im studying for a test and i have no idea where to even start for this practice problem..??
a 0.15M(molarity im assuming)solution of BrCl2 contains..
a).15MBr2+ ions and .30M Cl- ions
b).30MBr2+ ions and .15M Cl- ions
c).15MBr2+ ions and .15M Cl- ions
d).30MBr2+ ions and .30M Cl- ions
can you show me how you get the answer? thanks
Actually the correct answer is not listed. I would expect BrCl2 to be a covalent compound; therefore, it would not consist of ions. It's polar covalent, to be sure, but surely not ionic. However, I think the answer is a).
0.15M XY2 (if ionic) would consist of 0.15 M X^+ ions (there is 1 X^+ ion per molecule of XY2 and 1*0.15 = 0.15) and 0.30 M Y (there are two Y^- ions per molecule of XY2 and 2*0.15 = 0.30).
Sure! Let's break down the problem and figure out how to solve it step by step.
1. The given information is that we have a 0.15 M solution of BrCl2.
2. BrCl2 is a covalent compound. However, when it dissolves in water, it dissociates into ions, specifically Br2+ and Cl- ions.
3. The question is asking us to determine the concentration of each ion in the solution.
To solve this problem, we need to understand the concept of molarity and how it relates to the dissociation of the compound.
Molarity (M) is a measure of concentration defined as the number of moles of a solute dissolved in one liter of solution. In other words, it tells us the number of moles of the solute present per liter of solution.
To find the concentration of the ions, we need to consider the ratio of the ions produced when the compound dissociates.
The compound BrCl2 dissociates as follows:
BrCl2 → Br2+ + 2Cl-
Based on the coefficients in the balanced equation, we can see that for each BrCl2 molecule that dissociates, we get one Br2+ ion and two Cl- ions.
Since the concentration of BrCl2 is given as 0.15 M, we know that for every 1 liter of the solution, we have 0.15 moles of BrCl2. This means that we will have the same number of moles of Br2+ ions and 2 times that number of moles of Cl- ions.
To find the concentration of each ion, we can multiply the concentration of BrCl2 by the stoichiometric coefficients of the ions.
Concentration of Br2+ ions = 0.15 M x 1 = 0.15 M
Concentration of Cl- ions = 0.15 M x 2 = 0.30 M
So, the correct answer is option a): 0.15 M Br2+ ions and 0.30 M Cl- ions.
Remember, the key steps to solving this problem were:
1. Understanding that BrCl2 dissociates into Br2+ and Cl- ions.
2. Recognizing the stoichiometric coefficients in the balanced equation to determine the ratio of ions.
3. Using the concentration of BrCl2 to calculate the concentration of each ion.
I hope this helps you solve similar problems in the future! Let me know if you have any other questions.