Question #0a80d
1 Answer
- 46:
#K_(sp) = 1.1 * 10^-38# - 47:
#x = 1.3 * 10^-4 M# - 48:
#x = 0.0012 M#
Explanation:
- #46:
The first step to solving molar solubility problems is always to write down the balanced chemical equation of what's going on.
This would be:
Therefore the expression for
Setting up an ICE table would give you:
Note: Watch your parentheses when simplifying these expressions
Now, the jump to take with all such problems is to realize that
You're given a molar solubility, so all you need to do is plug and chug:
- #47:
Again, same process of setting up the expression:
By ICE Table:
The
- #48:
This problem is exactly the same process as the previous one, except with a different reaction:
By ICE Table:
The
To better understand what is exactly going on here, I'd recommend you watch these two videos.
Video 1 (Introduction to
Video 2 (Examples)
Hope that helps :)