Ionic Equation Answers
What is the net ionic equation for the decomposition reaction of hydrogen peroxide?
Q. I know that the molecular equation is 2H2O2(l) --> 2H2O(l)+O2(g). Would the net ionic equation be the same or different? Would you split up H2O2? Thanks!
Asked by paperhearts63 - Sat Feb 5 19:40:35 2011 - Chemistry - 1 Answers - Comments
A. Hi! you only split up ions which are in aqueous form. 2H202(l)---> 2 H20(l) + O2(g) In this reaction nothing is being displaced. Its just a decomposition reaction where H202 becomes water and oxygen gas is given out . net ionic equation for this would be the same as the molecular formula 2H202(l)---> 2 H20(l) + O2(g) (Molecular equation) Usually net ionic equation is more better for displacement type reaction. Here you can pretty much see what happens and how the reactions takes place! So the net ionic equation would be the same as molecular equation 2H202(l)---> 2 H20(l) + O2(g) (Net ionic equation)
Answered by chris j - Sat Feb 5 19:47:20 2011
Q. I know that the molecular equation is 2H2O2(l) --> 2H2O(l)+O2(g). Would the net ionic equation be the same or different? Would you split up H2O2? Thanks!
Asked by paperhearts63 - Sat Feb 5 19:40:35 2011 - Chemistry - 1 Answers - Comments
A. Hi! you only split up ions which are in aqueous form. 2H202(l)---> 2 H20(l) + O2(g) In this reaction nothing is being displaced. Its just a decomposition reaction where H202 becomes water and oxygen gas is given out . net ionic equation for this would be the same as the molecular formula 2H202(l)---> 2 H20(l) + O2(g) (Molecular equation) Usually net ionic equation is more better for displacement type reaction. Here you can pretty much see what happens and how the reactions takes place! So the net ionic equation would be the same as molecular equation 2H202(l)---> 2 H20(l) + O2(g) (Net ionic equation)
Answered by chris j - Sat Feb 5 19:47:20 2011
What is the net ionic equation for ammonium chloride + sodium hydroxide?
Q. NH4+ (aq) + Cl- (aq) + Na+(aq) + OH-(aq) --> NH4OH(aq) + Na+(aq) + Cl- (aq) This is the net ionic equation! I need help to calculate the net ionic equation? This is the total ionic equation. What is the net ionic equation?
Asked by Christopher M - Tue Oct 7 22:45:24 2008 - Chemistry - 2 Answers - Comments
A. NH4+ (aq) + OH-(aq) --> NH4OH(aq) Here ya go
Answered by gracelikerain_89 - Fri Oct 10 23:34:52 2008
Q. NH4+ (aq) + Cl- (aq) + Na+(aq) + OH-(aq) --> NH4OH(aq) + Na+(aq) + Cl- (aq) This is the net ionic equation! I need help to calculate the net ionic equation? This is the total ionic equation. What is the net ionic equation?
Asked by Christopher M - Tue Oct 7 22:45:24 2008 - Chemistry - 2 Answers - Comments
A. NH4+ (aq) + OH-(aq) --> NH4OH(aq) Here ya go
Answered by gracelikerain_89 - Fri Oct 10 23:34:52 2008
What is the total ionic equation for the following formula unit equation?
Q. What is the total ionic equation for the following formula unit equation? HF(aq) + KOH(aq)>>> KF(aq) + H2O(l)
Asked by Orgo V - Sun Jul 20 15:19:30 2008 - Chemistry - 1 Answers - Comments
A. H+ + F- + K+ + OH- >> K+ + F- + H2O
Answered by Dr.A - Mon Jul 21 05:25:19 2008
Q. What is the total ionic equation for the following formula unit equation? HF(aq) + KOH(aq)>>> KF(aq) + H2O(l)
Asked by Orgo V - Sun Jul 20 15:19:30 2008 - Chemistry - 1 Answers - Comments
A. H+ + F- + K+ + OH- >> K+ + F- + H2O
Answered by Dr.A - Mon Jul 21 05:25:19 2008
How do you write a net ionic equation in Chemistry?
Q. I'm not asking for you to do my homework, but I simply am asking for help. My teacher did not explain this well, and the Chemistry book is hopeless. One of the problems that I have to do is this: Phosphoric acid (H3PO4) and lithium hydroxide react to form a salt and water. I'm supposed to write the chemical (which I understand well) equation, complete ionic equation and net ionic equation. Please help me out here, I'm totally lost.
Asked by - Mon Feb 21 17:30:27 2011 - Chemistry - 1 Answers - Comments
Q. I'm not asking for you to do my homework, but I simply am asking for help. My teacher did not explain this well, and the Chemistry book is hopeless. One of the problems that I have to do is this: Phosphoric acid (H3PO4) and lithium hydroxide react to form a salt and water. I'm supposed to write the chemical (which I understand well) equation, complete ionic equation and net ionic equation. Please help me out here, I'm totally lost.
Asked by - Mon Feb 21 17:30:27 2011 - Chemistry - 1 Answers - Comments
How do you find the net ionic equation?
Q. We did a lab where we combined liquids and looked for precipitates and now we are required to write the Net ionic equation for each of them that had a precipitate. Problem is, i don't get how... He explained it in class in a ton of different ways, but i never kept up with him. I need someone to explain every step in finding the net ionic equation... One of the questions i have to do is Pb(NO3)2 (Lead (II) nitrate) and Na2CO3 (Sodium Carbonate). Many thanks ahead of time!
Asked by Flame - Tue Oct 27 19:02:41 2009 - Chemistry - 1 Answers - Comments
A. You should see a precipitate form when you combine lead (II) nitrate and sodium carbonate. Lead (II) carbonate will form, while the sodium and nitrate ions will remain in solution. Pb2+ + CO3^2- --> Pb CO3(s)
Answered by pisgahchemist - Tue Oct 27 19:14:17 2009
Q. We did a lab where we combined liquids and looked for precipitates and now we are required to write the Net ionic equation for each of them that had a precipitate. Problem is, i don't get how... He explained it in class in a ton of different ways, but i never kept up with him. I need someone to explain every step in finding the net ionic equation... One of the questions i have to do is Pb(NO3)2 (Lead (II) nitrate) and Na2CO3 (Sodium Carbonate). Many thanks ahead of time!
Asked by Flame - Tue Oct 27 19:02:41 2009 - Chemistry - 1 Answers - Comments
A. You should see a precipitate form when you combine lead (II) nitrate and sodium carbonate. Lead (II) carbonate will form, while the sodium and nitrate ions will remain in solution. Pb2+ + CO3^2- --> Pb CO3(s)
Answered by pisgahchemist - Tue Oct 27 19:14:17 2009
What is the total ionic and net ionic equation for the following?
Q. Write the complete ionic and net ionic equation for the following: Cr(NO3)3 (aq) + 3KOH (aq)--->Cr(OH)3 (s) + 3KNO (aq)
Asked by - Mon Dec 5 20:10:23 2011 - Chemistry - 1 Answers - Comments
A. Total Ionic Equation Cr^3+(aq) + 3NO3-(aq) + 3K+(aq) + 3OH-(aq) --> Cr(OH)3(s) + 3K+(aq) +3NO3-(aq) Net Ionic Equation Cr^3+(aq) + 3OH-(aq) --> Cr(OH)3(s)
Answered by - Mon Dec 5 20:20:07 2011
Q. Write the complete ionic and net ionic equation for the following: Cr(NO3)3 (aq) + 3KOH (aq)--->Cr(OH)3 (s) + 3KNO (aq)
Asked by - Mon Dec 5 20:10:23 2011 - Chemistry - 1 Answers - Comments
A. Total Ionic Equation Cr^3+(aq) + 3NO3-(aq) + 3K+(aq) + 3OH-(aq) --> Cr(OH)3(s) + 3K+(aq) +3NO3-(aq) Net Ionic Equation Cr^3+(aq) + 3OH-(aq) --> Cr(OH)3(s)
Answered by - Mon Dec 5 20:20:07 2011
What is the complete ionic equation and net equation for ?
Q. For---> Lead (II) nitrate (aq) + Sodium sulfide (aq) What is the complete ionic equation ? and What is the net ionic equation ?
Asked by - Wed Jul 28 15:30:01 2010 - Mathematics - 1 Answers - Comments
A. Never fear, Jaws is here! Lead (II) nitrate is Pb(NO3)2 and Sodium sulfide is Na2S Therefore, the chemical equation runs thus: Pb(NO3)2 + Na2S --> Pb S + 2 Na NO3 The complete ionic equation: Pb(+2) + 2 NO3(-1) + 2 Na(+1) + S(-2) --> Pb S + 2 Na(+1) + 2 NO3(-1) And the net ionic equation: Pb(+2) + S(-2) --> Pb S
Answered by Jaws - Thu Jul 29 20:20:46 2010
Q. For---> Lead (II) nitrate (aq) + Sodium sulfide (aq) What is the complete ionic equation ? and What is the net ionic equation ?
Asked by - Wed Jul 28 15:30:01 2010 - Mathematics - 1 Answers - Comments
A. Never fear, Jaws is here! Lead (II) nitrate is Pb(NO3)2 and Sodium sulfide is Na2S Therefore, the chemical equation runs thus: Pb(NO3)2 + Na2S --> Pb S + 2 Na NO3 The complete ionic equation: Pb(+2) + 2 NO3(-1) + 2 Na(+1) + S(-2) --> Pb S + 2 Na(+1) + 2 NO3(-1) And the net ionic equation: Pb(+2) + S(-2) --> Pb S
Answered by Jaws - Thu Jul 29 20:20:46 2010
Which of the following statements about writing molecular, complete and net ionic equation is false?
Q. 1. A molecular equation is a chemical equation showing the complete, neutral formulas for every compound in a reaction. 2. A complete ionic equation is a chemical equation showing all of the species as they are actually present in solution. 3. A net ionic equation is an equation showing only the species that actually change during the reaction. 4. A spectator ion remains unchanged in the reaction and appears on both sides of the equation. 5. All of the statements are true.
Asked by - Wed Mar 23 13:52:31 2011 - Chemistry - 2 Answers - Comments
A. 5
Answered by Soc the Poetic Chemist - Wed Mar 23 13:57:18 2011
Q. 1. A molecular equation is a chemical equation showing the complete, neutral formulas for every compound in a reaction. 2. A complete ionic equation is a chemical equation showing all of the species as they are actually present in solution. 3. A net ionic equation is an equation showing only the species that actually change during the reaction. 4. A spectator ion remains unchanged in the reaction and appears on both sides of the equation. 5. All of the statements are true.
Asked by - Wed Mar 23 13:52:31 2011 - Chemistry - 2 Answers - Comments
A. 5
Answered by Soc the Poetic Chemist - Wed Mar 23 13:57:18 2011
What is the net ionic equation of the reaction?
Q. What is the net ionic equation of the reaction of Mg SO4 with Ba Cl2 ? What is the net ionic equation of the reaction of Mg SO4 with Ba Cl2 ?
Asked by - Sun Aug 28 03:14:32 2011 - Chemistry - 1 Answers - Comments
A. The barium sulfate will precipitate; the magnesium ion and chloride ions will be spectator ions. Ba^2+ + SO4^2- ---> Ba SO4
Answered by - Sun Aug 28 04:13:12 2011
Q. What is the net ionic equation of the reaction of Mg SO4 with Ba Cl2 ? What is the net ionic equation of the reaction of Mg SO4 with Ba Cl2 ?
Asked by - Sun Aug 28 03:14:32 2011 - Chemistry - 1 Answers - Comments
A. The barium sulfate will precipitate; the magnesium ion and chloride ions will be spectator ions. Ba^2+ + SO4^2- ---> Ba SO4
Answered by - Sun Aug 28 04:13:12 2011
What is the balanced ionic equation including state symbols for these two reactions?
Q. What is the balanced ionic equation including state symbols for these two reactions?Also an explanation of what is the (aq) symbol would help. 1)copper sulphate+sodium carbonate 2)sodium hydroxide + hydrochloric acid Thankyou in advance.I need to complete this work in order to take chemistry A-level next year but because my school only offered double award science i am struggling with some parts. please answer
Asked by blanknameforanonymity - Fri Aug 20 10:49:27 2010 - Chemistry - 1 Answers - Comments
A. The (aq) symbol means that the substance is dissolved in water and surrounded by water molecules. Aq stands for aqueous; aqueous ions are mobile and free to move in the solution. For an ionic equation, you have to split the substances into their ions if they are dissolved. There are full ionic equations, which shows all ions present, and net ionic equations, which only show those ions that change state, such as from aqueous to solid (in a precipitation reaction). For the first reaction, first write out the normal equation. Cu SO4(aq) + Na2CO3(aq) Na2SO4(aq) + Cu CO3(s) The copper(II) carbonate is insoluble, so you write the (s); all the others are soluble, so you write (aq). Next, split the soluble substances into their ions. Cu2 (aq) +… [cont.]
Answered by kumorifox - Fri Aug 20 11:01:39 2010
Q. What is the balanced ionic equation including state symbols for these two reactions?Also an explanation of what is the (aq) symbol would help. 1)copper sulphate+sodium carbonate 2)sodium hydroxide + hydrochloric acid Thankyou in advance.I need to complete this work in order to take chemistry A-level next year but because my school only offered double award science i am struggling with some parts. please answer
Asked by blanknameforanonymity - Fri Aug 20 10:49:27 2010 - Chemistry - 1 Answers - Comments
A. The (aq) symbol means that the substance is dissolved in water and surrounded by water molecules. Aq stands for aqueous; aqueous ions are mobile and free to move in the solution. For an ionic equation, you have to split the substances into their ions if they are dissolved. There are full ionic equations, which shows all ions present, and net ionic equations, which only show those ions that change state, such as from aqueous to solid (in a precipitation reaction). For the first reaction, first write out the normal equation. Cu SO4(aq) + Na2CO3(aq) Na2SO4(aq) + Cu CO3(s) The copper(II) carbonate is insoluble, so you write the (s); all the others are soluble, so you write (aq). Next, split the soluble substances into their ions. Cu2 (aq) +… [cont.]
Answered by kumorifox - Fri Aug 20 11:01:39 2010
How would I write the molecular / net ionic equation for this?
Q. Lead is put into Zinc Sulfate. How would I write the net molecular / net ionic equation? Please provide a short explanation. Thanks!
Asked by onlineworld - Thu Nov 22 06:00:41 2007 - Chemistry - 2 Answers - Comments
A. Pb (s) + Zn SO4 (aq) >> Pb SO4 (s) + Zn(s) ionic Pb + Zn2+ + SO42- >> Pb SO4 + Zn
Answered by Dr.A - Thu Nov 22 13:20:25 2007
Q. Lead is put into Zinc Sulfate. How would I write the net molecular / net ionic equation? Please provide a short explanation. Thanks!
Asked by onlineworld - Thu Nov 22 06:00:41 2007 - Chemistry - 2 Answers - Comments
A. Pb (s) + Zn SO4 (aq) >> Pb SO4 (s) + Zn(s) ionic Pb + Zn2+ + SO42- >> Pb SO4 + Zn
Answered by Dr.A - Thu Nov 22 13:20:25 2007
Chemistry Problem: What is the net ionic equation of a dissolution of salt in water?
Q. What is the net ionic equation of a dissolution of salt in water?Basically we added salt in water and we want to know the net ionic equation for this.
Asked by Lola M - Mon Oct 27 09:45:26 2008 - Chemistry - 3 Answers - Comments
A. Na Cl(s) + H2O(l) ---> H2O(l) + Na+(aq) + Cl-(aq) This is the Ionic equation. Since H2O are on both sides of the equation and in the same state (both in the liquid state). They can be cancelled out to get a net ionic equation of: Na Cl(s) ---> Na+(aq) + Cl-(aq)
Answered by clamk - Mon Oct 27 10:00:25 2008
Q. What is the net ionic equation of a dissolution of salt in water?Basically we added salt in water and we want to know the net ionic equation for this.
Asked by Lola M - Mon Oct 27 09:45:26 2008 - Chemistry - 3 Answers - Comments
A. Na Cl(s) + H2O(l) ---> H2O(l) + Na+(aq) + Cl-(aq) This is the Ionic equation. Since H2O are on both sides of the equation and in the same state (both in the liquid state). They can be cancelled out to get a net ionic equation of: Na Cl(s) ---> Na+(aq) + Cl-(aq)
Answered by clamk - Mon Oct 27 10:00:25 2008
What is the net ionic equation of barium chloride and a chromate ion?
Q. barium chloride is Ba Cl2 and chromate ion is Cr O42- please show me all your work so i can understand how to write net ionic equations. like write the molecular equation and then show me how you get to the net ionic equation. THANKS so MUCH!! :)
Asked by sana i - Tue Mar 1 12:39:22 2011 - Chemistry - 2 Answers - Comments
A. Solubility rules are here Of course the chromate ion does not come by itself, it comes with a positive ion. I will take potassium so the formula will be K2Cr O4 In Ba Cl2(aq) you have Ba^2+ ions and Cl^- ions. In K2Cr O4 you have K^+ ions and Cr O4^2- ions. Now when you mix the two together you can get two new combninations of positive and negative ions: Ba^2+ with Cr O4^2- and K^+ with Cl^- Now, if one of these two new combinations would result in the formation of an insoluble compound you will get a reaction (a precipitate will form) According to the sol. rules the combination Ba^2+ with Cr O4^2- is not soluble so that will form a precipitate. The combination between K^+ and Cl^- is soluble so you won't see anything happen between these… [cont.]
Answered by - Tue Mar 1 12:54:22 2011
Q. barium chloride is Ba Cl2 and chromate ion is Cr O42- please show me all your work so i can understand how to write net ionic equations. like write the molecular equation and then show me how you get to the net ionic equation. THANKS so MUCH!! :)
Asked by sana i - Tue Mar 1 12:39:22 2011 - Chemistry - 2 Answers - Comments
A. Solubility rules are here Of course the chromate ion does not come by itself, it comes with a positive ion. I will take potassium so the formula will be K2Cr O4 In Ba Cl2(aq) you have Ba^2+ ions and Cl^- ions. In K2Cr O4 you have K^+ ions and Cr O4^2- ions. Now when you mix the two together you can get two new combninations of positive and negative ions: Ba^2+ with Cr O4^2- and K^+ with Cl^- Now, if one of these two new combinations would result in the formation of an insoluble compound you will get a reaction (a precipitate will form) According to the sol. rules the combination Ba^2+ with Cr O4^2- is not soluble so that will form a precipitate. The combination between K^+ and Cl^- is soluble so you won't see anything happen between these… [cont.]
Answered by - Tue Mar 1 12:54:22 2011
How do you write net ionic equation for the reaction between nitric acid and calcium hydroxide?
Q. I have to write a net ionic equation for nitric acid and calcium hydroxide and all the answers I've submitted have been rejected. If someone could explain how to create the equation that would be great.
Asked by psawyer - Sat Feb 27 17:03:41 2010 - Chemistry - 1 Answers - 1 Comments
A. Write your reactants as ions in solution, as well as your products as either ions or molecules. Then cancel out things that appear on either side of the reaction So: 2HNO3 + Ca(OH)2 -> Ca(NO3)2 + 2H2O becomes 2H+(aq) + 2NO3-(aq) + Ca2+(aq) + 2OH-(aq) -> Ca2+(aq) + 2NO3-(aq) + 2H2O(l) As you can see, 2NO3- and Ca2+ appears on both sides of the equation, so we cancel them out, and they are excluded from the net ionic equation Net ionic: 2H+ (aq) + 2OH- (aq) - 2H2O (l)
Answered by sharkness77 - Sat Feb 27 17:12:08 2010
Q. I have to write a net ionic equation for nitric acid and calcium hydroxide and all the answers I've submitted have been rejected. If someone could explain how to create the equation that would be great.
Asked by psawyer - Sat Feb 27 17:03:41 2010 - Chemistry - 1 Answers - 1 Comments
A. Write your reactants as ions in solution, as well as your products as either ions or molecules. Then cancel out things that appear on either side of the reaction So: 2HNO3 + Ca(OH)2 -> Ca(NO3)2 + 2H2O becomes 2H+(aq) + 2NO3-(aq) + Ca2+(aq) + 2OH-(aq) -> Ca2+(aq) + 2NO3-(aq) + 2H2O(l) As you can see, 2NO3- and Ca2+ appears on both sides of the equation, so we cancel them out, and they are excluded from the net ionic equation Net ionic: 2H+ (aq) + 2OH- (aq) - 2H2O (l)
Answered by sharkness77 - Sat Feb 27 17:12:08 2010
What is the net ionic equation for those cases in which no solid was produced? Why?
Q. I think that you could not write no net ionic equation because there is no solid at all. The purpose of the net ionic equation is to show us the solid in the end. Is this correct?
Asked by jmagdaleno666 - Tue Sep 30 00:45:27 2008 - Chemistry - 1 Answers - Comments
A. The net ionic equation removes like ions from the equation. A solid is not a requirement for a net ionic equation. It just makes finding a net ionic equation easier if there is a solid sometimes I think.
Answered by Devon - Tue Sep 30 01:09:37 2008
Q. I think that you could not write no net ionic equation because there is no solid at all. The purpose of the net ionic equation is to show us the solid in the end. Is this correct?
Asked by jmagdaleno666 - Tue Sep 30 00:45:27 2008 - Chemistry - 1 Answers - Comments
A. The net ionic equation removes like ions from the equation. A solid is not a requirement for a net ionic equation. It just makes finding a net ionic equation easier if there is a solid sometimes I think.
Answered by Devon - Tue Sep 30 01:09:37 2008
What is the net ionic equation for ammonium carbonate and Na2HPO4?
Q. What is the net ionic equation of ammonium carbonate and Na2HPO4. Include the states (s) (l) (g) (aq). (NH4)2CO3 + Na2HPO4.
Asked by - Fri Mar 18 13:29:45 2011 - Chemistry - 1 Answers - Comments
A. Since the ions involved will not produce a precipitate, there is no reaction and therefore no net ionic equation. I guess you could show all the hydrated ions on both sides of the equation but that looks a little silly.
Answered by - Tue Mar 22 12:00:14 2011
Q. What is the net ionic equation of ammonium carbonate and Na2HPO4. Include the states (s) (l) (g) (aq). (NH4)2CO3 + Na2HPO4.
Asked by - Fri Mar 18 13:29:45 2011 - Chemistry - 1 Answers - Comments
A. Since the ions involved will not produce a precipitate, there is no reaction and therefore no net ionic equation. I guess you could show all the hydrated ions on both sides of the equation but that looks a little silly.
Answered by - Tue Mar 22 12:00:14 2011
What is the total and net ionic equation?
Q. What is the total and net ionic equation for barium hydroxide solution mixed with hydrogen fluoride, please explain Thank you so much!
Asked by - Sun Nov 20 15:46:39 2011 - Chemistry - 1 Answers - Comments
Q. What is the total and net ionic equation for barium hydroxide solution mixed with hydrogen fluoride, please explain Thank you so much!
Asked by - Sun Nov 20 15:46:39 2011 - Chemistry - 1 Answers - Comments
How do you know whether a reaction has an ionic equation?
Q. Please help me. My exam is in less than a week and i need to know which types of reactions have an ionic equation and which don't!! Thanks A LOT!
Asked by kath(: - Fri Oct 10 03:49:23 2008 - Chemistry - 3 Answers - Comments
A. Hi, for an ionic equation to happen you need to have a substance made of a metal and a non metal. In aqueous solution the metals exit as + ions and the non metal as - ions. Example: Na OH Na sodium, is the metal and exits as Na + ions in solution OH hydroxide, is the non metal and exits as OH - ions in solution If you look up Redox reactions and oxidation/reduction you should find more about ionic equations somewhere there. Cheers
Answered by MJbetterdays - Fri Oct 10 04:32:58 2008
Q. Please help me. My exam is in less than a week and i need to know which types of reactions have an ionic equation and which don't!! Thanks A LOT!
Asked by kath(: - Fri Oct 10 03:49:23 2008 - Chemistry - 3 Answers - Comments
A. Hi, for an ionic equation to happen you need to have a substance made of a metal and a non metal. In aqueous solution the metals exit as + ions and the non metal as - ions. Example: Na OH Na sodium, is the metal and exits as Na + ions in solution OH hydroxide, is the non metal and exits as OH - ions in solution If you look up Redox reactions and oxidation/reduction you should find more about ionic equations somewhere there. Cheers
Answered by MJbetterdays - Fri Oct 10 04:32:58 2008
What is the net ionic equation for the hydrolysis of Zn Cl2?
Q. What is the net ionic equation for the hydrolysis of Zn Cl2 What is the expression for equilibrium constant? What is the value
Asked by Stephen's - Sat Mar 29 17:03:49 2008 - Chemistry - 1 Answers - Comments
A. Zn Cl2 (s) ==> Zn2+ (aq) _ 2Cl- (aq) Keq = [Zn2+] x [Cl-]^2
Answered by drbillmacmo - Sat Mar 29 17:20:05 2008
Q. What is the net ionic equation for the hydrolysis of Zn Cl2 What is the expression for equilibrium constant? What is the value
Asked by Stephen's - Sat Mar 29 17:03:49 2008 - Chemistry - 1 Answers - Comments
A. Zn Cl2 (s) ==> Zn2+ (aq) _ 2Cl- (aq) Keq = [Zn2+] x [Cl-]^2
Answered by drbillmacmo - Sat Mar 29 17:20:05 2008
What is the total ionic equation of this balanced equation?
Q. 2Na OH(aq) + Cu SO4(aq) ---> Na2SO4(aq) + Cu(OH)2(s) Also, what's the net ionic equation?
Asked by vitten - Wed Apr 22 14:32:32 2009 - Chemistry - 1 Answers - Comments
A. Total ionic 2Na^+(aq) + 2OH^-(aq) + Cu^2+(aq) + SO4^2-(aq) 2Na^+(aq) + SO4^2-(aq) + Cu(OH)2(s) Net ionic 2OH^-(aq) + Cu^2+(aq) Cu(OH)2(s)
Answered by kumorifox - Wed Apr 22 14:38:07 2009
Q. 2Na OH(aq) + Cu SO4(aq) ---> Na2SO4(aq) + Cu(OH)2(s) Also, what's the net ionic equation?
Asked by vitten - Wed Apr 22 14:32:32 2009 - Chemistry - 1 Answers - Comments
A. Total ionic 2Na^+(aq) + 2OH^-(aq) + Cu^2+(aq) + SO4^2-(aq) 2Na^+(aq) + SO4^2-(aq) + Cu(OH)2(s) Net ionic 2OH^-(aq) + Cu^2+(aq) Cu(OH)2(s)
Answered by kumorifox - Wed Apr 22 14:38:07 2009
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