Answer:
the correct answer is: All of the above pairs, a, b, c, and d.
Explanation:
To find the pair of acids that would each react with barium hydroxide [tex](\( \text{Ba(OH)_2} \))[/tex]
to form water [tex](\( \text{H}_2\text{O} \))[/tex] and have the net ionic equation
[tex]\( \text{H}^+ + \text{OH}^- \rightarrow \text{H}_2\text{O} \),[/tex]
we need to identify the acids that contain hydrogen ions [tex](\( \text{H}^+ \))[/tex]and hydroxide ions [tex](\( \text{OH}^- \))[/tex] in their chemical formulas.
Let's analyze each option:
a. HCl and HNO₃:
- HCl is hydrochloric acid, which contains[tex]\( \text{H}^+ \) ions.[/tex]
- HNO₃ is nitric acid, which also contains [tex]\( \text{H}^+ \) ions.[/tex]
- Both HCl and HNO₃ can react with \( \text{Ba(OH)_2} \) to form water.
b. H₂SO₄ and H₃PO₄:
- H₂SO₄ is sulfuric acid, which contains[tex]\( \text{H}^+ \)[/tex] ions.
- H₃PO₄ is phosphoric acid, which also contains [tex]\( \text{H}^+ \) ions.[/tex]
- Both H₂SO₄ and H₃PO₄ can react with \( \text{Ba(OH)_2} \) to form water.
c. H₃PO₄ and HCl:
- H₃PO₄ is phosphoric acid, which contains [tex]\( \text{H}^+ \) ions.[/tex]
- HCl is hydrochloric acid, which contains[tex]\( \text{H}^+ \) ions.[/tex]
- Both H₃PO₄ and HCl can react with \( \text{Ba(OH)_2} \) to form water.
d. H₂CO₃ and H₃PO₄:
- H₂CO₃ is carbonic acid, which contains [tex]\( \text{H}^+ \) ions.[/tex]
- H₃PO₄ is phosphoric acid, which also contains [tex]\( \text{H}^+ \) ions.[/tex]
- Both H₂CO₃ and H₃PO₄ can react with \( \text{Ba(OH)_2} \) to form water.
From the analysis, it is evident that all the given pairs contain acids that can react with \( \text{Ba(OH)_2} \) to produce water with the net ionic equation [tex]\( \text{H}^+ + \text{OH}^- \rightarrow \text{H}_2\text{O} \).[/tex]
Therefore, the correct answer is: All of the above pairs, a, b, c, and d.
