Question

Which volume of 2.0 M NaOH(aq) is needed to completely neutralize 24 milliliters of 1.0 M HCl(aq)?

Answer 1

Answer:

12mLd

Explanation:

Given parameters:

Concentration of base, NaOH = 2.0M

Volume of acid, HCl = 24mL = 24 x 10⁻³L = 0.024L

Concentration of HCl = 1.0M

Unknown parameter

Volume of NaOH = ?

The equation of the reaction is NaOH + HCl → NaCl + H₂O

Method

1. Starting the known values, we find the number of moles of acid used. From the reaction equation , we know that:

            1 mole of NaOH reacts with 1 mole of HCl

We use the above to find the number of moles of base used

2. From the number of moles of base, we plug it into the equation below:

              Volume of NaOH = $\frac{number of moles of NaOH}{concentration of NaOH}$

Solution

Number of moles of acid = concentration of acid x volume of acid

Number of moles = 1M x 0.024L = 0.024mol

              From the balanced equation we know that:

                   1 mole of NaOH reacts with 1 mole of HCl

                   Therefore, the number of moles of NaOH is 0.024mol

Using the equation below, we have:

Volume of NaOH = $\frac{number of moles of NaOH}{concentration of NaOH}$

Volume of NaoH = $\frac{0.024mol}{2.0M}$

Volume of NaOH = 0.012L = 12mL