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Chapter 4: Problem 99

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 a 1 L, 0.02 M potassium iodate solution with the required accuracy, use a 1 L volumetric flask and an analytical balance with a readability of 0.0001 g (0.1 mg). Weigh the potassium iodate within the acceptable mass range of 4.2372 g to 4.3228 g.

Step by step solution

01

Calculate the required mass of KIO3

First, we need to calculate the mass of KIO3 required to make the 1 L, 0.02 M solution. To do this, we can use the following formula: \(c = \frac{n}{V}\) Where: - c is the concentration (moles/L) - n is the number of moles - V is the volume in L Rearranging for n, we get: \(n = c * V\) Then, we can find the mass (m) using: \(m= n * M\) Where: - m is the mass in grams - M is the molar mass of the compound (in this case, KIO3) Combining these into one equation, we get: \(m = c * V * M\) Given, c = 0.02 M, V = 1 L, and the molar mass of KIO3 (M) is 214 g/mol, we can calculate the required mass as: \(m = 0.02 * 1 * 214\) \(m = 4.28~grams\)
02

Determine the acceptable mass range of KIO3

Since the solution must be within 1% of the desired concentration, we need to determine the acceptable range of mass for KIO3. We will find the lower and upper bounds for the mass as follows: Lower bound = (1 - 0.01) * required mass Upper bound = (1 + 0.01) * required mass Lower bound = (0.99) * 4.28 g Upper bound = (1.01) * 4.28 g Lower bound = 4.2372 g Upper bound = 4.3228 g The acceptable mass range for KIO3 is between 4.2372 g and 4.3228 g.
03

Select the appropriate glassware

To achieve the required accuracy to the fourth decimal place, we need to use precise volumetric glassware. In this case, a 1 L volumetric flask would be the most appropriate choice.
04

Choose a suitable balance

Since we need to measure the mass accurately to the fourth decimal place, a balance with a readability of at least 0.0001 g (0.1 mg) is needed. An analytical balance that meets this requirement should be used to weigh the KIO3. In summary, to prepare a 1 L, 0.02 M KIO3 solution with the required accuracy, we would use a 1 L volumetric flask, an analytical balance with a readability of 0.0001 g (0.1 mg), and measure the mass of KIO3 within the range of 4.2372 g to 4.3228 g.

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