1. Practice
Suppose that a solution containing 3.50 grams of Na3PO4 is mixed with a solution containing grams of Ba(NO3)2.
Na3PO4 + Ba(NO3)2  Ba3(PO4)2 + NaNO3
What is the limiting reactant and what is the excess reactant
How many grams of Ba3(PO4)2 can be formed?
How much of the excess reactant remains

2. Solution Dilution
Stock solutions – solutions stored in concentrated forms
HCl is stored as 12M stock solution
When diluting acids, always add concentrated acid to water

3. Dilution Equation
M1V1 =M2V2
Mol1=Mol2
The number of moles of a solute doesn’t change when we dilute a solution

4. Problems
To what volume (in ML) should you dilute 100 ML of a 5M CaCl2 Solution to obtain M CaCl2 solution ?
What volume of a 6M NaNO3 should you use to make 0.525L of a 1.20M NaNO3 solution?

5. Solution Stoichiometry
We can use the volume and concentration of a reactant or product to calculate its amount in moles
The conceptual plan is
Volume A Amount A( in moles )
Amount B in moles Volume B
Volume B

6. What mass in grams of CO2 forms?
Practice
What volume in ML of a 0.150M HNO3 solution will completely react with 35.7ml of a 0.108M Na2CO3 solution according to the following reaction?
 Na2CO3(aq) + 2HNO3(aq) ---> 2NaNO3(aq) + H2O(l) + CO2(g)
What mass in grams of CO2 forms?

7. Aqueous solutions and solubility
How do solids
such as salt and sugar dissolve in water?

8. Electrolyte and non electrolyte solutions
Salt solution conducts electricity while sugar solution doesn’t
Salt – Ionic compound
Sugar – Molecular compound
Ionic compounds completely dissociate in to ions in a solution and act as charge carriers and they are strong electrolytes
Molecular compounds dissolve in water as intact molecules

9. Solubility of Ionic compounds
A compound is said to be soluble - If it completely dissolves in water
A compound is insoluble - If its not completely dissolved in water
Solid AgNO3 in water is completely soluble and makes a strong electrolyte
Solid AgCl in water is insoluble and remains as a solid in water

10. Strong Electrolytes and Nonelectrolytes
Strong electrolytes: Substances that dissolves in water to form solutions that conducts electricity
Example: NaCl
Nonelectrolytes: substances that do not dissociate in to ions when dissolved in water are called nonelectrolytes
Example: All molecular compounds except acids

11. Strong acids and weak Acids
Strong acids dissociate completely in water
Example: HCl
Weak Acids: They do not completely dissociate in water
Example : acetic acid
Strong acids are strong electrolytes and weak acids are weak electrolytes

12. Solubility Rules for Ionic compounds in Water

13. Predict the solubility
NiS
Mg3(PO4)2
Li2CO3
NH4Cl