Question

3.65g HCl and 4g NaOH are mixed together to prepare 2litre aqueous solution.The resulting solution will be
1)alkaline
2)neutral
3) strongly acidic
4)weakly acidic

Answer 1

Answer:

neutral

Explanation:

Hcl+NaOH-------NaCl+H2O

Answer 2

Answer: The correct answer is Option 2.

Explanation:

Alkaline solutions are defined as the solutions where concentration of base is more than the concentration of acid.

Neutral solutions are defined as the solutions in which concentration of base and acid are equal.

Strongly acidic solutions are defined as the solutions where concentration of acid is very very high than the concentration of base.

Weakly acidic solutions are defined as the solutions where concentration of acid is slightly higher than the concentration of base.

We are given:

Mass of HCl = 3.65 g

Mass of NaOH = 4 g

Volume of solution = 2 L

To calculate the molarity of solution, we use the equation:

$\text{Molarity of the solution}=\frac{\text{Given mass of solute}}{\text{Molar mass of solute}\times \text{Volume of solution (in L)}}$

• For HCl:

Molar mass of HCl = 36.5 g/mol

Putting values in above equation, we get:

$\text{Molarity of HCl}=\frac{3.65g}{36.5g/mol\times 2L}=0.05mol/L$

• For NaOH:

Molar mass of NaOH = 0.4 g/mol

Putting values in above equation, we get:

$\text{Molarity of NaOH}=\frac{0.4g}{40g/mol\times 2L}=0.05mol/L$

The chemical equation for the reaction of HCl and NaOH follows:

$NaOH+HCl\rightarrow NaCl+H_2O$

By Stoichiometry of the reaction:

1 mole of NaOH reacts with 1 mole of HCl.

So, 0.05 moles/L of NaOH will react with = $\frac{1}{1}\times 0.05=0.05mol/L$ of HCl

Thus, total concentration of HCl are getting consumed in the reaction as well as total concentration of NaOH.

Hence, the solution becomes neutral.

Therefore, the correct answer is Option 2.