Write a molecular equation for the precipitation reaction if...

Write a molecular equation for the precipitation reaction (if any) that occurs when the following solutions are mixed. If no reaction occurs, write "no reaction". Express your answer as a chemical equation. Enter "no reaction" if no precipitate is formed. Identify all of the phases in your answer. 1) Potassium chloride and lead(II) acetate 2) Chromium(III) nitrate and potassium phosphate

Transcript

00:01 Okay, so here we want to write the molecular equation for these precipitation reactions when solutions are mixed.

00:09 So for our first one, we have potassium chloride and lead to acetate.

00:14 So potassium chloride is kcl, and this is going to be an aqueous solution that's mixed, and it's going to be mixed with lead to acetate.

00:28 So lead is pb, and acetate is a negative 1 charge, so we'll need 2 acetate groups.

00:35 And this is also going to be aqueous.

00:45 Then we want to see what these products end up forming.

00:48 So we're going to do a double displacement.

00:50 So now the lead will be combined with the chlorine.

00:53 Chlorine has a minus one charge, so we'll need two chlorines to counteract lead's plus two charge.

00:58 And then we'll make potassium acetate.

01:05 Each of those have a minus one and plus one charge.

01:08 So we just need one of each.

01:11 So potassium acetates are soluble.

01:14 But lead chlorides, if we look at what, if we look at our solubility rules, chlorides are typically insoluble with lead.

01:22 So this is going to form a precipitation reaction and form a solid.

01:26 Then we want to go ahead and balance this equation.

01:29 So we see that we have two chlorines on the right -hand side and we'll need two on the left.

01:33 So we can put a two here.

01:35 And then doing that means we'll need two chlorines, or sorry, two potassiums on the right side as well.

01:42 So we can put a two in front of potassium.

01:44 Acetate...

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