In aqueous solutions, the solvent used is:
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- Benzene
- Ether
- Alcohol
- Water
The Correct Option is D
Solution and Explanation
Aqueous Solutions and Solvent
An aqueous solution is a solution where the solvent is water. In such solutions, the solute is dissolved in water.
Understanding Aqueous Solutions
In an aqueous solution, the term "aqueous" specifically refers to water being the solvent. This is a key concept in chemistry because water is one of the most common solvents used to dissolve substances, especially ionic compounds.
Why Water is the Solvent
Water is used as a solvent in aqueous solutions due to its unique properties:
- Polarity: Water is a polar molecule, meaning it has a partial positive charge on one side and a partial negative charge on the other. This allows it to dissolve many ionic and polar substances.
- High Solubility: Water can dissolve a wide range of substances, including salts, acids, and gases, making it an excellent solvent for many chemical reactions.
- Ability to form hydrogen bonds: Water molecules can form hydrogen bonds with various solutes, enhancing the dissolving process.
Common Examples of Aqueous Solutions
Some examples of aqueous solutions include:
- Sodium chloride (NaCl) in water, commonly known as saltwater.
- Hydrochloric acid (HCl) in water, forming a strong acid solution.
- Sugar (C₆H₁₂O₆) dissolved in water to make a sweet solution.
Other Solvents and Their Roles
While water is the most common solvent for aqueous solutions, other solvents like benzene, ether, and alcohol are used in different types of solutions:
- Benzene: A non-polar solvent used in organic chemistry, but not in aqueous solutions.
- Ether: Another organic solvent used for dissolving non-polar substances, but not suitable for aqueous solutions.
- Alcohol: Commonly used as a solvent in both organic and aqueous solutions, depending on the substance being dissolved.
Conclusion
In summary, the solvent used in aqueous solutions is water, which provides an ideal environment for dissolving many substances due to its polarity, high solubility, and hydrogen bonding ability.
Top Questions on Solutions
- Consider the dissociation equilibrium of the following weak acid: \[ \mathrm{HA \rightleftharpoons H^+(aq) + A^-(aq)} \] If the \(pK_a\) of the acid is \(4\), then the pH of a \(10\ \text{mM}\) HA solution is ________ (Nearest integer). (Given: The degree of dissociation can be neglected with respect to unity)
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Assume complete dissociation of NaCl
(Given : Molar mass of Na and Cl are 23 and 35.5 g mol$^{-1}$ respectively.) A substance 'X' (1.5 g) dissolved in 150 g of a solvent 'Y' (molar mass = 300 g mol$^{-1}$) led to an elevation of the boiling point by 0.5 K. The relative lowering in the vapour pressure of the solvent 'Y' is $____________ \(\times 10^{-2}\). (nearest integer)
[Given : $K_{b}$ of the solvent = 5.0 K kg mol$^{-1}$]
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