What is the mass of 0.76 moles of the cupric sulfate salt CuSO4.5H2O?
What is the mass of 0.76 moles of the cupric sulfate salt CuSO4.5H2O?
What is the mass of 0.90moles of the cupric sulfate salt CuSO4∙5H2O
A. calculate moles of magnesium sulfate b.calculate moles of water c. The ratio of moles water: moles of magnesium sulfate. d. Identify any potential sources of error. Data Table 1 Sample 1 2 3 Mass of aluminum dish 1.24g 1.24g 1.24g Mass of aluminum dish + Epsom salt 1.99g 1.97g 2.14g .75g .73g 90g Epsom salt, original (hydrated) mass Mass of aluminum dish + Epsom salt after heating Epsom salt, heated (dehydrated) mass 1.62g 1.61g 1.72g .38g .37g .48g Mass...
CuSO4• 5H20 -------> Custy + D u 2) What is the color for anhydrous salt of copper (II) sulfate (CuSO4)? What is the color for ionic hydrate compound of copper (II) sulfate pentahydrate (CuSO4.5H2O)? 3) How would you test a colorless crystalline compound to determine whether it is a hydrate or not? 4) How many grams of CuSO4.5H20 are needed to prepare 50.0 mL of a 1.00 M CuSO4 solution? 5) Suppose you used the Procedure in this experiment to...
What is the mass of 4.5 moles of magnesium sulfate?
1. Calculate the mass of copper(II) sulfate pentahydrate (CuSO4.5H2O) needed to prepare 1.50 grams ol tetramminecopper (II) sulfate monohydrate (Cu(NH3)4] SO4 H2O according to the overall reaction on the first page of the lab. The overall net equation for the reaction is: Cu(H2O)2]SO4+H2O (aq) + 4 NH3 (aq) → [Cu(NH3)4]SO4+H2O + +4 H20 و اما الدم
calculate the molarity of the new solution 5. You prepare a stock solution of cupric sulfate pentahydrate by adding 3.745 g to a volumetric flask and filling the flask to the 100.0 mL mark with water. You then add 3.00 mL of the stock solution and 2.00 mL of water to a test tube and mix well. Calculate the molarity of the new solution. a. 0.225 moles b. 0.150 moles C. 0.100 moles d. 0.352 moles e. 0.0900 moles
Write an equation for the thermal dehydration of copper (II) sulfate pentahydrate (CuSO4.5H2O) and for the thermal decomposition of CuSO4 to CuO in air.
1. (DCH Page 23) Cupric sulfate is commonly sold as the pentahydrate, CuSO4-H2O, which has 5 moles of H20 for each mole of CuSO4 in the solid. The formula mass is 249.69 g/mol. How many grams of CuS04 H2O should be dissolved in a 250 mL volumetric flask to make a solution containing 8.00 mM Cu2* (a) 1.28 g (b) 0.499 g (c) 2.00 g (d) 0.319 g (e) 3.72 g
These questions will help you with your own data collection 1. What is the molar mass of cupric sulfate pentahydrate? (CuSO4.5H20) 2. How many grams of CuSO4.5H2O is needed to make a 0.1 M solution in 40 mL of water? 3. If you wanted to make 10 mL of a 0.06 M CuSO4 solution, what ml amount of 0.1 M CuSO4 solution and deionized water would you need? (Remember: M,V=MV)
Formula of salt NAO AC Mass of salt used 8.3145 Moles of salt 10 moles Change in Temperature (Tr-T) -1.6 Total mass of solution 150ml x.99 7g| ML) + 8.314. UUUUU 157.869 5.5% Weight percent of salt in solution (8.314/150 x 100 =5.5% Specific heat of solution 4.18J Ig t Heat change for solution (9soln) Heat change for the calorimeter (cal) Total heat change (total) Molar heat of solution of your salt