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Chemistry of the Environment - Fertilisers (NPK)

Grade 11IGCSEChemistry

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

🔑Concepts

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

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}.

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}.

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}.

Ammonium salts are prepared by reacting ammonia (NH3NH_{3}) with an appropriate acid. For example, NH3+HNO3NH4NO3NH_{3} + HNO_{3} \rightarrow NH_{4}NO_{3}.

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)2CaSO4+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) - Revision Notes & Key Formulas | IGCSE Grade 11 Chemistry