need help with finding molarity thanks! **Problem Statement:**An aqueous potassium iodate (KIO₃) solution is made by dissolving 548 grams of KIO₃ in sufficient water so that the final volume of the solution is 3.90 L. Calculate the molarity of the KIO₃ solution.**Equation to Solve:**\[ \text{[KIO}_3\text{]} = \]**Solution Approach:**To determine the molarity of the KIO₃ solution, use the formula:\[ \text{Molarity (M)} = \frac{\text{moles of solute}}{\text{liters of solution}} \]**Steps:**1. **Calculate the moles of KIO₃:** - Determine the molar mass of KIO₃ using atomic masses (K: 39.10 g/mol, I: 126.90 g/mol, O: 16.00 g/mol). - Molar mass of KIO₃ = 39.10 + 126.90 + 3(16.00) = 214.00 g/mol. - Moles of KIO₃ = \(\frac{548 \text{ g}}{214.00 \text{ g/mol}}\).2. **Calculate the molarity:** - Use the calculated moles of KIO₃ and the given volume of the solution (3.90 L) to find molarity.\[ \text{[KIO}_3\text{]} = \text{moles of KIO}_3 \div 3.90 \text{ L} \]

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An aqueous potassium iodate (KIO,) solution volume of the solution is 3.90 L. Calculate the molarity of the KIO, solution. made by dissolving 548 grams of KIO, in sufficient water so that the fir [KIO,]=

An aqueous potassium iodate (KIO,) solution volume of the solution is 3.90 L. Calculate the molarity of the KIO, solution. made by dissolving 548 grams of KIO, in sufficient water so that the fir [KIO,]=

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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