Textbook Question
Which of the following are not acids?
CH3COOH, CO2 , HNO2 , HCOOH, CCl4
3. Acids and Bases
Acids and Bases
2:39 minutesProblem 4b
Textbook Question
What is the conjugate base of each of the following?
1. NH3
2. HBr
3. HNO3
4. H2O
Verified step by step guidance1
Step 1: Understand the concept of a conjugate base. A conjugate base is formed when an acid donates a proton (H⁺). The conjugate base will have one less hydrogen atom and a negative charge compared to the original acid.
Step 2: For NH₃ (ammonia), identify the acid and remove one proton (H⁺). The conjugate base will be NH₂⁻. This is because NH₃ loses a hydrogen atom and gains a negative charge.
Step 3: For HBr (hydrobromic acid), remove one proton (H⁺) from the molecule. The conjugate base will be Br⁻, as HBr loses its hydrogen atom and becomes negatively charged.
Step 4: For HNO₃ (nitric acid), remove one proton (H⁺) from the molecule. The conjugate base will be NO₃⁻, as HNO₃ loses its hydrogen atom and gains a negative charge.
Step 5: For H₂O (water), remove one proton (H⁺) from the molecule. The conjugate base will be OH⁻, as H₂O loses a hydrogen atom and becomes negatively charged.
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Video duration:
2mKey Concepts
Here are the essential concepts you must grasp in order to answer the question correctly.
Conjugate Acid-Base Theory
The conjugate acid-base theory, developed by Brønsted and Lowry, defines acids as proton donors and bases as proton acceptors. When an acid donates a proton (H+), it forms its conjugate base, while the base that accepts the proton becomes its conjugate acid. Understanding this relationship is crucial for identifying conjugate pairs in chemical reactions.
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Ammonia (NH3) and its Conjugate Base
Ammonia (NH3) acts as a weak base in aqueous solutions. When it accepts a proton, it forms its conjugate acid, ammonium (NH4+). The conjugate base of ammonia, however, is the amide ion (NH2-), which is formed when ammonia donates a proton. Recognizing this transformation is essential for solving the question.
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Strong Acids and Their Conjugate Bases
Strong acids, such as HBr and HNO3, completely dissociate in water, meaning they donate protons readily. The conjugate bases of strong acids are typically very weak and have negligible basicity. For example, the conjugate base of HBr is bromide ion (Br-), and for HNO3, it is nitrate ion (NO3-). Understanding the strength of acids and their corresponding conjugate bases is vital for this question.
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