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Write balanced molecular and net ionic equations for each of the following neutralization reactions.?

Write balanced molecular and net ionic equations for each of the following neutralization reactions.? Topic: Homework writing ionic compound formulas
May 26, 2019 / By Garnette
Question: Aqueous acetic acid is neutralized by aqueous potassium hydroxide. Solid chromium (III) hydroxide reacts with nitric acid. Aqueous nitrous acid and aqueous calcium hydroxide react. Nitrites are soluble compounds.
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Best Answers: Write balanced molecular and net ionic equations for each of the following neutralization reactions.?

Debbie Debbie | 8 days ago
Frankly, if you get somebody to do all your homework, you're not going to learn. Start off with the formulae HAc H2O KOH Cr(OH)3 HNO3 HNO2 H2O Ca(OH)2 You need to know what's soluble e.g. HAc + H2O <-> Ac- & H3O+ KOH + H2O <-> K+ OH- so H3O+ & OH- <-> 2H2O about the only thing to remember is that all of your elements H, O, C, Cr, Ca, N, you must have the same number of each on both sides of your equation and the sum of the charges on each side of the equation must be equal.
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Debbie Originally Answered: How to write total ionic and net ionic equations for the following chemical reactions?
I am puzzled about these equations. Because in both cases, no chemical reaction will occur. If you take you first example: BaCl2(aq) + Ca(NO3)2(aq) → Ba(NO3)2(aq) + CaCl2(aq) This indicates that you have started off with two soluble compounds, and all that can be "produced" are two soluble compounds. Under these conditions all that you actually have is a solution of soluble ions - no new product has been formed. So no reaction has taken place. Chemically speaking it is not possible to write any equation for this mixture. Exactly the same applies to your second example. No reaction occurs. Where did you get these equations?
Debbie Originally Answered: How to write total ionic and net ionic equations for the following chemical reactions?
OH, I might forget, but here I will give you some helpful tips. The first one, Barium Chloride and Calcium Nitrate? Now, you will have to see which one will dissolve, and if it does, it gets crossed out. So, you will left only with the strong acids. Supposedly, BaCl2+ Ca(NO3)2? If BaCl2 is weak, it will dissolve, and you are left with only Ca(NO3)2. I will check the Activity Series, stong acids and Weak Acids and get back to your question, but let me assure you that, Molecular equation is when you write the whole thing out. Net Ionic equation is most likely when you have everything else dissolved.

Britannia Britannia
(b) Solid chromium (III) hydroxide reacts with nitrous acid. Cr(OH)3 (s) + 3HNO3(aq) → Cr(NO3)3(aq) + 3H20(l) Cr(OH)3(s) + 3H(+)(aq) + 3NO3(-)(aq) → Cr(+3)(aq) + 3NO3(-)(aq) + 3H2O(l) Cr(OH)3(s) + 3 H(+)(aq) → Cr(3+)(aq) + 3H2O(l)
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Britannia Originally Answered: How would you write a balanced net ionic equation for each of the following two reactions? PLEASE HELP?
H3PO4 + 3NaOH = Na3Po4 + 3H20 Cu(NO3)2 + 2 KOH = Cu(OH)2 + 2 KNO3 you just need to make sure there is the same number of each ion on each side of the equation. i.e. there is two nitrates on the left so you need a two in front of the potassium nitrate, which means you need a 2 in front of the potassium hydroxide (to balance the number of potassiums) then you will notice that it works out because then you have two hydroxides on the left and two on the right.
Britannia Originally Answered: How would you write a balanced net ionic equation for each of the following two reactions? PLEASE HELP?
A) H3PO4 (aq) + 3NaOH (aq) = Na3PO4 (aq) + 3 H2O ==> H3PO4 (aq) + 3NaOH (aq) = Na3PO4 (aq) + 3 H2O<== B) Cu(NO3)2 (aq) + 2 KOH (aq) = Cu(OH)2 + 2KNO3 ==> Cu(NO3)2 (aq) + 2 KOH (aq) = Cu(OH)2 + 2KNO3 <== :)

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