SOLUTIONS
Introduction to Solutions:
- A solution is a homogeneous mixture of two or more substances that are uniformly dispersed at the molecular or atomic level.
- Solutions can exist in all three states of matter: solid, liquid, and gas.
- The solute is the substance being dissolved in the solvent, and the resulting mixture is a single-phase solution.
Types of Solutions:
- Solid solutions have a solid solute and a solid solvent. An example of a solid solution is an alloy.
- Liquid solutions have a liquid solute and a liquid solvent. An example of a liquid solution is sugar dissolved in water.
- Gas solutions have a gas solute and a gas solvent. An example of a gas solution is air.
Solubility and Saturated Solutions:
- Solubility is the maximum amount of solute that can be dissolved in a given amount of solvent at a particular temperature and pressure.
- An unsaturated solution is a solution in which the amount of solute present is less than its solubility.
- A saturated solution is a solution in which the amount of solute present is equal to its solubility.
- A supersaturated solution is a solution in which the amount of solute present is greater than its solubility.
Concentration Units:
- Molarity (M) is the number of moles of solute present in one liter of solution.
- Molality (m) is the number of moles of solute present in one kilogram of solvent.
- Mole fraction (X) is the ratio of the number of moles of solute to the total number of moles of solute and solvent in the solution.
- Percentage composition is the percentage of the mass of the solute in the total mass of the solution.
Solubility and Factors Affecting Solubility:
- Factors that affect solubility include temperature, pressure, and the nature of the solute and solvent.
- Henry's Law states that the solubility of a gas in a liquid is directly proportional to the partial pressure of the gas above the liquid.
Colligative Properties of Solutions:
- Colligative properties are properties of a solution that depend on the concentration of the solute particles, regardless of the nature of the solute.
- The four colligative properties are vapor pressure lowering, boiling point elevation, freezing point depression, and osmotic pressure.
Ideal and Non-Ideal Solutions:
- Ideal solutions follow Raoult's law, which states that the vapor pressure of each component in an ideal solution is proportional to its mole fraction in the solution.
- Non-ideal solutions deviate from Raoult's law and have activity coefficients that vary from unity.
Abnormal Molar Masses:
- Abnormal molar masses can occur when a solute undergoes association or dissociation in solution.
- The molar mass of a solute can be determined using colligative properties, such as boiling point elevation and freezing point depression.
Osmosis and Osmotic Pressure:
- Osmosis is the movement of solvent molecules across a semi-permeable membrane from a region of low solute concentration to a region of high solute concentration.
- Osmotic pressure is the pressure required to stop the flow of solvent molecules across a semi-permeable membrane.
Applications of Solutions:
- Solutions are used in various applications, including in industry, medicine, and everyday life.
- Some common solutions used in industry include acid-base solutions, metal plating solutions, and electrolytes.
- In medicine, solutions are used as drugs, vaccines, and medical solutions.
These are some of the key concepts and ideas covered in the chapter on Solutions in Chemistry
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