Net ionic equations with no ions

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The molecular equation for the reaction between lithium hydroxide (LiOH) and hydrobromic acid (HBr) is correctly represented as LiOH (aq) + HBr (aq) → LiBr (aq) + H2O (l). The net ionic equation simplifies to OH(-) + H(+) → H2O, as the reaction involves the hydroxide ion reacting with the hydrogen ion to form water. LiBr is soluble in water, which is relevant when considering the ionic species present in solution. In aqueous solutions, the focus should be on the ions produced, similar to how sodium chloride (NaCl) dissociates into Na(+) and Cl(-) ions. Additionally, consulting a physical chemistry text on ionic equations can provide further clarity on these reactions and the behavior of ions in solution.
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Just a short question:
Now the molecular equation between LiOH (aq) with HBr (aq) is (I presume):
LiOH (aq) + HBr (aq) ----> LiBr (aq) + H(2)O (l)
Now I'm confused about the net ionic, since there are no ions.
Would it just be:
OH(-) + H(+) ---> H(2)O?
 
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What is the solubility of LiBr?

Think of a solution of NaCl. What are the ions?
 
Additionally, I recommend you look up the chapter on Ionic Equations in your favorite physical chemistry text. I like Atkins, but any decent text will show you how to go about this.
 
Astronuc has shown a good way, in aqueous solutions we don't have LiBr on hand, this is in another form. And look for cross-ionic reactions to give the final product. You wrote (aq) for three compounds, but not for H2O, this may give you a cue.
 

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