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
Which of the following represents the balanced complete ionic equation for the reaction between HF(aq) and LiOH(aq)?
A
H+(aq) + F-(aq) + Li+(aq) + OH-(aq) → H2O(l) + Li+(aq) + F-(aq)
B
H+(aq) + F-(aq) + LiOH(aq) → H2O(l) + LiF(aq)
C
HF(aq) + Li+(aq) + OH-(aq) → H2O(l) + LiF(aq)
D
HF(aq) + LiOH(aq) → H2O(l) + LiF(aq)
Verified step by step guidance1
Identify the reactants and products in the molecular equation: HF(aq) + LiOH(aq) → H2O(l) + LiF(aq).
Write the complete ionic equation by dissociating all strong electrolytes into their ions. HF is a weak acid and does not dissociate completely, while LiOH is a strong base and dissociates into Li+(aq) and OH-(aq).
The complete ionic equation is: HF(aq) + Li+(aq) + OH-(aq) → H2O(l) + Li+(aq) + F-(aq).
Identify the spectator ions, which are ions that appear on both sides of the equation without undergoing any change. In this case, Li+(aq) is a spectator ion.
Remove the spectator ions to write the net ionic equation: HF(aq) + OH-(aq) → H2O(l) + F-(aq).
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