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In the table below, use your most important scientific instrument (your calculator) to fill in the little boxes that are highlighted: 2. Data Table Identity of Dehydrated salt (for afterwards) Mass of empty dish 70.874g Mass of dish + hydrated salt 71.346g Mass of hydrated salt Mass of dish + dehydrated salt a) first heating 71.194g b) second heating 71.174g Mass of dehydrated salt Mass of water lost Wt. % of water in hydrated salt Moles of dehydrated salt Moles of water driven off Empirical formula of hydrated salt In your notebooks, the following must be clearly visible. I won't hunt for it...LABEL IT PROPERLY! Show the calculation for obtaining the mass of your hydrated salt used. b. a. Show the calculation for obtaining the mass of your dehydrated salt after the second heating. C. Show the calculation for obtaining the mass of water that was driven off (based on second heating). Show the calculation for obtaining the weight percent of water that was in your hydrated salt. Show the calculation for obtaining the moles of dehydrated salt left after the second heating. f. d. е. Show the calculation for obtaining the moles of water that were driven off. Show the calculation for obtaining the empirical formula for your hydrated salt. g.

In the table below, use your most important scientific instrument (your calculator) to fill in the little boxes that are highlighted: 2. Data Table Identity of Dehydrated salt (for afterwards) Mass of empty dish 70.874g Mass of dish + hydrated salt 71.346g Mass of hydrated salt Mass of dish + dehydrated salt a) first heating 71.194g b) second heating 71.174g Mass of dehydrated salt Mass of water lost Wt. % of water in hydrated salt Moles of dehydrated salt Moles of water driven off Empirical formula of hydrated salt In your notebooks, the following must be clearly visible. I won't hunt for it...LABEL IT PROPERLY! Show the calculation for obtaining the mass of your hydrated salt used. b. a. Show the calculation for obtaining the mass of your dehydrated salt after the second heating. C. Show the calculation for obtaining the mass of water that was driven off (based on second heating). Show the calculation for obtaining the weight percent of water that was in your hydrated salt. Show the calculation for obtaining the moles of dehydrated salt left after the second heating. f. d. е. Show the calculation for obtaining the moles of water that were driven off. Show the calculation for obtaining the empirical formula for your hydrated salt. g.

Introduction to Chemical Engineering Thermodynamics
Introduction to Chemical Engineering Thermodynamics
8th Edition
ISBN:9781259696527
Author:J.M. Smith Termodinamica en ingenieria quimica, Hendrick C Van Ness, Michael Abbott, Mark Swihart
Publisher:J.M. Smith Termodinamica en ingenieria quimica, Hendrick C Van Ness, Michael Abbott, Mark Swihart
Chapter1: Introduction
Section: Chapter Questions
Problem 1.1P
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In the table below, use your most important scientific instrument (your calculator) to fill in the little boxes that are highlighted: 2. Data Table Identity of Dehydrated salt (for afterwards). Mass of empty dish 70.874g Mass of dish + hydrated salt 71.346g Mass of hydrated salt Mass of dish + dehydrated salt a) first heating 71.194g b) second heating 71.174g Mass of dehydrated salt Mass of water lost Wt. % of water in hydrated salt Moles of dehydrated salt Moles of water driven off Empirical formula of hydrated salt In your notebooks, the following must be clearly visible. I won't hunt for it...LABEL IT PROPERLY! Show the calculation for obtaining the mass of your hydrated salt used. b. а. Show the calculation for obtaining the mass of your dehydrated salt after the second heating. Show the calculation for obtaining the mass of water that was driven off (based on second heating). Show the calculation for obtaining the weight percent of water that was in your hydrated salt. Show the calculation for obtaining the moles of dehydrated salt left after the second heating. f. C. d. е. Show the calculation for obtaining the moles of water that were driven off. Show the calculation for obtaining the empirical formula for your hydrated salt. g.
Transcribed Image Text:In the table below, use your most important scientific instrument (your calculator) to fill in the little boxes that are highlighted: 2. Data Table Identity of Dehydrated salt (for afterwards). Mass of empty dish 70.874g Mass of dish + hydrated salt 71.346g Mass of hydrated salt Mass of dish + dehydrated salt a) first heating 71.194g b) second heating 71.174g Mass of dehydrated salt Mass of water lost Wt. % of water in hydrated salt Moles of dehydrated salt Moles of water driven off Empirical formula of hydrated salt In your notebooks, the following must be clearly visible. I won't hunt for it...LABEL IT PROPERLY! Show the calculation for obtaining the mass of your hydrated salt used. b. а. Show the calculation for obtaining the mass of your dehydrated salt after the second heating. Show the calculation for obtaining the mass of water that was driven off (based on second heating). Show the calculation for obtaining the weight percent of water that was in your hydrated salt. Show the calculation for obtaining the moles of dehydrated salt left after the second heating. f. C. d. е. Show the calculation for obtaining the moles of water that were driven off. Show the calculation for obtaining the empirical formula for your hydrated salt. g.
The only thing you are doing differently here is you are NOT in the lab so you DO NOT have to physically weigh out the salt, put it in a crystallizing dish, heat the dish too strongly, causing the salt to spray all over the place, stop, clean up, and start again whilst I stand behind you and hound you to keep your goggles on. That's because we aren't there. Angels and ministers of grace defend us from such joy..5 Have fun. ACT 2: YOUR DATA Today's salt in question appears as below left. A flame test confirms it is a salt of manganese, which confirms your suspicions; manganese salts are often uniquely pink in appearance. There are several different formulations, however; which one is this? Your next step would be to take a small amount and drop it in distilled water to see if it is soluble in water. It is! That certainly narrows the possibilities. On a hunch, you take a solution of silver nitrate AGNO3(a9) and put a few drops in the solutions. INSTANTLY the vessel is full of a milky precipitate. Hmm, that narrows it down again to ONE of THREE possibilities. Examining the precipitate closely, you notice the precipitate is WHITE (not colored in the visible). Okay, NOW you know what it is. What is your guess (check one)?: CIt- Br1- But what is the formula? Sending it off for elemental analysis, you find the formula weight is 125.944 g mol-1 NOW you know enough to do the calculation, to figure the exact formula by calculating the empirical formula FIRST. THIS IS THE POINT OF TODAY'S LABORATORY. You data table is given on the next page; this is the information you will use to accomplish your mission. Hamlet, Prince of Denmark, Act 1, Scene 4. With apologies to William Shakespeare.
Transcribed Image Text:The only thing you are doing differently here is you are NOT in the lab so you DO NOT have to physically weigh out the salt, put it in a crystallizing dish, heat the dish too strongly, causing the salt to spray all over the place, stop, clean up, and start again whilst I stand behind you and hound you to keep your goggles on. That's because we aren't there. Angels and ministers of grace defend us from such joy..5 Have fun. ACT 2: YOUR DATA Today's salt in question appears as below left. A flame test confirms it is a salt of manganese, which confirms your suspicions; manganese salts are often uniquely pink in appearance. There are several different formulations, however; which one is this? Your next step would be to take a small amount and drop it in distilled water to see if it is soluble in water. It is! That certainly narrows the possibilities. On a hunch, you take a solution of silver nitrate AGNO3(a9) and put a few drops in the solutions. INSTANTLY the vessel is full of a milky precipitate. Hmm, that narrows it down again to ONE of THREE possibilities. Examining the precipitate closely, you notice the precipitate is WHITE (not colored in the visible). Okay, NOW you know what it is. What is your guess (check one)?: CIt- Br1- But what is the formula? Sending it off for elemental analysis, you find the formula weight is 125.944 g mol-1 NOW you know enough to do the calculation, to figure the exact formula by calculating the empirical formula FIRST. THIS IS THE POINT OF TODAY'S LABORATORY. You data table is given on the next page; this is the information you will use to accomplish your mission. Hamlet, Prince of Denmark, Act 1, Scene 4. With apologies to William Shakespeare.
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