What is the conjugate acid of each of the following? 1. NH 3 2. Cl − 3. HO − 4. H 2 O

Alright. Hi, everyone. So for this question, let's draw the conjugate acid for the below given species. And before we do that, let's go ahead and recall a few things about um the Bronson Lowry as a base theory. So recall that according to the Bronston Lowry theory, acids are chemical species that donate protons. And by contrast, bases are chemical species that accept protons. So there's kind of a back and forth there. And in order to figure out the conjugate acid of a base or the conjugate base of an acid, I like to kind of treat it as a formula. So if we start with our acids, if we take our acid and we go ahead and we subtract a proton from it, we end up with our conjugate base. So this is going to be our conjugate base and we can do the same thing or a similar thing with our base because we can take our base and we can add a proton to it to come up with our conjugate acid. So now because we have to figure out the conjugate acids for each of the species that were given, let's go ahead and let's add a proton to each of them, right. So if we start with our bromide in part A, when we add a proton to that, we end up with HBR, we end up with HBR and recall that when you add a proton to a chemical species, you're increasing its charge by plus one. So we're going from a charge of minus one in our bromide to a charge of zero or neutral charge in HBR the conjugate acid. So let's go ahead and let's do the same thing with our N H two minus. Let's add our proton. And let's give that nitrogen An additional hydrogen making it NH three. And similarly to bromide, here are charges increased from -1-0 after adding a proton to it. So our NH three is going to be neutral. And, and now for our H C 03 minus, let's go ahead and add a proton, right? And that's gonna give us H two C 03 because we're going from one hydrogen to two hydrogen in our molecule And are starting charge was once again -1. So we have neutral charge um by the end of this process, after adding our proton and last but not least, let's add our proton here to H S minus to generate H two S. And once again, our charge has increased from -1-0. So these are going to be your four conjugate acid here and we determined that by going ahead and adding a proton to each base that we are given. So this is going to correspond to choice a within the multiple choice. And so with that being said, thank you very much for watching. And I hope you found this helpful.

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1. A Review of General Chemistry5h 5m
2. Molecular Representations1h 14m
3. Acids and Bases2h 46m
4. Alkanes and Cycloalkanes4h 17m
5. Chirality3h 39m
6. Thermodynamics and Kinetics1h 22m
7. Substitution Reactions1h 48m
8. Elimination Reactions2h 30m
9. Alkenes and Alkynes2h 9m
10. Addition Reactions3h 19m
11. Radical Reactions1h 58m
12. Alcohols, Ethers, Epoxides and Thiols2h 42m
13. Alcohols and Carbonyl Compounds2h 17m
14. Synthetic Techniques1h 26m
15. Analytical Techniques:IR, NMR, Mass Spect7h 3m
16. Conjugated Systems6h 13m
17. Ultraviolet Spectroscopy51m
18. Aromaticity2h 34m
19. Reactions of Aromatics: EAS and Beyond5h 1m
20. Phenols55m
21. Aldehydes and Ketones: Nucleophilic Addition4h 56m
22. Carboxylic Acid Derivatives: NAS2h 51m
23. The Chemistry of Thioesters, Phophate Ester and Phosphate Anhydrides1h 10m
24. Enolate Chemistry: Reactions at the Alpha-Carbon1h 53m
25. Condensation Chemistry2h 9m
26. Amines1h 43m
27. Heterocycles2h 0m
28. Carbohydrates5h 53m
29. Amino Acids4h 20m
30. Peptides and Proteins2h 42m
31. Catalysis in Organic Reactions1h 30m
32. Lipids 2h 50m
33. The Organic Chemistry of Metabolic Pathways2h 52m
34. Nucleic Acids1h 32m
35. Transition Metals6h 14m
36. Synthetic Polymers1h 49m

3. Acids and Bases

Acids and Bases

Organic Chemistry

3. Acids and Bases

Acids and Bases

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3:56 minutes

Problem 4a

Textbook Question

What is the conjugate acid of each of the following?
1. NH₃
2. Cl⁻
3. HO⁻
4. H₂O

Verified step by step guidance

Step 1: Understand the concept of a conjugate acid. A conjugate acid is formed when a base gains a proton (H⁺). This involves identifying the base and adding an H⁺ to it.

Step 2: For NH₃ (ammonia), add an H⁺ to the molecule. This results in NH₄⁺ (ammonium ion). Write the chemical equation: NH₃ + H⁺ → NH₄⁺.

Step 3: For Cl⁻ (chloride ion), add an H⁺ to the ion. This results in HCl (hydrogen chloride). Write the chemical equation: Cl⁻ + H⁺ → HCl.

Step 4: For HO⁻ (hydroxide ion), add an H⁺ to the ion. This results in H₂O (water). Write the chemical equation: HO⁻ + H⁺ → H₂O.

Step 5: For H₂O (water), add an H⁺ to the molecule. This results in H₃O⁺ (hydronium ion). Write the chemical equation: H₂O + H⁺ → H₃O⁺.

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Key Concepts

Here are the essential concepts you must grasp in order to answer the question correctly.

Conjugate Acid-Base Theory

In acid-base chemistry, a conjugate acid is formed when a base accepts a proton (H+). This theory, primarily based on the Brønsted-Lowry definition, emphasizes the transfer of protons between species. Understanding this concept is crucial for identifying the conjugate acids of various bases, as it allows for the prediction of their behavior in chemical reactions.

Ammonia (NH3) as a Base

Ammonia (NH3) is a common weak base that can accept a proton to form its conjugate acid, ammonium (NH4+). This reaction illustrates the basic nature of ammonia, which is often involved in acid-base reactions. Recognizing ammonia's role as a base is essential for determining its conjugate acid.

Water (H2O) as an Amphoteric Substance

Water (H2O) is an amphoteric substance, meaning it can act as both an acid and a base. When it acts as a base, it can accept a proton to form the hydronium ion (H3O+), which is its conjugate acid. This dual behavior is important for understanding the conjugate acids of other species, such as hydroxide (HO−) and chloride (Cl−), in aqueous solutions.

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Related Practice

Textbook Question

Calculate the pH of the following solutions.

a. 5.00 g of HBr in 100 mL of aqueous solution

b. 1.50 g of NaOH in 50 mL of aqueous solution

Textbook Question

Consider the following reaction:

HBr + ^-C≡N ⇌ Br⁻+ HC≡N

g. What is the conjugate base of the acid on the right?

h. What is the conjugate acid of the base on the right?

Textbook Question

Consider the following reaction:

HBr + ^-C≡N ⇌ Br⁻+ HC≡N

c. What is the conjugate base of the acid on the left?

d. What is the conjugate acid of the base on the left?

Textbook Question

Draw the conjugate acid of each of the following:

a. CH₃CH₂OH

b. CH₃CH₂O⁻

Textbook Question

In the following acid–base reactions,

1. draw Lewis structures of the reactants and the products.

2. determine which species are acting as electrophiles (acids) and which are acting as nucleophiles (bases).

3. use the curved-arrow formalism to show the movement of electron pairs in these reactions, as well as the imaginary movement in the resonance hybrids of the products.

4. indicate which reactions are best termed Brønsted–Lowry acid–base reactions.

(b)

Textbook Question

Predict the products of the following acid–base reactions.

(c)

(d)

Textbook Question

Predict the products of the following acid–base reactions.

(a) H₂SO₄ + CH₃COO^– ⇌

(b) CH₃COOH + (CH₃)₃N: ⇌

Textbook Question

Label the reactants in these acid–base reactions as Lewis acids (electrophiles) or Lewis bases (nucleophiles). Use curved arrows to show the movement of electron pairs in the reactions.

(c)

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What is the conjugate acid of each of the following? 1. NH3 2. Cl− 3. HO− 4. H2O

Key Concepts

Conjugate Acid-Base Theory

Ammonia (NH3) as a Base

Water (H2O) as an Amphoteric Substance

Watch next

What is the conjugate acid of each of the following?
1. NH₃
2. Cl⁻
3. HO⁻
4. H₂O