a buffer with PH of 9.85 contains CH3NH2 and CH3NH3Cl in water. what can you conclude about the relative concentrations of CH3NH2 and CH3NH3Cl in this buffer
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pH = 9.85
pH + pOH = 14
pOH = 14 - pH
pOH = 14 - 9.85 = 4.15
The solution will be basic buffer.
As,
pOH = pKb + log [ conjugate acid / base ]
4.15 = 3.36 + log [ CH3 NH3 Cl / CH3 NH2 ]
[ CH3 NH3 Cl / CH3 NH2 ] = 6.16
CH3 NH3 Cl > CH3 NH2
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