Problems involving moles in solute, oxidation numbers and concentration

Please see the attached file for the complete problems.


1. Calculate the moles of solute for the following solutions:
10mL of .898M KMnO4
100 mL of .651 M FeSO4
50.0 mL of .762 M FeSO4
20.0 Ml of 1.11 M K2Cr2O7

2. Write a net ionic equation for:
-the precipitation reaction resulting form mixing a BaCl2 solution with a K2SO4 solution.
-the reaction between AgNO3 (aq) and Na2SO4 (aq)

3. 10.0 g of KCl and 26.5g of CaCl2 were dissolved in 500 mL of water.  How many mL of 1.57 M AgNO3 solution would be required to precipitate all Cl- from the solution?

4. Water is added to 25.0 mL of a .666 M KNO3 solution until the volume of the solution is exactly 500mL.  What is the concentration of the final solution.
5.  What is the acid:base mole ratio for the reaction between H2SO4 and NaOH?
6. Look at the following redox reaction and identify which element is oxidized and which is reduced?
2Li + H2 2LiH
7. Give the oxidation numbers for the specified atoms in the following molecules and ions:
* Mg3N2   nitrogen:
*CaC2    carbon:
*ZnO2-2    Oxygen:
* NaBH4   Boron:
*C2O4-2          Carbon:
*WO4-2      tungsten:

Attached file(s):

unknown chem ?s.docx  View File