Without Doing Any Calculations, Which Of The Following Aqueous Acids Is The Least Acidic? Assume All Act As Monoprotic Acids.A) Saccharin, $Ka = 2.1 \times 10^{-12}$B) Boric Acid, $Ka = 5.8 \times 10^{-10}$C) Lactic Acid, $Ka =
In the realm of chemistry, acids are substances that donate a proton (H+ ion) in a solution, resulting in a pH level lower than 7. The strength of an acid is often measured by its acid dissociation constant (Ka), which indicates the extent to which the acid dissociates in water. In this article, we will explore three aqueous acids - Saccharin, Boric acid, and Lactic acid - and determine which one is the least acidic based on their Ka values.
Understanding Acid Dissociation Constant (Ka)
The acid dissociation constant (Ka) is a measure of the strength of an acid. It is defined as the ratio of the concentration of the conjugate base to the concentration of the acid at equilibrium. A higher Ka value indicates a stronger acid, while a lower Ka value indicates a weaker acid.
The Three Aqueous Acids
Saccharin
Saccharin is a synthetic sweetener commonly used as a sugar substitute. It has a Ka value of 2.1 × 10^(-12). This value indicates that Saccharin is a very weak acid.
Boric Acid
Boric acid is a weak acid commonly used in various applications, including as an antiseptic and a pH buffer. It has a Ka value of 5.8 × 10^(-10). This value indicates that Boric acid is a relatively weak acid.
Lactic Acid
Lactic acid is a naturally occurring acid found in various foods, including milk and fruits. It has a Ka value of 1.4 × 10^(-4). This value indicates that Lactic acid is a relatively strong acid compared to the other two acids.
Determining the Least Acidic Aqueous Acid
Based on the Ka values of the three aqueous acids, we can determine which one is the least acidic. The acid with the lowest Ka value is the least acidic.
- Saccharin has a Ka value of 2.1 × 10^(-12), which is the lowest among the three acids.
- Boric acid has a Ka value of 5.8 × 10^(-10), which is higher than Saccharin's Ka value.
- Lactic acid has a Ka value of 1.4 × 10^(-4), which is higher than both Saccharin's and Boric acid's Ka values.
Therefore, Saccharin is the least acidic aqueous acid among the three.
Conclusion
In conclusion, the least acidic aqueous acid among Saccharin, Boric acid, and Lactic acid is Saccharin, with a Ka value of 2.1 × 10^(-12). This value indicates that Saccharin is a very weak acid and is the least acidic among the three.
References
- "Acid Dissociation Constant (Ka)" by Wikipedia
- "Saccharin" by Wikipedia
- "Boric Acid" by Wikipedia
- "Lactic Acid" by Wikipedia
Frequently Asked Questions (FAQs) About the Least Acidic Aqueous Acid ====================================================================
In our previous article, we determined that Saccharin is the least acidic aqueous acid among Saccharin, Boric acid, and Lactic acid. However, we understand that you may have more questions about this topic. In this article, we will address some of the frequently asked questions (FAQs) about the least acidic aqueous acid.
Q: What is the significance of the acid dissociation constant (Ka) in determining the acidity of an acid?
A: The acid dissociation constant (Ka) is a measure of the strength of an acid. It is defined as the ratio of the concentration of the conjugate base to the concentration of the acid at equilibrium. A higher Ka value indicates a stronger acid, while a lower Ka value indicates a weaker acid.
Q: Why is Saccharin considered the least acidic aqueous acid?
A: Saccharin is considered the least acidic aqueous acid because it has the lowest Ka value among the three acids. Its Ka value is 2.1 × 10^(-12), which is significantly lower than the Ka values of Boric acid (5.8 × 10^(-10)) and Lactic acid (1.4 × 10^(-4)).
Q: What are the applications of Saccharin?
A: Saccharin is a synthetic sweetener commonly used as a sugar substitute. It is also used in various applications, including as a food additive, a pharmaceutical ingredient, and a research chemical.
Q: How does the acidity of an acid affect its properties and behavior?
A: The acidity of an acid affects its properties and behavior in several ways. For example, a strong acid will completely dissociate in water, resulting in a high concentration of hydrogen ions (H+). This can lead to a decrease in pH, making the solution more acidic. On the other hand, a weak acid will only partially dissociate in water, resulting in a lower concentration of hydrogen ions (H+).
Q: Can the acidity of an acid be changed by altering its concentration?
A: Yes, the acidity of an acid can be changed by altering its concentration. For example, increasing the concentration of a weak acid will increase its acidity, while decreasing its concentration will decrease its acidity.
Q: How does the pH of a solution relate to the acidity of an acid?
A: The pH of a solution is a measure of its acidity or basicity. A pH of 7 is neutral, while a pH below 7 is acidic and a pH above 7 is basic. The acidity of an acid is directly related to its pH, with stronger acids having a lower pH and weaker acids having a higher pH.
Q: Can the acidity of an acid be changed by altering its temperature?
A: Yes, the acidity of an acid can be changed by altering its temperature. For example, increasing the temperature of a weak acid will increase its acidity, while decreasing its temperature will decrease its acidity.
Conclusion
In conclusion, the least acidic aqueous acid among Saccharin, Boric acid, and Lactic acid is Saccharin, with a Ka value of 2.1 × 10^(-12). We hope that this article has addressed some of the frequently asked questions (FAQs) about the least acidic aqueous acid and has provided a better understanding of the topic.
References
- "Acid Dissociation Constant (Ka)" by Wikipedia
- "Saccharin" by Wikipedia
- "Boric Acid" by Wikipedia
- "Lactic Acid" by Wikipedia