Use Lowry-Brönstes theory to write the balanced equation for the following reaction: HNO3(aq) +OH(aq)><_+_
The Lowry-Brönsted theory states that an acid donates a proton (H+) and a base accepts a proton. In the given reaction, HNO3 acts as the acid since it donates a proton, and OH acts as the base since it accepts a proton.
The balanced equation for the reaction is:
HNO3(aq) + OH(aq) -> H2O(l) + NO3-(aq)
Lowry-Brönsted theory describes acid-base reactions in terms of the donation and acceptance of protons (H+ ions). In order to write a balanced equation using this theory, we need to identify the acid and base present in the reaction.
In this case, HNO3(aq) is a strong acid, which can donate a proton (H+ ion), and OH(aq) is a strong base, capable of accepting a proton. Therefore, HNO3(aq) is the acid, and OH(aq) is the base.
The balanced equation using Lowry-Brönsted theory for this reaction is:
HNO3(aq) + OH(aq) ↔ H2O(l) + NO3-(aq)
In this equation, HNO3 donates a proton (H+) to OH, forming water (H2O) as a product, and leaving the NO3- ion behind. The double arrows in the equation indicate that the reaction can proceed in both directions, with the reactants forming products and the products potentially reverting back to reactants.