A solution is prepared by mixing 0.10 of 0.12 M sodium chloride with 0.23 L of a 0.18 M magnesium chloride solution. What is the pCl- of the

Question

A solution is prepared by mixing 0.10 of 0.12 M sodium chloride with 0.23 L of a 0.18 M magnesium chloride solution. What is the pCl- of the resulting solution?

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Tryphena 5 years 2021-07-14T06:45:53+00:00 1 Answers 62 views 0

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  1. Gerda
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    2021-07-14T06:46:57+00:00
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    Answer:

    pCl⁻ = 0.54

    Explanation:

    First we calculate how many Cl⁻ moles are coming from each substance, using the given volumes and concentrations:

    • 0.12 M NaCl * 0.10 L = 0.012 mol NaCl = 0.012 mol Cl⁻
    • 0.18 M MgCl₂ * 0.23 L = 0.0414 mol MgCl₂ = (0.0414 * 2) 0.0828 mol Cl⁻

    The final volume of the mixture is = 0.10 L + 0.23 L = 0.33 L

    Now we calculate [Cl⁻], using the total number of Cl⁻ moles and the final volume:

    • [Cl⁻] = (0.012 mol + 0.0828 mol) / 0.33 L = 0.29 M

    Finally we calculate the pCl⁻ of the resulting solution:

    • pCl⁻ = -log[Cl⁻]
    • pCl⁻ = 0.54

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