Understanding the Nature of an Aqueous Solution: A Detailed Analysis of 10 mL 0.50M HCl and 10 mL 1.0M NaOH

Introduction

The determination of the nature of an aqueous solution often involves a careful understanding of the chemical reaction between acids and bases. This analysis focuses on the interaction between 10 mL of 0.50M HCl and 10 mL of 1.0M NaOH to determine the resulting solution's pH and its nature.

Calculations and Steps Involved

Step 1: Calculate the Moles of the Reactants

The first step in our analysis involves calculating the moles of the reactants, HCl and NaOH, to proceed with the reaction balance and chemical equilibrium.

Moles of HCl:

Using the formula Moles of HClConcentration×VolumeMoles of HCl Concentration times Volume

Concentration 0.50 mol/L, Volume 0.010 L Moles of HCl 0.50 mol/L × 0.010 L 0.005 mol

Moles of NaOH:

Using the same formula as above,

Concentration 1.0 mol/L, Volume 0.010 L Moles of NaOH 1.0 mol/L × 0.010 L 0.010 mol

Step 2: Determine the Reaction

Next, we consider the reaction between HCl and NaOH. These reactants combine in a 1:1 molar ratio based on the reaction equation:

text{HCl} text{NaOH} rightarrow text{NaCl} text{H}_2text{O}

Step 3: Identify the Limiting Reactant

With 0.005 mol of HCl and 0.010 mol of NaOH, it is clear that HCl is the limiting reactant due to its lesser quantity.

Step 4: Calculate Remaining Moles Post-Reaction

After the reaction, the remaining moles of NaOH can be calculated as follows:

Remaining NaOH 0.010 mol - 0.005 mol 0.005 mol

Step 5: Calculate the Total Volume and Solution Concentration

The total volume of the solution is the sum of the two volumes:

Total Volume 10 mL 10 mL 20 mL 0.020 L

The concentration of the remaining NaOH in the solution is then:

Concentration of NaOH frac{0.005 mol}{0.020 L} 0.25 M

Conclusion

Given the presence of excess NaOH, the resulting solution is alkaline. The pH of the solution will be greater than 7, confirming its basic nature.

Understanding the nature of aqueous solutions is crucial in many chemical applications, from everyday cleaning agents to industrial processes. The principles demonstrated in this case study can be applied to a wide variety of acid-base reactions and scenarios where understanding the pH is essential.

This detailed analysis of the interaction between 10 mL of 0.50M HCl and 10 mL of 1.0M NaOH provides a clear pathway for determining the nature of the resulting solution. Whether you are a student or a professional in the field of chemistry, this understanding is invaluable.