What is Solution?
A solution is a homogeneous mixture, Which composed of two or more substances. The substances involved in a solution can be in any state of matter - solid, liquid, or gas. The component's particles are evenly distributed at the molecular level, resulting in a uniform appearance throughout the mixture & the size of components particles in solution is less than 1nm.
The two main components of solution :
Solvent:
It is the component present in the larger quantity and serves as the dissolving medium. It has the ability to dissolve other substances. Water is one of the most common solvents, but other substances can also act as solvents depending on the specific solution.
Solute:
It is the component present in the smaller quantity and gets dissolved in the solvent. The solute may exist in various forms, such as ions, molecules, or particles.
Based on the states of the solvent and solute, solutions can be categorized into different types:
Solid solutions: Where the solvent is a solid, and the solute is also a solid, for example, alloys like brass (copper dissolved in zinc).
Liquid solutions: Where both the solvent and solute are liquids, for example, ethanol dissolved in water.
Gaseous solutions: Where both the solvent and solute are gases, for example, air (a mixture of gases dissolved in nitrogen).
What is Concentration of a solution?
Concentration of Solution gives an idea of the amount of solute that has been dissolved in the solution.
Concentration is defined as the quantity of solute dissolved in a solvent. Concentration can be expressed in both qualitative and quantitative (numerically) terms.
Qualitative Expressions of Concentration
Quantitative Expressions of Concentration
In order to characterize the concentrations in an accurate and precise manner, we need quantitative expressions of concentration of solution.
Following terms are used to express concentration of any solution quantitatively,
Mass Percentage (w/w%)
Mass percentage which is also known as weight by weight concentration of solute and it is defined as the amount of solute (in grams) present in 100 gm of the solution.
Mass Percentage = (Mass of Solute / Mass of Solution) × 100
It has no unit because the ratio of the mass of solute and solution.
Volume Percentage (v / v %)
Volume Percentage is also called as volume by volume concentration of solute and is defined as the amount of solute (in ml) present in 100 ml of the solution.
Volume Percentage = (Volume of Solute × 100 / Volume of Solution)
Volume percentage has no unit as it is the ratio of the volume of solute and solution.
Mass by Volume Percentage (w / v %) It is defined as the amount of solute (in grams) present in the 100ml of the solution. Mass by Volume Percentage = Mass of Solute (in gm) × 100 / Volume of Solution (in ml) Unit of mass by volume percentage is gram per millilitre as it is the ratio of the mass of the solute and volume of the solution. Parts per Million (PPM) Parts per million or PPM is used to measure the trace amount of solute dissolved in the Solvent. PPM of solute = Mass of solute (grams) x 10⁶ /Mass of solution (grams) Molarity Molarity of a solution is defined as the number of moles of solute present in the 1 liter of solution. For example, if 2 moles of NaOH are dissolved in 1 liter of water, the molarity of the resulting solution would be 2M, and the Formula for Molarity is given as follows: Molarity (M) = Moles of solute /Volume of solution (in Liter) Molality Molality of a solution is defined as the number of moles present in 1 kg of solution. For example, if 3 moles of NaOH are dissolved in 3 kilogram of water , the molality of the resulting solution would be 1 m means 1 mole of NaOH present in each Kg of water. The formula for molality: Molality (m) = Moles of solute / Mass of solvent (Kg) Mole Fraction Mole fraction is defined as the ratio of the number of moles of one component to the total number of moles present in the solution. Mole fraction of A (Xа) = Moles of A / (Moles of A + Moles of B) Mole fraction of B (X ᵦ) = Moles of A / (Moles of A + Moles of B)
Question 1: Find the number of electrons constituting one coulomb of charge.
Explanation:
