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Chapter 2: Problem 12

Among sodium phosphate, sodium sulphate and sodium chloride the solubility in water decreases as : (a) sulphate \(>\) phosphate \(>\) chloride \(-0\) (b) chloride \(>\) sulphate \(>\) phosphate \(\square\) (c) chloride \(>\) phosphate \(>\) sulphate \(\square\) (d) phosphate \(>\) chloride \(>\) sulphate

Short Answer

Expert verified
Option (b): chloride > sulphate > phosphate.

Step by step solution

01

Understand Solubility Rules

Solubility rules help us predict the solubility of ionic compounds in water. Generally, sodium salts such as sodium chloride (NaCl) and sodium sulfate (Na2SO4) are known to be very soluble. However, sodium phosphate (Na3PO4) has comparatively lower solubility in water.
02

Compare Solubility of Sodium Compounds

Based on typical solubility behavior, sodium chloride (NaCl) is highly soluble in water, often more so than sodium sulfate (Na2SO4). Sodium phosphate (Na3PO4) typically has the lowest solubility among the three in water.
03

Rank the Solubilities

Considering the solubility properties: NaCl is generally more soluble than Na2SO4, and both are more soluble than Na3PO4. Therefore, the correct order, from most to least soluble, is chloride > sulfate > phosphate.
04

Identify the Correct Option

Match the order determined in Step 3 with the options provided in the question. The order matches option (b): chloride > sulfate > phosphate.

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Key Concepts

These are the key concepts you need to understand to accurately answer the question.

Sodium Compounds
Sodium compounds play a vital role in both chemical reactions and everyday life. These compounds, containing sodium ions ( ext{Na}^+), readily dissolve in water due to their ionic nature. Some well-known sodium compounds include sodium chloride, sodium phosphate, and sodium sulfate.
  • Sodium chloride (NaCl): Commonly known as table salt, is universally recognized for its essential roles in food seasoning and preservation.
  • Sodium phosphate (Na鈧働O鈧�): Often used in cleaning agents, it stabilizes fluids and contributes to neutralizing acidic solutions.
  • Sodium sulfate (Na鈧係O鈧�): Widely used in the paper and textile industries, known for its utility in manufacturing processes.
Understanding the distinct solubility characteristics of these compounds is crucial when predicting their behavior in different solutions.
Ionic Solubility
The concept of ionic solubility refers to an ionic compound's ability to dissolve in water. This ability is influenced by the charges and sizes of the ions present.
  • Most sodium-based compounds are highly water-soluble, allowing them to dissociate into individual ions.
  • The solubility of an ionic compound can vary widely, dependent on factors like lattice energy and the hydration energy of ions.
When dissolved, these ionic compounds separate into sodium ions and their respective partner ions, enabling them to participate in chemical reactions or conduct electricity. Understanding this process is key to predicting how substances will behave in aqueous environments.
Sodium Phosphate
Sodium phosphate, chemically represented as Na鈧働O鈧�, is a compound comprising three sodium ions and one phosphate ion. Despite its role in many industrial and cleaning applications, it has a lower solubility in water compared to other sodium compounds like sodium chloride.
  • Its limited solubility is due to the phosphate ion which forms a strong lattice structure that is more challenging to break apart.
  • Water solubility affects its utility, making it suitable for uses that do not require complete dissolving.
Its performance in applications where partial solubility is needed showcases the unique properties of sodium phosphate compared to other sodium salts.
Sodium Sulfate
Sodium sulfate, with the formula Na鈧係O鈧�, consists of two sodium ions and one sulfate ion. It is known for its good solubility in water, although not as great as sodium chloride.
  • The compound dissociates easily in water, releasing its ions readily, which enables its effective use in several industrial applications.
  • Its solubility is higher than that of sodium phosphate, allowing for more versatile applications.
Understanding sodium sulfate's solubility helps in determining its suitability for various industries, whether in detergents or in textiles manufacturing processes.
Sodium Chloride
Sodium chloride is the most soluble among the sodium compounds discussed. Represented as NaCl, it separates easily into sodium and chloride ions in water.
  • Its high solubility makes it a primary choice for many applications, including culinary and industrial processes.
  • It is crucial for biological systems, particularly in maintaining fluid balance and conducting nerve impulses.
With its simple ionic structure and significant solubility, sodium chloride's role stretches from the kitchen table to crucial industrial functions, illustrating its versatility and importance in both daily life and specialized processes.

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Most popular questions from this chapter

Hybridisation of the atom changes in : (a) \(\mathrm{AlH}_{3}\) to \(\mathrm{AlH}_{4}^{-}\) \(\square\) (b) \(\mathrm{H}_{2} \mathrm{O}\) to \(\mathrm{H}_{3} \mathrm{O}^{+}\) (c) \(\mathrm{NH}_{3}\) to \(\mathrm{NH}_{4}^{+}\) \(\square\) (d) all of these

Which molecule has zero dipole moment? (a) \(\mathrm{CH}_{2} \mathrm{Cl}_{2}\) \(\square\) (b) \(\mathrm{BF}_{3}\) (c) \(\mathrm{NF}_{3}\) \(\square\) (d) \(\mathrm{ClO}_{2}\)

Electrovalent bond is formed by: (a) sharing of electrons \(\square\) (b) donation of electrons (c) transfer of electrons \(\square\) (d) none of these

Multiple covalent bonds exist in a molecule of: (a) \(\mathrm{F}_{2}\) \(\square\) (b) \(\mathrm{N}_{2}\) (c) \(\mathrm{CH}_{4}\) \(\square\) (d) \(\mathrm{H}_{2}\)

The bond angles of \(\mathrm{NH}_{3}, \mathrm{NH}_{4}^{+}\) and \(\mathrm{NH}_{2}^{-}\) are in the order (a) \(\mathrm{NH}_{2}^{-}>\mathrm{NH}_{3}>\mathrm{NH}_{4}^{+} \square\) (b) \(\mathrm{NH}_{4}^{+}>\mathrm{NH}_{3}>\mathrm{NH}_{2}^{-}\) (c) \(\mathrm{NH}_{3}>\mathrm{NH}_{2}^{-}>\mathrm{NH}_{4}^{+}\) \(\square\) (d) \(\mathrm{NH}_{3}>\mathrm{NH}_{4}^{+}>\mathrm{NH}_{2}\)
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