Chem I
Name: ______________ ______________
Chapter 4: Chemical Quantities and Aqueous Reactions
Homework: 4.8, 4.26, 4.46, 4.50, 4.62, BONUS: 4.70
1. The numerical relationship between chemical amounts in a reaction is called ______________________.
2. How many moles of CO2 can be made from 4 moles of CH4 in the combustion of CH4?.
3. How many grams of CO2 is produced from 10.0 g CH4?
4. Homework 4.8: Sulfuric acid dissolved aluminum metal according to the following reaction:
2Al(s) + 3H2SO4(aq) → Al2(SO4)3(aq) + 3H2(g)
What minimum mass of H2SO4 is needed to dissolve an aluminum block of mass 15.2 g?
5. Write definition of limiting reagent. (Slide 11)
Example Slide 13-15.
6. Define: solution, solute and solvent.
7. Concentration = no. moles (mols) / Volume (L) = mols/L = Molarity, M
How many liters of 0.125 M NaOH contain 0.255 mol NaOH?
8. How would you make a 1.0 M solution of potassium bromide?
9. Dilution, M1V1 = M2V2
What volume (mL) of 12.0 M HCl is required to make 1.0 L of 1.0 M HCl?
10. Solution stoichiometry. (Slide 39-40)
What volume of 0.150 M KCl is required to completely react with 0.150 L of 0.175 M Pb(NO 3)2 in the reaction
2 KCl(aq) + Pb(NO3)2(aq)  PbCl2(s) + 2 KNO3(aq)
Chem I
Name: ______________ ______________
11. Define electrolyte and non electrolyte. (Slide 43)
12. Define strong acid and weak acid. (Slide 46)
13. Define soluble and insoluble.
14. Solubility rules. (Slide 51-52)
15. Example 4.10 – Write the equation for the precipitation reaction between an aqueous solution of potassium carbonate
and an aqueous solution of nickel(II) chloride.
16. Remove the spectator ions and write a net ionic equation for the above reaction.
17. Give an example of a neutralization reaction (acid-base) and its net ionic equation.
18. Gas evolving reactions. (Slide 82 + 84)
e.g. reaction between sodium carbonate and nitric acid
19. Redox reactions. (Slide 88-96)
20. Identify the redox reagents:
MnO2 + 4 HBr → MnBr2 + Br2 + 2 H2O