Problem: A 500.0-mL buffer solution is 0.100 M in HNO2 and 0.150 M in KNO2. Determine whether or not 250 mg NaOH would exceed the capacity of the buffer to neutralize it.

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FREE Expert Solution

(1) Recall the Henderson-Hasselbalch equation:

pH=pKa+logconjugate baseweak acidpH=pKa+log[KNO2][HNO2]pH=3.33+log0.150.10

pH = 3.5

(2) Calculating for the moles of NaOH, HNO2 and KNO2

mol NaOH= 0.25 g39.996 g/mol

mol NaOH = 0.0063 moles

mol HNO2 = (0.1 M) (0.5 L) = 0.050 moles

mol KNO2 = (0.15 M) (0.5 L) = 0.075 moles

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Problem Details

A 500.0-mL buffer solution is 0.100 M in HNO2 and 0.150 M in KNO2. Determine whether or not 250 mg NaOH would exceed the capacity of the buffer to neutralize it.

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What professor is this problem relevant for?

Based on our data, we think this problem is relevant for Professor Paesani's class at UCSD.