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Chapter 6: Problem 91

You wish to prepare 1 L of a \(0.02-M\) potassium iodate solution. You require that the final concentration be within \(1 \%\) of \(0.02 M\) and that the concentration must be known accurately to the fourth decimal place. How would you prepare this solution? Specify the glassware you would use, the accuracy needed for the balance, and the ranges of acceptable masses of \(\mathrm{KIO}_{3}\) that can be used.

Short Answer

Expert verified
To prepare 1 L of a 0.02-M potassium iodate solution within 1% of the target concentration and known accurately to the fourth decimal place, weigh out between 4.2452 g and 4.3148 g of KIO3 using a high precision analytical balance with at least 0.0001 g readability. Transfer the KIO3 to a 1 L Class A volumetric flask, dissolve it in approximately 800 mL of distilled water, and fill up to the 1 L mark with distilled water. Stopper the flask and mix well to ensure a homogeneous solution.

Step by step solution

01

Calculate the mass of potassium iodate (KIO3) required

To calculate the mass of potassium iodate needed, we can use the formula: mass = volume × molarity × molar mass where volume = 1 L, molarity = 0.02 M, and molar mass of KIO3 = 39.10 (K) + 126.90 (I) + 48.00 (O3) = 214.00 g/mol. mass = \(1 \times 0.02 \times 214.00\) g mass = 4.28 g
02

Determine the acceptable mass range of KIO3

The final concentration should be within 1% of 0.02 M. So the range of acceptable molarities is: Min. molarity = 0.02 M × (1 - 0.01) = 0.0198 M Max. molarity = 0.02 M × (1 + 0.01) = 0.0202 M Convert the acceptable molarities to mass: Min. mass = \(1 \times 0.0198 \times 214.00\) g = 4.2452 g Max. mass = \(1 \times 0.0202 \times 214.00\) g = 4.3148 g The mass of KIO3 should be within the range of 4.2452 g to 4.3148 g.
03

Choose the appropriate glassware and balance

To know the concentration accurately up to the fourth decimal place, we need a balance with at least 0.0001 g readability and accuracy. A high precision analytical balance would be suitable for this task. For glassware, use a volumetric flask to prepare the 1 L solution accurately. A 1 L volumetric flask with a high-quality Class A or equivalent certification would be appropriate, ensuring the final volume is within the specified error range.
04

Prepare the solution

1. Weigh out the required amount of KIO3 (between 4.2452 g and 4.3148 g) on the high precision analytical balance. 2. Transfer the KIO3 to the 1 L volumetric flask. 3. Add approximately 800 mL of distilled water to the flask, ensuring all the KIO3 dissolves. 4. Fill the volumetric flask up to the 1 L mark with distilled water. 5. Stopper the flask and mix well to ensure a homogeneous solution. The 1 L of 0.02 M potassium iodate solution is now prepared with the concentration within 1% of the target concentration and known accurately to the fourth decimal place.

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