Solution Concept Map

1. pOH

1.1. The pOH of an acidic solution is larger than 7, whereas that of a basic solution is less than 7.

1.1.1. Based on the hydroxide ion, the pOH scale determines how basic or acidic a solution is.

2. Spectator Ions

2.1. The ions that are present on both sides of chemical reactions but do not participate in them.

3. Preparation of standard solutions

3.1. 1. Weigh out substance.

3.2. 2. Dissolve solid in beaker with small amount of distilled water.

3.3. 3. Move the solution into a volumetric flask.

3.4. 4. Add distilled water until you reach the etch on the volumetric flask.

3.5. 5. Put stopper on the volumetric flask and start flipping it to make the make the solution homogeneous.

4. Ionic equations

4.1. An ionic equation shows spectator ions.

5. Net ionic equations

5.1. A net ionic equation does not show the speactator ions.

6. Acids and bases

6.1. defintion

6.1.1. base - Any molecule or ion that can take up a hydrogen ion from an acid is considered a base.

6.1.1.1. Properties of acids

6.1.1.1.1. taste = sour

6.1.1.1.2. pH = less than 7

6.1.1.1.3. Texture = rough

6.1.2. Acid - Any compound that contains hydrogen and has the ability to transfer a hydrogen ion, to another substance is considered an acid.

6.1.2.1. Properties of bases

6.1.2.1.1. Taste = bitter

6.1.2.1.2. pH = more than 7

6.1.2.1.3. Texture = slippery

6.2. Conjugate pairs

6.2.1. Example - H2O+NH3→NH4+OH−

6.2.1.1. 1st pair = H20 , OH-

6.2.1.1.1. H20 is the proton receiver and 0H- is the proton donator.

6.2.1.2. 2nd pair = NH3 , NH4

6.2.1.2.1. NH3 is the proton donator and NH4 is the proton acceptor.

7. What is a solution

7.1. A homogeneous mixture of two or more components is called a solution.

7.1.1. Types of solutions

7.1.1.1. gas solution

7.1.1.2. Solid solution

7.1.1.3. Liquid solution

8. Concentration

8.1. Molarity

8.1.1. M is the solute's moles per litre of solution. One liter of a 1.00 molar (abbreviated 1.00 M) solution contains one mole of solute per liter of solution.

8.1.2. Formula is moles of solute / litres of solution = molar concentration.

8.2. Molality

8.2.1. The formula for molality is m = moles of solute / kilograms of solvent.

9. Mass

9.1. Mass of solute = volume of solution × concentration of solution.

10. Volume

10.1. Divide the mass of the solute by the mass concentration of the solution.

11. pH?

11.1. pH is a quantitative gauge of how basic or acidic aqueous or liquid solutions are.

12. pH is a unit of measurement for hydrogen ion concentration in a solution.

13. Process of dissolving in water

13.1. 1. If the solute is in solid form use heat or some other method like stirring to separate the solutes particles.

13.2. 2. water is a polar molecule which means it has a partial postive charge and partial negative charge so that polarity allows the water to affect the solutes particles.

13.3. 3. now the water is surrounding the solutes particles and destroys the bonds that were holding them together.

13.4. 4. now the particles scatter making a solution.

14. solution stoichiometry vs simple stoichiometry

14.1. Solution stoichiometry applies the major concepts to reactions that take place in solutions, whereas simple stoichiometry deals with reactions in the gas or aqueous phase and concentrates on fundamental calculations using moles. This includes taking into account variables like volume, molarity, and ion activity in solution stoichiometry.