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

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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)


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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