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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 KIO3 that could be used.(a) To make this solution (ideally) you would need ________ grams of potassium iodide dissolved in enough water to make up 1 L of solution.fill in the blank(b)What is the least accurate balance that could be used to make this solution?

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dvelasquez90

Answer:

4.28 g of KIO3

Explanation:

[tex]\frac{0.02 mol}{L} *1L*\frac{214 g}{1 mol KIO3}=4.28 g[/tex]

You must use an analytical balance with a precision of 0.1 mg and the measure can be since 4.2372 (0.0198 M) g until 4.3228 (0.0202 M) g to preserve the accurate of 1%. Then dissolve the salt with 100 mL in a beaker with water. Put it into a volumetric flask of 1L and fill with water until the mark.

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