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Chapter 27: Q10P (page 767)
A 50.00-mL solution containingwas treated with excess AgNo3 to precipitate 0.2146 g of AgBr (FM 187.772). What was the molarity of NaBr in the solution?
The Molarity of NaBr in a solution is .
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Thermogravimetric analysis and propagation of error. 16 Crystals of deuteratedpotassium dihydrogen phosphate,are used in optics as a light valve, as a light deflector, and for frequency doubling of lasers. The optical properties are sensitive to the fraction of deuterium in the material. A publication states that deuterium content can be determined by measuring the mass lost by dehydration of the crystal after slow heating to in a Pt crucible under
(a) Let be the mass of product divided by the mass of reactant:
Show that the coefficient xin is related to by the equation
What would be the value ofif starting material were 100% deuterated?
(b) One crystal measured in triplicate gave an average value of.Find x for this crystal.
(c) From equation B.1 in Appendix B, show that the uncertainty in is related to the uncertainty inby the equation
(d) The uncertainty in deuterium: hydrogen stoichiometry isThe authors estimate that their uncertainty in is From compute. Write the stoichiometry in the form Ifwere 0.001 (which is perfectly reasonable), what wouldbe?
Why are many ionic precipitates washed with electrolyte solution instead of pure water?
Why is tin used to encapsulate a sample for combustion analysis?
Explain how the quartz crystal microbalance at the opening of Chapter 2 measures small masses
Statistics of coprecipitation. 17In Experiment 1,200.0mL of solution containing 10.0mg of (from ) were treated with excess solution to precipitate containing some coprecipitated . To find out how much coprecipitated was present, the precipitate was dissolved in 35mL of 98wt% and boiled to liberate , which was removed by bubbling gas through the . The HCI/ stream was passed into a reagent solution that reacted with to give a color that was measured. Ten replicate trials gave values of 7.8,9.8,7.8,7.8,7.8,7.8,13,7,12.7,13.7, and 12.7. Experiment 2 was identical to the first one, except that the mL solution also contained of from ). Ten replicate trials gave 7.8,10,8,8.8,7.8,6.9, 8.8, 15.7 , 12.7 , 13.7and .
(a) Find the mean, standard deviation, and 95% confidence interval for in each experiment.
(b) Is there a significant difference between the two experiments? What does your answer mean?
(c) If there were no coprecipitate, what mass of (FM 233.39) would be expected?
(d) If the coprecipitate is (FM 208.23), what is the average mass of precipitatein Experiment 1. By what percentage is the mass greater than the mass in part (c)?
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