To determine the number of moles of HCl needed to neutralize 0.10 L of 2.0 M NaOH, we need to follow these steps:
1. Understand the neutralization reaction:
- The balanced chemical equation for the neutralization of sodium hydroxide (NaOH) with hydrochloric acid (HCl) is:
[tex]\[
\text{NaOH} + \text{HCl} \rightarrow \text{NaCl} + \text{H}_2\text{O}
\][/tex]
- From the equation, the mole ratio of NaOH to HCl is 1:1. This means one mole of NaOH reacts with one mole of HCl to form one mole of NaCl and one mole of water.
2. Calculate the moles of NaOH:
- We know the volume of NaOH solution is 0.10 liters and the concentration is 2.0 M (moles per liter).
- To find the number of moles of NaOH, we use the formula:
[tex]\[
\text{moles of NaOH} = \text{volume (L)} \times \text{concentration (M)}
\][/tex]
- Plugging in the values:
[tex]\[
\text{moles of NaOH} = 0.10 \, \text{L} \times 2.0 \, \text{M}
\][/tex]
- This gives:
[tex]\[
\text{moles of NaOH} = 0.20 \, \text{moles}
\][/tex]
3. Determine the moles of HCl required:
- According to the balanced equation, the mole ratio of NaOH to HCl is 1:1. Therefore, the number of moles of HCl required will be equal to the number of moles of NaOH.
- Thus:
[tex]\[
\text{moles of HCl} = 0.20 \, \text{moles}
\][/tex]
Therefore, 0.20 moles of HCl are needed to neutralize 0.10 L of 2.0 M NaOH.
