During a titration, it is found that 25.0 mL of an unknown molarity NaOH is required to fully titrate 10.0 mL of 1.00 M HCl. What is the concentration of the unknown NaOH?

[tex]\[ \text{HCl} + \text{NaOH} \rightarrow \text{NaCl} + \text{H}_2\text{O} \][/tex]

A. 0.400 M
B. 2.50 M
C. 4.00 M
D. 0.250 M



Answer :

Sure, let's solve the problem step-by-step to find the concentration of the unknown NaOH.

Given Values:
- Volume of hydrochloric acid (HCl), [tex]\( V_{\text{HCl}} = 10.0 \)[/tex] mL
- Molarity of HCl, [tex]\( M_{\text{HCl}} = 1.00 \)[/tex] M
- Volume of sodium hydroxide (NaOH), [tex]\( V_{\text{NaOH}} = 25.0 \)[/tex] mL
- We need to find the molarity of NaOH, [tex]\( M_{\text{NaOH}} \)[/tex].

Chemical Equation:
[tex]\[ \text{HCl} + \text{NaOH} \rightarrow \text{NaCl} + \text{H}_2\text{O} \][/tex]

This equation tells us that HCl and NaOH react in a 1:1 molar ratio.

Step-by-Step Solution:

1. Identify the titration formula:

When a solution of known concentration (HCl) is used to determine the concentration of another solution (NaOH), we use the titration formula:
[tex]\[ M_1 \times V_1 = M_2 \times V_2 \][/tex]
Where:
[tex]\( M_1 \)[/tex] = Molarity of HCl
[tex]\( V_1 \)[/tex] = Volume of HCl
[tex]\( M_2 \)[/tex] = Molarity of NaOH
[tex]\( V_2 \)[/tex] = Volume of NaOH

2. Substitute the given values into the titration formula:
[tex]\[ (1.00 \, \text{M}) \times (10.0 \, \text{mL}) = M_{\text{NaOH}} \times (25.0 \, \text{mL}) \][/tex]

3. Calculate the unknown concentration:
[tex]\[ 10.0 \, \text{M} \cdot \text{mL} = M_{\text{NaOH}} \times 25.0 \, \text{mL} \][/tex]
[tex]\[ M_{\text{NaOH}} = \frac{10.0 \, \text{M} \cdot \text{mL}}{25.0 \, \text{mL}} \][/tex]
[tex]\[ M_{\text{NaOH}} = \frac{10.0}{25.0} \][/tex]
[tex]\[ M_{\text{NaOH}} = 0.4 \, \text{M} \][/tex]

So, the concentration of the unknown NaOH is [tex]\( 0.4 \, \text{M} \)[/tex].

The correct answer is:
[tex]\[ \boxed{0.4 \, \text{M}} \][/tex]