Describe how you would prepare 250.0 mL of a 0.500 M solution of NaCl by using apparatus found in a chemistry lab.
no
did you try putting it in a 600mL beaker?
write the steps something like this
1. Place 0.125 moles NaCl (7.305 grams) in a 250 mL volumetric flask, add some water, swirl to dissolve all of the NaCl, then make to the mark with water. You PROBABLY should round the 7.305 g to 7.31 grams.
To prepare a 0.500 M solution of NaCl using apparatus found in a chemistry lab, you will need the following equipment:
1. A 250.0 mL volumetric flask: This flask is used to accurately measure and prepare a specific volume of solution.
2. A balance: This is used to measure the mass of the NaCl powder.
3. A weighing boat or container: This is used to hold the NaCl powder during weighing.
4. Deionized water: This is used as the solvent to dissolve the NaCl powder.
Here's a step-by-step guide on how to prepare the solution:
1. Weigh the appropriate amount of NaCl powder: The molar mass of NaCl is approximately 58.44 g/mol. To prepare a 0.500 M solution, we need to calculate the amount of NaCl needed. The formula to calculate the mass is mass = molarity × volume × molar mass. Rearranging the formula, we get mass = molarity × volume × molar mass. Plugging in the values, we get mass = 0.500 mol/L × 0.250 L × 58.44 g/mol. This gives us approximately 7.305 grams of NaCl.
2. Use a balance to measure out the calculated mass of NaCl accurately.
3. Transfer the measured NaCl powder into the volumetric flask using a weighing boat or container.
4. Add a small amount of deionized water to dissolve the NaCl. Swirl gently to aid dissolution.
5. Once the NaCl is dissolved, slowly add more deionized water to fill the volumetric flask up to the mark on the neck.
6. Stopper the flask and invert it several times to ensure the solution is thoroughly mixed.
7. Finally, label the volumetric flask with the concentration, the solute (NaCl), and the date of preparation.
By following these steps, you will have successfully prepared a 250.0 mL of a 0.500 M NaCl solution using apparatus commonly found in a chemistry lab.
The definition of molarity is
M = #mols/Liter of solution.
If you want to do this by math (instead of reasoning), you first plug in 0.5 for M and 0.250 for L and calculate #moles.
0.5=moles/0.250 L
moles NaCl = 0.5 x 0.250 = 0.125 moles.
1 mole NaCl = approximately 58.5 grams. So 0.125 moles NaCl is ......
Or by reasoning, we want 0.5 mole for 0.5 M in 1 L and divide that by 4 for only 1/4 of a liter (250 mL). So we want 1/4 of 1/2 = 1/8 of a mole (or 0.125 mol).
But this isn't the tricky part. The tricky part is telling the prof HOW to prepare the solution. You will want to take 1/8 mole NaCl (about 7 grams or so), place it in a 250 mL volumetric flask, add a little water, swirl until all of the NaCl is dissolved, then make to the mark with water. That will prepare 0.5 M solution in a 250 mL volumetric flask. (Note that I DID NOT say to add about 7 grams NaCl to 250 mL water.).