Net ionic equation for Cu(NO3)2 (aq) + K2CO3 (aq) --> CuCO3 + 2KNO3?
Cu(NO3)2 (aq) + K2CO3 (aq) --> CuCO3 + 2KNO3 When I try to figure out the net ionic equation for the above reaction, I write out the complete ionic equation and it seems like everything breaks down the same on both sides, but I know that's not right :( What is the complete ionic and net ionic equation for this?
Do you know these net ionic equations?
AlBr3(aq) + 3LiOH(aq) → Al(OH)3(s) + 3LiBr(aq) Net ionic equation: Al^3+(aq) + 3 OH^-(aq) --> Al(OH)3(s) both Li^+ and Br^- are spectator ions. LiClO(aq) + HI(aq) → LiI(aq) + HClO(aq) HClO is a weak acid and will not be appreciably ionized in solution. Net ionic equation: ClO^-(aq) + H^+(aq) --> HClO(aq) Pb(NO3)2(aq) + 2HCl(aq) → PbCl2(s) + 2HNO3(aq) Net ionic equation: Pb^2+(aq) + 2 Cl^-(aq) --> PbCl2(s) Mg(s) + 2HI(aq) → MgI2(aq) + H2(g) I^- is the spectator ion in this equation. HI is a strong acid and ionizes 100% in water. Net ionic equation: Mg(s) + 2 H^+(aq) --> Mg^2+(aq) + H2(g) Mg(s) + Cu(CH3COO)2(aq) → Mg(CH3COO)2(aq) + Cu(s) Net ionic equation: Mg(s) + Cu^2+(aq) --> Mg^2+(aq) + Cu(s) LiOH(aq) + HCN(aq) → LiCN(aq) + H2O(l) This is an acid base reaction. HCN is a weak acid. Net ionic equation: OH^-(aq) + HCN --> H2O(l) + CN^-(aq) Mg(s) + 2HI(aq) → MgI2(aq) + H2(g) This is a repeat. See above. NaF(aq) + HCl(aq) → NaCl(aq) + HF(aq) HF is a weak acid. Net ionic equation: F^-(aq) + H^+(aq) --> HF(aq) MgCl2(aq) + 2LiOH(aq) → Mg(OH)2(s) + 2LiCl(aq) Net ionic equation: Mg^2+(aq) + 2 OH^-(aq) --> Mg(OH)2(s) Hope this is helpful. JIL HIR
Complete and balance each of the following equations. If no reaction occurs, write NOREACTION.?
Pb(NO3)2(aq) + 2KCl(aq) --> PbCl2 (s) + 2KNO3 (aq) 2NaI(aq) + Hg2(C2H3O2)2(aq) --> Hg2I2 (s) + 2NaC2H3O2 (aq) NH4)2S(aq) + SrCl2(aq) --> SrS (s) + 2NH4Cl (aq) Note: SrS is slightly soluble. NH4Cl(aq) + AgNO3(aq) --> AgCl (s) + NH4NO3 (aq)
Which combination will produce a precipitate?
d. would form NaNO3 and Fe(OH)3 (solid) it's based on the solubility rules.. All compounds of NH4+, Na+ (and other alkali metals), C2H3O2- are soluble A Cl compounds are soluble except for Ag, Hg and Pb here's a link i found for the solubility rule of compounds: http://www.csudh.edu/oliver/chemdata/sol...
Help me find the ionic and net ionic equations for these reactions PLEASE!?
Write the balanced complete ionic equations and net ionic equations for the reactions that occur when each of the following pairs of solution are mixed. (a) Na2CO3(aq) and MgSO4(aq) ionic equation? net ionic equation? (b) Pb(NO3)2(aq) and Na2S(aq) ionic equation? net ionic equation? (c) (NH4)3PO4(aq) and CaCl2(aq) ionic equation? net ionic equation? ***Explanation These are metathesis or double displacement reactions. So the cation of the first compound combines with the anion of the second compound to form one product. Then the cation of the second compound combines with the anion of the first compound to form the second product. Look at the solubility guidelines in Table 4.1 to determine which products are insoluble (and therefore a solid) and which are soluble (and therefore will break apart into ions.) Then all soluble ionic compounds will break apart into their constituent ions in the Ionic Equation. The insoluble ionic compounds will remain together as a molecule. If an ion appears on both sides of the equation, then it is a spectator ion. You will cancel the spectator ions out to achieve the NET IONIC equation. This only contains the ions and compounds that are involved in the reaction.
Net Ionic Equations Help ?!?
Pb(NO3)2(aq) + 2KCl(aq) => PbCl2(s) + 2KNO3(aq) Pb2+(aq) + 2[NO3]-(aq) + 2K+(aq) + 2Cl-(aq) => PbCl2(s) + 2K+(aq) + 2[NO3]-(aq) Pb2+(aq) + 2Cl-(aq) => PbCl2(s) CaCl2(aq) + Na2CO3(aq) => CaCO3(s) + 2NaCl(aq) Ca2+(aq) + 2Cl-(aq) + 2Na+(aq) + [CO3]2- (aq) => CaCO3(s) + 2Na+(aq) + 2Cl-(aq) Ca2+(aq) + [CO3]2-(aq) => CaCO3(s)
Net Ionic Chemistry Equation?
It's good to know that a carbonate and an acid will produce CO2, H2O, and a salt. So your equation would become Li2CO3 + H2SO4 --> Li2SO4 + H2O + CO2 Ionically, you would have 2 Li+ (aq) + CO3-2(aq) + 2H+(aq) + SO4-2(aq) --> 2 Li+ (aq) + SO4-2(aq) + H2O(l) + CO2(g) The net ionic equation would be 2H+(aq) + CO3-2(aq) -----> H2O + CO2
Net Ionic Equations Help?
I have had a quick look through your question and answers. You can only have a net ionic equation where the product(s) is either (g) (s) or (l) . The equation cannot include a product that is (aq) because that indicates that the product is in solution and has dissociated. You must establish a habit of writing out the equations in full in an orderly manner preferably in one line indicating for every compound or ion whether it is (aq), (s) (g) or (l) In your list : A) KC2H3O2 (aq) + HNO3 (aq) →2K+(aq) + C2H3O2-(aq) + H+(aq) + NO3-(aq) Because all the products are (aq) there is no reaction and no net ionic equation. See how I have written out the balanced equation in one line showing states for everything B) H2SO4(aq) + 2KOH(aq) → K2SO4(aq) + 2H2O (l) 2H+ (aq) + SO4 2-(aq) + 2K+(aq) + 2OH-(aq) → 2K+(aq) + SO4 2-(aq) + 2H2O(l) Net ionic : H+ (aq) + OH-(aq) → H2O(l) C. AgNO3 (aq) + HCl (aq) → AgCl(s) + NO3-(aq) + H+(aq) Net ionic : Ag+(aq) + Cl-(aq) → AgCl(s) This is probably one of the best known net ionic equations you learn I am not going to go through all the equations in full: I will give some advice for each: D) BaS consider as (aq) Net ionic equation: H+(aq) + OH-(aq) → H2O (l) E), F), G) H) Correct answers Good work J Ba+2(aq) + SO4-2(aq) ---> BaSO4 (s) is the net ionic equation. K - All products are (aq) - no reaction L Na+(aq) + Br- (aq) ---> NaBr(aq) is not a net ionic equation - in fact the answer is : Na2CO3 (aq) + BaBr2 (aq) → BaCO3(s) + 2NaBr(aq) Net ionic equation: Ba 2+ (aq) + CO3 2-(aq) → BaCO3 (s) M) Correct answer. Do you have a list which shows you how to check if compounds are soluble or insoluble. You must know this otherwise you cannot do these net ionic equation problems. For instance you have: "KNO3 (s)". This is not possible - one of the first thinhgs that you learn about solubility is that all nitrates are soluble. This was a very long question - I hope taht I have clarified some things for you Be free to email me if you want more help.
Net ionic equations!!!!!!!!!!!?
Looks like you need the products as well as the net ionic equations. First the products. Decide what type of reaction each one is to find the products. The first is an acid-base reaction that forms carbonic acid, H2CO3 (aq), which is unstable. H2CO3 (aq) decomposes to H2O (l) and CO2 (g). The second reaction is a precipitation reaction, since BaCO3 is not soluble. The last reaction isn't really a reaction, i.e. nothing will happen when HCl is mixed with Na2SO4. Then, balance each equation by making sure the same number of each type of atom appears on both sides of the equation. So here are the balanced equations for the first two, where something actually reacts: a. Na2CO3 (aq) + 2HCl (aq) -> 2NaCl (aq) + H2O (l) + CO2 (g) b. Na2CO3 (aq) + BaCl2 (aq) -> 2NaCl (aq) + BaCO3 (s). If your teacher wants you to write something for the third reaction, you might try this: c. HCl (aq) + Na2SO4 (aq) -> no reaction To get the net ionic equations, recognize that all (aq) compounds are really individual cations and anions separated in the solvent (water). So the balanced equations can also be written as full ionic equations, where the (aq) compounds are written as separated ions: a. 2Na+ (aq) + CO3(-2) (aq) + 2H+ (aq) + 2Cl- (aq) -> 2Na+ (aq) + 2Cl- (aq) + H2O (l) + CO2 (g) b. 2Na+ (aq) + CO3(-2) (aq) + Ba(+2) (aq) + 2Cl- (aq) -> 2Na+ (aq) + 2Cl- (aq) + BaCO3 (s). Any cation or anion that appears on both sides of the equation is called a spectator ion because it really doesn't participate in the reaction. You can cancel the spectator ions out. The net ionic equations are thus: a. CO3(-2) (aq) + 2H+ (aq) -> H2O (l) + CO2 (g) The Na+ (aq) and Cl- (aq) cancel. b. CO3(-2) (aq) + Ba(+2) (aq) -> BaCO3 (s) The Na+ (aq) and Cl- (aq) cancel again.
What are the following molecular and net ionic equations?
I had to do an unknown solutions experiment, what are the following molecular and net ionic equations? AgNO3 + BaCl2 AgNO3+Cu(NO3)2 AgNO3+CuSO4 AgNO3+Pb(NO3)2 AgNO3+KI BaCl2+Cu(NO3)2 BaCl2+CuSO4 BaCl2+Pb(NO3)2 BaCl2+KI BaCl2+Na2CO3 Cu(NO3)2+CuSO4 Cu(NO3)2+Pb(NO3)2 Cu(NO3)2+KI Cu(NO3)2+Na2CO3 CuSO4+Pb(NO3)2 CuSO4+KI CuSO4+Na2CO3 Pb(NO3)2+KI Pb(NO3)2+Na2CO3 KI+Na2CO3