You may want to reference (Page) section 16.3 while completing this problem.
Write the formula for the conjugate acid of each of the following bases
The Correct Answer and Explanation is :
Answers:
- Conjugate Acid of NH₃ (Ammonia):
[
\text{NH}_4^+ (\text{Ammonium Ion})
] - Conjugate Acid of OH⁻ (Hydroxide Ion):
[
\text{H}_2\text{O} (\text{Water})
] - Conjugate Acid of CO₃²⁻ (Carbonate Ion):
[
\text{HCO}_3^- (\text{Bicarbonate Ion})
] - Conjugate Acid of HPO₄²⁻ (Hydrogen Phosphate Ion):
[
\text{H}_2\text{PO}_4^- (\text{Dihydrogen Phosphate Ion})
]
Explanation:
In acid-base chemistry, the conjugate acid of a base is formed by adding a proton (( H^+ )) to the base. This is based on the Brønsted-Lowry acid-base theory, which defines acids as proton donors and bases as proton acceptors.
1. NH₃ (Ammonia) → NH₄⁺ (Ammonium Ion)
Ammonia (( \text{NH}_3 )) is a weak base that can accept a proton to form ammonium ion (( \text{NH}_4^+ )). This process occurs in water and is common in biological and chemical systems:
[
\text{NH}_3 + H^+ \rightarrow \text{NH}_4^+
]
2. OH⁻ (Hydroxide Ion) → H₂O (Water)
Hydroxide ion (( \text{OH}^- )) is a strong base that readily accepts a proton to form neutral water:
[
\text{OH}^- + H^+ \rightarrow \text{H}_2\text{O}
]
This is one of the most fundamental acid-base reactions, forming the basis of pH and neutralization reactions.
3. CO₃²⁻ (Carbonate Ion) → HCO₃⁻ (Bicarbonate Ion)
Carbonate (( \text{CO}_3^{2-} )) is a polyatomic anion that can accept a proton to form the bicarbonate ion:
[
\text{CO}_3^{2-} + H^+ \rightarrow \text{HCO}_3^-
]
Bicarbonate is an important buffer in biological and environmental chemistry.
4. HPO₄²⁻ (Hydrogen Phosphate Ion) → H₂PO₄⁻ (Dihydrogen Phosphate Ion)
Hydrogen phosphate (( \text{HPO}_4^{2-} )) can accept a proton to form dihydrogen phosphate:
[
\text{HPO}_4^{2-} + H^+ \rightarrow \text{H}_2\text{PO}_4^-
]
This reaction plays a key role in the phosphate buffer system, important for maintaining pH in biological fluids.
These conjugate acids are essential in chemical equilibrium, buffer solutions, and biological systems, ensuring pH stability.
Here is the scientific illustration of acid-base conjugate pairs, visually representing the transformation of bases into their conjugate acids. Let me know if you need any modifications!
