I need help with 5, 6 and the last three questions.

5. Calculate the ratio of the mole of water lost to the mole of anhyfrous salt.

6. Formula of the hydrate.....

1. Explain why the mass of the sample decreased after it was heated, despite the law of conservation of mass.

2. Why do you have to calculate the mole of water and salt in this lab?

3. Analyze the percent of water in your sample and compare it with the theoretical value which is 36.0%. What conclusion can you draw with this difference of % hydrate?

Molecules/substances to be studied: once we calculate the armant of water. 1) CuSO4H2O Copper(ii) salfate xhydrate Materials and Methods: Googles, gloves and apron Crucible Crucible tong lusb, conver t it be mole. Top balance Water Hot plate Procedure: 1) Clean and dry your evaporating dish. 2) Prepare your hot plate set up heat to number 5 . 3) Place the emply crucible and cover on the bot plate for 2 minates to dry the crucible. (between 5+1 4) Using a crucible tong, remove the cracible and cover from the hot plate and allow to cool for several minutes. Necer put a hot crucible on a fop halance, it will damage the halance. 5) Using a balance, determine the mass of the cooled crucible with its lid. Record this mass in the observations and Data section. 6) With the erucible on the talance, meaure into it approximatcly 2, 000 grams of copper (i1) sulfate Xlydrate with a spatula. Dote the color and appearance of the CuSO2xH2O. Record the mass of the crucible with lid and hydratc copper (II) sufate. 7) Place the crucible and hydrate on the hot plate. Gently heat at first and increase the heat grodually for 5 minutes until all of blue color has disspeared. Dering the heating. a glass-stirring nod can be used to break up langer lumps of the hydrate. If the edge of the solid appear to be turning brown, remove the heat momentarily and resume heating with a cooler setting. Record the color and appearance of anlydrous salt. 8) Allow the crucible to cool for two minutes. Immediately find the mass of the crucible plus the anhydrous salt using a tong. Record the mass in the dana section. The erucible must be weight before it neabsorbs water from the atmosphere. 9) When you have finished weighing the crucible and sall, place the erucible back on the counter top and squirt sone water onto it. Record any change in appearince in the Data section. 10) When you have finished, the anhydrous salt can be thrown into the waste container, and wash the crucible. Report Sheet Show all calculation and take note of significant figures. CiSO2xH2O Mass of crucible, 26. 6.11g Mass of erucible and CuSOxH2O hydrate salt ..2.8. .11....g Mass of CuSO4,xH2O..2.....g Appearance and color of CuSO4H2O... Blue sobid powaler Mass of crucible and CuSO4 anhydrous...2.7.48 8.8 Mass of CuSO4 anhydrous..... 1,37 Mass of water lost..... 6.3.......s Moles of CuSO4 anhydrous. mol Moles of water lost. mol Formula of hydrate. Appearance before addition of water. vercy pale ble pe poucler sub.Stance (Gimost white Appearance after addition of water...Turns blok color Calculations: the Same Remember to show all of your work 1. Find the percent of water lost from the original hydrate (remember that percentage is "the part divided by the whole, multiplied by 1007 ?). %hydrate=massoftydratesaltmassofwateriost100%28.11.63100% 2. Calculate the mass of water lost from the hydrate 5. Calculate the ratio of the mole of water lost to the mole of anhydrocas saly. 6. Formula of the hydrate: liscussion and Conclusion: 1) Explain why the mass of the sample decreased after it was heated, despite the law of conservation of mass. 2) Why do you have to ealculate the mole of water and salt in this lab? 3) Analyze the percent of water in your-sample and compare it with the theoretical value which is 36.0%. What conclusion can you draw with this difference of % hydrate? Molecules/substances to be studied: once we calculate the armant of water. 1) CuSO4H2O Copper(ii) salfate xhydrate Materials and Methods: Googles, gloves and apron Crucible Crucible tong lusb, conver t it be mole. Top balance Water Hot plate Procedure: 1) Clean and dry your evaporating dish. 2) Prepare your hot plate set up heat to number 5 . 3) Place the emply crucible and cover on the bot plate for 2 minates to dry the crucible. (between 5+1 4) Using a crucible tong, remove the cracible and cover from the hot plate and allow to cool for several minutes. Necer put a hot crucible on a fop halance, it will damage the halance. 5) Using a balance, determine the mass of the cooled crucible with its lid. Record this mass in the observations and Data section. 6) With the erucible on the talance, meaure into it approximatcly 2, 000 grams of copper (i1) sulfate Xlydrate with a spatula. Dote the color and appearance of the CuSO2xH2O. Record the mass of the crucible with lid and hydratc copper (II) sufate. 7) Place the crucible and hydrate on the hot plate. Gently heat at first and increase the heat grodually for 5 minutes until all of blue color has disspeared. Dering the heating. a glass-stirring nod can be used to break up langer lumps of the hydrate. If the edge of the solid appear to be turning brown, remove the heat momentarily and resume heating with a cooler setting. Record the color and appearance of anlydrous salt. 8) Allow the crucible to cool for two minutes. Immediately find the mass of the crucible plus the anhydrous salt using a tong. Record the mass in the dana section. The erucible must be weight before it neabsorbs water from the atmosphere. 9) When you have finished weighing the crucible and sall, place the erucible back on the counter top and squirt sone water onto it. Record any change in appearince in the Data section. 10) When you have finished, the anhydrous salt can be thrown into the waste container, and wash the crucible. Report Sheet Show all calculation and take note of significant figures. CiSO2xH2O Mass of crucible, 26. 6.11g Mass of erucible and CuSOxH2O hydrate salt ..2.8. .11....g Mass of CuSO4,xH2O..2.....g Appearance and color of CuSO4H2O... Blue sobid powaler Mass of crucible and CuSO4 anhydrous...2.7.48 8.8 Mass of CuSO4 anhydrous..... 1,37 Mass of water lost..... 6.3.......s Moles of CuSO4 anhydrous. mol Moles of water lost. mol Formula of hydrate. Appearance before addition of water. vercy pale ble pe poucler sub.Stance (Gimost white Appearance after addition of water...Turns blok color Calculations: the Same Remember to show all of your work 1. Find the percent of water lost from the original hydrate (remember that percentage is "the part divided by the whole, multiplied by 1007 ?). %hydrate=massoftydratesaltmassofwateriost100%28.11.63100% 2. Calculate the mass of water lost from the hydrate 5. Calculate the ratio of the mole of water lost to the mole of anhydrocas saly. 6. Formula of the hydrate: liscussion and Conclusion: 1) Explain why the mass of the sample decreased after it was heated, despite the law of conservation of mass. 2) Why do you have to ealculate the mole of water and salt in this lab? 3) Analyze the percent of water in your-sample and compare it with the theoretical value which is 36.0%. What conclusion can you draw with this difference of % hydrate