A presentation on Solution and Solubility it includes type of solutions and about solubility with few examples.

1. Solutions and Solubility
Made By : Sudhanshu Tripathi

2. Solutions
• Solution is a homogenous mixture of a
solute dissolved in a solvent. The
solubility (ability to dissolve) of a solute in
a solvent is dependent on the
1. Temperature
For solid solutes: as temperature
increases, solubility increases.
For gas solutes: as temperature
increases, solubility decreases.

3. 2. Pressure
For solid solutes: as pressure increases,
solubility remains the same.
For gas solutes: as pressure increases,
solubility increases
3. Nature of Solute/Solvent
“Like dissolves in like.”

4. Solute/Solvents concentration.
Solubility Summary
Solute Type Nonpolar
solvent
Polar Solvent
Nonpolar (Fat
Grease)
Soluble (soap) Insoluble
(water)
Polar Insoluble Soluble (water)
Ionic (salt) insoluble Soluble (water)
High solubility-soluble Low solubility-insoluble

5. Solubility Curves
• Shows the number of grams of solute that can be
dissolved in 100.g of water at temperatures between 0
degrees C and 100 degrees C.
• Each line represents the maximum amount of that
substance that can be dissolved at a given temperature.
• Lines that show an increase in solubility as temperatures
increase represent solids being dissolved in water.
• Lines that show a decrease in solubility as temperatures
increase represent gases being dissolved in water.
These are NH3, SO2, and HCl

6. There are three types of solutions
• 1. An unsaturated solution is a solution in which
more solute can be dissolved at a given
temperature.
• 2. a saturated solution is a solution containing
the maximum amount of solute that will dissolve
at a given temperature.
• 3. a supersaturated solution is a solution that
contains more solute than would dissolve in a
saturated solution at a given temperature.

7. Solubility Rules
• Not all ionic compounds are water soluble
• There are some general rules for
compounds that are water soluble:
– Group 1 ionic cmpds and ammonium (NH4
+)
are always water soluble
– Group 17 ionic cmpds are water soluble
except when paired with Ag, Pb, and Hg ions
– See Table F for full rules and exceptions

8. Examples
• AgNO3 = water soluble
• AgCl = insoluble
• Na2S = soluble
• NaCl = soluble
• CaCO3 = insoluble
• AlPO4 = insoluble

9. Concentrations of Solutions
• Because solutions are homogeneous
mixtures, their compositions can vary.
Sometimes it is adequate to refer to a
solution as dilute or concentrated. These
are qualitative descriptions of
concentration. It is more precise to
describe the concentration of solutions in
quantitative measures.

10. Molarity
• Molarity (M)- number of moles of solute in 1L of
solution. Table T
Molarity= moles of solute
liters of solution

11. Calculating molarity
Highly concentrated HCl(aq) has a molarity
of 12M
This means there are 12 moles of HCl
dissolved in 1 Liter of water
12M = 12 moles
1 Liter

12. Parts Per Million
• Parts per million is another way of
measuring the concentration of a solution
• The general formula is:
Parts per million = grams of solute x 1,000,000
grams of solution

13. Parts per million example
• 5 grams of NaCl is dissolved in 2.5L of
water. What is the concentration of NaCl
in parts per million (ppm)?
• Remember 1mL water = 1 g
ppm = 5g NaCl x 1,000,000 = 2000 ppm
2500 g H2O