Calculating the pH of the Resulting Solution

Oct 13, 2025 by talynt.org 18 views

Introduction

Titration is a fundamental technique in chemistry used to determine the concentration of a substance in a solution. In this article, we will explore the titration of a polyprotic acid, specifically 70.0 mL of 0.10 M H3A, with 0.10 M KOH. We will calculate the pH of the resulting solution at 175 mL of KOH added.

Theoretical Background

H3A is a polyprotic acid with three dissociable protons. Its dissociation constants are given as Ka1 = 7.7 × 10^−4, Ka2 = 1.0 × 10^−8, and Ka3 = 8.8 × 10^−11. The dissociation of H3A can be represented by the following equations:

H3A ⇌ H+ + H2A^− (Ka1) H2A^− ⇌ H+ + HA2^−− (Ka2) HA2^−− ⇌ H+ + A3^−−− (Ka3)

Calculating the pH of the Resulting Solution

To calculate the pH of the resulting solution, we need to consider the amount of KOH added and the resulting concentration of H3A. At 175 mL of KOH added, the total volume of the solution is 245 mL (70.0 mL of H3A + 175 mL of KOH).

The number of moles of KOH added can be calculated as follows:

moles KOH = Molarity × Volume (L) moles KOH = 0.10 M × 0.175 L moles KOH = 0.0175 mol

Since KOH is a strong base, it completely dissociates in water to produce OH^− ions. The concentration of OH^− ions can be calculated as follows:

[OH^−] = moles KOH / Total Volume (L) [OH^−] = 0.0175 mol / 0.245 L [OH^−] = 0.0714 M

The pOH of the solution can be calculated using the following equation:

pOH = -log[OH^−] pOH = -log(0.0714) pOH = 1.15

The pH of the solution can be calculated using the following equation:

pH = 14 - pOH pH = 14 - 1.15 pH = 12.85

Discussion

The pH of the resulting solution is 12.85, which is slightly basic. This is due to the presence of OH^− ions produced by the dissociation of KOH. The pH of the solution is also influenced by the dissociation of H3A, which produces H+ ions.

Conclusion

In conclusion, the titration of 70.0 mL of 0.10 M H3A with 0.10 M KOH results in a solution with a pH of 12.85 at 175 mL of KOH added. This calculation demonstrates the importance of considering the dissociation constants of polyprotic acids in titration calculations.

Calculating the Number of Moles of H3A

To calculate the number of moles of H3A, we need to know the initial volume and molarity of H3A.

moles H3A = Molarity × Volume (L) moles H3A = 0.10 M × 0.070 L moles H3A = 0.007 mol

Calculating the Concentration of H3A

The concentration of H3A can be calculated as follows:

[H3A] = moles H3A / Total Volume (L) [H3A] = 0.007 mol / 0.245 L [H3A] = 0.0286 M

Calculating the pH of the Resulting Solution Using the Henderson-Hasselbalch Equation

The Henderson-Hasselbalch equation can be used to calculate the pH of the resulting solution:

pH = pKa + log([A^−]/[HA]) pH = pKa1 + log([H2A^−]/[H3A])

To calculate the pH of the resulting solution, we need to know the concentrations of H2A^− and H3A.

[H2A^−] = [H3A] × (Ka1 / (Ka1 + Ka2)) [H2A^−] = 0.0286 M × (7.7 × 10^−4 / (7.7 × 10^−4 + 1.0 × 10^−8)) [H2A^−] = 0.0286 M × 0.9999 [H2A^−] = 0.0286 M

[H3A] = 0.0286 M

pH = pKa1 + log([H2A^−]/[H3A]) pH = -log(7.7 × 10^−4) + log(0.0286/0.0286) pH = 3.11 + 0 pH = 3.11

Conclusion

In conclusion, the pH of the resulting solution can be calculated using the Henderson-Hasselbalch equation. The pH of the solution is 3.11, which is slightly acidic.

Calculating the pH of the Resulting Solution Using the Titration Curve

The titration curve can be used to calculate the pH of the resulting solution. The titration curve is a plot of pH against the volume of KOH added.

The pH of the resulting solution can be calculated as follows:

pH = 14 - pOH pH = 14 - log(0.0714) pH = 14 - 1.15 pH = 12.85

Conclusion

In conclusion, the pH of the resulting solution can be calculated using the titration curve. The pH of the solution is 12.85, which is slightly basic.

Calculating the pH of the Resulting Solution Using the Quadratic Equation

The quadratic equation can be used to calculate the pH of the resulting solution.

The quadratic equation is:

x^2 + bx + c = 0

where x is the pH of the resulting solution, b is the sum of the dissociation constants, and c is the product of the dissociation constants.

The quadratic equation can be written as:

pH^2 + (pKa1 + pKa2 + pKa3) × pH + pKa1 × pKa2 × pKa3 = 0

The pH of the resulting solution can be calculated as follows:

pH = (-b ± √(b^2 - 4ac)) / 2a

where a = 1, b = pKa1 + pKa2 + pKa3, and c = pKa1 × pKa2 × pKa3.

The pH of the resulting solution can be calculated as follows:

pH = (-(-3.11 + 1.15 + 10.95) ± √((-3.11 + 1.15 + 10.95)^2 - 4 × 1 × 7.7 × 10^−4 × 1.0 × 10^−8 × 8.8 × 10^−11)) / 2 pH = (-12.85 ± √((-12.85)^2 - 4 × 1 × 7.7 × 10^−4 × 1.0 × 10^−8 × 8.8 × 10^−11)) / 2 pH = (-12.85 ± √(164.22 - 3.43 × 10^−11)) / 2 pH = (-12.85 ± √164.22) / 2 pH = (-12.85 ± 12.86) / 2 pH = 0.005 or 12.85

The pH of the resulting solution is 12.85, which is slightly basic.

Conclusion

Q: What is titration and why is it important in chemistry?

A: Titration is a laboratory technique used to determine the concentration of a substance in a solution. It involves the addition of a known amount of a reagent to a solution containing the substance to be analyzed, until a specific endpoint is reached. Titration is an important technique in chemistry because it allows us to accurately determine the concentration of a substance, which is essential in many fields such as medicine, environmental science, and industry.

Q: What is a polyprotic acid and how does it differ from a monoprotic acid?

A: A polyprotic acid is an acid that can donate more than one proton (H+ ion) per molecule. In contrast, a monoprotic acid can only donate one proton per molecule. Polyprotic acids are also known as polybasic acids. H3A is an example of a polyprotic acid, as it can donate three protons per molecule.

Q: What is the Henderson-Hasselbalch equation and how is it used in titration calculations?

A: The Henderson-Hasselbalch equation is a mathematical formula used to calculate the pH of a solution containing a weak acid and its conjugate base. It is given by the equation:

pH = pKa + log([A^−]/[HA])

where pH is the pH of the solution, pKa is the acid dissociation constant, [A^−] is the concentration of the conjugate base, and [HA] is the concentration of the weak acid.

Q: How is the pH of a solution calculated using the Henderson-Hasselbalch equation?

A: To calculate the pH of a solution using the Henderson-Hasselbalch equation, we need to know the concentrations of the weak acid and its conjugate base. We can then plug these values into the equation and solve for pH.

Q: What is the significance of the dissociation constants (Ka) in titration calculations?

A: The dissociation constants (Ka) are a measure of the strength of an acid. A higher Ka value indicates a stronger acid, while a lower Ka value indicates a weaker acid. In titration calculations, the Ka values are used to determine the pH of a solution at different stages of the titration.

Q: How is the pH of a solution calculated using the titration curve?

A: The titration curve is a plot of pH against the volume of a reagent added to a solution. To calculate the pH of a solution using the titration curve, we need to know the volume of the reagent added and the pH of the solution at that point. We can then use the titration curve to determine the pH of the solution.

Q: What is the significance of the quadratic equation in titration calculations?

A: The quadratic equation is a mathematical formula used to calculate the pH of a solution at different stages of the titration. It is given by the equation:

pH^2 + (pKa1 + pKa2 + pKa3) × pH + pKa1 × pKa2 × pKa3 = 0

where pH is the pH of the solution, pKa1, pKa2, and pKa3 are the acid dissociation constants, and pKa1 × pKa2 × pKa3 is the product of the acid dissociation constants.

Q: How is the pH of a solution calculated using the quadratic equation?

A: To calculate the pH of a solution using the quadratic equation, we need to know the acid dissociation constants (pKa1, pKa2, and pKa3) and the pH of the solution at different stages of the titration. We can then plug these values into the equation and solve for pH.

Q: What are the limitations of the Henderson-Hasselbalch equation in titration calculations?

A: The Henderson-Hasselbalch equation is a simplified equation that assumes a weak acid and its conjugate base are present in equal concentrations. However, in real-world titration calculations, the concentrations of the weak acid and its conjugate base may not be equal. In such cases, the Henderson-Hasselbalch equation may not provide accurate results.

Q: What are the limitations of the titration curve in titration calculations?

A: The titration curve is a graphical representation of the pH of a solution against the volume of a reagent added. However, the titration curve may not provide accurate results if the pH of the solution is not measured at regular intervals.

Q: What are the limitations of the quadratic equation in titration calculations?

A: The quadratic equation is a mathematical formula used to calculate the pH of a solution at different stages of the titration. However, the quadratic equation may not provide accurate results if the acid dissociation constants (pKa1, pKa2, and pKa3) are not known accurately.

Conclusion

In conclusion, titration is an important technique in chemistry that allows us to accurately determine the concentration of a substance in a solution. The Henderson-Hasselbalch equation, titration curve, and quadratic equation are all useful tools in titration calculations. However, each of these tools has its limitations, and the choice of which tool to use depends on the specific requirements of the titration calculation.