Problem: Calculate the pH of the following solution.a. 0.12 M KNO2

FREE Expert Solution

We are asked to Calculate the pH of 0.12 M KNO2

KNO2 → K+ + NO2- 

  • NO2- → conjugate base of HNO2

ICE Chart: 

Calculate x: 

Kb = [HNO2][OH-][NO2-]KwKa = [HNO2][OH-][NO2-]1 × 10-147.2 × 10-4 = [x][x][0.12-x]

Kb is small so x is negligible in denominator. 

1 × 10-147.2 × 10-4 = [x][x][0.12]x2 = [1 × 10-14][0.12]7.2 × 10-4 x = [1 × 10-14][0.12]7.2 × 10-4 

[OH-] = x= 1.29 x10-6

Calculate pOH: 

pOH = -log[OH-]pOH = -log[1.29 ×10-6]

pOH = 5.89

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Problem Details

Calculate the pH of the following solution.

a. 0.12 M KNO2

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Our tutors have indicated that to solve this problem you will need to apply the Weak Bases concept. If you need more Weak Bases practice, you can also practice Weak Bases practice problems.

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

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Our data indicates that this problem or a close variation was asked in Chemistry: An Atoms First Approach - Zumdahl Atoms 1st 2nd Edition. You can also practice Chemistry: An Atoms First Approach - Zumdahl Atoms 1st 2nd Edition practice problems.