How do you figure out that say potassium phosphate= K3PO4? or barium chloride is BaCl2? ?
Q. How do you figure out the number of the individual atoms?
Asked by erik - Mon Oct 13 18:29:11 2008 - - 1 Answers - 0 Comments
A. because barium has a charge of +2 and chloride has a charge of -1. so to balance out the molecule, you have to have 1 barium and 2 chlorides. its the same thing for the potassium phosphate. the potassium has a charge of +1 i think and phosphate has a charge of -3 since theres 3 potassiums.
Answered by Diane L - Mon Oct 13 18:36:20 2008
Q. How do you figure out the number of the individual atoms?
Asked by erik - Mon Oct 13 18:29:11 2008 - - 1 Answers - 0 Comments
A. because barium has a charge of +2 and chloride has a charge of -1. so to balance out the molecule, you have to have 1 barium and 2 chlorides. its the same thing for the potassium phosphate. the potassium has a charge of +1 i think and phosphate has a charge of -3 since theres 3 potassiums.
Answered by Diane L - Mon Oct 13 18:36:20 2008
Write a net ionic equation for the precipitation reaction resulting from mixing a BaCl2 sol. with a K2SO4 sol?
Q. Write a net ionic equation for the precipitation reaction resulting from mixing a BaCl2 solution with a K2SO4 solution... i do not know how to make the numbers smaller so i just put them the way they are.
Asked by Jared S - Thu Nov 15 15:18:24 2007 - - 1 Answers - 0 Comments
A. Molecular : BaCl2 (aq) + K2SO4 (aq) >> BaSO4 (s) + 2 KCl (aq) Ionic : Ba2+ + 2Cl- + 2K+ + SO42- >> BaSO4 + 2Cl- + 2 K+ Net ionic : Ba2+ + SO42- >> BaSO4 (s)
Answered by Dr.A - Thu Nov 15 15:22:47 2007
Q. Write a net ionic equation for the precipitation reaction resulting from mixing a BaCl2 solution with a K2SO4 solution... i do not know how to make the numbers smaller so i just put them the way they are.
Asked by Jared S - Thu Nov 15 15:18:24 2007 - - 1 Answers - 0 Comments
A. Molecular : BaCl2 (aq) + K2SO4 (aq) >> BaSO4 (s) + 2 KCl (aq) Ionic : Ba2+ + 2Cl- + 2K+ + SO42- >> BaSO4 + 2Cl- + 2 K+ Net ionic : Ba2+ + SO42- >> BaSO4 (s)
Answered by Dr.A - Thu Nov 15 15:22:47 2007
What are the spectator ions when BaCl2 combines with H2SO4?
Q. How do you figure this out? When you are given two compounds like that how would you even determine what the ions are? Struggling with chemistry.. thanks for the help!
Asked by sunrisesover12th - Thu Jun 12 10:32:10 2008 - - 1 Answers - 0 Comments
A. Both the substances are strong electrolytes, fully dissociated (near enough for introductory chemistry) into their separate ions. So you actually have Ba2+, Cl-, H+(aq) and SO4 2-. Overall equation: BaCl2 + H2SO4 = BaSO4(s) + 2 HCl (s means solid precipitate) Write out the ions actually present: Ba2+ + 2Cl- + 2H+ + SO4 2- = BaSO4(s) + 2H+ + 2Cl- The chloride and hydrogen ions are unchanged by the reaction, so they are spectators. BaSO4 is a salt, containing ions, but these are no longer moving freely in solution. So the net ionic equation, which shows you what is really happening, is simply Ba2+ + SO4 2- = BaSO4 Hope this helps.
Answered by Paul B - Thu Jun 12 10:40:53 2008
Q. How do you figure this out? When you are given two compounds like that how would you even determine what the ions are? Struggling with chemistry.. thanks for the help!
Asked by sunrisesover12th - Thu Jun 12 10:32:10 2008 - - 1 Answers - 0 Comments
A. Both the substances are strong electrolytes, fully dissociated (near enough for introductory chemistry) into their separate ions. So you actually have Ba2+, Cl-, H+(aq) and SO4 2-. Overall equation: BaCl2 + H2SO4 = BaSO4(s) + 2 HCl (s means solid precipitate) Write out the ions actually present: Ba2+ + 2Cl- + 2H+ + SO4 2- = BaSO4(s) + 2H+ + 2Cl- The chloride and hydrogen ions are unchanged by the reaction, so they are spectators. BaSO4 is a salt, containing ions, but these are no longer moving freely in solution. So the net ionic equation, which shows you what is really happening, is simply Ba2+ + SO4 2- = BaSO4 Hope this helps.
Answered by Paul B - Thu Jun 12 10:40:53 2008
How do I prepare a solution of BaCl2 from BaCl2-H2O?
Q. I need to prepare 2 litres of 0.108M BaCl I need to prepare 2 litres of 0.108M BaCl2
Asked by Karz - Tue Apr 22 09:28:23 2008 - - 1 Answers - 0 Comments
A. It doesn't matter that it's the hydrate when you prepare the solution! Since BaCl2 2H2O(s) + H2O(l) --> BaCl2(aq) 1 mole BaCl2 2H2O will give 1 mole BaCl2 BaCl2 2H2O MW = 244.264 g/mole you need 2 L of 0.108 M 0.108 M = .108 mole/L 0.108 moles = 0.108 mole * 244.264 g/mole = 26.4 g Take 52.8 g of the hydrate and dissolve it in 2 Liter of water and you will have 2 L of 0.018 M BaCl2
Answered by Dr Dave P - Tue Apr 22 09:41:35 2008
Q. I need to prepare 2 litres of 0.108M BaCl I need to prepare 2 litres of 0.108M BaCl2
Asked by Karz - Tue Apr 22 09:28:23 2008 - - 1 Answers - 0 Comments
A. It doesn't matter that it's the hydrate when you prepare the solution! Since BaCl2 2H2O(s) + H2O(l) --> BaCl2(aq) 1 mole BaCl2 2H2O will give 1 mole BaCl2 BaCl2 2H2O MW = 244.264 g/mole you need 2 L of 0.108 M 0.108 M = .108 mole/L 0.108 moles = 0.108 mole * 244.264 g/mole = 26.4 g Take 52.8 g of the hydrate and dissolve it in 2 Liter of water and you will have 2 L of 0.018 M BaCl2
Answered by Dr Dave P - Tue Apr 22 09:41:35 2008
How do I calculate the number of mL of 0.2 M BaCl2 that will be needed to carry out?
Q. a complete precipitation of .300 grams of barium sulfate? Afterwards, how do you calculate the percent yield of sodium sulfate recovered?
Asked by Mack O - Sat Feb 28 09:09:23 2009 - - 1 Answers - 0 Comments
A. moles BaSO4 = 0.300 g /233.43 g/mol=0.00129 BaCl2 + SO42- >> BaSO4(s) + 2 Cl- moles BaCl2 needed = 0.00129 V = 0.00129 / 0.2 M =0.00695 L =>>6.95 mL
Answered by Dr.A - Sat Feb 28 09:27:21 2009
Q. a complete precipitation of .300 grams of barium sulfate? Afterwards, how do you calculate the percent yield of sodium sulfate recovered?
Asked by Mack O - Sat Feb 28 09:09:23 2009 - - 1 Answers - 0 Comments
A. moles BaSO4 = 0.300 g /233.43 g/mol=0.00129 BaCl2 + SO42- >> BaSO4(s) + 2 Cl- moles BaCl2 needed = 0.00129 V = 0.00129 / 0.2 M =0.00695 L =>>6.95 mL
Answered by Dr.A - Sat Feb 28 09:27:21 2009
What would be observed in the redox reaction between BaCl2 solution and dilute H2SO4?
Q. What would be observed in the redox reaction between BaCl2 solution and dilute H2SO4?
Asked by ka - Wed Mar 11 11:38:40 2009 - - 2 Answers - 0 Comments
A. HCl will be formed, and a white precipitate of BaSO4 will be produced.
Answered by time.travel - Thu Mar 12 06:30:02 2009
Q. What would be observed in the redox reaction between BaCl2 solution and dilute H2SO4?
Asked by ka - Wed Mar 11 11:38:40 2009 - - 2 Answers - 0 Comments
A. HCl will be formed, and a white precipitate of BaSO4 will be produced.
Answered by time.travel - Thu Mar 12 06:30:02 2009
What is the ion concentration in a 0.12 M solution of BaCl2?
Q. So, what are the molarities of Ba+2 and Cl-1?
Asked by some teenager - Wed Sep 24 19:27:07 2008 - - 1 Answers - 0 Comments
A. Hint: The subscript 2 tells you something about the concentration of the Cl ion compared to the barium.
Answered by paul1 - Wed Sep 24 19:34:36 2008
Q. So, what are the molarities of Ba+2 and Cl-1?
Asked by some teenager - Wed Sep 24 19:27:07 2008 - - 1 Answers - 0 Comments
A. Hint: The subscript 2 tells you something about the concentration of the Cl ion compared to the barium.
Answered by paul1 - Wed Sep 24 19:34:36 2008
why are NaCl, BaCl2 and CrCl3 chloride fomulas different?
Q. why are NaCl, BaCl2 and CrCl3 chloride fomulas different?
Asked by hussain h - Mon Dec 10 18:23:08 2007 - - 2 Answers - 0 Comments
A. That's easy. Because NaCl (sodium chloride), BaCl2 (barium dichloride) and CrCl3 (chromium trichloride) are different compounds. The formula just tells you what the compound is made of. NaCl has one sodium atom ionically bonded with one chlorine atom. BaCl2 has one barium atom ionically bonded to two chlorine atoms. That's all I have to say about that.
Answered by alex l - Mon Dec 10 18:38:56 2007
Q. why are NaCl, BaCl2 and CrCl3 chloride fomulas different?
Asked by hussain h - Mon Dec 10 18:23:08 2007 - - 2 Answers - 0 Comments
A. That's easy. Because NaCl (sodium chloride), BaCl2 (barium dichloride) and CrCl3 (chromium trichloride) are different compounds. The formula just tells you what the compound is made of. NaCl has one sodium atom ionically bonded with one chlorine atom. BaCl2 has one barium atom ionically bonded to two chlorine atoms. That's all I have to say about that.
Answered by alex l - Mon Dec 10 18:38:56 2007
You want to prepare barium chloride, BaCl2, using an exchange reaction of some type. To do so...?
Q. You want to prepare barium chloride, BaCl2, using an exchange reaction of some type. To do so you have the following reagents from which to select reactants: BaSO4, BaBr2, BaCO3, Ba(OH)2, HCl, HgSO4, AgNO3, and HNO3. Write a complete, balanced equation for the reaction chosen. (There are several possibilities)
Asked by beeboroachgoingon197 - Mon Oct 1 04:47:54 2007 - - 1 Answers - 0 Comments
A. I would, personally use Ba(OH)2 and HCl. Since the ending formula is BaCl2, you need to balance out your equation on the left side, so place a 2 in front of the HCl, to balance the number of Cl's on each side. This is a simple acid base reaction and when those occur an Acid and a Base form a salt and water. In general: Ba(OH)2+HCl ---> BaCl2 H2O Balanced we get: Ba(OH)2+2HCl ---> BaCl2+H2O
Answered by Another 2 Cents - Mon Oct 1 05:06:56 2007
Q. You want to prepare barium chloride, BaCl2, using an exchange reaction of some type. To do so you have the following reagents from which to select reactants: BaSO4, BaBr2, BaCO3, Ba(OH)2, HCl, HgSO4, AgNO3, and HNO3. Write a complete, balanced equation for the reaction chosen. (There are several possibilities)
Asked by beeboroachgoingon197 - Mon Oct 1 04:47:54 2007 - - 1 Answers - 0 Comments
A. I would, personally use Ba(OH)2 and HCl. Since the ending formula is BaCl2, you need to balance out your equation on the left side, so place a 2 in front of the HCl, to balance the number of Cl's on each side. This is a simple acid base reaction and when those occur an Acid and a Base form a salt and water. In general: Ba(OH)2+HCl ---> BaCl2 H2O Balanced we get: Ba(OH)2+2HCl ---> BaCl2+H2O
Answered by Another 2 Cents - Mon Oct 1 05:06:56 2007
What is the net Ionic and Complete Ionica equation for NaSO4+BaCl2----->2NaCl +BaSO4?
Q. What is the net Ionic and Complete Ionica equation for NaSO4+BaCl2--->2NaCl+B aSO4?
Asked by Mary T - Mon Dec 3 20:38:34 2007 - - 2 Answers - 0 Comments
A. Complete: 2Na+ + SO4= + Ba++ + 2Cl- ===> 2Na+ + 2Cl- + BaSO4 Net: Ba++ + SO4= ==> BaSO4
Answered by steve_geo1 - Mon Dec 3 20:43:06 2007
Q. What is the net Ionic and Complete Ionica equation for NaSO4+BaCl2--->2NaCl+B aSO4?
Asked by Mary T - Mon Dec 3 20:38:34 2007 - - 2 Answers - 0 Comments
A. Complete: 2Na+ + SO4= + Ba++ + 2Cl- ===> 2Na+ + 2Cl- + BaSO4 Net: Ba++ + SO4= ==> BaSO4
Answered by steve_geo1 - Mon Dec 3 20:43:06 2007
Assuming that BaCl2+NaSO4--->BaSO4+N aCl is correct(I know it isn't correct), how would you balance it?
Q. I know it is incorrect, but how would I balance it if it was?
Asked by pokefan022194 - Sat May 31 17:45:43 2008 - - 1 Answers - 0 Comments
A. BaCl2+Na2SO4--->BaSO4+2Na Cl No other way of balancing the reaction
Answered by mob3 - Sat May 31 17:52:56 2008
Q. I know it is incorrect, but how would I balance it if it was?
Asked by pokefan022194 - Sat May 31 17:45:43 2008 - - 1 Answers - 0 Comments
A. BaCl2+Na2SO4--->BaSO4+2Na Cl No other way of balancing the reaction
Answered by mob3 - Sat May 31 17:52:56 2008
What volume of 0.131M BaCl2 is required to react completely with 42.0 ml of 0.453M Na2SO4?
Q. I'm not sure how to set this up, any help would be greatly appreciated!
Asked by Jennifer - Thu Oct 29 19:34:45 2009 - - 1 Answers - 0 Comments
Q. I'm not sure how to set this up, any help would be greatly appreciated!
Asked by Jennifer - Thu Oct 29 19:34:45 2009 - - 1 Answers - 0 Comments
which solution below when mixed with an aqueous solution of BaCl2 will result in a the formation of a solid?
Q. percipitate? a) NH4Br b) Pb(NO3)2 C)KNO3 D)LiCl Please explain!
Asked by tooba - Thu Jun 18 02:25:03 2009 - - 1 Answers - 0 Comments
A. From the list provided, Pb(NO3)2 Pb(NO3)2(aq) + BaCl2(aq) PbCl2(s) + Ba(NO3)2(aq) A reaction occurs between the two reactants resulting in the formation of insoluble lead chloride.
Answered by Trevor H - Thu Jun 18 03:18:22 2009
Q. percipitate? a) NH4Br b) Pb(NO3)2 C)KNO3 D)LiCl Please explain!
Asked by tooba - Thu Jun 18 02:25:03 2009 - - 1 Answers - 0 Comments
A. From the list provided, Pb(NO3)2 Pb(NO3)2(aq) + BaCl2(aq) PbCl2(s) + Ba(NO3)2(aq) A reaction occurs between the two reactants resulting in the formation of insoluble lead chloride.
Answered by Trevor H - Thu Jun 18 03:18:22 2009
How many milliliters of 0.150 M BaCl2 are needed to react completely with 36.0 mL of 0.200 M Na2SO4?
Q. Also how many grams of BaSO4 will be formed? Thank you so much! I understand it now!
Asked by Redirkulous - Fri Nov 6 15:22:45 2009 - - 1 Answers - 0 Comments
A. The reaction that occurs ( double replacement ) is : BaCl2 (aq) + Na2SO4 (aq) = BaSO4 (s) + 2 NaCl (aq) moles Na2SO4 = 0.0360 L x 0.200 M=0.00720 the ratio between Na2SO4 and BaCl2 is 1 : 1 moles BaCl2 needed = 0.00720 Volume BaCl2 = 0.00720 mol/ 0.150 M=0.0480 L => 48.0 mL moles BaSO4 = 0.00720 mass BaSO4 = 0.00720 mol x 233.43 g/mol=1.68 g
Answered by Dr.A - Fri Nov 6 15:32:45 2009
Q. Also how many grams of BaSO4 will be formed? Thank you so much! I understand it now!
Asked by Redirkulous - Fri Nov 6 15:22:45 2009 - - 1 Answers - 0 Comments
A. The reaction that occurs ( double replacement ) is : BaCl2 (aq) + Na2SO4 (aq) = BaSO4 (s) + 2 NaCl (aq) moles Na2SO4 = 0.0360 L x 0.200 M=0.00720 the ratio between Na2SO4 and BaCl2 is 1 : 1 moles BaCl2 needed = 0.00720 Volume BaCl2 = 0.00720 mol/ 0.150 M=0.0480 L => 48.0 mL moles BaSO4 = 0.00720 mass BaSO4 = 0.00720 mol x 233.43 g/mol=1.68 g
Answered by Dr.A - Fri Nov 6 15:32:45 2009
How many grams of BaCl2 is formed when 2.9gms hydrated BaCl2 is heated to remove all H2O??? help please?
Q. I think that hydrated BaCl2 has the formula: BaCl2.2H2O thanks
Asked by Freshy - Thu Apr 3 05:58:54 2008 - - 2 Answers - 1 Comments
A. M(BaCl2) = 137.3 + 35.5 = 208.3 M(BaCl2.2H2O) = 172.8 + 2 ( 18 ) =244.3 So we know that when you heat a BaCl.2H2O compound, all the water evaporates, leaving BaCl. This means that the mass that remains after heating is the part of the compound that was BaCl, not H2O Therefore the mass of BaCl2 formed is 208.3/244.3 x 2.9 = 2.47g
Answered by HybridSnap - Thu Apr 3 06:09:10 2008
Q. I think that hydrated BaCl2 has the formula: BaCl2.2H2O thanks
Asked by Freshy - Thu Apr 3 05:58:54 2008 - - 2 Answers - 1 Comments
A. M(BaCl2) = 137.3 + 35.5 = 208.3 M(BaCl2.2H2O) = 172.8 + 2 ( 18 ) =244.3 So we know that when you heat a BaCl.2H2O compound, all the water evaporates, leaving BaCl. This means that the mass that remains after heating is the part of the compound that was BaCl, not H2O Therefore the mass of BaCl2 formed is 208.3/244.3 x 2.9 = 2.47g
Answered by HybridSnap - Thu Apr 3 06:09:10 2008
What is the weight of BaCl2 in a 0.250 L bottle of 0.200 M BaCl2?
Q. I'm stuck on this homework problem and need a little help! Could you please also show steps used to solve or get the answer that you got? Best will go to the first person to answer and show steps! Thanks, also please note the "2's" are intended to be subscripts.
Asked by [Sunkissed] - Sat Oct 24 10:32:10 2009 - - 2 Answers - 0 Comments
A. Moles of BaCl2 = L * M = (.250L) (.200M) = .0500 moles of BaCl2 .0500 mol * 208.23 g/ 1 mol = 10.4 g of BaCl2
Answered by x52raylewis - Sat Oct 24 10:42:14 2009
Q. I'm stuck on this homework problem and need a little help! Could you please also show steps used to solve or get the answer that you got? Best will go to the first person to answer and show steps! Thanks, also please note the "2's" are intended to be subscripts.
Asked by [Sunkissed] - Sat Oct 24 10:32:10 2009 - - 2 Answers - 0 Comments
A. Moles of BaCl2 = L * M = (.250L) (.200M) = .0500 moles of BaCl2 .0500 mol * 208.23 g/ 1 mol = 10.4 g of BaCl2
Answered by x52raylewis - Sat Oct 24 10:42:14 2009
2 clear aqueous solutions BaCl2 and Na2SO4 are mixed and a white solid forms?
Q. what is the solvent and most importantly how you got it
Asked by davidishere - Tue Jun 3 06:41:39 2008 - - 3 Answers - 0 Comments
A. The solvent is water as it states that you have AQUEOUS solutions. The precipitate will be barium sulphate (BaSO4) as all other ion combinations are soluble in water..
Answered by cstspeedy - Tue Jun 3 06:48:01 2008
Q. what is the solvent and most importantly how you got it
Asked by davidishere - Tue Jun 3 06:41:39 2008 - - 3 Answers - 0 Comments
A. The solvent is water as it states that you have AQUEOUS solutions. The precipitate will be barium sulphate (BaSO4) as all other ion combinations are soluble in water..
Answered by cstspeedy - Tue Jun 3 06:48:01 2008
How could you separate barium chloride, BaCl2, from calcium sulfate CaSO4?
Q. Stuck on a chem question... any input would be greatly appreciated. Working on the separation of components of a mixture... Thanks!
Asked by Erin B - Mon Oct 30 17:57:40 2006 - - 2 Answers - 0 Comments
A. BaCl2 is very soluble in water but CaSO4 is not. So add water. Then filtrated to get the BaSO4. Evaporate the solution and you get back BaCl2
Answered by Dimos F - Mon Oct 30 19:25:15 2006
Q. Stuck on a chem question... any input would be greatly appreciated. Working on the separation of components of a mixture... Thanks!
Asked by Erin B - Mon Oct 30 17:57:40 2006 - - 2 Answers - 0 Comments
A. BaCl2 is very soluble in water but CaSO4 is not. So add water. Then filtrated to get the BaSO4. Evaporate the solution and you get back BaCl2
Answered by Dimos F - Mon Oct 30 19:25:15 2006
How many moles of BaCl2 are formed in the neutralization of 393 mL of .171 M Ba(OH)2 with aueous HCL?
Q. How many moles of BaCl2 are formed in the neutralization of 393 mL of .171 M Ba(OH)2 with aueous HCL?
Asked by Monee - Sat Nov 7 00:51:55 2009 - - 1 Answers - 0 Comments
Q. How many moles of BaCl2 are formed in the neutralization of 393 mL of .171 M Ba(OH)2 with aueous HCL?
Asked by Monee - Sat Nov 7 00:51:55 2009 - - 1 Answers - 0 Comments
Why from MgCl2 to BaCl2 ( down a group) lattice enrgy becomes less exothermic?
Q. i wrote due to the distrortion of the electron cloud of chlourine, and because the Mg 2+ is very polarising. But what else? its a 3 mark question. I also wrote due to a covalent character in the ionic bond. If you go down, i thought it becomes more exothermic due to the size of the particle gets bigge
Asked by Shivraj B - Wed Oct 29 13:45:05 2008 - - 1 Answers - 0 Comments
Q. i wrote due to the distrortion of the electron cloud of chlourine, and because the Mg 2+ is very polarising. But what else? its a 3 mark question. I also wrote due to a covalent character in the ionic bond. If you go down, i thought it becomes more exothermic due to the size of the particle gets bigge
Asked by Shivraj B - Wed Oct 29 13:45:05 2008 - - 1 Answers - 0 Comments
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