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27 February, 16:09

What volume of a concentrated HCl solution, which is 36.0% HCl by mass and has a density of 1.179 g/mL, should be used to make 5.20 L of an HCl solution with a pH of 1.70

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  1. 27 February, 16:37
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    The volume we need is 8.89 mL

    Explanation:

    We analyse dа ta:

    36 % by mass → 36 g of HCl in 100 g of solution

    Solution's density = 1.179 g/mL

    5.20L → Volume of diluted density

    pH = 1.70 → [H⁺] = 10⁻¹'⁷⁰ = 0.0199 M

    HCl → H⁺ + Cl⁻

    0.0199

    pH can gives the information of protons concentrations, so as ratio is 1:1, 0.0199 M is also the molar concentration of HCl

    Let's verify the molar concentration of the concentrated solution:

    We convert the mass to moles: 36 g / 36.45 g/mol = 0.987 moles

    As the solution mass is 100 g, we apply density to find out the volume:

    Density = Mass / volume → Volume = Mass / Density

    Volume = 100 g / 1.179 g/mL → 84.8 mL

    Let's convert the volume from mL to L in order to define molarity

    84.8 mL. 1L / 1000mL = 0.0848 L

    Molarity → 0.987 mol / 0.0848L = 11.6M

    Let's apply the dilution formula:

    M concentrated. V concentrated = M diluted. V diluted

    11.6 M. V concentrated = 0.0199M. 5.20L

    V concentrated = (0.0199M. 5.20L) / 11.6M → 8.89*10⁻³L

    We can say, that the volume we need is 8.89 mL
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