Question

How many milliliters of 0.100 M NaOH are required to neutralize the following solutions?5.00 mL of 0.0500 M HCl_____ mL NaOH

Answer 1

So,

The balanced reaction for this situation is:

`NaOH_((aq))+HCl_((aq))\to NaCl_((s))+H_2O_((l))`

The first thing we're going to do is to determine the # of moles of HCl from its volume and molarity: (Remember that 5mL are 0.005 liters)

`\begin{gathered} M=(n)/(V)\to n=M\cdot V \\ \\ n=0.0500M\cdot0.005L \\ n=0.00025molesHCl \end{gathered}`

Now, we're going to convert these moles to moles of NaOH using stoichiometry:

`0.00025molesHCl\cdot(1molNaOH)/(1molHCl)=0.00025molesNaOH`

And then, use the calculated moles of NaOH and its molarity (0.100 M) to figure out the volume needed.

`V=(n)/(M)=(0.00025molesNaOH)/(0.1)=0.0025L`

If we pass this answer to mL:

`0.0025L=2.5mL`

Therefore, we need 2.5mL of NaOH to neutralize the solution.