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Chemistry HW - Balancing Equations?

Chemistry HW - Balancing Equations? Topic: Chemistry HW - Balancing Equations?
July 18, 2019 / By Debbi
Question: So I have homework on balancing chemical equations. I'm a bit confused on whether I'm balancing the chemical equations correctly or not. Please help. I will write a chemical equation that I balanced and I want to know if I balanced it correctly. 6 AgI + Fe2(CO3)3 --> 2 FeI3 + 3 Ag2CO3 * sorry that I can't put the subscripts on the bottom right of the atom. Any useful help will be super appreciated!(:
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Best Answers: Chemistry HW - Balancing Equations?

Briony Briony | 7 days ago
Just keep on doing what you are doing. Practice. Your equation is correct. Keep posting when you get stuck. You'll get it. Balancing programs work but you can't take them into a test.
👍 242 | 👎 7
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Briony Originally Answered: Need Chemistry help - Balancing chemical equations?
Your balanced equation is this: Al(NO3)3 + 3NaOH -> Al(OH)3 + 3NaNO3 Since there are three hydroxide ions in Al(OH)3, you need to start with three OH- ions. You would need 3 NaOH. If you actually did this, it would be more likely to produce a precipitate that dissolved as more NaOH was added. The reaction is as follows: Al(NO3)3(aq) + 4NaOH(aq) --> 4Na+ + Al(OH)4^- + 3NO3^- or, the net ionic equation is Al^3+ + 4OH- --> Al(OH)4^-
Briony Originally Answered: Need Chemistry help - Balancing chemical equations?
You need to end up with the same number of each molecule on either side of the equation. I would start with the aluminum hydroxide in the product. If you look at OH- there are now 3 of them, so there has to be 3 sodium hydroxide in the reactants to even out the number of -OH molecules on either side of the equation, giving you Al(NO3)3 + 3NaOH -> Al(OH)3 + NaNO3 Now you have three sodium molecules in the reactants that have to be accounted for in the products, so you have Al(NO3)3 + 3NaOH -> Al(OH)3 + 3NaNO3 Now there are an equal number molecules of each in the reactants and products and the equation is balanced.

Alica Alica
6AgI + Fe2(CO3)3 --> 2 FeI3 + 3 Ag2CO3 ..... this is a disaster. Whoever put this "equation" together is missing some fundamental chemistry. Silver iodide is insoluble in water and won't take part in a double replacement reaction. Iron(III) carbonate does not exist. Solutions of Fe3+ are so acidic, that if combined, the carbonate ion will react forming CO2 gas. Therefore, you can't "balance" the equation as you have written it, because there is no such reaction. In fact, there are no carbonate compounds in which the metal exhibits an oxidation state of +3 or greater. If you want to come up with something similar, then you could go with the following: 3Ba(NO2)2(aq) + Fe2(SO4)3(aq) --> 3BaSO4(s) + 2Fe(NO3)3(aq) or better yet.... 6AgNO3(aq) + Fe2(SO4)3(aq) --> 3Ag2SO4(s) + 2Fe(NO3)3(aq)
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Tyrrell Tyrrell
Ca3(PO4)2(s) + 2H2SO4(aq) ---> 2CaSO4(s) + Ca(H2PO4)2(aq) The equation as presented is a little bit dodgy given that there will probably be many more species than these in reality in solution. Calcium phosphate is insoluble in water, but will react with sulfuric acid. Calcium sulfate is relatively insoluble. Additionally to the "monocalcium phosphate", which is relatively soluble in water, there will be the following ions in answer: Ca2+, H+, H2PO4^-, HPO4^2-, PO4^three-, and H3PO4. The concentrations of these relies on the pH, with the intention to rely on the amount of any extra sulfuric acid in the reaction combination.
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Tyrrell Originally Answered: Gr10 Science Homework Help (Chemistry Equations)?
I'll give you the chemical formulas for these, but you should be balancing these equations yourself. If you don't practice that, it'll be over for you on the test and exam. CuSO4 + H2O Fe + O2 MnO2 + H2O2 CuSO4 * 5H2O Mg + AgNO3 Cu + AgNO3 Ag + Cu(NO3)2

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