Problem: Determine the pH of a solution that is 3.65% KOH by mass. Assume that the solution has density of 1.01 g / mL.
FREE Expert Solution
We’re being asked to calculate the pH of a solution that is of 3.65% KOH by mass. Assume that the solution has density of 1.01 g/mL.
KOH is a strong base.
Remember that strong bases completely dissociate in water and that bases accept H+ from the acid (water in this case).
The dissociation of KOH is as follows:
KOH (aq) ⇌ K+ (aq) + OH-(aq)
For strong base, an ICE table is not necessary because it can be assumed that all of the acid or base will dissociate.
The concentration of the strong base is the same as its dissociated particles.
Determine the pH of a solution that is 3.65% KOH by mass. Assume that the solution has density of 1.01 g / mL.
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 Strong Acid-Base Calculations concept. If you need more Strong Acid-Base Calculations practice, you can also practice Strong Acid-Base Calculations practice problems .
What professor is this problem relevant for?
Based on our data, we think this problem is relevant for Professor Billman's class at Abilene Christian University.