The weak base-conjugate acid buffer used in this laboratory consists of a weak base ammonia, NH3, and its conjugate acid ammonium chloride, NH4Cl. If the NH3 concentration is 0.05 M and the NH4Cl concentration is 0.05 M, what is the pH of the buffer? Kb for NH3 is 1.8*10^-5

asked by E

15 years ago

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1 answer

Use the Henderson-Hasselbalch equation.
base = 0.05 M
acid = 0.05 M

answered by DrBob222

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Question

The weak base-conjugate acid buffer used in this laboratory consists of a weak base ammonia, NH3, and its conjugate acid ammonium chloride, NH4Cl. If the NH3 concentration is 0.05 M and the NH4Cl concentration is 0.05 M, what is the pH of the buffer? Kb for NH3 is 1.8*10^-5

1 answer

Use the Henderson-Hasselbalch equation.
base = 0.05 M
acid = 0.05 M

DrBob222 · Answer

Use the Henderson-Hasselbalch equation. base = 0.05 M acid = 0.05 M