1. Which of the following has the incorrect assignment of oxidation numbers?
a. Fe2O3 (Fe: 2+, O: 2-)
b. H2SO4 (H:1+, S: 6+, O: 2-)
c. Cr2O72- (Cr: 6+, O: 2-)
d. KCl (K: 1+, Cl: 1-)
2. Which of the following has the incorrect assignment of oxidation numbers?
a. H2O2 (H: 1+, O: 2-)
b. NO3– (N: 5+, O: 2-)
c. NO2 (N: 4+, O: 2-)
d. K3PO4: (K: 1+, P: 5+, O: 2-)
3. Which of the following has the incorrect assignment of oxidation numbers?
a. SiO2 (Si: 4+, O: 2-)
b. KNO2 (K: 1+, N: 3+, O: 2-)
c. HNO3 (H: 1+, N: 3+, O: 2-)
d. NH4Cl (N: 3-, H: 1+, Cl: 1-)
Based on the reaction, Sn + Cu2+ ⇌ Sn2+ + Cu+ (in acidic medium)
Calculate the following values:
a. E°cell
b. ΔG°
c. K
d. E (when [Cu2+] = 0.0200 M, [Sn2+] = 0.0100 M, and [Cu+] = 0.0300 M)
BALANCE THE FOLLOWING REDOX REACTION.. Show your full solution/method. Label each step. Briefly explain what you did in each step (few phrases and direct to the point, example: Balanced the oxygen atoms by adding water.).
a. Fe2O3 + CO ⇌ Fe + CO2 (in acidic medium)
b. Mg + NiO2 ⇌ Mg(OH)2 + Ni(OH)2 (in basic medium)
A water was tested for water hardness. A 50.00 mL aliquot was prepared and buffered to pH 10.0, it required 23.55 mL of 0.0250 M EDTA. A second aliquot, prepared with NaOH, was titrated with 14.53 mL of the same EDTA titrant. Calculate the following:
a. total hardness (in ppm CaCO3)
b. magnesium hardness (in ppm MgCO3)
The chloride ion content of a 250.0-mL seawater sample was titrated against 0.1102 M silver nitrate, requiring 13.56 mL to reach end point. What is the molarity of the chloride ion in the seawater sample?
The purity of a sample of sodium oxalate, Na2C2O4, is determined by titrating with a standard solution of KMnO4. If a 0.5116-g sample requires 35.62 mL of 0.0400 M KMnO4 to reach the titration’s end point, what is the %w/w Na2C2O4 in the sample.
1. For the following reaction at 25 oC, under these conditions: [Fe2+] = 0.50 M, [Fe3+] = 0.10 M, [MnO4−] = 0.025 M, [Mn2+] = 0.015 M, and a pH of 7.00.
5Fe2+(aq) + MnO4−(aq) + 8H+(aq) ⇌ 5Fe3+(aq) + Mn2+(aq) + 4H2O(l)
Calculate
(a) the standard potential
(b) the equilibrium constant
(c) the potential
A 25.ID-mL sample containing Fe³° and Cu°° required
16.06 mL of 0.050 83 M EDTA for complete titration. A 50.IXI-mL sample of the unknown was treated
with NH F to protect the Fe°°. Then Cu²° was reduced and masked by thiourea. Addition of
25.00 mL of 0.050 83 M EDTA liberated Fe from its fluoride complex to form an EDTA complex. The
excess EDTA required
19.77 mL of 0.018 83 M Pb'+ to reach a xylenol orange end point.
Find (Cu' ) in the unknown.
A 10.231-9 sample of window cleaner containing amnmnia was diluted with 39.466 g of water.
Then 4.373 g of solution were iitraied with 14.22 mL of 0.106 3 M HCI to reach a bromocresol green
end point. Find the weight percent of NH (FM 17.031) in the cleaner.
Ni(CNi42 + 2AgBr(i) 2Ag(C 2 + Ni²+ + 2Br°
The liberated nickel ion required 26.73 mL of 0.02089 M EDTA. The bromate in a 10.00-mL aliquot was
reduced to bromide with arsenic(UI) priof to the addition of silver nitrate. The same procedure
was followed, and the released nickel ion was titrated with 21.94 mL of the EDTA solution.
Calculate the percentages of NaBr and NaBrO3 in the sample.