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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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"A commerically available sample of sulphuric acid is 15% "H_(2)SO_(4)" by mass" ("density "= 1.10 g mL^(-1)). Calculate : Molarity Normality Molality of solution.

Commercially available sulphuric acid contains 93% acid by mass and has a density of 1.84 g mL^(-1) . Calculate (i) the molarity of the solution (ii) volume of concentrated acid required to prepare 2.5 L of 0.50 M H_(2)SO_(4)

Knowledge Check

  • Concentrated aqueous sulphuric acid is 98% H_(2)SO_(4) by weight and has a density of 1.80 gmL^(-1) . Molarity of solution

    A
    1 M
    B
    1.8 M
    C
    18 M
    D
    1.5 M

  • The molarity of H_(2)SO_(4) is 18 M. Its density is 1.8 g mL^(-) . Hence, molality is:

    A
    36
    B
    200
    C
    500
    D
    18

  • The molarity of 90% H_(2)SO_(4) solution is [density = 1.8 gm/ml]

    A
    `1.8`
    B
    `48.4`
    C
    `91.83`
    D
    `94.6`

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    A solution of glucose in water is labelled as 10% (w/W). The density of the solution is 1.20 g mL^(-1) Calculate (i) molality (ii) molarity and (iii) mole fraction of each component in solution.

    Calculate the volume of 80% H_(2)SO_(4) by weight (density = 1.80 g mL^(-1) ) required to preapre 1L of 0.2 M H_(2)SO_(4) .

    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.

    Concentrated aqueous sulphuric acid is 98% H_(2)SO_(4) by mass and has a density of "1.80 g mL"^(-1) . Volume of the acid required to make one litre of 0.1 M H_(2)SO_(4) solution is

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