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Chapter 27: Q3P (page 767)
Why is high relative supersaturation undesirable in a gravimetric precipitation?
The high relative supersaturation undesirable in a gravimetric precipitation due to the fast nucleation- suspension of colloids would be higher would isn鈥檛 desirable.
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What is the purpose of the and Cu in Figure 27-8?
What measures can be taken to decrease the relative supersaturation during a precipitation?
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)?
Propagation of error. A mixture containing only silver nitrate and mercurous nitrate was dissolved in water and treated with excess sodium cobalticyanide, to precipitate both cobalticyanide salts:
(a) The unknown weighed 0.4321g and the product weighed 0.4515g. Find wt% in the unknown. Caution: Keep all the digits in your calculator or else serious rounding errors may occur. Do not round off until the end.
(b) Even a skilled analyst is not likely to have less than a 0.3% error in isolating the precipitate. Suppose that thege is negligible error in all quantities, except the mass of product, which has an uncertainty of0.30%. Calculate the relative uncertainty in the mass of in the unknown.
How many grams of AgBr would have been formed from 0.100 g of?
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