When HCl(aq) is exactly neutralized by NaOH(aq), the hydrogen ion concentration in the resulting mixture is
a. always equal than the concentration of the hydroxide ions
b.sometimes greater and sometimes less than the concentration of the hydroxide ion
c. always greater than the concentration of the hydroxide ions
d. always less than the concentration of the hydroxide ion.
The correct ans. will be (c)- always equal to the concentration of hydroxide ions.
When. Hcl is exactly neutralise by NaoH the hydrogen ion concentration in the resulting mixture is
To determine the hydrogen ion concentration in the resulting mixture when HCl(aq) is exactly neutralized by NaOH(aq), we need to understand the concept of a neutralization reaction and the stoichiometry involved.
In a neutralization reaction between an acid (such as HCl) and a base (such as NaOH), the acid donates hydrogen ions (H+) and the base donates hydroxide ions (OH-) to form water (H2O). The stoichiometry of the reaction is such that the number of moles of hydrogen ions donated by the acid is equal to the number of moles of hydroxide ions donated by the base.
The balanced chemical equation for the neutralization reaction between HCl(aq) and NaOH(aq) is:
HCl(aq) + NaOH(aq) -> H2O(l) + NaCl(aq)
From this equation, we can see that 1 mole of HCl reacts with 1 mole of NaOH to produce 1 mole of water.
Since the reaction is stoichiometric, when the acid is exactly neutralized by the base, the number of moles of hydrogen ions will be equal to the number of moles of hydroxide ions. Therefore, the correct answer is:
a. always equal to the concentration of the hydroxide ions
In other words, when HCl is completely neutralized by NaOH, the resulting solution will have the same concentration of hydrogen ions as the concentration of hydroxide ions.