USING EQUATION SHOW HOW AQUEOUS SOLUTION OF HYDROCHLORIC ACID CONTAINING HYDROXONIUM ION NEUTRALISED POTASSIUM HYDROXIDE
I'm guessing that the author wants this.
H3O^+(aq) + Cl^-(aq) + KOH ==> KCl(aq) + 2H2O(l)
OK, that makes sense... The ionic equation.
KOH + HCl => KCl + H23^+
To show how an aqueous solution of hydrochloric acid containing hydroxonium ions neutralizes potassium hydroxide, we need to write and balance the equation representing the chemical reaction between these two compounds.
Hydrochloric acid is a strong acid that dissociates completely in water, yielding hydrogen ions (H+) and chloride ions (Cl-). Potassium hydroxide, on the other hand, is a strong base that dissociates fully in water, producing potassium ions (K+) and hydroxide ions (OH-).
The reaction between hydrochloric acid and potassium hydroxide can be represented by the following balanced equation:
HCl + KOH → KCl + H2O
In this equation, hydrochloric acid (HCl) reacts with potassium hydroxide (KOH) to form potassium chloride (KCl) and water (H2O).
The hydroxonium ion (H3O+) is formed when a water molecule reacts with a hydrogen ion (H+). In this case, since hydrochloric acid is a strong acid, it completely dissociates in water, resulting in the formation of hydroxonium ions:
HCl + H2O → H3O+ + Cl-
Therefore, to account for the presence of hydroxonium ions in the reaction, we can modify the balanced equation as follows:
H3O+ + OH- + K+ + Cl- → K+ + Cl- + H2O
In this equation, the hydroxonium ion (H3O+) and hydroxide ion (OH-) combine to form water (H2O), while the potassium ions (K+) and chloride ions (Cl-) do not participate in the neutralization reaction and remain unchanged.
So, an aqueous solution of hydrochloric acid containing hydroxonium ions neutralizes potassium hydroxide by reacting the hydroxonium ion (H3O+) and hydroxide ion (OH-) to form water, while the remaining ions (K+ and Cl-) remain unchanged.