What is molarity of pure water?
What is molarity of pure water?
- $18.36\, M$
- $1.16 \,M$
- $55.56 \,M$
- $5.56\, M$
The Correct Option is C
Solution and Explanation
Density of water = 1 g/cm3 and its molecular weight is 18. So, 1000 cm3 of water will weigh 1000 g of water.
Now, we know that molarity \(=\frac{\text { Mass of water }}{\text { Molecular weight }}\) \(=\frac{1000}{18}\) \(=55.56 \,M\)
\(Molarity = \frac{\text { Mass of water }}{\text { Molecular weight }}\)
\(Molarity = \frac{1000}{18}\)
\(Molarity = 55.56 M\)
Hence, the molarity of water is 55.56 M.
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Concepts Used:
Solutions
A solution is a homogeneous mixture of two or more components in which the particle size is smaller than 1 nm.
For example, salt and sugar is a good illustration of a solution. A solution can be categorized into several components.
Types of Solutions:
The solutions can be classified into three types:
- Solid Solutions - In these solutions, the solvent is in a Solid-state.
- Liquid Solutions- In these solutions, the solvent is in a Liquid state.
- Gaseous Solutions - In these solutions, the solvent is in a Gaseous state.
On the basis of the amount of solute dissolved in a solvent, solutions are divided into the following types:
- Unsaturated Solution- A solution in which more solute can be dissolved without raising the temperature of the solution is known as an unsaturated solution.
- Saturated Solution- A solution in which no solute can be dissolved after reaching a certain amount of temperature is known as an unsaturated saturated solution.
- Supersaturated Solution- A solution that contains more solute than the maximum amount at a certain temperature is known as a supersaturated solution.