We’re being asked to calculate the molarity (M) of lithium ions (Li+) in 4.57 L of 2.35 M Li3P solution. Recall that molarity is the ratio of the moles of solute and the volume of solution (in liters). In other words:
Since the Li3P is an ionic compound, it forms ions when dissociating in water. The dissociation of Li3P in water is as follows:
Li3P(s) → 3 Li+(aq) + P–3(aq)
What is the concentration (M) of lithium ions in 4.57 L of a 2.35 M Li 3P solution?
a. 45.0 M
b. 14.1 M
c. 2.35 M
d. 7.05 M
e. 99.0 M
Frequently Asked Questions
What scientific concept do you need to know in order to solve this problem?
Our tutors have indicated that to solve this problem you will need to apply the Molarity concept. You can view video lessons to learn Molarity. Or if you need more Molarity practice, you can also practice Molarity practice problems.
What is the difficulty of this problem?
Our tutors rated the difficulty ofWhat is the concentration (M) of lithium ions in 4.57 L of a...as medium difficulty.
How long does this problem take to solve?
Our expert Chemistry tutor, Dasha took 3 minutes and 17 seconds to solve this problem. You can follow their steps in the video explanation above.
What professor is this problem relevant for?
Based on our data, we think this problem is relevant for Professor Bushey's class at TOWSON.