1. A lab tech needs 1.00 L of 0.125 mol/L sulfuric acid solution for a quantitative analysis experiment. A commercial 5.00 mol/L sulfuric acid solution is available from a chemical supply company. Write out what steps he/she would follow to prepare the needed solution. Include all necessary calculations.
Do I just solve for final volume and then write what to do?
Calculate the mass of solid cobalt(II) chloride hexahydrate you need to prepare 100.0 mL of a 0.100 mol/L cobalt(II) chloride solution.
Yes, solve for the final volume and explain what to do. Remember to add the ACID to the water, let cool (if needed) and make to final volume.
For the CoCl2.6H2O, how many mols do you need. That's mols = M x L = ?
Then mols = grams/molar mass. YOu know molar mass and mols, solve for grams.
Yes, to prepare the desired sulfuric acid solution, you need to calculate the final volume and then outline the steps to follow. Here are the calculations and steps:
Step 1: Determine the amount of sulfuric acid needed.
Moles of acid needed = concentration × volume
= 0.125 mol/L × 1.00 L
= 0.125 mol
Step 2: Determine the amount of the commercial sulfuric acid solution required.
Moles of commercial solution required = moles of acid needed / concentration of commercial solution
= 0.125 mol / 5.00 mol/L
= 0.025 L
= 25 mL
Step 3: Calculate the amount of water needed.
Water volume = final volume - volume of commercial solution
= 1.00 L - 0.025 L
= 0.975 L
= 975 mL
Step 4: Prepare the solution.
a) Measure 25 mL of the commercial 5.00 mol/L sulfuric acid solution using a graduated cylinder.
b) Add the measured sulfuric acid solution to a 1.00 L volumetric flask.
c) Fill the volumetric flask with distilled water up to the 1.00 L mark.
d) Mix the solution thoroughly to ensure proper dissolution.
Now, you have successfully prepared the 1.00 L of 0.125 mol/L sulfuric acid solution required for your experiment.
To prepare the 0.125 mol/L sulfuric acid solution, the lab tech can follow these steps:
1. Determine the desired final volume of the 0.125 mol/L sulfuric acid solution. In this case, it is 1.00 L.
2. Calculate the amount of sulfuric acid needed by using the formula:
Amount (in moles) = Concentration (in mol/L) x Volume (in L)
Let's denote the amount of sulfuric acid needed as n. Since the desired concentration is 0.125 mol/L and the final volume is 1.00 L, we can write:
n = 0.125 mol/L x 1.00 L = 0.125 mol
Therefore, the lab tech needs 0.125 moles of sulfuric acid.
3. Determine the volume of the 5.00 mol/L sulfuric acid solution needed to obtain 0.125 moles of sulfuric acid. To do this, we use the formula:
Volume (in L) = Amount (in moles) / Concentration (in mol/L)
Let's denote the volume of the 5.00 mol/L sulfuric acid solution as V. We can substitute the values into the formula:
V = 0.125 mol / 5.00 mol/L = 0.025 L
Therefore, the lab tech needs 0.025 L (or 25 mL) of the 5.00 mol/L sulfuric acid solution.
4. Using a graduated cylinder or a pipette, measure 25 mL of the 5.00 mol/L sulfuric acid solution.
5. Transfer the measured sulfuric acid solution into a clean and dry container.
6. Add distilled water to the container until the final volume reaches 1.00 L.
7. Mix the solution thoroughly to ensure uniform distribution.
By following these steps, the lab tech will obtain the required 0.125 mol/L sulfuric acid solution for the quantitative analysis experiment.