Textbook Question
Write balanced complete ionic and net ionic equations for each acid–base reaction. a. HI(aq) + RbOH(aq) →
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6. Chemical Quantities & Aqueous Reactions
Complete Ionic Equations
Multiple Choice
2H3PO4 + 3Ba(OH)2 → Ba3(PO4)2 + 6H2O. What is the total ionic equation of this reaction?
A
6H⁺(aq) + 6OH⁻(aq) → 6H₂O(l)
B
2H₃PO₄(aq) + 3Ba²⁺(aq) + 6OH⁻(aq) → Ba₃(PO₄)₂(s) + 6H₂O(l)
C
2H₃PO₄(aq) + 3Ba(OH)₂(aq) → Ba₃(PO₄)₂(s) + 6H₂O(l)
D
6H⁺(aq) + 2PO₄³⁻(aq) + 3Ba²⁺(aq) + 6OH⁻(aq) → Ba₃(PO₄)₂(s) + 6H₂O(l)
Verified step by step guidance1
Identify the compounds involved in the reaction: phosphoric acid (H₃PO₄), barium hydroxide (Ba(OH)₂), barium phosphate (Ba₃(PO₄)₂), and water (H₂O).
Write the balanced molecular equation: 2H₃PO₄(aq) + 3Ba(OH)₂(aq) → Ba₃(PO₄)₂(s) + 6H₂O(l).
Break down the aqueous compounds into their ions. For H₃PO₄, it dissociates into 6H⁺(aq) and 2PO₄³⁻(aq). For Ba(OH)₂, it dissociates into 3Ba²⁺(aq) and 6OH⁻(aq).
Recognize that Ba₃(PO₄)₂ is a solid and does not dissociate into ions in the solution. Water (H₂O) is a liquid and remains as molecules.
Combine the ions from the reactants and products to form the total ionic equation: 6H⁺(aq) + 2PO₄³⁻(aq) + 3Ba²⁺(aq) + 6OH⁻(aq) → Ba₃(PO₄)₂(s) + 6H₂O(l).
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