1. Solution

2. Solution homogeneous mixture composed of only one phase
a solute is a substance dissolved in another substance, known as a solvent.

3. How to prepare 800mL of 2M Sodium chloride
How to prepare 100 mL of 1.0 M hydrochloric acid from concentrated (12.1 M ) hydrochloric acid.

4. How to prepare 800mL of 2M Sodium chloride

5. How to prepare 100 mL of 1.0 M hydrochloric acid from concentrated (12.1 M ) hydrochloric acid.

7. Molarity
The most common unit of solution concentration is molarity (M)
The molarity of a solution is defined as the number of moles of solute per one liter of solution.
Note that the unit of volume for molarity is liters, not milliliters or some other unit.
Also note that one liter of solution contains both the solute and the solvent.
Molarity, therefore, is a ratio between moles of solute and liters of solution.
To prepare laboratory solutions, usually a given volume and molarity are required.
To determine molarity, the formula weight or molar mass of the solute is needed.

10. Percent solution

15. Simple dilution
Simple diluttion - A unit volume of liquid material of interest is combine with an appropriate volume of a solvent liquid to archieve the desired concentration
Dilution factor – the total number of unit volume in which material will be dissolved
Diluted material must be thoroughly mixed to achieve the true dilution
1:10 dilution

16. 1:10 dilution (verbalize as 1 to 10) = 1 unit volume of diluent (material to be diluted) + 9 unit volumes of the solvent
Hence, 1+9=10
1:300 = 1 unit volume of diluent volumes of solvent medium

17. Sometimes, solution are expressed in term of ‘X’, an indicator of relative solute concentration.
Eg. Buffer – made up to 20X stock solution.
1X buffer = 1 unit volume of buffer + 19 volumes of water

18. Mixing parts or volumes
Not to confused with simple dilution
Instruction:
Add 1 part glacial acetic acid with 3 parts water
Mix 1 volume of glacial acetic acid with 3 volume water
Make up a 1:3 acetic ethanol solution
(just add accordingly)
But, if the instruction to make a 1:3 dilution of acetic acid in ethanol = 1 unit acetic acid with 2 unit volumes of ethanol

19. Serial dilution

20. V1C1 = V2C2
V= volume;
C=concentration (In what ever units you are working)
Eg: Suppose you have 3 ml of stock solution of 100 mg/ml ampicilin and you want to make 200 ul of solution having 25 mg/ml. What is the volume of the stock to use?

22. Stoichiometry
Refers to quantities of reactants and products in a balanced chemical reaction.
aA + bB cC + dD
i.e. a moles of A react with b moles of B to give c moles of C and d moles of D.
a,b,c,d are stoichiometric quantities
Paul Ashall, 2008

23. Tutorial
How would you prepare 400 ml of a 0.24 M NaCl solution (MW=58.44 g/mole)?
How would you prepare 750 ml of a 0.35 M Na2PO4(MW=141.96)?
How would you prepare 225 ml of a 0.15 M citric acid solution (MW=453.6)?
What volume of stock 0.24 NaCl is needed to prepare 75 ml of 0.1 M NaCl
What volume of stock 0.35 M Na2PO4 is needed to prepare 150 ml of 0.2 M Na2PO4 ?

24. What volume of stock 0.15 M citric acid is needed to prepare 230 ml of 2.5x10-3M citric acid.
How much (ml) 3x10-3 M Na2PO4can be prepared from 20 ml of 0.2 M Na2PO4
If you have 35 ml of 0.1 M NaCl, is it enough to prepare 200 ml of 0.06 M NaCl?

25. For each of the following, indicate the mass (g) of reagent needed to prepare 125 ml of the indicated percent solution
A protocol calls for using a working concentration of 1.5X10-4M boric acid. To save shelf space, you decide to make up a 20X stock solution. What will be the molarity of that stock solution?
Reagent
Molecular weight
Percent solution needed (125 ml)
Mass of reagent (g)
NaCl
58.44
10%
Na2PO4
141.96
4.5%
Citric Acid
453.6
2.5%

26. Stoichiometry