Problem: Find [OH−] of a 0.33 M methylamine (CH3NH2) solution. (Methylamine has a Kb value of 4.4×10−4.) Express the concentration in moles per liter to two significant figures.Find the pH of the 0.33 M methylamine (CH3NH2) solution. Express the pH of the solution to two decimal places

FREE Expert Solution

Step 1

Step 2

Kb =[CH3NH3+][OH-][CH3NH2]Kb =(x)(x)0.33 - xKb =x20.33 - x


[CH3NH2]initialKb =0.334.4×10-4 > 500→ remove (-x)


92% (277 ratings)
View Complete Written Solution
Problem Details

Find [OH] of a 0.33 M methylamine (CH3NH2) solution. (Methylamine has a Kb value of 4.4×10−4.) Express the concentration in moles per liter to two significant figures.

Find the pH of the 0.33 M methylamine (CH3NH2) solution. Express the pH of the solution to two decimal places

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.