We’re being asked to calculate the equilibrium concentration of the hydroxide ion (OH-) in a 0.150 M C6H5NH2 solution.
To solve this problem, we need to:
Step 1. Determine the dissociation of the base in water.
Step 2. Construct the ICE chart.
Step 3. Determine the equilibrium concentration of OH-
Step 1. Since C6H5NH2 has a low Kb value, it’s a weak base. Remember that weak bases partially dissociate in water and that bases accept H+ from the acid (water in this case). The dissociation of C6H5NH2 is as follows:
Aniline, C6H5NH2, is a weak base that dissociates in water. At 25 °Celsius, the base dissociation constant, Kb , for aniline is 4.3 x 10 -10.
(A) Determine the hydroxide ion concentration and the percentage dissociation of a 0.150 molar solution of aniline at 25 °Celsius.
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 Weak Bases concept. If you need more Weak Bases practice, you can also practice Weak Bases practice problems.
What professor is this problem relevant for?
Based on our data, we think this problem is relevant for Professor Jones' class at University of Guelph.