Question

State whether the statement is true or false:
$LiOH$ is treated as a strong base because it reacts with acids and the reaction is known as neutralization reaction.
A.True
B.False

Answer 1

Approach this question with a clear understanding of Arrhenius acid and bases.
The strength of acids and bases could be determined by their dissociative properties.

Complete step by step answer:
The Arrhenius theory of acids and bases was originally proposed by the Swedish chemist Svante Arrhenius in 1884. He proposed classifying definite compounds as acids or bases based on what kind of ions formed when the compound was added to water.
An Arrhenius acid can be defined as the species which increases the concentration of ${{H}^{+}}$in the solution. Similarly Arrhenius' base is the species which increases the concentration of $O{{H}^{-}}$in the solution. The ${{H}^{+}}$interacts with ${{H}_{2}}O$molecules to form hydronium ions ${{H}_{3}}{{O}^{+}}$.
An example of an Arrhenius base is the highly soluble sodium hydroxide, $NaOH$.
The strong bases are those species which dissociates completely in water, into its respective ions. The OH- ions released from the base increases the overall OH- concentration of the solution which makes it basic in nature. Weak bases on the other hand, dissociate partially in the solution hence they have comparatively lower concentration of $O{{H}^{-}}$ions.
When an Arrhenius acid reacts with an Arrhenius base, the products are usually water plus a salt. These reactions are also sometimes called neutralization reactions.
$LiOH$ is treated as a strong base as it completely dissociates in water in lithium ions and hydroxide ions.
$LiOH\rightleftharpoons L{{i}^{+}}+O{{H}^{-}}~$
LiOH reacts with acids to form salt and water and the reaction, as mentioned earlier, is called neutralisation reaction.
Thus, the statement is false.

Additional Information:
The Arrhenius theory is limited in that it can only define acid-base chemistry in aqueous solutions. Similar reactions can also occur in solvents which are non-aqueous in nature, however, as well as between molecules in the gas phase. As a result, modern chemists usually prefer the Bronsted-Lowry theory, which is useful in a broader range of chemical reactions.

Note:

${{H}^{+}}$ doesn’t exist in this form, in fact it exists in ${{H}_{3}}{{O}^{+}}$ form in solution.
While writing any mechanism in organic chemistry, the arrows always point towards the ${{H}^{+}}$ and not the opposite, as the electrons jump to fill the proton.