A solution is made by mixing exactly 500.0 mL of 0.167 M NaOH with exactly 500.0 mL of 0.100 M CH3COOH. Calculate the equilibrium concentrations of H3O+, CH3COOH, CH3COO-, OH-, and Na+.
[H3O+] = M
[CH3COOH] = M
[CH3COO-] = M
[OH-] = M
[Na+] = M
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In the chemiluminesence reaction, a diene is generated on the luminol molecule. Why does the reaction not progress from that point forward as a Diels-Alder reaction with molecular oxygen acting as the dienophile? How does ground state molecular oxygen exist and does this affect the possibility of a Diels-Alder mechanism with O2?
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The complex ion Cu(NH3)42 is formed in a solution made of 0.0400 M Cu(NO3)2 and 0.500 M NH3. What are the concentrations of Cu2 , NH3, and Cu(NH3)42 at equilibrium? The formation constant*, Kf, of Cu(NH3)42 is 1.70 × 1013.
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|
Drops of Stock Solutions |
Temp. (K) |
Reaction Time |
||||
|
Test Tube |
KMnO4 |
H2O |
H3O^+/H2SO4 |
C2O4H2 |
||
|
E-1 |
15 |
15 |
15 |
5 |
278 K |
3 min 1 sec |
|
E-2 |
15 |
15 |
15 |
5 |
300 K |
6 min 13 sec |
a. What effect does the temperature of the solutions have on the rate of the reaction?
b. How does heating the reaction mixture affect the energy of the species in solution? What effect would cooling the reaction mixture have on the energy of the species in solution?
c. Write a general, qualitative, statement about how the rate of a reaction depends on the temperature at which the reaction is carried out.
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A solution containing 10.00 mL of 0.0500 M metal ion buffered to pH = 10.00 was titrated with 0.0400 M EDTA. Calculate the fraction (αY4-) of free EDTA in the form Y4−. Keep 2 significant figures.
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A rigid container has water of 2 kg at 120 C with a quality of 25%. The container is heated to the temperature of 140 Celsius, calculate the new quality?
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HClO is a weak acid (Ka = 4.0 × 10–8) and so the salt NaClO acts as a weak base. What is the pH of a solution that is 0.017 M in NaClO at 25 °C
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1.For the reaction,
PCl5(g) <-----> PCl3(g) + Cl2(g) Kp = 24.6 at 500 K
calculate the equilibrium partial pressures of the reactants and
products if the initial pressures are PPCl5 =
0.610 atm, PPCl3 = 0.400 atm and
PCl2 = 0.000 atm.
PPCl5 = PPCl3 = PCl2 =
2.
H2O(g) + Cl2O(g) <-----> 2HClO(g) Kc = 0.14 at 298.15 K
calculate the equilibrium concentrations of the reactants and
products if the initial concentrations are [H2O(g)] =
0.00482 mol L-1, [Cl2O(g)] = 0.00482 mol
L-1 and [HClO(g)] = 0.000 mol L-1.
[H2O(g)] = [ClO2(g)] = [HClO(g)] =
3.A flask that initially contained pure NO2 was
heated to 1000 K, a temperature at which the value of Kp
for the decomposition of NO2 is 128.8.
2NO2(g) <-----> 2NO(g) + O2(g)
Given that the partial pressure of O2 at equilibrium
equals 0.168 atm calculate the partial pressures of NO2
and NO at equilibrium.
PNO = PNO2 =
4.The equilibrium constant Kp for the
reaction,
2 SO3(g) <-------> 2 SO2(g) + O2(g)
is 8.440 at 789 °C. If a vessel at this temperature initially
contains pure SO3 and if the partial pressure of
SO3 at equilibrium is 0.050 atm, what is the partial
pressure of O2 in the flask at equilibrium?
What was the initial pressure of SO3 in the flask?
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Calculate the percent dissociation of HF (Ka= 3.5x10^-4) in
(a) 0.050 M HF
(b) 0.50 M HF
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Write:
a) balanced equation
b) total ionic equation
c) net ionic equation
d) type of reaction
e)limiting reactant
1) Cu(s) + HNO3(aq) -> Cu(NO3)2 (aq)+ NO2(g) +H2O(l)
2) Cu(NO3)2(aq) + NaOH(aq) -> Cu(OH)2(s) + NaNO3
3) Cu(OH)2(s) -> CuO(s) +H2O
4) CuO(s) + H2SO4(aq) ->CuSO4(aq) +H2O(l)
5)CuSO4(aq) + Zn(s) -> Cu(s) +ZnSO4 (aq)
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Calculate enthalpy for the following reaction Ca(s) + 1/2O2 + CO2 = CaCo3 Given the following reactions: Ca(s) + 1/2 O2 = CaO (s) H= -635.1 kj CaCo3 = CaO (s) + CO2 H= 178.3 kj
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Consider a solution formed by mixing
50.0 mL of 0.100 M H2SO4,
30.0 mL of 0.1000 M HOCl,
25.0 mL of 0.200 M NaOH,
25.0 mL 0.100 M Ba(OH)2, and
10.0 mL of 0.150 M KOH.
Calculte the pH of this solution.
Ka (HOCl) = 3.5 x 10-8
What is the pH?
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Chromatography explained in details highlighting important things to know for test.
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Exothermic Vs. Endothermic Reaction
Reaction progress diagrams for single-step endothermic and exothermic reactions.
a. Devise a general statement about the relationship between Ea and the rate of a reaction.
b. Describe the effect of temperature on the energy of collisions, and explain how this effect changes the rate of a reaction.
c. State three things that resulted in an increase in the rate of the reaction. For each of the three things, explain at a molecular level what happens to cause the rate of the reaction to increase.
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A 12.9 mL solution of 0.100 mol L-1 HOCl is titrated using 0.150 mol L-1 NaOH.
What is the pH of the solution after 5.18 mL of the NaOH solution is added? Express your answer to 2 decimal places.
You have 5 attempts at this question.
Remember you can find KA and/or KB values in your textbook in chapter 15.
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