What is the molarity of a saline solution that contains 3.6 g NaCl (58.44 g/mol) dissolved in 100.0 mL of solution?
1.00
3,6/58,44 = 0,0616
0,0616/o,1L = 0,616 M
To calculate the molarity of a solution, you need to know the amount of solute (in moles) and the volume of the solution (in liters). Here's how you can calculate the molarity of the saline solution:
Step 1: Convert the mass of the solute to moles.
Given that the mass of NaCl is 3.6 g and the molar mass of NaCl is 58.44 g/mol, you can use the formula:
moles = mass / molar mass
Substituting the given values:
moles = 3.6 g / 58.44 g/mol
Step 2: Convert the volume from milliliters to liters.
Given that the volume of the solution is 100.0 mL, you can use the conversion factor:
1 L = 1000 mL
So, the volume in liters is:
volume = 100.0 mL / 1000 mL/L
Step 3: Calculate the molarity.
Molarity is defined as moles of solute per liter of solution. Therefore, you divide the number of moles by the volume in liters:
molarity = moles / volume
Let's calculate the molarity step by step:
moles = 3.6 g / 58.44 g/mol ≈ 0.0616 mol
volume = 100.0 mL / 1000 mL/L = 0.100 L
Now, substitute the values into the formula:
molarity = 0.0616 mol / 0.100 L ≈ 0.616 M
Thus, the molarity of the saline solution is approximately 0.616 M.