In standardization of KMNO, againstNa,C,04 (134 g/mol), if 35 mL of the 0.02 MKMNO, is used find the mass of Na,C,042MN0, + 5 H,C,04 + 6 H* ==> 2 Mn2 + 10co, + 8 H20a. 0.0375 gb. 0.0523c. 0.101 gd. 0.235 gIn the reactionCe +Fe s>+]Knowing that Fe +e => Fe2 E 0.767 VCe +e sa> Ce E= 1.70 VAnd Hydrogen reference electrode was used.In titrating 25 ml of 0.2 M Fe against 0.1 M ofCe, it the volume of titrant is half theequivalence volume, then the2O a Ereaction = E of Fe*O b. E reaction = 0OC.E reaction E" of Ce4+O d. E reaction 1//2 (E of Fe + E of Ce

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In standardization of KMNO, against NazC,04 (134 g/mol), if 35 mL of the 0.02 M KMNO, is used find the mass of Na2C204 2Mno, + 5 H2C204+6 H* ==> 2 Mn2+ + 10 co, + 8 H,0 1 a. 0.0375 g b. 0.0523 C. 0.101 g d. 0.235 g

In standardization of KMNO, against NazC,04 (134 g/mol), if 35 mL of the 0.02 M KMNO, is used find the mass of Na2C204 2Mno, + 5 H2C204+6 H* ==> 2 Mn2+ + 10 co, + 8 H,0 1 a. 0.0375 g b. 0.0523 C. 0.101 g d. 0.235 g

Chemistry: An Atoms First Approach

2nd Edition

ISBN:9781305079243

Author:Steven S. Zumdahl, Susan A. Zumdahl

Publisher:Steven S. Zumdahl, Susan A. Zumdahl

Chapter7: Chemical Energy

Section: Chapter Questions

Problem 134IP: On Easter Sunday, April 3, 1983, nitric acid spilled from a tank car near downtown Denver, Colorado....

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On Easter Sunday, April 3, 1983, nitric acid spilled from a tank car near downtown Denver, Colorado. The spill was neutralized with sodium carbonate: 2HNO3(aq)+Na2CO3(aq)2NaNO3(aq)+H2O(l)+CO2(g) a. Calculate H for this reaction. Approximately 2.0 104 gal nitric acid was spilled. Assume that the acid was an aqueous solution containing 70.0% HNO3 by mass with a density of 1.42 glcm3. What mass of sodium carbonate was required for complete neutralization of the spill, and what quantity of heat was evolved? (Hf for NaNO3(aq) = 467 kJ/mol) b. According to The Denver Post for April 4, 1983, authorities feared that dangerous air pollution might occur during the neutralization. Considering the magnitude of H, what was their major concern?
The present average concentration (mass percent) of magnesium ions in seawater is 0.13%. A chemistry textbook estimates that if 1.00 × 108 tons Mg were taken out of the sea each year, it would take one million years for the Mg concentration to drop to 0.12%. Do sufficient calculations to either verify or refute this statement. Assume that Earth is a sphere with a diameter of 8000 mi, 67% of which is covered by oceans to a depth of 1 mi, and that no Mg is washed back into the oceans at any time.
The aluminum in a 2.200-g sample of impure ammonium aluminum sulfate was precipitated with aqueous ammonia as the hydrous ‍‍Al2O3⋅xH2O. The precipitate was filtered and ignited at 1000°C to give anhydrous Al2O3, which weighed 0.3006 g. Express the result of this analysis in terms of a. %NH4Al(SO4)2 b. %Al2O3 c. %Al
When Na3PO4 and Ca(NO3)2 are combined , the following reactions occurs:2PO4 3- (aq) + 3 Ca2+ (aq) ------ Ca3PO4)2How many grams of Ca3(PO4)2 (MM = 310.18 g/mol) are obtained from 15.00 ml of 0.1386 M Na3PO4 are mixed with 20.00 ml of 0.2118 M Ca(NO3)2 ?
A 0.6214-g portion of manganese dioxide was added to an acidic solution in which 1.1444 9 of a chloride-containing sample was dissolved. Evolution of chlorine took place as a consequence of the following reaction: MnO2 (s) + 2Cl- + 4H+ → Mn2+ + Cl2 (g) + 2H2O After the reaction was complete, the excess MnO2 was collected by filtration, washed, and weighed, and 0.3153 g was recovered. Express the results of this analysis in terms of percent aluminum chloride. _____% AlCl3
A 0.6447 g portion of manganese dioxide was added to an acidic solution in which 1.1402 g of a chloride containing sample was dissolved. Evolution of chlorine took place as a consequence of the following reaction: MnO2(s) + 2Cl- + 4H+ ® Mn2+ + Cl2(g) + 2H2O After the reaction was complete, the excess MnO2 was collected by filtration, washed, and weighed, and 0.3521 g was recovered. Express the results of this analysis in terms of percent aluminum chloride. (Al:27.0 ; Mn:55.0 ; O:16.0 ; Cl:35.5 ; H:1.0 g/mol)
How many milliliters of silver nitrate is required in the standardization? If wt. of silver nitrate (precipitate) = 0.600 g mw of silver nitrate = 170 g/mol mw of silver chloride = 143 g/mol meq of silver nitrate = 0.170 initial volume of silver nitrate = 40 mL N of silver nitrate = 0.105 N Choices: A. 4.995; B. 49.950; C. 49.590; D. 45.990 I tried to compute for the required amount using 0.105 N but my answer isn't in the choices. Please help me, thanks!
Alum [KAl(SO₄)₂.xH2O] is used in food preparation, dyefixation, and water purification. To prepare alum, aluminum isreacted with potassium hydroxide and the product with sulfuricacid. Upon cooling, alum crystallizes from the solution.(a) A 0.5404-g sample of alum is heated to drive off the watersof hydration, and the resulting KAl(SO₄)₂weighs 0.2941 g. De-termine the value of xand the complete formula of alum.(b) When 0.7500 g of aluminum is used, 8.500 g of alum forms.What is the percent yield?
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For the analysis of unknown soda and vinegar samples, 25.0 mL soda and 1.0 mL vinegar samples were diluted to 50.0 mL in separate Erlenmeyer flasks. KHP, 0.85 g, (Purity = 99.98%; Molar mass = 204.22 g/mol) was titrated with 11.5 mL of NaOH. After the standardization step, it required 0.0143 L of NaOH to reach the endpoint with the soda sample while it took 0.00885 L with the vinegar sample. Phenolphthalein was used as the indicator for the experiment. Express all final answers in 2 significant figures. a. Determine the concentration of the titrant (NaOH) b. Determine the concentration of the unknown vinegar sample. c. Determine the concentration of the unknown soda sample.
another question The aluminum in a 1.200g sample of impure ammonium aluminum sulfate was precipitatedwith aqueous ammonia as the hydrous Al2O3 · XH2O. The precipitate was filtered and ignitedat 100°C to give anhydrous Al2O3, which weighed 0.2001 g. Express the result of this analysisin terms of % Al.
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