Solution, solute, and solvent
by qit villorante
SOLUTION- A life supporting homogeneous or one-phase system mixture of two or more substances or particles (ions, atoms, or molecules).
Example: softdrinks, air, soil, medicines, disinfectants etc.
Each 100mL bottle of rubbing alcohol contains 70mL Isopropyl Alcohol
Components of a Solution
SOLVENT- the less active dissolving medium in a solution (solid, liquid, gas) and
has the greater amount.
SOLUTE- the more active material (solid, liquid gas) that has dissolved in a solution
and has a smaller amount.
Example: The price of a solution of 100mL gasoline and 50mL kerosene has
increased in 5%.
Solvent: gasoline Solute: kerosene
Types of Solution
SOLID + SOLID, LIQUID, GAS
LIQUID + LIQUID, SOLID, GAS
GAS + GAS, LIQUID, SOLID
Concentration of solution
By qit villorante
Concentration of Solutions
1) Unsaturated Solution- solution that can hold more solute because it has not yet reached its maximum point of saturation.
2) Saturated Solution- solution that contains a maximum amount of solute that can hold in a certain temperature.
3) Supersaturated Solution- solution that contains more solute that it can normally hold at a certain temperature.
4) Diluted Solution- solution that contains a large amount of solvent and a small amount of solute.
5) Concentrated- solution that contains a large amount of solute compared to the amount of solvent.
1) Unsaturated Solution- solution that can hold more solute because it has not yet reached its maximum point of saturation.
2) Saturated Solution- solution that contains a maximum amount of solute that can hold in a certain temperature.
3) Supersaturated Solution- solution that contains more solute that it can normally hold at a certain temperature.
4) Diluted Solution- solution that contains a large amount of solvent and a small amount of solute.
5) Concentrated- solution that contains a large amount of solute compared to the amount of solvent.
solubility
by qit villorante
SOLUBILITY- the quality or state of a material to be dissolve. The measure of the amount of solute that dissolves in a given solvent at a particular temperature.
![Picture](/uploads/2/2/5/2/22529028/1620329.png?900)
Example: What is the Molarity (M) of a 60g Sodium Hydroxide (NaOH)?
Using the Formula:
M=gsolute/Fm(Lsolution)
Gsolute= mass of solute
Fm= formula mass
Lsolution= volume of solution
Find out the value of fm (Formula mass) number of atoms multiplied by the atomic weight of the element.
NaOH = Na (1X 22.O4) + O (1X16.00) + H (1X1.01) =40g/mol
The Sodium Hydroxide (NaOH) is soluble in the solution.
1.5 or 2 mol/L
The Sodium Hydroxide (NaOH) is soluble in the solution.
Using the Formula:
M=gsolute/Fm(Lsolution)
Gsolute= mass of solute
Fm= formula mass
Lsolution= volume of solution
Find out the value of fm (Formula mass) number of atoms multiplied by the atomic weight of the element.
NaOH = Na (1X 22.O4) + O (1X16.00) + H (1X1.01) =40g/mol
The Sodium Hydroxide (NaOH) is soluble in the solution.
1.5 or 2 mol/L
The Sodium Hydroxide (NaOH) is soluble in the solution.
Factors Affecting the Solubility of a Solute:
1) Size of Solute and Solvent- it really affects the result of a solution especially the concentration. There are instances when all the solutes that were mixed with a solvent aren’t dissolve or the solvent was too many or large in amount resulting for a very thinness solution.
Example: A 25g of sugar was dissolved in 100L of water.
2) Nature of solute and solvent- Polar liquids dissolves polar compounds and non-polar liquids dissolve non-polar compounds.
Example: Water is a polar liquid and dissolves polar compounds such as sodium chloride NaCl.
3) Effect of Temperature- solute dissolves in high temperature (hot) and slows down in low temperature (cold).
Example: A teaspoon of coffee powder was dissolved in a newly boiled water, faster than a hot water that was left for several minutes and evaporated.
4) Stirring- when you are going to make a liquid solution like fruit juices, etc.,applying pressure or stirring will really helps in dissolving the solute.
Example: A teaspoon of orange juice was dissolved when stirred, faster than leaving it undisturbed.
1) Size of Solute and Solvent- it really affects the result of a solution especially the concentration. There are instances when all the solutes that were mixed with a solvent aren’t dissolve or the solvent was too many or large in amount resulting for a very thinness solution.
Example: A 25g of sugar was dissolved in 100L of water.
2) Nature of solute and solvent- Polar liquids dissolves polar compounds and non-polar liquids dissolve non-polar compounds.
Example: Water is a polar liquid and dissolves polar compounds such as sodium chloride NaCl.
3) Effect of Temperature- solute dissolves in high temperature (hot) and slows down in low temperature (cold).
Example: A teaspoon of coffee powder was dissolved in a newly boiled water, faster than a hot water that was left for several minutes and evaporated.
4) Stirring- when you are going to make a liquid solution like fruit juices, etc.,applying pressure or stirring will really helps in dissolving the solute.
Example: A teaspoon of orange juice was dissolved when stirred, faster than leaving it undisturbed.
Reference
Chemistry Lectures
http://en.wikipedia.org/wiki/Solution
http://chemwiki.ucdavis.edu/Physical_Chemistry/Physical_Properties_of_Matter/Solutions_and_Mixtures/Solubilty/Solubility_and_Factors_Affecting_Solubility
Chemistry Lectures
http://en.wikipedia.org/wiki/Solution
http://chemwiki.ucdavis.edu/Physical_Chemistry/Physical_Properties_of_Matter/Solutions_and_Mixtures/Solubilty/Solubility_and_Factors_Affecting_Solubility