Applied chem

summative tmrw ohno

Tyndall Effect

the scattering of light by particles in a colloid or suspension, making the light beam visible.

Brownian movement

the random, continuous motion of particles caused by collisions with surrounding molecules.

Solution

a homogeneous mixture in which one or more solutes are uniformly dissolved in a solvent.

Solute

the substance in a solution that is dissolved by the solvent, usually present in the smaller amount.

Solvent

the substance in a solution that dissolves the solute, usually present in the greater amount.

A. Classification of Solution Accdg, to Phase

• Solid solution — a homogeneous mixture in which the solvent is in the solid phase.

• Liquid solution — a homogeneous mixture in which the solvent is in the liquid phase.

• Gaseous solution — a homogeneous mixture in which the solvent is in the gas phase.

Solution formation

occurs when solvent molecules are attracted to and surround solute particles, overcoming the forces holding the solute particles together and dispersing them uniformly throughout the solvent.

Miscible liquids

liquids that mix completely in all proportions to form a homogeneous solution.

Immiscible liquids

liquids that do not mix completely and separate into distinct layers.

Dissolution

the process in which a solute disperses uniformly in a solvent without forming a new substance.

reaction

a chemical process in which substances undergo rearrangement of atoms and form one or more new substances.

Bronze

78-95% copper, 5-22% tin

18K gold

75% gold , 12,5% copper,12.5% silver

sterling silver

92.5% silver, 7.5% copper

Brass

60-90% copper, 10-35% zinc

Cast Iron

96-98% Iron, 2-4% Carbon

Unsaturated solution

a solution containing less solute than the maximum amount that can dissolve at a given temperature.

Saturated solution

a solution containing the maximum amount of solute that can dissolve at a given temperature.

Saturated solution

a solution containing more dissolved solute than the normal maximum amount at a given temperature.

electrolytes

a substance that produces ions when dissolved in water, allowing the solution to conduct electricity.

Electrical conductivity of a solution

the ability of a solution to conduct electric current through the movement of ions.

strong electrolytes

a solution in which the dissolved electrolyte completely ionizes or dissociates into ions, allowing it to conduct electricity strongly.

Weak electrolytes

a solution in which the dissolved electrolyte partially ionizes into ions, allowing it to conduct electricity weakly.

solubility

maximum amount of solute that can be dissolved in a give amount of solvent

1. nature of solute

2. nature of the solvent

3. temperature of the solution

4. pressure in case of gases

factors affecting solubility of a solvent

Henrys law

the solubility of a gas in a liquid is directly proportional to the pressure of the gas above the liquid at constant temperature.

Mole fraction (X)

the ratio of the number of moles of a component to the total number of moles in a solution.

Parts per million (ppm)

the number of parts of solute per one million parts of solution.

Molarity (M)

the number of moles of solute dissolved per liter of solution.

Molar (1 M)

a solution containing 1 mole of solute per liter of solution.

Decimolar (0.1 M)

a solution containing 0.1 mole of solute per liter of solutio

Semimolar (0.5 M)

a solution containing 0.5 mole of solute per liter of solution.

Dilution Law

states that the concentration and volume of a solution are inversely related, expressed as M₁V₁ = M₂V₂.

molality

Molality (m): The concentration of a solution expressed as moles of solute per kilogram of solvent.

Mass Percent (% by mass)

The percentage of solute by mass in a solution.

percent concentration

The amount of solute present in a solution, expressed as a percentage.