How much NaCl (mol. wt. 58.5 g/mol) would be needed to make a 10% solution of NaCl in a final volume of 1 liter of water?
To make a 10% solution of NaCl with a final volume of 1 liter, we need to determine how much NaCl is needed.
A 10% solution means that 10 grams of NaCl is dissolved in 100 mL of water. However, to simplify calculations, we will convert 10% into a decimal form: 10/100 = 0.1.
Since the final volume is 1 liter (1000 mL), we need to calculate 10% of 1000 mL:
0.1 * 1000 mL = 100 mL
Therefore, we need 100 mL of NaCl solution, which contains 10 grams of NaCl, for a final volume of 1 liter.
To convert 100 mL into grams, we use the fact that the density of water is approximately 1 g/mL (at room temperature):
100 mL * 1 g/mL = 100 grams
So, we need 100 grams of NaCl to make a 10% solution in a final volume of 1 liter of water.
To determine the amount of NaCl needed to make a 10% solution in a final volume of 1 liter, we can follow these steps:
Step 1: Convert the percentage (10%) to a decimal by dividing it by 100.
10% / 100 = 0.1
Step 2: Calculate the mass of NaCl required using the formula:
Mass = Percentage × Volume
Mass = 0.1 × 1 liter
Step 3: Multiply the mass by the molar mass of NaCl to convert it to moles:
Moles = Mass / Molar mass of NaCl
Molar mass of NaCl = 58.5 g/mol
Moles = (0.1 × 1) / 58.5
Therefore, the amount of NaCl needed to make a 10% solution in a final volume of 1 liter is approximately 0.0017 moles (or 0.0994 grams).