A calcium chloride hydrate has a mass of 4.72g, after heating for several minutes the mass...
determining the formula of a hydrate of calcium chloride (CaCl2·X H2O). Mass (g) Crucible and Lid 28.4735 Crucible and Lid + hydrate salt 33.1938 Crucible and Lid + anhydrous residue 32.0339 What is the mass of the hydrate? mass = ___ g What is the mass of the anhydrous residue? mass = ___ g What is the mass of water lost upon heating the sample? mass = ___ g How many mol of H2O were lost upon heating? (H2O: 18.016...
A hydrate of Cobalt(ii)Chloride had mass of 166.04g before heating. After heating, the anhydrous CoCl2 weighed 130.9g. - what is the mass of the water that was driven off? - how many moles of water were driven off? - how many moles of anhydrous CoCl2 remain? - what is the hydration number (moles of water per mole compound)?
Laboratory 12 Report Sheet - Lab 12 B. Formula of a Hydrate B.1 Mass of crucible B.2 Mass of crucible and salt (hydrate) B3 Mass of crucible and salt (anhydrate) after first heating after second heating (optional) 25.10 26.38 2573 Calculations B.4 Mass of salt (hydrate) B5 Mass of salt (anhydrate) OR B.6 Mass of water lost B.7 Percent water (Show calculations.) _mole B.8 Moles of water (Show calculations.) mole B.9 Moles of salt (anhydrate) (Show calculations.) B.10 Ratio of...
If an unknown hydrate, AC XH20, has a mass of 1.555 g before heating, and a mass of 0.994 g after heating, what is the experimental percentage of water in the hydrate? f the anhydrous compound (AC) in the preceding problem has a molar mass of 160 g/mol, hat are the water of crystallization (X) and formula for the hydrate?
You placed a sample of a hydrate of calcium chloride (CaCl2) in a weighed test tube, and weighed the filled test tube Then you heated it until no more water was evolved. After cooling, you weighed the test tube again. Mass of empty tube (g) 13.89 Mass of filled tube before heating (g) 18.55 Mass after cooling (g) 16.9 Calculate the following: Moles of anhydrous CaC12
After Heating .320 g of NaSO4•xH2O,The residue has a mass of .140g. Calculate the percentage of water in the hydrate. Write the hydrate formula 3. After heating,0320 g of Na2S04 Hydrate XH20, the residue has a mass of o, 140 g. Calculate the percentage (%) of water in the hydrate. What is the hydrate formula?
3. What happens when a hydrate is heated? 4. A hydrate of CoCl, with a mass of 6.00 g is heated strongly. After cooling, the mass of the anhydrate is 3.27 g. a. How many grams of H2O were lost from the hydrate? b. What is the % water in the hydrate? c. What is the formula of the CoCl, hydrate? d. Write the equation for the dehydration of the CoCl, hydrate.
Cacl2 has a mass of .101g before heating, after heating it has a mass of .013 find the stoichiometric waters of hydration and the name of the hydrate
4. A hydrate of CoCl2 with a mass of 6.00 g is heated strongly. After cooling, the mass of the anhydrate is 3.27 g. a. How many grams of H2O were lost from the hydrate? b. What is the % water in the hydrate? c. What is the formula of the Cocl, hydrate? d. Write the equation for the dehydration of the CoCl, hydrate. Moles and Chemical Formulas Questions and Problems Q1 Using the rules for writing the formulas of...
From your data, determine the mass of the water present in your hydrate, the number of moles of water present in your hydrate, and the number of moles of compound present in your hydrate. Determine the formula of your hydrate. Data collected: mass of crucible 19.214g mass of crucible and unknown hydrate: 20.208g mass of crucible after heating w/ hydrate: 19.701 mass of hydrate: 0.994g formula of compound that forms hydrate: MgSO4 . nH2O