The properties of solutions

Solution

is a homogeneous mixture of two or more substances whose composition are uniformly distributed

Unsaturated solution

there is less amount of solute dissolve in a given solvent

saturated solution

the amount of solute dissolve in a given amount of solvent is in its maximum

supersaturated solution

the amount of solute is dissolved in a given amount of solvent is more than the maximum

hypertonic solution

the concentration of solution inside the cell is lower than the outside of the cell

isotonic solution

the concentration outside the cell is equal to the concentration inside of the cell

hypotonic solution

the concentration of the solution inside the cell is higher than the outside of the cell

solubility

refers to the ability of a chemical substance (solute), to form a solution with another substance (solvent)

nature of solute

likes dissolves likes, ionic and polar solutes dissolves in polar solvents while non polar solutes dissolved in nonpolar solvents

temperature

the solubility of liquids and solids is directly proportional to the absolute temperature while that of gas is inversely proportional

pressure

on the surface of the solvent has minimal effect on solubility of solids and liquids but has a vast effect on the solubility of gases

stirring

affects how fast a solute dissolved in a solvent but it has an effect on how much solute will dissolve

heating

gives the solvent particles more kinetic energy. The faster the motion of the solvent particles, the greater is the collision with the solute particles

powdering

the smaller the size of the solute particles, the greater is the surface area in contact with the solvent.

concentration

is defines as the amount of a substance divided by the total volume of the mixture

percent by mass

mathematically defines as the mass of the solute divided by the mass of solution multiplied by 100%

percent by volume

mathematically defines as the quotient between volume of solute and volume of solution multiplied by 100%

percent by mass volume

defined as the quotient between the mass of the solute and the volume of the solution multiplied by 100%

mole fraction

mathematically expressed in terms of the quotient between the mole of the solute and mole of the solution = m/MW

Molality

mathematically defined as the number of moles of solute divided by the mass of solvent in kilograms

molarity

mathematically defined as the number of moles of solute divided by the volume of the solution in Liters

Normality

defined as the molarity multiplied by the number of replaceable H+ for acids and OH- for bases

Parts per million

defined as the concentration expressed in milligrams of one substance per liter of water or per kilogram of soil.

stoichiometry

introduced by the german chemist, Jeremias Benjamin Richter, the word stoichiometry was derived from the Greek words stoicheion which means element and metron which means measure

Colligative properties

A Physical property of matter that does not depend on the intensive properties but more specifically on the amount of solute present in a solution

Boiling point elevation

the increase in the boiling point of the solvent due to the addition of solute to form solution and can be expressed mathematically in T=Kbmi

Freezing Point Depression

the decrease in the freezing point of the solvent due to the addition of solute to form solution and can be expressed mathematically in T=Kfmi

electrolyte

a solution that contains ions, atoms, or molecules that lost or gained electrons, thus is electrically conductive

Non electrolyte

a solution that does not conduct electricity due to the absence of ions or charged particles