We wish to determine the mass of Mg required to react completely with 250 mL of 1.0 M HCl. HCl reacts with Mg according to the equation below.

[tex]\[2 \text{HCl} ( \text{aq} ) + \text{Mg} ( \text{s} ) \rightarrow \text{MgCl}_2 ( \text{aq} ) + \text{H}_2 ( \text{g} )\][/tex]

How many moles of HCl are present in 250 mL of 1.0 M HCl?



Answer :

To determine how many moles of HCl are present in 250 mL of 1.0 M HCl, we'll proceed as follows:

1. Convert Volume from mL to L:
Given the volume of HCl solution is 250 mL, we need to convert this volume to liters (L) since molarity (M) is defined as moles per liter (mol/L).

[tex]\[ \text{Volume in liters} = \frac{250 \text{ mL}}{1000 \text{ mL/L}} = 0.25 \text{ L} \][/tex]

2. Identify the Molarity (Concentration) of HCl:
We are given that the molarity of the HCl solution is 1.0 M, which means there are 1.0 moles of HCl in every 1 liter of solution.

3. Calculate the Moles of HCl:
Now we use the relationship between volume, molarity, and moles. The formula to find the number of moles (n) from molarity and volume is:

[tex]\[ \text{moles of HCl} = \text{Molarity (M)} \times \text{Volume (L)} \][/tex]

Substituting the given values:

[tex]\[ \text{moles of HCl} = 1.0 \text{ M} \times 0.25 \text{ L} = 0.25 \text{ moles} \][/tex]

Therefore, there are 0.25 moles of HCl present in 250 mL of a 1.0 M HCl solution.