2}SO_{4} + Ca(OH)_{2} \rightarrow CaSO_{4} + 2H_{2}O + 2NH_{3}(g).

Explanation:

Ammonium salts react with alkalis to undergo a displacement reaction. This releases NH3NH_{3} as a gas, which escapes into the atmosphere. This reduces the nitrogen content available in the soil for the plants, making the fertiliser application ineffective.

Fertilisers (NPK) Grade 11 Notes & Examples