pH and pOH
If I have a solution with a pH of 4 is it acidic, basic or neutral?
Acidic
If my rate of rxn = k[A][B]2 what is the overall order of this rxn?
Third order
The following endothermic reaction is at equilibrium. What effect will increasing the temperature have on the system?
Fe3O4 (s) + CO (g) ⇌ 3 FeO (s) + CO2 (g)
Shift to the right. More products formed
Write the keq for the following reaction
CO(g) + H2O(g) <-> CO2(g) + H2 (g)
K= [CO2][H2 ]/[H2O][CO]
Give the old name for the following:
Pb(C2O4)2
Plumbic oxalate
If I have a solution with a pOH of 9 what is the pH and is the solution acidic, basic, or neutral?
Acidic pH=5
I found a reaction to be second order in reactant A and zero order in reactant B. What is my rate law?
rate=k[A]2
CH4(g) + 2H2S(g) <-> 4H2(g) + CS2 (g)
What will happen to the equilibrium as 1)Volume increases? 2) CH4 is removed? 3) H2(g) is added?
1) equilibrium shifts right
2) and 3) equilibrium shifts left
Write the keq for
Zn3(PO4)2 <-> 3 Zn 2+ (aq) + 2 PO4 3- (aq)
K= [Zn 2+]3[PO4 3-]2
Magnesium bromite
Mg(BrO2)2
Calculate the pH for a solution of 0.00154 M HNO3
pH=2.812
The following reaction was studied using the method of initial rates: A + 2B → 2C + D. Use the data table to determine the rate law.
Go to picture
rate=k[A]
4NH3(g) + 5O2 (g) <-> 6H2O(l) + 4NO (g) + 905 kJ
1)What happens to Oxygen as volume increase? 2) energy when the concentration of ammonia decreases?
3) water when temperature decreases?
1) oxygen increases
2) energy decreases
3) water increases
Consider a solution of HCN. List all of the aqueous species in this solution. If the solution has a pH of 5.3, determine the concentration of all of the species you listed. Ka of HCN is 6.2 x 10-10
[HCN]=0.04M [CN-]=[H3O+]=5x10-6M
[OH-]=2x10-9M
HCO3-
bicarbonate ion
hydrogen carbonate ion
Calculate the pH for a solution of 1.099 x 10-6 M KOH
pH=8.0140
Consider the reaction A + B → C + D with an experimental rate law of rate = k[B]2 . Is the following a plausible mechanism?
Step 1: B + B → C + E (slow)
Step 2: C + A → D + B (fast)
No, we would end up with an intermediate (E) in our overall rxn and no product C.
Consider the following reaction
4NH3(g) + 5O2 (g) <-> 6H2O(l) + 4NO (g) + 905 kJ
What happens to equilibrium as volume is decreased?
Shift to the side with fewer moles. To the right.
A solution is 0.045 M H2C2O4. Determine the pH of the solution and [C2O42-].
Ka H2C2O4=5.6 x 10-2
Ka HC2O4-=5.4 x 10-5
pH=1.54
[C2O42-]=5.4x 10-5M
DOUBLE POINTS
1)HCl(g)
2) Acetic acid
1)hydrogen chloride
2) HC2H3O2
A saturated solution of solution made by dissolving 1.00 g of Ba(OH)2 ⋅ 8 H2O(s) in enough water to make 100 mL of solution. What is the pH
pH=12.802
Use the steady state approximation to derive a rate law for the following two step reaction:
O3 ⇄ O2 + O
O + O3 → 2O2
rate=k2k1[O3]2 / k2[O3]+k-1[O2]
Hydrolisis:
Calculate the pH of 0.05 M Na2CO3.(H2CO3:Ka1=4×10−7, Ka2=4.7×10−11)
pH=11.5
What is the molarity of an aqueous solution of NH3 if it is 4.1% ionized? (Kb, NH3 = 1.8 x 10-5 )
0.011M NH3
H2O2
Hydrogen peroxide