After Heating .320 g of NaSO4•xH2O,The residue has a mass of .140g. Calculate the percentage 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?
6. The following data are compiled during water of hydration experiment of BaCl2.xH2O. Mass of beaker + watch glass 35.82 grams Mass of beaker + watch glass + sample 37.80 grams Mass of beaker + watch glass + residue after first heating 37.52 grams Mass of beaker + watch glass + residue after second heating 37.51 grams What is the formula of the hydrate?
- Part A After 0.61 g of CoCl2.6H2O is heated, the residue has a mass of 0.308 8. Calculate the % H20 in the hydrate. IV AERO? | % H₂O Submit Request Answer Part B What was the actual number of moles of water per formula unit CoCl2? 0 AED RO? Submit Request Answe
Part A After 0.62g of CoCl2 · 6H2O is heated, the residue has a mass of 0.302 g . Calculate the % H20 in the hydrate. ΑΣΦ H20 Part B What was the actual number of moles of water per formula unit CoCl2? ΑΣΦ
5. Extensive heating of 245.2 g of FeCl3 • xH2O produces 137.2 g of FeCl3. a. Calculate the mass of water lost b. Calculate the number of moles of water lost c. Calculate the number of moles of anhydrous salt d. Calculate the mole : mole ratio of salt to water e. Determine the formula for the hydrated salt
2. Using the data from the experiment, calculate the mass of copper (II) sulfate residue and the mass of water (Items 5 and 6 from the Data Form). Express your answers in grams to the nearest hundredth (+ 0.01 g). Show your work. 3. Calculate the moles of copper (II) sulfate present from the mass of the copper (II) sulfate. Express your answer in moles as three significant digits. Show your work. 4. Calculate the moles of water driven off...
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...
just write the answers. Part A After 0.64g of CoCl2 6H2O is heated, the residue has a mass of 0.32 g . Calculate the % H20 in the hydrate. ΑΣΦ H20 Submit Request Answer Part B What was the actual number of moles of water per formula unit CoCl2? ΑΣΦ Consider the following precipitation reaction: 2 Na3PO4 (aq) + 3 CuCl2 (aq) + Cu3(PO4)2 (s) + 6 NaCl(aq) Part A What volume of 0.193 M Na3PO4 solution is necessary to...
Data Table 1. CuSO4 Data Mass of empty cup (grams) Mass of CuSO, hydrate (erams)S Cuso, hydrate after 1st heating (grams) CuSO, hydrate after 2nd heating (grams) Mass of released H20 (grams) Number of moles of released H201 Mass of anhydrous Cuso (grams) Number of moles of anhydrous CuSO 02a mo Questions: A) Calculate the ratio of moles of H2O to moles of anhydrous Cuso4. Note: Report the ratio to the closest whole number. B) Write the empirical formula for...
A student is given a sample of a calcium sulfate hydrate. He places the sample in a dry, covered crucible and weighs it. The total mass (crucible, cover, and hydrate) is 19.39219.392 g. The crucible and cover together had previously weighed 17.98717.987 g. He then heats the crucible to redness for 10 minutes with the cover slightly ajar. After the crucible cools, he weighs the crucible and its contents; the mass is now 19.09819.098 g, due to the loss of...