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Question 5

Complete the table below using the Bronsted-Lowry definition by entering the missing chemical formulas:

(Do not use subscripts and superscripts in your answer. For example, [tex]$H_2CO_4$[/tex] would be written as H 2 CO 4.)

Sagot :

GinnyAnsweridn
It seems like you posted part of a question about Bronsted-Lowry acids and bases, but the details of the specific table are missing. Since no chemical formulas or specific reactions were provided, I'll explain the general concept and how to complete such a table.

The Bronsted-Lowry definition describes acids as proton (H^+) donors and bases as proton acceptors. When an acid donates a proton, it forms its conjugate base. Conversely, when a base accepts a proton, it forms its conjugate acid.

Assume the table has pairs of acids and bases along with their conjugates. Here's a step-by-step explanation on how to complete such a table:

1. Identify Acid and Conjugate Base Pair:
An acid will donate a proton (H^+), forming its conjugate base. For instance, HCl (acid) donates a proton to form Cl^- (conjugate base).

2. Identify Base and Conjugate Acid Pair:
A base will accept a proton, forming its conjugate acid. For example, NH_3 (base) accepts a proton to form NH_4^+ (conjugate acid).

### Sample Table:

| Acid | Conjugate Base | Base | Conjugate Acid |
|------------|----------------|----------|----------------|
| HCl | Cl^- | NH_3 | NH_4^+ |
| H_2SO_4 | HSO_4^- | OH^- | H_2O |
| H_2O | OH^- | HCO_3^- | H_2CO_3 |
| NH_4^+ | NH_3 | CO_3^2^- | HCO_3^- |

### Explanation for Each:

1. HCl (acid) and Cl^- (conjugate base):
HCl can donate a proton (H^+), which leaves behind Cl^-.

2. H_2SO_4 (acid) and HSO_4^- (conjugate base):
Sulfuric acid (H_2SO_4) donates one proton to form HSO_4^-.

3. H_2O (water) and OH^- (hydroxide ion, conjugate base):
Water (H_2O) donates a proton to form OH^-.

4. NH_4^+ (ammonium ion, acid) and NH_3 (ammonia, conjugate base):
NH_4^+ donates a proton to form NH_3.

5. NH_3 (base) and NH_4^+ (conjugate acid):
Ammonia (NH_3) accepts a proton to form NH_4^+.

6. OH^- (hydroxide ion, base) and H_2O (conjugate acid):
OH^- accepts a proton to form H_2O.

7. HCO_3^- (bicarbonate ion, base) and H_2CO_3 (carbonic acid, conjugate acid):
HCO_3^- accepts a proton to form H_2CO_3.

8. CO_3^2^- (carbonate ion, base) and HCO_3^- (conjugate acid):
CO_3^2^- accepts a proton to form HCO_3^-.

This approach will guide you in completing any Bronsted-Lowry acid-base table, provided you know the initial substances and their reactions.
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