how would you prepare 60.0 mL of 0.200 M HNO3 from a stock solution of 4.00 M HNO3?
3ml
225ml
3ml
Answer
To prepare 60.0 mL of 0.200 M HNO3 from a stock solution of 4.00 M HNO3, you can use the dilution formula:
C1V1 = C2V2
where:
C1 = concentration of the stock solution
V1 = volume of the stock solution taken
C2 = desired concentration of the diluted solution
V2 = final volume of the diluted solution
Let's break down the steps to prepare the desired solution:
Step 1: Calculate the volume of the stock solution needed.
Using the dilution formula, we can rearrange it to solve for V1:
V1 = (C2 * V2) / C1
Substituting the given values:
C1 = 4.00 M
V2 = 60.0 mL
C2 = 0.200 M
V1 = (0.200 M * 60.0 mL) / 4.00 M
V1 = 3.00 mL
So, you would need to take 3.00 mL of the 4.00 M HNO3 stock solution.
Step 2: Calculate the volume of solvent (water) needed.
To determine the volume of water needed, subtract the volume of the stock solution taken from the final volume of the diluted solution:
V_water = V2 - V1
V_water = 60.0 mL - 3.00 mL
V_water = 57.0 mL
So, you would need to add 57.0 mL of water.
Step 3: Combine the stock solution and water.
Take 3.00 mL of the 4.00 M HNO3 and add 57.0 mL of water to it. Mix thoroughly to ensure uniformity.
Now, you have prepared 60.0 mL of 0.200 M HNO3 from the stock solution.