Calculating the pH of a Strong Base Solution

Oct 13, 2025 by pinkandtrash.com 83 views

Introduction

pH is a measure of the concentration of hydrogen ions in a solution, and it plays a crucial role in various chemical reactions. In this article, we will discuss the pH of a 0.014 M Ca(OH)2 solution. Calcium hydroxide, also known as slaked lime, is a strong base that completely dissociates in water to produce calcium ions and hydroxide ions. Understanding the pH of a Ca(OH)2 solution is essential in various fields, including chemistry, biology, and environmental science.

The pH Scale

The pH scale is a measure of the concentration of hydrogen ions in a solution, ranging from 0 to 14. A pH of 7 is considered neutral, while a pH less than 7 is acidic and a pH greater than 7 is basic. The pH scale is logarithmic, meaning that each unit change represents a tenfold change in the concentration of hydrogen ions.

The Strong Base Ca(OH)2

Calcium hydroxide, Ca(OH)2, is a strong base that completely dissociates in water to produce calcium ions (Ca2+) and hydroxide ions (OH-). The dissociation reaction is as follows:

Ca(OH)2 (s) → Ca2+ (aq) + 2OH- (aq)

Calculating the pH of a Strong Base Solution

To calculate the pH of a strong base solution, we can use the formula:

pH = -log[OH-]

where [OH-] is the concentration of hydroxide ions in moles per liter (M).

Calculating the Concentration of Hydroxide Ions

Since Ca(OH)2 is a strong base, it completely dissociates in water to produce calcium ions and hydroxide ions. Therefore, the concentration of hydroxide ions is twice the concentration of calcium ions. Given that the concentration of Ca(OH)2 is 0.014 M, the concentration of hydroxide ions is:

[OH-] = 2 × [Ca(OH)2] = 2 × 0.014 M = 0.028 M

Calculating the pH of the Solution

Now that we have the concentration of hydroxide ions, we can calculate the pH of the solution using the formula:

pH = -log[OH-] = -log(0.028) = 1.55

Conclusion

In conclusion, the pH of a 0.014 M Ca(OH)2 solution is 1.55. This is because Ca(OH)2 is a strong base that completely dissociates in water to produce calcium ions and hydroxide ions, resulting in a high concentration of hydroxide ions and a low pH.

Frequently Asked Questions

Q: What is the pH of a 0.014 M Ca(OH)2 solution? A: The pH of a 0.014 M Ca(OH)2 solution is 1.55.
Q: Why is Ca(OH)2 a strong base? A: Ca(OH)2 is a strong base because it completely dissociates in water to produce calcium ions and hydroxide ions.
Q: How do you calculate the pH of a strong base solution? A: To calculate the pH of a strong base solution, you can use the formula: pH = -log[OH-], where [OH-] is the concentration of hydroxide ions in moles per liter (M).

References

"Chemistry: The Central Science" by Theodore L. Brown, H. Eugene LeMay, Jr., and Bruce E. Bursten
"General Chemistry: Principles and Modern Applications" by Linus Pauling
"Chemical Principles: The Quest for Insight" by Steven S. Zumdahl

Introduction

In our previous article, we discussed the pH of a 0.014 M Ca(OH)2 solution. Calcium hydroxide, also known as slaked lime, is a strong base that completely dissociates in water to produce calcium ions and hydroxide ions. Understanding the pH of a Ca(OH)2 solution is essential in various fields, including chemistry, biology, and environmental science. In this article, we will answer some frequently asked questions about the pH of a 0.014 M Ca(OH)2 solution.

Q&A

Q: What is the pH of a 0.014 M Ca(OH)2 solution?

A: The pH of a 0.014 M Ca(OH)2 solution is 1.55.

Q: Why is Ca(OH)2 a strong base?

A: Ca(OH)2 is a strong base because it completely dissociates in water to produce calcium ions and hydroxide ions.

Q: How do you calculate the pH of a strong base solution?

A: To calculate the pH of a strong base solution, you can use the formula: pH = -log[OH-], where [OH-] is the concentration of hydroxide ions in moles per liter (M).

Q: What is the concentration of hydroxide ions in a 0.014 M Ca(OH)2 solution?

A: Since Ca(OH)2 is a strong base, it completely dissociates in water to produce calcium ions and hydroxide ions. Therefore, the concentration of hydroxide ions is twice the concentration of calcium ions. Given that the concentration of Ca(OH)2 is 0.014 M, the concentration of hydroxide ions is:

[OH-] = 2 × [Ca(OH)2] = 2 × 0.014 M = 0.028 M

Q: How does the pH of a Ca(OH)2 solution change with concentration?

A: The pH of a Ca(OH)2 solution changes with concentration. As the concentration of Ca(OH)2 increases, the concentration of hydroxide ions also increases, resulting in a higher pH.

Q: What are some common applications of Ca(OH)2?

A: Ca(OH)2 has several common applications, including:

Water treatment: Ca(OH)2 is used to remove impurities and contaminants from water.
Construction: Ca(OH)2 is used as a cement additive to improve its strength and durability.
Agriculture: Ca(OH)2 is used as a soil conditioner to improve soil fertility and structure.

Q: What are some safety precautions when handling Ca(OH)2?

A: When handling Ca(OH)2, it is essential to wear protective gear, including gloves, goggles, and a mask. Ca(OH)2 can cause skin and eye irritation, and inhalation of its dust can lead to respiratory problems.

Conclusion

In conclusion, understanding the pH of a 0.014 M Ca(OH)2 solution is essential in various fields, including chemistry, biology, and environmental science. By answering some frequently asked questions, we hope to provide a better understanding of the pH of a Ca(OH)2 solution and its applications.

Frequently Asked Questions

Q: What is the pH of a 0.014 M Ca(OH)2 solution? A: The pH of a 0.014 M Ca(OH)2 solution is 1.55.
Q: Why is Ca(OH)2 a strong base? A: Ca(OH)2 is a strong base because it completely dissociates in water to produce calcium ions and hydroxide ions.
Q: How do you calculate the pH of a strong base solution? A: To calculate the pH of a strong base solution, you can use the formula: pH = -log[OH-], where [OH-] is the concentration of hydroxide ions in moles per liter (M).

References

"Chemistry: The Central Science" by Theodore L. Brown, H. Eugene LeMay, Jr., and Bruce E. Bursten
"General Chemistry: Principles and Modern Applications" by Linus Pauling
"Chemical Principles: The Quest for Insight" by Steven S. Zumdahl