Given a \(0.250 \mathrm{M} \mathrm{K}_{2} \mathrm{CrO}_{4}\) stock solution, describe how you would prepare a solution that is \(0.0125 \mathrm{M}\) \(\mathrm{K}_{2} \mathrm{CrO}_{4} .\) That is, what combination(s) of pipet and volumetric flask would you use? Typical sizes of volumetric flasks found in a general chemistry laboratory are \(100.0,250.0,500.0,\) and \(1000.0 \mathrm{mL},\) and typical sizes of volumetric pipets are 1.00,5.00,10.00 \(25.00,\) and \(50.00 \mathrm{mL}\)

Short Answer

Expert verified
For the desired \(0.0125 \mathrm{M} \mathrm{K}_{2} \mathrm{CrO}_{4}\) solution, use a 50.00 mL pipette to measure stock solution and mix in a 1000.0 mL volumetric flask by adding solvent until the mark.

Step by step solution

01

Using Dilution Formula

Let's use the dilution formula \( M1V1 = M2V2 \) , where \( M1 = 0.250 \mathrm{M}\), the molarity of stock solution, and \( M2 = 0.0125 \mathrm{M}\), the molarity of the desired diluted solution. Let's calculate \( V1 \), the volume of stock solution required, while \( V2 \), the total volume of the final diluted solution will be selected from one of the given typical volumetric flask sizes.
02

Determine Volume of stock solution (V1)

Rearranging the dilution formula to calculate for \( V1 = \(\frac{M2}{M1} \cdot V2\).
03

Final Volume Option Iteration

Iterate through typical volumetric flask sizes, for each \( V2 \), calculate \( V1 \) using step 2 formula. Ensure that calculated \( V1 \) matches one of the given typical sizes of pipettes. This ensures accurate and efficient measurement.
04

Verify volumes for pipetting and total solution

Cross-verify that the calculated \( V1 \) can be accurately measured with availabe pipette and that the total volume \( V2 \) can be held by the selected volumetric flask.

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Most popular questions from this chapter

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