How to calculate moles of Cu in CuSO4*5H2O?
Q. I have 2g of CuSO4*5H2O. How do I calculate how many moles of Cu that I have?
Asked by Dyproti - Sun Jun 14 20:21:12 2009 - - 1 Answers - 0 Comments
Q. I have 2g of CuSO4*5H2O. How do I calculate how many moles of Cu that I have?
Asked by Dyproti - Sun Jun 14 20:21:12 2009 - - 1 Answers - 0 Comments
How do you write the equation when you heat CuSO4 * 5H2O ???
Q. How do your write the chemical equation when you heat CuSO4 * 5H2O??? What type of reaction is it? Is it a decomposition reaction???
Asked by sexy_chick_California - Tue Sep 19 14:28:28 2006 - - 1 Answers - 0 Comments
A. CuSO4*5H20 ---t ---> CuSO4 + 5*H2O It's a physical reaction and not a decomposition reaction. the hydrate loses the water.
Answered by andreicnx - Tue Sep 19 14:33:33 2006
Q. How do your write the chemical equation when you heat CuSO4 * 5H2O??? What type of reaction is it? Is it a decomposition reaction???
Asked by sexy_chick_California - Tue Sep 19 14:28:28 2006 - - 1 Answers - 0 Comments
A. CuSO4*5H20 ---t ---> CuSO4 + 5*H2O It's a physical reaction and not a decomposition reaction. the hydrate loses the water.
Answered by andreicnx - Tue Sep 19 14:33:33 2006
How do I found the number of moles in 35 g of CuSO4 X 5H2O?
Q. How do I find the number of moles in a compound like in the question? How do I find the number of moles in something that is attached with an H2O molecule? How do I convert back to grams like 3.2 moles of CuSO4 X 5H2O?
Asked by Gug N - Mon Oct 27 19:00:38 2008 - - 1 Answers - 0 Comments
A. 35g CuSO4x5H2O x (1mole/250 g) = 0.14 moles CuSO4x5H2O Use the number of moles of CuSO4 in CuSO4x 5H2O. So it's 1 mole:1 mole. :)
Answered by kookiekim77 - Tue Oct 28 01:01:01 2008
Q. How do I find the number of moles in a compound like in the question? How do I find the number of moles in something that is attached with an H2O molecule? How do I convert back to grams like 3.2 moles of CuSO4 X 5H2O?
Asked by Gug N - Mon Oct 27 19:00:38 2008 - - 1 Answers - 0 Comments
A. 35g CuSO4x5H2O x (1mole/250 g) = 0.14 moles CuSO4x5H2O Use the number of moles of CuSO4 in CuSO4x 5H2O. So it's 1 mole:1 mole. :)
Answered by kookiekim77 - Tue Oct 28 01:01:01 2008
Why does CuSO4.5H2O change color from blue to White when the water molecules are separated by heating?
Q. Does it have to do anything with the last orbital?
Asked by khalid_parvoni - Sun May 4 15:50:50 2008 - - 1 Answers - 0 Comments
A. No, it has to do with making it anhydrous (free from water). Basically, the current formula states that for each CuSO4 molecule there are 5 H2O molecules surrounding it (they are not covalently bonded to the CuSO4). When water is removed via heating, you're left with pure, crystallized CuSO4.
Answered by DesertFox OIC - Sun May 4 16:06:02 2008
Q. Does it have to do anything with the last orbital?
Asked by khalid_parvoni - Sun May 4 15:50:50 2008 - - 1 Answers - 0 Comments
A. No, it has to do with making it anhydrous (free from water). Basically, the current formula states that for each CuSO4 molecule there are 5 H2O molecules surrounding it (they are not covalently bonded to the CuSO4). When water is removed via heating, you're left with pure, crystallized CuSO4.
Answered by DesertFox OIC - Sun May 4 16:06:02 2008
hydrated copper sulphate CuSO4. 5H2O weighs 50g. How many moles of water molecules does it contain?
Q. hydrated copper sulphate CuSO4. 5H2O weighs 50g. How many moles of water molecules does it contain?
Asked by Cat S - Sat Nov 1 09:57:36 2008 - - 1 Answers - 0 Comments
A. molar mass CuSO4 = 143.612 g/mol molar mass CuSO4 *5H2O = 143.612 + ( 5 x 18.02)= 233.712 g/mol Moles CuSO4 * 5H2O = 50 g / 233.712 g/mol = 0.214 moles water = 5 x 0.214 = 1.07
Answered by Dr.A - Sat Nov 1 10:04:39 2008
Q. hydrated copper sulphate CuSO4. 5H2O weighs 50g. How many moles of water molecules does it contain?
Asked by Cat S - Sat Nov 1 09:57:36 2008 - - 1 Answers - 0 Comments
A. molar mass CuSO4 = 143.612 g/mol molar mass CuSO4 *5H2O = 143.612 + ( 5 x 18.02)= 233.712 g/mol Moles CuSO4 * 5H2O = 50 g / 233.712 g/mol = 0.214 moles water = 5 x 0.214 = 1.07
Answered by Dr.A - Sat Nov 1 10:04:39 2008
how do you prepare a 100mL solution w/ a molar concentration of 0.5 mol/L using CuSO4 5H2O ?
Q. what are the kinds of calculations required? and how can you calculate it? Also, how can you calculate the same thing (100 mL of solution using copper (II) sulfate pentahydrate) but with a molar concentration of 0.200 mol/L by dilution? This is for a grade 11 chemistry course, thanks for any help you can provide.
Asked by Mikal - Mon Dec 3 16:22:27 2007 - - 1 Answers - 0 Comments
A. This is a simple conversion problem. -Find the mass of copper (II) sulfate pentahydrate (249.75 g/mol) -Now, use the information you have to find the mass of the copper sulfate that you need. (.5mol/1L) * .1L solution = .05 mol copper sulfate 0.05 mol * (249.75 g/mol) = 12.49g copper sulfate So, the answer to the first part of your question is: add 12.49g copper sulfate pentahydrate to 100mL water. For the next part, use the equation M1V1=M2V2 (M is molarity in mols/liter, V is volume) So... 0.5M * V1 = 0.2M * 0.1 L V1=0.04 L (40 mL) The answer to the second part would be to add 40 mL of the .5M solution and 60 mL water. Good luck in your class.
Answered by David R - Mon Dec 3 16:35:17 2007
Q. what are the kinds of calculations required? and how can you calculate it? Also, how can you calculate the same thing (100 mL of solution using copper (II) sulfate pentahydrate) but with a molar concentration of 0.200 mol/L by dilution? This is for a grade 11 chemistry course, thanks for any help you can provide.
Asked by Mikal - Mon Dec 3 16:22:27 2007 - - 1 Answers - 0 Comments
A. This is a simple conversion problem. -Find the mass of copper (II) sulfate pentahydrate (249.75 g/mol) -Now, use the information you have to find the mass of the copper sulfate that you need. (.5mol/1L) * .1L solution = .05 mol copper sulfate 0.05 mol * (249.75 g/mol) = 12.49g copper sulfate So, the answer to the first part of your question is: add 12.49g copper sulfate pentahydrate to 100mL water. For the next part, use the equation M1V1=M2V2 (M is molarity in mols/liter, V is volume) So... 0.5M * V1 = 0.2M * 0.1 L V1=0.04 L (40 mL) The answer to the second part would be to add 40 mL of the .5M solution and 60 mL water. Good luck in your class.
Answered by David R - Mon Dec 3 16:35:17 2007
What is the mass percentage of water in the hydrate CuSO4 5H2O?
Q. What is the mass percentage of water in the hydrate CuSO4 5H2O?
Asked by Drums12 - Tue Aug 25 20:29:12 2009 - - 1 Answers - 0 Comments
A. FW (formula weight) of 5 H2O = 90.076 g/mol FW of hydrate = 249.685 g/mol % (mass/mass) of water in hydrate = (FW 5 H2O / FW of hydrate) x 100 = (90.076 g/mol / 249.685 g/mol) x 100 = 36.07586 % *** Answer: 36.1 % *** (at 3 sig. figs.)
Answered by MyAnswerIs - Wed Aug 26 15:17:32 2009
Q. What is the mass percentage of water in the hydrate CuSO4 5H2O?
Asked by Drums12 - Tue Aug 25 20:29:12 2009 - - 1 Answers - 0 Comments
A. FW (formula weight) of 5 H2O = 90.076 g/mol FW of hydrate = 249.685 g/mol % (mass/mass) of water in hydrate = (FW 5 H2O / FW of hydrate) x 100 = (90.076 g/mol / 249.685 g/mol) x 100 = 36.07586 % *** Answer: 36.1 % *** (at 3 sig. figs.)
Answered by MyAnswerIs - Wed Aug 26 15:17:32 2009
How does CuSo4.5H2o differ from CuSo4?
Q. My experiment calls for CuSo4, but I have been unable to locate it with just that formula How does CuSO4.5H2O differ from CuSO4? If I knew how it differs I could determine if it will work for me. Thanks, Back Porch Willie
Asked by Back Porch Willy - Tue Jul 15 22:54:58 2008 - - 2 Answers - 0 Comments
A. CuSO4 * 5H2O is a hydrate. A hydrate is a compound with several water molecules attached to it. CuSO4*5H2O has 5 water molecules attached to it. A compound with no water molecules attached to it is called anhydrate.
Answered by tsangalfred - Tue Jul 15 23:08:43 2008
Q. My experiment calls for CuSo4, but I have been unable to locate it with just that formula How does CuSO4.5H2O differ from CuSO4? If I knew how it differs I could determine if it will work for me. Thanks, Back Porch Willie
Asked by Back Porch Willy - Tue Jul 15 22:54:58 2008 - - 2 Answers - 0 Comments
A. CuSO4 * 5H2O is a hydrate. A hydrate is a compound with several water molecules attached to it. CuSO4*5H2O has 5 water molecules attached to it. A compound with no water molecules attached to it is called anhydrate.
Answered by tsangalfred - Tue Jul 15 23:08:43 2008
What is the amount of mol of: H2O molecules in 20.0g of CuSO4.5H2O?
Q. I need help with the working out. the answer is 0.401 mol thank Chong J =D. best answer, i would rate you but then i am unable to vote yet. hehe thanks Chong J =D. best answer, i would rate you but then i am unable to vote yet. hehe
Asked by Cookiie_ - Sat Jan 17 09:15:04 2009 - - 3 Answers - 0 Comments
A. 1 mole of CuSO4.5H2O=63.5+32+(4*16) +(5*(2*1+16))= 249.5g x mole of CuSO4.5H2O= 20 g X =20/249.5=0.08 mole since 1 mole of CuSO4.5H2O cotains 5 mole of H2O then 0.08 mole of CuSO4.5H2O contains Y mole of H2O Y = 5*0.08/1=0.4 mole of H2O
Answered by vertigo - Sat Jan 17 09:39:49 2009
Q. I need help with the working out. the answer is 0.401 mol thank Chong J =D. best answer, i would rate you but then i am unable to vote yet. hehe thanks Chong J =D. best answer, i would rate you but then i am unable to vote yet. hehe
Asked by Cookiie_ - Sat Jan 17 09:15:04 2009 - - 3 Answers - 0 Comments
A. 1 mole of CuSO4.5H2O=63.5+32+(4*16) +(5*(2*1+16))= 249.5g x mole of CuSO4.5H2O= 20 g X =20/249.5=0.08 mole since 1 mole of CuSO4.5H2O cotains 5 mole of H2O then 0.08 mole of CuSO4.5H2O contains Y mole of H2O Y = 5*0.08/1=0.4 mole of H2O
Answered by vertigo - Sat Jan 17 09:39:49 2009
How many grams of CuSO4*5H2O are needed to prepare 50 mL, .3M CuSO4 solution?
Q. the 5 H2O at the end is throwing me off, do i ignore it when doing the calculation or do i include its molar mass in that of the copper sulfate?
Asked by jav_7792 - Sun Oct 21 17:24:45 2007 - - 1 Answers - 0 Comments
A. the 5 H2O is to calculated in the molar mass as it part of the compound. Molar mass of H2) is 18.02 Molar Mass CuSO4*5H2O Cu 63.55 gmol-1 S 32.07 gmol-1 O4 4(16.00) =64.00 gmol-1 5 H2O 5(18.02) = 90.08 gmol-1 total Molar Mass CuSO4*5H2O is 249.70 gmol-1 #moles = M x V x =0.3 M x 0.05 L x = 0.015 moles CuSO4*5H2O Mass = moles x Molar Mass Mass = 0.015 moles x 249.70 gmol-1 mass = 3.74 g CuSO4*5H2O remember M is express as mol L-1 so volume should be in L (50 mL divided by 1000 gives 0.05 L (1L =1000 mL))
Answered by Penny M - Sun Oct 21 19:58:19 2007
Q. the 5 H2O at the end is throwing me off, do i ignore it when doing the calculation or do i include its molar mass in that of the copper sulfate?
Asked by jav_7792 - Sun Oct 21 17:24:45 2007 - - 1 Answers - 0 Comments
A. the 5 H2O is to calculated in the molar mass as it part of the compound. Molar mass of H2) is 18.02 Molar Mass CuSO4*5H2O Cu 63.55 gmol-1 S 32.07 gmol-1 O4 4(16.00) =64.00 gmol-1 5 H2O 5(18.02) = 90.08 gmol-1 total Molar Mass CuSO4*5H2O is 249.70 gmol-1 #moles = M x V x =0.3 M x 0.05 L x = 0.015 moles CuSO4*5H2O Mass = moles x Molar Mass Mass = 0.015 moles x 249.70 gmol-1 mass = 3.74 g CuSO4*5H2O remember M is express as mol L-1 so volume should be in L (50 mL divided by 1000 gives 0.05 L (1L =1000 mL))
Answered by Penny M - Sun Oct 21 19:58:19 2007
please help, how many grams of water would 3 g CuSo4 absorb in becoming CuSO4 5H2O?
Q. I tried doing this problem and I can't get it right. Please help if you can. I know CuSO4 has an atomic weight of 159 and that has something to do with the problem. Do you divide 159 (CuSO4) by 1 mole (6.022 times 10^23) then times that by 3 since there are three grams of CuSO4?
Asked by Sam - Tue Nov 21 18:59:20 2006 - - 1 Answers - 0 Comments
A. You bet the molecular weight of copper sulfate has something to do with the answer! If you divide the weight of the copper sulphate (3 grams) by the molecular weight you'll get the number of moles of copper sulfate present. The hydrated form has 5 moles of water for each mole of copper sulfate. So, the answer above times 5 gives the moles of water. Multiply this by the molecular weight of water and you'll have your answer.
Answered by Flyboy - Tue Nov 21 19:10:06 2006
Q. I tried doing this problem and I can't get it right. Please help if you can. I know CuSO4 has an atomic weight of 159 and that has something to do with the problem. Do you divide 159 (CuSO4) by 1 mole (6.022 times 10^23) then times that by 3 since there are three grams of CuSO4?
Asked by Sam - Tue Nov 21 18:59:20 2006 - - 1 Answers - 0 Comments
A. You bet the molecular weight of copper sulfate has something to do with the answer! If you divide the weight of the copper sulphate (3 grams) by the molecular weight you'll get the number of moles of copper sulfate present. The hydrated form has 5 moles of water for each mole of copper sulfate. So, the answer above times 5 gives the moles of water. Multiply this by the molecular weight of water and you'll have your answer.
Answered by Flyboy - Tue Nov 21 19:10:06 2006
What is the molar mass of CUSO4 * 5H2O? What is the percent composition of O in CUSO4 * 5H2O? HELP!!!?
Q. What is the molar mass of CUSO4 * 5H2O? What is the percent composition of O in CUSO4 * 5H2O???# help pleazzz???
Asked by LNLNLN - Sun Nov 2 06:46:48 2008 - - 2 Answers - 0 Comments
A. well to find molar mass just add all the RAM of each element in the compound. Cu= 64 S= 32 O= 16 H= 1 63.5+32+16*4+10+5*16 = 250 How many O's are in the compound? theres 9 so 9*16= 144 144/250*100= 57.6%
Answered by celinex - Sun Nov 2 08:22:09 2008
Q. What is the molar mass of CUSO4 * 5H2O? What is the percent composition of O in CUSO4 * 5H2O???# help pleazzz???
Asked by LNLNLN - Sun Nov 2 06:46:48 2008 - - 2 Answers - 0 Comments
A. well to find molar mass just add all the RAM of each element in the compound. Cu= 64 S= 32 O= 16 H= 1 63.5+32+16*4+10+5*16 = 250 How many O's are in the compound? theres 9 so 9*16= 144 144/250*100= 57.6%
Answered by celinex - Sun Nov 2 08:22:09 2008
Determine the percentage by mass of water in the hydrate CuSo4*5H2O?
Q. Determine the percentage by mass of water in the hydrate CuSo4*5H2O?
Asked by Bayern - Wed Dec 19 21:59:56 2007 - - 2 Answers - 1 Comments
A. First of all, it's CuSO4*5H2O (notice the capital "O" in the first part of the formula). The compound is called copper(II) sulfate pentahydrate, and if we wish to find the percent by mass of water, we need to find the molar mass of the hydrate first. Cu = 63.55 g/mol S = 32.07 g/mol O x 4 = 16.00 g/mol x 4 = 64.00 g/mol H2O x 5 = 18.02 g/mol x 5 = 90.10 g/mol Now add them all together and you get a molar mass of 249.72 g/mol Of that 249.72 grams, 90.10 grams is water, so to find the percentage by mass that is water, simply divide 90.10 g by 249.72 g and multiply the result by 100%: 90.10 g / 249.72 g x 100% = 36.08% water I hope that helps. Good luck!
Answered by Lucas C - Wed Dec 19 22:09:43 2007
Q. Determine the percentage by mass of water in the hydrate CuSo4*5H2O?
Asked by Bayern - Wed Dec 19 21:59:56 2007 - - 2 Answers - 1 Comments
A. First of all, it's CuSO4*5H2O (notice the capital "O" in the first part of the formula). The compound is called copper(II) sulfate pentahydrate, and if we wish to find the percent by mass of water, we need to find the molar mass of the hydrate first. Cu = 63.55 g/mol S = 32.07 g/mol O x 4 = 16.00 g/mol x 4 = 64.00 g/mol H2O x 5 = 18.02 g/mol x 5 = 90.10 g/mol Now add them all together and you get a molar mass of 249.72 g/mol Of that 249.72 grams, 90.10 grams is water, so to find the percentage by mass that is water, simply divide 90.10 g by 249.72 g and multiply the result by 100%: 90.10 g / 249.72 g x 100% = 36.08% water I hope that helps. Good luck!
Answered by Lucas C - Wed Dec 19 22:09:43 2007
What percentage of water is found in CuSO4 5H2O?
Q. What percentage of water is found in CuSO4 5H2O?
Asked by John X - Sun Nov 5 04:17:08 2006 - - 2 Answers - 0 Comments
A. Miss Science, you have all the facts but you missed out the most important one, which is that the percentage by mass of water in CuSO4.5H2O is always the same. the Mr of CuSO4 is 159.6 and that of 5 water molecules is 90.0. no matter what mass of hydrated copper(ii)sulphate, the masses of CuSO4 and H2O will always be in the ratio of 159.6:90.0 this means that the percentage mass of water would be 90/(90+159.6)x100% = 36.06%
Answered by Dr Greg - Sun Nov 5 06:22:44 2006
Q. What percentage of water is found in CuSO4 5H2O?
Asked by John X - Sun Nov 5 04:17:08 2006 - - 2 Answers - 0 Comments
A. Miss Science, you have all the facts but you missed out the most important one, which is that the percentage by mass of water in CuSO4.5H2O is always the same. the Mr of CuSO4 is 159.6 and that of 5 water molecules is 90.0. no matter what mass of hydrated copper(ii)sulphate, the masses of CuSO4 and H2O will always be in the ratio of 159.6:90.0 this means that the percentage mass of water would be 90/(90+159.6)x100% = 36.06%
Answered by Dr Greg - Sun Nov 5 06:22:44 2006
What mass of bluestone, CuSO4.5H2O would contain 175 g of water?
Q. I know the answer is 4.85 x 10 exp.2 g. I don't know what formula to use to arrive at that. Could someone please help me?
Asked by scarletxvi - Sun Nov 8 12:51:34 2009 - - 1 Answers - 0 Comments
A. Moles water = 175 g/ 18 g/mol= 9.72 the ratio between CuSO4 and H2O is 1 : 5 moles CuSO4 = 9.72 x 1 /5=1.94 molar mass CuSO4 = 159.61 g/mol mass CuSO4 = 159.61 g/mol x 1.94 mol= 310 g total mass = 310 + 175 = 485 g => 4.85 x 10^2 g
Answered by Dr.A - Sun Nov 8 12:59:02 2009
Q. I know the answer is 4.85 x 10 exp.2 g. I don't know what formula to use to arrive at that. Could someone please help me?
Asked by scarletxvi - Sun Nov 8 12:51:34 2009 - - 1 Answers - 0 Comments
A. Moles water = 175 g/ 18 g/mol= 9.72 the ratio between CuSO4 and H2O is 1 : 5 moles CuSO4 = 9.72 x 1 /5=1.94 molar mass CuSO4 = 159.61 g/mol mass CuSO4 = 159.61 g/mol x 1.94 mol= 310 g total mass = 310 + 175 = 485 g => 4.85 x 10^2 g
Answered by Dr.A - Sun Nov 8 12:59:02 2009
What mass of Cu(IO3)2 can be formed from 0.500g of CuSO4-5H2O?
Q. What mass of Cu(IO3)2 can be formed from 0.500g of CuSO4-5H2O?
Asked by Steve M - Wed Oct 15 23:45:59 2008 - - 1 Answers - 0 Comments
A. First we need to figure out what is the limiting reagent. Since it is not given lets assume it is CuSO4-5H2O. Now we need to find a formula for this reaction, the most simple reaction is the following: CuSO4.5H2O + 2HIO3 --> Cu(IO3)2 + H2SO4 + 5H2O If we assume the reaction goes to completion every mole of CuSO4-5H2O will result in one mole Cu(IO3)2 (1:1 reaction). So now we calculate the number of moles of CuSO4-5H2O there are in 0.500g. For this we divide the given mass by the sum of the atomic weight of all the components of the molecule. These are the weights I'll use (out of wikipedia) I'll use 3 decimal places. Cu --> 63.546 S --> 32.065 O --> 15.9994 ~ 15.999 H --> 1.00794 ~ 1.010 I --> 126.90447 ~ 126.904 For CuSO4-5H2O… [cont.]
Answered by Diego S - Thu Oct 16 03:37:52 2008
Q. What mass of Cu(IO3)2 can be formed from 0.500g of CuSO4-5H2O?
Asked by Steve M - Wed Oct 15 23:45:59 2008 - - 1 Answers - 0 Comments
A. First we need to figure out what is the limiting reagent. Since it is not given lets assume it is CuSO4-5H2O. Now we need to find a formula for this reaction, the most simple reaction is the following: CuSO4.5H2O + 2HIO3 --> Cu(IO3)2 + H2SO4 + 5H2O If we assume the reaction goes to completion every mole of CuSO4-5H2O will result in one mole Cu(IO3)2 (1:1 reaction). So now we calculate the number of moles of CuSO4-5H2O there are in 0.500g. For this we divide the given mass by the sum of the atomic weight of all the components of the molecule. These are the weights I'll use (out of wikipedia) I'll use 3 decimal places. Cu --> 63.546 S --> 32.065 O --> 15.9994 ~ 15.999 H --> 1.00794 ~ 1.010 I --> 126.90447 ~ 126.904 For CuSO4-5H2O… [cont.]
Answered by Diego S - Thu Oct 16 03:37:52 2008
Explain and discuss the reaction of :CuSO4 oH20 and CuSO4 5H2O?
Q. Explain and discuss the reaction of :CuSO4 oH20 and CuSO4 5H2O? What is the delta H? What is the q=.What is the mass values? Table 1.1: title Given:0.783 M CuSO4 10g M1 H2O80mL Ti22.20 C Tf32.60 C T10.4 C H= (q / # moles)(-435.24) / (0.0626)= -6952.7g Q= -mass x (4.184 J K-1g-1) T ( -10g)(4.184 J K-1g-1 )( 283 K) = Table 1.2: title Given:0.5 M CuSO4 5H20 10g M1 H2O80mL Ti22.85 C Tf21.40 C T-1.45 C H= (q / # moles)(60.7) / (0.0400)= 1516.7 Q= -mass x (4.184 J K-1g-1) T ( -10g)(4.184 J K-1g-1 )( 271.55K ) = Table 1.3: title Given:0.626 M CuSO4 5g M1 H2O50mL Ti-22.40 C Tf-34.40 C T12.0 C H= (q / # moles)(-251.0) / (0.0313)= 1516.7 Q= -mass x (4.184 J K-1g-1) T ( -5g)(4.184 J K-1g-1 )( 285K ) = Table 1.4: title… [cont.]
Asked by Gabriel Z - Tue Jun 19 12:24:17 2007 - - 1 Answers - 0 Comments
A. Discuss ??? This is an experimental problem. Do the experiment first !!!
Answered by ag_iitkgp - Tue Jun 19 12:34:24 2007
Q. Explain and discuss the reaction of :CuSO4 oH20 and CuSO4 5H2O? What is the delta H? What is the q=.What is the mass values? Table 1.1: title Given:0.783 M CuSO4 10g M1 H2O80mL Ti22.20 C Tf32.60 C T10.4 C H= (q / # moles)(-435.24) / (0.0626)= -6952.7g Q= -mass x (4.184 J K-1g-1) T ( -10g)(4.184 J K-1g-1 )( 283 K) = Table 1.2: title Given:0.5 M CuSO4 5H20 10g M1 H2O80mL Ti22.85 C Tf21.40 C T-1.45 C H= (q / # moles)(60.7) / (0.0400)= 1516.7 Q= -mass x (4.184 J K-1g-1) T ( -10g)(4.184 J K-1g-1 )( 271.55K ) = Table 1.3: title Given:0.626 M CuSO4 5g M1 H2O50mL Ti-22.40 C Tf-34.40 C T12.0 C H= (q / # moles)(-251.0) / (0.0313)= 1516.7 Q= -mass x (4.184 J K-1g-1) T ( -5g)(4.184 J K-1g-1 )( 285K ) = Table 1.4: title… [cont.]
Asked by Gabriel Z - Tue Jun 19 12:24:17 2007 - - 1 Answers - 0 Comments
A. Discuss ??? This is an experimental problem. Do the experiment first !!!
Answered by ag_iitkgp - Tue Jun 19 12:34:24 2007
Finding the percentage of water in CuSO4 5H2O?
Q. i have a chemistry teacher that wants us to think of a few ways to find the percentage of water in copper(II) sulfate pentahydrate in a lab experiment what are other ways besides using evaporation to do so...i have been working on this for a few hours and only can think of using evaporation... and we cant just do the math for it ...it has to be in a lab
Asked by jbfan223 - Fri Nov 28 18:33:06 2008 - - 1 Answers - 0 Comments
A. 1. Karl Fischer titration...look it up in wiki...measures water content directly. 2. Measure Cu content... eg by precipitation of CuS via H2S, weighing the washed/dried ppt, and back-calculating to find H2O content. 3. Measure SO4 content...eg by ppting out BaSO4 via a soluble barium salt, then working up as above. ADDED For KF titration see Plug Karl Fischer into search box.
Answered by L. A. L. - Fri Nov 28 19:02:43 2008
Q. i have a chemistry teacher that wants us to think of a few ways to find the percentage of water in copper(II) sulfate pentahydrate in a lab experiment what are other ways besides using evaporation to do so...i have been working on this for a few hours and only can think of using evaporation... and we cant just do the math for it ...it has to be in a lab
Asked by jbfan223 - Fri Nov 28 18:33:06 2008 - - 1 Answers - 0 Comments
A. 1. Karl Fischer titration...look it up in wiki...measures water content directly. 2. Measure Cu content... eg by precipitation of CuS via H2S, weighing the washed/dried ppt, and back-calculating to find H2O content. 3. Measure SO4 content...eg by ppting out BaSO4 via a soluble barium salt, then working up as above. ADDED For KF titration see Plug Karl Fischer into search box.
Answered by L. A. L. - Fri Nov 28 19:02:43 2008
CuSO4 to CuSO4.5H2O?
Q. CuSO4 + H2O --> CuSO4.5H2O When water is added to the CuSO4 WHY does it form blue crystals?? ...but why does it from crystal when the water is added? cuso4 is a powder substance
Asked by sweetflower - Sun Apr 15 08:38:17 2007 - - 2 Answers - 0 Comments
A. Hey, The reaction is that a reactive metal + water -> metal hydroxide + hydrogen gas. This also applies to your equation. Since copper is a transition metal, its compounds are coloured, with copper being blue, thus forming blue crystals. Another example is copper(II) hydroxide which is also blue. I hope this answers your answer. ^.^ --- *New part... It forms crystals cause the method you're doing is preparation of salts and its called neutralization as the copper sulphate is soluble in water. So crystalisation - where crystals are formed - occurs as **when you saturate the solution, there's too much salt but too little solution, thus the salts form as the solution cant hold it anymore**
Answered by Zaki M - Sun Apr 15 09:09:12 2007
Q. CuSO4 + H2O --> CuSO4.5H2O When water is added to the CuSO4 WHY does it form blue crystals?? ...but why does it from crystal when the water is added? cuso4 is a powder substance
Asked by sweetflower - Sun Apr 15 08:38:17 2007 - - 2 Answers - 0 Comments
A. Hey, The reaction is that a reactive metal + water -> metal hydroxide + hydrogen gas. This also applies to your equation. Since copper is a transition metal, its compounds are coloured, with copper being blue, thus forming blue crystals. Another example is copper(II) hydroxide which is also blue. I hope this answers your answer. ^.^ --- *New part... It forms crystals cause the method you're doing is preparation of salts and its called neutralization as the copper sulphate is soluble in water. So crystalisation - where crystals are formed - occurs as **when you saturate the solution, there's too much salt but too little solution, thus the salts form as the solution cant hold it anymore**
Answered by Zaki M - Sun Apr 15 09:09:12 2007
Calculate the theoretical % by mass of water in CuSO4*5H2O?
Q. Calculate the theoretical % by mass of water in CuSO4*5H2O?
Asked by criki964 - Thu Jun 1 01:27:53 2006 - - 2 Answers - 0 Comments
A. First of all work out the molar mass of CuSO4*5H2O Cu + S + (9 * O) * (10 * H) Sorry I don't have a chemical table next to me Call this A Secondary work out the mass of 5 moles of water. Call this B (5 * O) + (10 * H) the theoretical % is then B/A * 100 = x%
Answered by unknown - Thu Jun 1 01:33:05 2006
Q. Calculate the theoretical % by mass of water in CuSO4*5H2O?
Asked by criki964 - Thu Jun 1 01:27:53 2006 - - 2 Answers - 0 Comments
A. First of all work out the molar mass of CuSO4*5H2O Cu + S + (9 * O) * (10 * H) Sorry I don't have a chemical table next to me Call this A Secondary work out the mass of 5 moles of water. Call this B (5 * O) + (10 * H) the theoretical % is then B/A * 100 = x%
Answered by unknown - Thu Jun 1 01:33:05 2006
From Yahoo Answer Search: 'CuSo4 5H2O'
Sun Nov 22 13:02:02 2009 [ refresh local cache ]
