Write the balanced formula, complete ionic, and net ionic...

Write the balanced formula, complete ionic, and net ionic equations for each of the following acid-base reactions. (Be sure to specify states such as (aq) or (s). If a box is not needed, leave it blank. If no reaction occurs, leave all boxes blank and click on Submit.) a. Balanced formula equation: HNO3(aq) + Al(OH)3(s) Complete ionic equation: Net ionic equation: b. Balanced formula equation: HC2H3O2(aq) + KOH(aq) Complete ionic equation:

Transcript

00:01 Okay, it looks like we have some acid -based reactions here.

00:03 We want to look for balanced formula equations, complete ionic equations, and net ionic equations.

00:11 So for our first one with the nitric acid, and that's going to react with our aluminum hydroxide.

00:19 Now, the nitric acid it says is aqueous.

00:25 Aluminum hydroxide is solid.

00:27 So let's start with the overall process.

00:29 Now, in an acid -based reaction, the hydrogens from the acid are, going to react with the hydroxides from the base to form water.

00:38 And that's going to be a liquid.

00:40 So the thing is if we have three hydroxides from our base, then we're going to need three hydrogens from our acids.

00:48 So i'm going to put a three there.

00:51 And so three hydrogens from the acid and three hydroxides are going to give us three waters, right? h and oh makes h2o.

00:58 So at this point, i've got the reactants balanced.

01:03 So what's left then? well, we have one aluminum and three nitrates.

01:08 So the last product is aluminum nitrate.

01:13 And it's going to be aqueous because nitrates will dissolve in water.

01:17 And that's consistent.

01:18 You know, the leftover pieces, i have three no3s left over and one al.

01:23 And that's consistent with what we know about balanced charges, because aluminum is plus three and nitrate is minus one.

01:29 So those charges are balanced when we have three of that nitrate group.

01:35 Okay, now taking that.

01:37 And turning it into a complete ionic equation, the key is to separate anything that is aqueous.

01:44 Because when it's aqueous, when it's dissolved in water, it really doesn't exist as that compound.

01:48 It exists as a bunch of dissolved ions.

01:51 So let's go ahead and just start from left to right.

01:53 I have my nitric acid is aqueous.

01:56 So that really is going to exist as three aqueous hydrogen ions and three aqueous nitrate ions, right? because that three in front means we have three of both of those ions.

02:09 Now, solids, like the aluminum hydroxide, we do not split apart.

02:15 It's a solid compound.

02:18 Likewise, the water is a molecule.

02:22 It doesn't exist as ions.

02:25 But our aluminum nitrate does.

02:27 So we'll have aluminum, which is a positive three ion.

02:31 It's going to be aqueous.

02:32 And then we have those same three nitrate ions, which are also aqueous.

02:39 Now, so that's our complete, because complete.

02:42 Meaning it's showing all the ions that are there...

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