1. Solutions, Acids, & Bases

2. Solutions

3. Solutions
Solutions
type of homogeneous mixture (no visibly different particles)

4. Solutions Solutions solute is dissolved in a solvent
(Not always solid dissolved in a liquid)

5. Solutions
Solutions
solubility – how much solute is able to be dissolved in a given solvent

6. Solutions Solutions solubility factors temperature pressure
surface area
stirring

7. Solutions Solutions solubility degrees
unsaturated – more solute may theoretically be dissolved
saturated – maximum theoretical amount of solute is dissolved
supersaturated – more solute dissolved than predicted at given temp.

8. Solutions
Solutions
concentration – measure of amount of solute dissolved per quantity of solvent

9. Solutions Solutions concentration
dilute solution – low amount of solute
concentrated solution – high amount of solute

10. Solutions Solutions Concentration
molarity (M) – moles of solute dissolved per liter of solution
also called molar concentration

11. Solutions Molarity sample problems
A solution has a volume of 2.0 L and contains 36.0 g glucose. If the molar mass of glucose is 180 g/mol, find the molarity.

12. Solutions Molarity sample problems
A saline solution contains 0.90 g NaCl per 100 mL of solution. What is the molarity?

13. Solutions Molarity sample problems
How many moles of solute are present in 1.5 L of 0.24 M Na2SO4?

14. Solutions Molarity sample problems
How many moles of ammonium nitrate are in 335 mL of M NH4NO3?

15. Solutions Solutions concentration
diluting – lowering amount of solute in solution by adding more solvent (usually water)
M1 × V1 = M2 × V2

16. Solutions Diluting sample problems
How many milliliters of a stock solution of 4.00 M KI would you need to prepare mL of M KI?

17. Solutions Diluting sample problems
How many milliliters of a stock solution of 2.00 M MgSO4 would you need to prepare mL of M MgSO4?

18. Acids & Bases

19. Acids & Bases
Acids
substances that donate hydrogen ions to form hydronium ions (H3O1+) when dissolved in water
strong acids fully ionize in water
weak acids do not fully ionize in water

20. Acids & Bases
Bases
substances that either contain hydroxide ions or react with water to form hydroxide ions
strong bases fully ionize in water
weak bases do not fully ionize in water

21. Acids & Bases Acids & Bases degrees of acidity or basicity
measured by pH
concentration of hydronium ions in solution
pH < 7.0 → acidic
pH = 7.0 → neutral
pH > 7.0 → basic

23. Acids & Bases Acids & Bases at home… cleaning products are often basic
food products are often acidic

24. Acids & Bases Acids & Bases
mixing acids & bases may cause neutralization, forming water and a salt
Ex:
HCl(aq) + NaOH(aq)  NaCl(aq) + H2O