Calculate the pH of the solution resulting from the addition of 10.0 mL of 0.10 M NaOH to 50.0 mL of a 0.10 M solution of aspirin (acetylsalicic acid, Ka = 3.0 × 10–4) solution.
| A. |
2.9 |
|
| B. |
10.5 |
|
| C. |
4.1 |
|
| D. |
3.5 |
|
| E. |
1.8 |
In: Chemistry
Calculate the amount of heat that must be absorbed by 50.0 grams of ice at -12.0oC to convert it to water at 20.0oC. (specific heat capacity of ice = 2.09 J/g.K; specific heat capacity of liquid water = 4.18 J/g.K; specific heat capacity of water vapor = 1.84 J/g.K; heat of fusion of ice = 334 J/g
In: Chemistry
Some NH4I is palced in a reaction placed in a closed container, which is then heated to 400 deg. C. If the total pressure in the container is (7.47x10^2) , mm Hg, what is the value of Kp. Remember to convert the pressures to atm's.
In: Chemistry
For the reaction 2SO2(g) + O2(g) → 2SO3(g), ΔH° and ΔS° are both negative at 298 K, and the process is spontaneous at 298 K. Which of the following statements must also be true?
A.ΔG is positive for the reaction at 298 K.
B.The change in entropy is the driving force of the reaction.
C.ΔG is temperature independent.
D.The direction of the reaction may be reversed at high temperatures.
E.At high temperature, ΔH becomes positive.
In: Chemistry
What is the mass of potassium oxalate monohydrate and
iron (III) chloride required to synthesize 3g of potassium tris
(oxalato)iron (III). water should not be included in
equation.
Please include equation and explain in detail. thank you!
In: Chemistry
What is chemical equilibrium? Describe the factors that can affect chemical equilibrium, including the presence of catalysts. Explain Le Châtelier’s principle and explain how chemists might use it to increase the amount of products produced in a reaction. (Equilibrium)
In: Chemistry
You have a concentration cell in which the cathode has a silver
electrode with 0.10 M Ag+. The anode also has a silver electrode
with Ag+ (aq), 0.050 M S2O3^2-, and 1.0 x 10^-3 M Ag (S2O3)2^3-.
You read the voltage to be 0.76 V
a. Calculate the concentration of Ag+ at the anode.
b. Determine the value of the equilibrium constant for the
formation of Ag(S2O3)2 ^3-.
Ag+ (aq) + 2S2O3 ^2- (aq) --> Ag(S2O3)2 ^3- (aq) K=?
In: Chemistry
a) Calculate the solubility (in grams per 1.00×10^2mL of solution) of magnesium hydroxide in a solution buffered at pH = 12.
S1 = _________________ g/(1.00×10^2mL)
b) Calculate the solubility (in grams per 1.00×10^2mL of solution) of magnesium hydroxide in pure water.
S = __________________ g/(1.00×10^2mL)
c) How does the solubility of Mg(OH)2 in a buffered solution compare to the solubility of Mg(OH)2 in pure water?
S1/S = ________________
TIA.
In: Chemistry
In: Chemistry
A voltaic cell is constructed that is based on the following
reaction:
Sn2+(aq)+Pb(s)→Sn(s)+Pb2+(aq).
Part A If the concentration of
Sn2+ in the cathode compartment is 1.50 M and the cell generates an emf of 0.18 V , what is the concentration of Pb2+ in the anode compartment?
Part B If the anode compartment contains
[SO2−4]= 1.40 M in equilibrium with PbSO4(s), what is the Ksp of PbSO4?
In: Chemistry
Complete and Balance:
a. Fe3+ + NH3OH+ = Fe2+ + N2
b. Fe3+ + NH3OH+ = Fe2+ + N2O
c. Fe3+ + NH3OH+ = Fe2+ + NO
d. Fe3+ + NH3OH+ = Fe2+ + NO2
e. Fe3+ + NH3OH+ = Fe2+ + NO3-
In: Chemistry
Complete the following table of data for Ce2(SO4)3 · 9 H2O. (Assume the density of water is 1.00 g/mL.)
| T (°C) |
Solubility (g/100. g) |
Concentration (M) |
Ksp |
?G (kJ/mol) |
|---|---|---|---|---|
| 27.0 | 9.27 | ____ | ____ | ____ |
| 34.0 | 7.82 | ____ | ____ | ____ |
| 41.0 | 6.54 | ____ | ____ | ____ |
| 48.0 | 5.45 | ____ | ____ | ____ |
| 55.0 | 4.54 | ____ | ____ | ____ |
| 62.0 | 3.81 | ____ | ____ | ____ |
| 69.0 | 3.26 | ____ | ____ | ____ |
Use a graph of ?G vs. T to determine the following. (Enter your answers to three significant figures.)
What is the value of ?H for the system?
_________kJ/mol
What is the value of ?S for the system?
__________J/mol·K
In: Chemistry
According to the hard and soft acid and bases indicate with arrow the direction of the favored reaction ,balance the equation and indicate which is a harder or softer acid and harder or softer base.
a)CuCl + LiCH2CH3 ______________ CuCH2CH3 + LiCl
b)KN3 + FeCO3----------K2CO3 + Fe(N3)2
c)Sr(ClO4 )2 + AgI ----------AgClO4 + SrI2
d)NaCN + FeCl2 ----------NaCl + Na4Fe(CN)6
e) KOCH3 + PdS2O3-------- K2S2O3 + Pt(OCH3)2
In: Chemistry
EDTA is a hexaprotic system with the following pKa values: pKa1 = 0.00 pKa4 = 2.69 pKa2 = 1.50 pKa5 = 6.13 pKa3 = 2.00 pKa6 = 10.37 The distribution of protonated forms of EDTA will therefore vary with pH. For equilibrium calculations involving metal complexes with EDTA, it is convenient to calculate the fraction of EDTA that is in the completely unprotonated form, Y4– . This fraction is designated αY4–. Calculate αY4– at the following two pH values:
pH=3.45
pH=10.85
In: Chemistry