How could you use a precipitation reaction to separate each of the following pairs of anions? Write the formula for each reactant you would add, and write a balanced net ionic equation for each reaction. (a)

Video transcript

Hello everyone today. We have the following problem identify the reactant that you can use to separate the an ions acetate and hydroxide provide the chemical formula of the reaction and give the balanced net ionic equation. So this question has many different steps to it. So let's take it one at a time first. It's important to identify what we're working with. So we have acetate and hydroxy side with acetate. All acetate are soluble. So anything with an acetate will be soluble. And for hydro oxides they're going to be insoluble unless when they're paired with calcium, barium or strontium. Now that that's out of the way, we can go ahead and identify these separate reactant. So we have a reactant of strontium chloride. And so if we react strontium chloride in the aggregate swarm of course with our acetate. Also acquis we're going to form strontium acetate And two chloride ions. So as you said before, anything paired with struck with with acetate is going to be soluble And since chloride is a Group, one element, it is going to also be soluble. So we now need to pair strontium chloride with our hydroxide. So due to hydroxide ions of course and they will form strontium hydroxide Aquarius and two chloride ions once again we said that hydroxide are going to be soluble unless paired with strontium barium or calcium. And so this strontium is paired this hydroxide is paired up with strontium making it soluble. So we essentially have soluble and soluble to separate and ions. We are going to need something that is insoluble. So any answer choice that involves strontium chloride will be incorrect. And we can cross out answer choices A and B. Moving on to our second reactant, we have nickel nitrate N. 03 and I N 032. We're going to form nickel nitrate with our acetic or acetate. And of course user on the acquis form and it's a form nickel acetate and two nitrate ions. And so once again we said anything paired with acetate is going to be all soluble. And so lastly we're going to pair our nickel nitrate with our hydroxide. This is gonna give us a nickel hydroxide which will actually be a solid and form our precipitate. And so why does this form of precipitate? As we said before, hydroxide is only soluble when it is paired with calcium, barium and strontium intent. It is not in this situation, it is going to be insoluble, leaving us with answer choices C. Or D. To be correct. And so lastly we have barium nitrate. And so as routine as we did before we pair our barium nitrate with our acetate. And of course we get barium acetate Aquarius as well as to nitrate ions. We're then going to form or react barium nitrate with our hydroxide. This is going to form barium hydroxide of course and to nitrate ions and they're all nucleus. And so we said here that anything paired with hydroxide as a barium is going to be soluble and anything paired with acetate is going to be soluble as well. And so now we can focus on our nickel nitrate for our net ionic equation. So for our net ionic equation, we're going to do that down here three step three. Our net ionic equation, That's simply going to be what happens when we have our Nickel two plus in the acquis form Reacting with our two nitrate ions and our two hydroxide ions to yield nickel hydroxide and our two nitrate ions. And so if you notice here, we have two nitrates on the left and two nitrous on the right. That can be crossed out and we will be left with our final equation of nickel two plus Aquarius plus two hydroxide ions to give us a nickel hydroxide solid as our final answer. And with that we've answered the question overall, I hope this helped. And until next time.