Question

In a titration, 5.0 ml of a 2.0 M NaOH (aq) solutions exactly neutralizes 10.0 ml of an HCL (aq) solution. what is the concentration of the HCl (aq) solution?

Answer 1

`M_(acid)=1.0M`

Step-by-step explanation:

Hello,

In this case, since the reaction between HCl and NaOH is:

`NaOH+HCl\rightarrow NaCl+H_2O`

We notice a 1:1 molar ratio between the acid and the base, for that reason, in the equivalent point we find:

`n_(acid)=n_(base)`

Thus, in terms of concentrations, we have:

`M_(acid)V_(acid)=M_(base)V_(base)`

Hence, we solve for the concentration of the acid to obtain:

`M_(acid)=(M_(base)V_(base))/(V_(acid)) =(2.0M*5.0mL)/(10.0mL)\\ \\M_(acid)=1.0M`

Regards.