Which of the following does not cause hardness of water?

Explanation

## Correct Answer: A. Calcium carbonate Calcium carbonate (CaCO₃) is **insoluble** in water and does not contribute to water hardness. Water hardness is defined as the concentration of dissolved minerals—specifically **calcium and magnesium ions**—that remain in solution. CaCO₃ precipitates out as a solid and is therefore not bioavailable in the aqueous phase. This is why CaCO₃ deposits form as scale in pipes and kettles but do NOT increase the ionic hardness of the water itself. In contrast, the bicarbonates and sulphates listed in options B, C, and D are all soluble salts that dissociate into free Ca²⁺ and Mg²⁺ ions, which directly contribute to **temporary hardness** (bicarbonates, removable by boiling) and **permanent hardness** (sulphates, non-removable by boiling). The discriminating principle: only dissolved ions cause hardness; precipitated minerals do not. This distinction is critical in public health engineering and water quality assessment in India, where hardness testing (by EDTA titration or conductivity) measures only soluble ionic species. ## Why the other options are wrong **B. Calcium bicarbonate** — Calcium bicarbonate [Ca(HCO₃)₂] is **soluble** and dissociates completely in water to release Ca²⁺ ions, which are the primary cause of **temporary hardness**. It is removable by boiling (converts back to insoluble CaCO₃ precipitate). This is a classic cause of water hardness in India, especially in limestone and chalk regions. NBE trap: students may confuse the salt form (bicarbonate) with the insoluble carbonate. **C. Magnesium bicarbonate** — Magnesium bicarbonate [Mg(HCO₃)₂] is soluble and releases Mg²⁺ ions, contributing to **temporary hardness** alongside calcium. Magnesium is the second most important hardness-causing cation in natural waters. Like calcium bicarbonate, it is removable by boiling. This is a standard cause of hardness in Indian groundwater, particularly in volcanic and metamorphic regions. **D. Calcium sulphate** — Calcium sulphate (CaSO₄) is soluble (though less so than the bicarbonates) and dissociates to release Ca²⁺ ions, causing **permanent hardness** that cannot be removed by boiling. It is a major contributor to hardness in industrial and agricultural water supplies in India. The sulphate ion does not precipitate on heating, making this a true permanent hardness agent. ## High-Yield Facts - **Temporary hardness** is caused by bicarbonates of Ca²⁺ and Mg²⁺; removable by boiling (converts to insoluble carbonates). - **Permanent hardness** is caused by sulphates, chlorides, and nitrates of Ca²⁺ and Mg²⁺; NOT removable by boiling. - **CaCO₃ is insoluble** and precipitates out; it does NOT dissolve to form hardness-causing ions. - Water hardness is measured by **EDTA titration** (complexometric titration) in Indian public health labs; only dissolved ions are titrated. - **Hardness = 2.5 × [Ca²⁺ mg/L] + 4.1 × [Mg²⁺ mg/L]** (in terms of CaCO₃ equivalents); only soluble ionic species count. ## Mnemonics **BICARBONATE = Temporary (Boilable)** **B**icarbonates → **B**oilable (temporary hardness). Sulphates, chlorides, nitrates → Permanent. Use this when distinguishing hardness types in water quality questions. **CaCO₃ is SOLID, not SOLUTE** Calcium **Carbonate** (not bicarbonate) is insoluble—it's the white scale you see in kettles, NOT dissolved in water. Hardness requires dissolved ions, not precipitates. ## NBE Trap NBE pairs "calcium carbonate" with "hardness" to exploit the common misconception that any calcium salt causes hardness. Students see CaCO₃ deposits in pipes and assume it contributes to hardness, when in fact only the **dissolved bicarbonate and sulphate salts** do. The trap conflates visible mineral deposits with actual ionic hardness. ## Clinical Pearl In Indian villages relying on groundwater, hardness complaints (scale in vessels, soap wastage) correlate with dissolved bicarbonates and sulphates, not with visible CaCO₃ deposits. A water sample may show white precipitate (CaCO₃) yet have low hardness if the precipitate is filtered out—hardness is always a measure of what **remains dissolved**. _Reference: Park's Textbook of Preventive and Social Medicine, Ch. 8 (Water and Health); KD Tripathi Essentials of Medical Pharmacology, Ch. 60 (Water and Electrolytes)_