Refer to the figure to answer questions 4 and 5. The images are a molecular representation of three different substances, AX3, AY3, and AZ3, dissolved in water. (Water molecules are omitted for clarity.) What are the molar concentrations of A ions and X ions in a 0.500 M solution of AX3? (LO 4.7) (a) 0.500 M A and 0.500 M X (b) 0.500 M A and 0.167 M X (c) 1.500 M A and 0.500 M X (d) 0.500 M A and 1.500 M X

Video transcript

Hello everyone today. We have the following question, calculate the polarity of each ion and a . 00 Bowler, B. Y. two Solution. And this is a made up chemical formula. So first we want to show this compound dissociating. So we're going to take our starting material, our B. Y two. And we're going to show it dissociating into one B plus acquis ion and two y minus ions. We then can calculate the polarity of each individual ion. So for our B two plus we're going to take the polarity Shared here are .4 Polarity which would be equal to . moles over one leader. Since the unit for morality is moles over leader. And we could then multiply this by our one mole of B two plus is equal to R one mole and B. Y two. So for every one mole of B Y two we have one mole of B. Meaning that whenever you see B. Y two, you only have one B adam present. And so when these units cross out we're left with 10. polarity of B two plus. Now for our why minus? We're going to take that polarity which is once again 0.4 moles of B. Y 2/1 leader. And for every one mole for every one mole of our B. Y two we have two moles of our Y two or y minus. And so when our units cancel we are left with .8 polarity of our Y -. And these are going to be our answers Overall. I hope this helped until next time