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Week 9
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Week 12
Lab
Miscellaneous
100
What are the product of the reaction between a strong acid and a strong base
water and a salt
100

How much iron can be made from 495 g of aluminum by the following process
Fe2O3  +  2 Al   ➝   Al2O3  +  3 Fe 

 1540 g   

100

Determine the oxidation number of each element in the following compound:

 BaO2

If the oxidation number of the oxygen in BaO2 were -2, the oxidation number of the barium would have to be +4.  But elements in Group IIA can't form +4 ions.  This compound must be barium peroxide, [Ba2+][O22-].   Barium therefore is +2 and oxygen is -1.

100

What volume (in mL) of a 0.203 M NaOH solution is needed to neutralize 25.0 mL of a 0.188 M H2SO4 solution? 

 46.3 mL NaOH

100

What ions and how many of each are formed for every one formula unit of Al(NO3)3 that dissociates in water? 

 One Al3+ ion and three NO3–  ions 

200

What type of reaction is the one below: 

CH4 + 2O2 -> 2H2O + CO2

Combustion!
200

__CO + __H2 → C8H18 + __H2O

8 CO + 17 H2 → C8H18 + 8 H2O

200

Ag(s) + AuCl3(aq) →
Which element is oxidized? Which element is reduced? Which is the spectator ion? 



Oxidized: Ag

Reduced: Au 

Spectator: Cl 

200

An aqueous solution of Pb(NO3)2 is mixed with an aqueous solution of KOH.  A precipitate forms.  What is the chemical formula for the precipitate?  

The precipitate is Pb(OH)2 (s) 

200
Who is your favorite TA?
:)
300

What type of reactions is this: 
CoCl2(aq)  +Na2SO4(aq)  →CoSO4(aq)  +2NaCl (aq)

Precipitation 
300

_HClO4 + _P4O10 → __H3PO4 + _ Cl2O7

2 HClO4 + P4O10 → 4 H3PO4 + 6 Cl2O7

300
Two aqueous solution of AgNO3 and NaCl are mixed. What do the products look like?  Indicate the phases 

AgCl(s)

NO3- (aq)

Na+ (aq)

300

 Use the solubility rules to determine which compounds listed below are soluble or insoluble in water: 
a. PbI2 
b. (NH4)2CO3 
c. CaSO4
d. Ba(OH)2 

a. Insoluble
b. Soluble
c. Insoluble
d. Insoluble

300

 What is the mass of mercury that can be prepared from 1.25 g of cobalt metal? 

2 Co (s)  +  3 HgCl2 (aq)   -->  2 CoCl3 (aq)  +  3 Hg(l) 

6.38 g Hg

400
sulfuric acid is neutralized by sodium hydroxide. Write the balanced equation. 

H2SO4+ 2NaOH -->2H2O+ Na2SO4

400

__NH4OH + __KAl(SO4)2·__H2O → __Al(OH)3 + __(NH4)2SO4 + __KOH + __H2O

4NH4OH + KAl(SO4)2·12H2O → Al(OH)3 + 2 (NH4)2SO4 + KOH + 12 H2O

400

Determine the oxidation states of the elements in:

 1) Cl2;    2) NaH;    3) H2CO;
 1) Cl       2) H         3) C

1. 0 
2. 1- 
3. 0
400
You generated a standard curve in lab for red dye of lambda max 550nm. The fitted line for your scatter plot is  y= 10735x + 0.0612. You measured the absorbance of a solution of unknown concentration at wavelength 400nm. What is the concentration? 
TRICK QUESTION! You can't use the standard curve to figure out the concentration because you did not use the same wavelength for your unknown. 
400

How many ions (total) are present in 1 L of 1.00 M of a fully dissolved NaH2PO4 solution?  

2.41 x 1024 ions

500

 Which of the following is not a redox reaction?   
a) 2 H2(g) + O2(g) → 2 H2O(l)
 b) Zn(s) + H2SO4(aq) → ZnSO4(aq) + H2(g) 
c) H2O(l) + NH3(g) → NH4+(aq) + OH–(aq) 
d) Cl2(g) + 2 KBr(aq) → Br2(l) + 2 KCl(aq) 
e) CH4(g) + O2(g) → CO2(g) + H2O(g) 

c) H2O(l) + NH3(g) → NH4+(aq) + OH–(aq) 

500

__(NH4)2CO3 (aq) + __Al(NO3)3 (aq) --> __NH4NO3 (aq) + __Al2(CO3)3 (s)

Complete Ionic Equation:  6 NH4+ (aq) + 3 CO32- (aq) + 2 Al3+ (aq) + 6 NO3- (aq) --> 6 NH4+ (aq) + 6 NO3- (aq) + Al2(CO3)3 (s)    

Net Ionic Equation:  2 Al3+ (aq) + 3 CO32- (aq) --> Al2(CO3)3 (s) 

500

Oxidation states of the elements in:

1) S2O32-  2)HClO2;    3)CuSO4

1) S        2)Cl           3)S 

1.  2
2. 3
3. 6
500

You have 35 mL of H3PO4 with a concentration of 0.29 M. You a titrating this with 0.5 M NaOH. How much volume NaOH would you expect to use? 

60 mL of NaOH
500
Which of these have restrictions on the solubility rules: 
ammonium 
sulfate 
alkali metals 
halogens
sulfates & halogens