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1. Chemical Measurements1h 50m
2. Tools of the Trade1h 17m
3. Experimental Error1h 52m
4 & 5. Statistics, Quality Assurance and Calibration Methods1h 57m
6. Chemical Equilibrium3h 41m
7. Activity and the Systematic Treatment of Equilibrium1h 0m
8. Monoprotic Acid-Base Equilibria1h 53m
9. Polyprotic Acid-Base Equilibria2h 17m
10. Acid-Base Titrations2h 37m
11. EDTA Titrations1h 34m
12. Advanced Topics in Equilibrium1h 16m
13. Fundamentals of Electrochemistry2h 19m
14. Electrodes and Potentiometry41m
15. Redox Titrations1h 14m
16. Electroanalytical Techniques57m
17. Fundamentals of Spectrophotometry50m

8. Monoprotic Acid-Base Equilibria

Buffers

Analytical Chemistry

8. Monoprotic Acid-Base Equilibria

Buffers

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Multiple Choice

Which of the following molar ratios is the correct equilibrium ratio of BASE : ACID for a solution made of aniline (Kb = 3.8 x 10^-10) and anilinium nitrate where the pH is 4.80?

1:2

3:5

7:2

2:1

5:3

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Verified step by step guidance

First, understand that aniline is a weak base and anilinium nitrate is its conjugate acid. The equilibrium involves the base (aniline) and its conjugate acid (anilinium ion).

Use the Henderson-Hasselbalch equation for a base: \( \text{pOH} = \text{pK}_b + \log \left( \frac{[\text{conjugate acid}]}{[\text{base}]} \right) \).

Calculate the pOH from the given pH: \( \text{pOH} = 14 - \text{pH} = 14 - 4.80 = 9.20 \).

Determine the \( \text{pK}_b \) from the given \( K_b \): \( \text{pK}_b = -\log(3.8 \times 10^{-10}) \).

Substitute the values into the Henderson-Hasselbalch equation and solve for the ratio \( \frac{[\text{conjugate acid}]}{[\text{base}]} \) to find the correct equilibrium ratio.