Balance the following equations, and then write the net...

Balance the following equations, and then write the net ionic equation. (a) $\left(\mathrm{NH}_{4}\right)_{2} \mathrm{CO}_{3}(\mathrm{aq})+\mathrm{Cu}\left(\mathrm{NO}_{3}\right)_{2}(\mathrm{aq}) \rightarrow$ $\mathrm{CuCO}_{3}(\mathrm{s})+\mathrm{NH}_{4} \mathrm{NO}_{3}(\mathrm{aq})$ (b) $\mathrm{Pb}(\mathrm{OH})_{2}(\mathrm{s})+\mathrm{HCl}(\mathrm{aq}) \rightarrow \mathrm{PbCl}_{2}(\mathrm{s})+\mathrm{H}_{2} \mathrm{O}(\ell)$ (c) $\mathrm{BaCO}_{3}(\mathrm{s})+\mathrm{HCl}(\mathrm{aq}) \rightarrow$ $\mathrm{BaCl}_{2}(\mathrm{aq})+\mathrm{H}_{2} \mathrm{O}(\ell)+\mathrm{CO}_{2}(\mathrm{g})$ (d) $\mathrm{CH}_{3} \mathrm{CO}_{2} \mathrm{H}(\mathrm{aq})+\mathrm{Ni}(\mathrm{OH})_{2}(\mathrm{s}) \rightarrow$ $\mathrm{Ni}\left(\mathrm{CH}_{3} \mathrm{CO}_{2}\right)_{2}(\mathrm{aq})+\mathrm{H}_{2} \mathrm{O}(\ell)$

Balance the following equations, and then write the net ionic equation. (a) $\left(\mathrm{NH}_{4}\right)_{2} \mathrm{CO}_{3}(\mathrm{aq})+\mathrm{Cu}\left(\mathrm{NO}_{3}\right)_{2}(\mathrm{aq}) \rightarrow$
$\mathrm{CuCO}_{3}(\mathrm{s})+\mathrm{NH}_{4} \mathrm{NO}_{3}(\mathrm{aq})$
(b) $\mathrm{Pb}(\mathrm{OH})_{2}(\mathrm{s})+\mathrm{HCl}(\mathrm{aq}) \rightarrow \mathrm{PbCl}_{2}(\mathrm{s})+\mathrm{H}_{2} \mathrm{O}(\ell)$
(c) $\mathrm{BaCO}_{3}(\mathrm{s})+\mathrm{HCl}(\mathrm{aq}) \rightarrow$
$\mathrm{BaCl}_{2}(\mathrm{aq})+\mathrm{H}_{2} \mathrm{O}(\ell)+\mathrm{CO}_{2}(\mathrm{g})$
(d) $\mathrm{CH}_{3} \mathrm{CO}_{2} \mathrm{H}(\mathrm{aq})+\mathrm{Ni}(\mathrm{OH})_{2}(\mathrm{s}) \rightarrow$
$\mathrm{Ni}\left(\mathrm{CH}_{3} \mathrm{CO}_{2}\right)_{2}(\mathrm{aq})+\mathrm{H}_{2} \mathrm{O}(\ell)$

Key Concepts

Precipitation Reactions

Precipitation reactions occur when two soluble salts react in solution to form an insoluble product, known as a precipitate. The formation of the precipitate is a key signature of these reactions, and balancing such equations correctly is crucial to understanding the ion exchange process that leads to precipitation.

Spectator Ions

Spectator ions are ions that appear unchanged on both sides of a chemical reaction. They do not participate in the reaction itself and are removed when writing the net ionic equation. Recognizing spectator ions is important for correctly identifying the species that contribute to the actual chemical transformation.

Acid-Base Reactions

Acid-base reactions generally involve the transfer of protons from an acid to a base, typically resulting in the formation of water and a salt. These reactions can be represented by molecular equations, but often require conversion to ion-based equations for clarity, especially when identifying the active species involved in the neutralization process.

Balancing Chemical Equations

Balancing chemical equations involves ensuring that the number of atoms for each element and the net charge are the same on both sides of a reaction. This is a fundamental aspect of chemical stoichiometry, reflecting the law of conservation of mass, and it is essential for accurately representing the quantitative relationships between reactants and products.

Net Ionic Equations

A net ionic equation simplifies a chemical reaction by including only the ions and molecules that participate directly in the reaction, omitting spectator ions that do not change during the reaction. This format helps to highlight the actual chemical change taking place, making it easier to understand the underlying reaction mechanism.

Transcript

00:01 Hi everybody.

00:02 We're going to balance and then write net ionic equations for four equations.

00:07 And these are so long that i did something i don't usually do.

00:10 I have these all written out for you.

00:15 So you don't have to sit and listen to me, write them out.

00:18 Okay, so for the first chemical equation, we have ammonium carbonate reacting with copper two nitrate.

00:26 Yep, copper two nitrate.

00:28 Can't even read my own writing here.

00:30 This is in...

00:34 O3 to produce copper two carbonate solid and ammonium nitrate.

00:41 So those are my four substances.

00:43 Let's get rid of these lines so that we can balance this equation.

00:50 Okay, so this equation is pretty simple to balance by inspection.

00:54 I can see that i have two ammoniums and two nitrates here and here.

01:00 So i need two of each right there.

01:02 I put a two here in front of the ammonium nitrate and this is now a balanced chemical equation.

01:10 So this one we are now going to write our net ionic equation, but i think we'll go ahead and write this as our complete ionic equation first.

01:23 Remember we split all the aqs.

01:26 So here goes.

01:27 I have two ammonia's and i have one carbonate ion.

01:39 My first species.

01:42 My second species, i have one copper two ion plus two nitrate ions.

01:58 On the product side, i don't split the solids precipitate, and i have two ammonium ions and two nitrate ions.

02:20 Okay, so now let's go to a green and cross out our spectators.

02:27 I have nitrates on each side so they can cross out and i have ammoniums on each side so they can cross out and when we write this, rewrite this and i'm going to cheat i always like to put my metal first.

02:44 Cu 2 plus a q plus co3 2 plus or 2 minus a q yields co co3s.

03:02 And there is the final answer for a net ionic.

03:07 Okay.

03:08 And i'm going to circle these species here, here, and here.

03:13 Okay, let's do the same thing for a second equation.

03:17 First we need to balance this.

03:19 And this one is also pretty easy to balance.

03:22 I see that i have two chlorine, so i'm going to need a two here.

03:28 And if i put a two here, i'm also going to need a two here.

03:32 So here's my balanced chemical equation.

03:35 And i have a solid and a solid and a liquid.

03:39 So the only one that i can split is this.

03:42 So this isn't going to be much of an ionic equation.

03:49 So let me go ahead and write this one out.

03:50 P b oh h2 oops oh h 2 s plus now when i write my h plus my 2 h plus a q um the text that we're using for this is going to have us report these as h3 oh so i'm going to go ahead and do that make a little note underneath.

04:27 This is going to be 2h.

04:31 It's 2 hydronium because this is an aqueous solution, which is sort of similar to us going like this.

04:39 But we're going to go like this and you'll see what happens on the next side when i do that.

04:45 The only ones i split are my aqs, so this isn't going to change.

04:51 Now, i added an h2o right here.

04:54 So this two, actually i added two, i added two waters.

05:01 Right here.

05:03 So i have to add two more waters right here, which will give me an h2o, a 4 h2o...