. T Locate where the fire safety equipment like blankets, fire extinguisher, fire alarms etc are in the lab so that in case of an accident you know where to look for one. Special precautions on how to use the instrument First light the splinter before turning on the Bunsen burner and use the valves and collar to control the amount of gas and oxygen flowing in through the hole so that the flame burns blue and not yellow. Blue flames are oxygen-rich therefore they burn hotter and yellow flames are oxygen-deprived so they are comparatively cooler than blue flames. Also, yellow flames tend to be uncontrolled, and in comparison blue flames then to be controlled. Since the Bunsen burner is a source of open flame, care must be taken to locate and operate it away from flammable material.

. T Locate where the fire safety equipment like blankets, fire extinguisher, fire alarms etc are in the lab so that in case of an accident you know where to look for one. Special precautions on how to use the instrument First light the splinter before turning on the Bunsen burner and use the valves and collar to control the amount of gas and oxygen flowing in through the hole so that the flame burns blue and not yellow. Blue flames are oxygen-rich therefore they burn hotter and yellow flames are oxygen-deprived so they are comparatively cooler than blue flames. Also, yellow flames tend to be uncontrolled, and in comparison blue flames then to be controlled. Since the Bunsen burner is a source of open flame, care must be taken to locate and operate it away from flammable material.

Chemical Principles in the Laboratory

11th Edition

ISBN:9781305264434

Author:Emil Slowinski, Wayne C. Wolsey, Robert Rossi

Publisher:Emil Slowinski, Wayne C. Wolsey, Robert Rossi

Chapter6: Properties Of Hydrates

Section: Chapter Questions

Problem 1ASA: A student is given a sample of a pink manganese (II) chloride hydrate. She weighs the sample in a...

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A student is given a sample of a pink manganese (II) chloride hydrate. She weighs the sample in a dry, covered crucible and obtains a mass of 26.742g for the crucible, cover, and sample. Earlier she had found that the crucible and cover weighed 23.599g. She then heats the crucible to drive off the water of hydration, keeping the crucible at red heat for about 10 minutes with the cover slightly ajar. She then lets the crucible cool and finds it has a lower mass; the crucible, cover and contents then weigh 25.598g. In the process the sample was converted to off-white anhydrous MnCl2. a. What was the mass of the hydrate sample? _ghydrate b. What is the mass of the anhydrous MnCl2? _gMnCl2 c. How much water was driven off? _gH2O d. What is the percent by mass of water in the hydrate? water=massofwaterinsamplemassofhydrateinsample100 _massH2O e. How many grams of water would there be in 100.0g hydrate? How many moles? _gH2O; _molesH2O f. How many grams of MnCl2 are there in 100.0g hydrate? How many moles? What percentage of the hydrate is MnCl2? Convert the mass of MnCl2 to moles. The molar mass of MnCl2 is 125.85g/mol. _gMnCl2; _molesMnCl2 g. How many moles of water are present per mole MnCl2? _ h. What is the formula of the hydrate? _