1. 1) In the lab, students follow the chemical reaction above using 30 grams of Barium chloride. If 39 grams of silver chloride are actually produced, what is the percent yield?
2) Calculate the energy in Joules, of a quantum of radiant energy (the energy of a photon) that has a frequency of 5.00 x Hz.
3) A compound has an empirical formula of CH2O. The molecular mass is about 90g. What is the molecular formula?

2. 4) What volume of 1. 75 M sodium hydroxide must be used to prepare 150
4) What volume of 1.75 M sodium hydroxide must be used to prepare 150. mL of M NaOH solution?
5)What percentage of H3PO4 is made of oxygen?
6) If we dissolve 0.20 mol glucose in enough water to give precisely 0.50 L of solution, what will be the concentration?

3. There are two types of acids:
Binary Acids – contain hydrogen and another element.
Ex.s: HCl, HBr
Ternary Acids– contain hydrogen and a polyatomic ion.
Ex.s: HNO2, H3PO4

4. Use the root of the element name Add the suffix “ic”
Rules for Naming Binary Acids:
Begin with “hydro”
Use the root of the element name
Add the suffix “ic”
Add the word acid to the end

5. Examples of Binary Acids
HCl = hydrogen chloride
Hydro + chloride + ic = Hydrochloric acid
H2S = hydrogen sulfide
Hydro + sulfide + ic = Hydrosulfuric acid

6. Start with the name of the polyatomic ion.
Rules for Naming Ternary Acids:
Start with the name of the polyatomic ion.
If it ends with “ite” swap it out for “ous.”
If it ends with “ate” swap it out for “ic.”
Add the word acid to the end

7. Examples of Ternary Acids
H2SO3 =
SO3 = sulfite
sulfite = sulfurous acid
H2SO4
SO4 = sulfate
sulfate = sulfuric acid

8. Left Side Practice
Write the name of the acids on the left side of your notebook.
1) Hydrogen fluoride (HF)
2) Hydrogen bromide (HBr)
3) Hydrogen nitrite (HNO2)
4) Hydrogen nitrate (HNO3)
5) Hydrogen phosphate (H3PO4)
6) Hydrogen iodide (HI)