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A buffer with a ph of 9.85 contains ch3nh2and ch3nh3cl in water. what can you conclude about the relative concentrations of ch3nh2and ch3nh3cl in this buffer? for ch3nh2, pkb= 3.36.
a.ch3nh2 > ch3nh3cl
b.ch3nh2 c.ch3nh2 = ch3nh3cld) nothing can be concluded about the relative concentrations of ch3nh2 and ch3nh3cl.

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ChemistryHelper2024
pH = 9.85
so pOH = 14 - pH = 4.15
As the solution is basic buffer,
pOH = pKb + log [tex] \frac{[conjugate acid]}{[base]} [/tex]
4.15 = 3.36 + log [tex] \frac{[CH_{3}NH_{3}Cl]}{[CH_{3}NH_{2}]} [/tex]
so:
[tex] \frac{[CH_3NH_3Cl ]}{[CH_3NH_2]} = 6.16 [/tex]
∴ [CH₃NH₃Cl] > [CH₃NH₂]

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