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A student forgets to weigh a mixture of sodium bromide dihydrate and magnesium bromide hexahydrate. Upon strong heating, the sample loses 252.1 mg of water. The mixture of anhydrous salts reacts with excess $\mathrm{AgNO}_{3}$ solution to form $6.00 \times 10^{-3} \mathrm{mol}$ of solid AgBr. Find the mass $\%$ of each compound in the original mixture.

   A student forgets to weigh a mixture of sodium bromide dihydrate and magnesium bromide hexahydrate. Upon strong heating, the sample loses 252.1 mg of water. The mixture of anhydrous salts reacts with excess $\mathrm{AgNO}_{3}$ solution to form $6.00 \times 10^{-3} \mathrm{mol}$ of solid AgBr. Find the mass $\%$ of each compound in the original mixture.

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Chemistry: The Molecular Nature of Matter and Change

Chemistry: The Molecular Nature of Matter and Change

Martin S.… 7th Edition

Chapter 4, Problem 140

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Given that the mass of water lost is 252.1 mg, we can convert this to moles using the molar mass of water (18.015 g/mol). \[ \text{Moles of water} = \frac{252.1 \, \text{mg}}{18.015 \, \text{g/mol}} \times \frac{1 \, \text{g}}{1000 \, \text{mg}} = 0.014 \, Show more…

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