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A commerically availabe sample of sulphu...

A commerically availabe sample of sulphuric acid is 15% `H_(2)SO_(4)` by weight (density `= 1.10 g mL^(-1)`). Calculate (i) molarity (ii) normality and (iii) molality of the solution.

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To solve the problem, we need to calculate the molarity, normality, and molality of a 15% (by weight) solution of sulfuric acid (H₂SO₄) with a density of 1.10 g/mL. Let's go through the calculations step-by-step. ### Step 1: Calculate the mass of H₂SO₄ in the solution Given that the solution is 15% H₂SO₄ by weight, this means: - In 100 grams of the solution, there are 15 grams of H₂SO₄. ### Step 2: Calculate the number of moles of H₂SO₄ To find the number of moles, we use the formula: ...
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Molarity: A sample of commercial sulphuric acid is 98% H_(2) SO_(4) by mass and its specfic gravity is 1.84 . Caculate the molartiy of this sulburic acid solution. Strategy: The density of a solution (grams per milliliter) is numercially equal to its specific gravity. Thus, the density of the solution is 98% H_(2) SO_(4) by mass. Thus, every 100g of soultuon contains 98g of pure H_(2) SO_(4) . From the mass of H_(2) SO_(4) . we calculate its moles and from the density , we calculate its volume. Finally, we calculate molartity using its definition.