Question 30 ( A 2.47 g sample of hydrated cobalt(II) nitrate is heated. After heating, 1.55 g of pure Co(NO3)2 is obtained. What is the formula for this hydrate? O Co(NO3)2 8H₂O Co(NO3)2 6H₂O O CO(NO3)2 4H₂O O CO(NO3)2 2H₂O

Question 30 ( A 2.47 g sample of hydrated cobalt(II) nitrate is heated. After heating, 1.55 g of pure Co(NO3)2 is obtained. What is the formula for this hydrate? O Co(NO3)2 8H₂O Co(NO3)2 6H₂O O CO(NO3)2 4H₂O O CO(NO3)2 2H₂O

Chemistry & Chemical Reactivity

10th Edition

ISBN:9781337399074

Author:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel

Publisher:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel

Chapter4: Stoichiometry: Quantitative Information About Chemical Reactions

Section: Chapter Questions

Problem 37PS: Nickel forms a compound with carbon monoxide, Nix(CO)y. To determine its formula, you carefully heat...

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1)When Jack performed a flame test on his unknown solid, he observed a violet-colored flame. Given this result and the answer to Question 16, what is the chemical formula of Jack's unknown solid? a)KHCO 3 b)NaHCO 3 c)K 2CO 3 d)Na 2CO 3 2) A Mass of empty evaporating dish + watch glass 65.362 g B Mass of dish + watch glass + initial solid 65.864 g C Mass of dish + watch glass + carbonate 65.705 g D Mass of dish + watch glass + chloride 65.716 g Calculate the mass (in grams) of the final chloride product that Jack obtained after reacting his carbonate with HCl. This mass represents the actual yield of Jack's overall reaction.Include the appropriate number of significant figures. 3)Use your answer to Question 1 and the appropriate balanced chemical equation (see page 2 in the procedure handout) to calculate the theoretical yield (in grams) of MCl in Jack's reaction (M = Na or K, depending on the chemical formula of the…
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Question 2 : Many chemical salts come as hydrated crystals, i.e. there is a specific ratio of water molecules associated with the salt crystals. For example: CaCl2. 2H2O (Calcium chloride dihydrate; FW = 147.01 g/mol) has 2 water molecules to every CaCl2 molecule. The difference between anhydrate and dihydate is that anhydrate form CaCl2 does not contain any water molecules whereas dihydrate form contains two H2O molecules per CaCl2 molecule. Therefore since it is possible to have CaCl2 as an anhydrous (without water) powder the molecular weight of the anhydrate is 36 g/mol lighter than the dihydrate form (FW = 110.98 g/mol). Once dissolved in water, these salts have the same chemical properties, but in the solid state they obviously have different FWs. You are given a recipe for a buffer that contains 8% (w/v) CaCl2.2H2O, however, you only have CaCl2 anhydrous available to you. How much CaCl2 anhydrous do you need to make 3.5 L of the buffer with the same molar concentration as in the…