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6 April, 10:39

Calculate the molarity of a solution, given that its volume is 820 mL and that it contains 7.4 g of ammonium chloride, NH, CI.

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Answers (2)
  1. 6 April, 10:56
    0
    Molarity = 0.169M

    Explanation:

    Applying n = CV

    V=820ml = 0.82dm3

    n = m/M = 7.4/53.5 = 0.138mol

    0.138 = C * 0.82

    C = 0.169M
  2. 6 April, 10:59
    0
    The correct answer is 0.17 M

    Explanation:

    We have the following dа ta:

    V = 820 ml x 1 L/1000 ml = 0.82 L

    m = 7.4 g

    Ammonium chloride has the chemical formulae NH₄Cl. So, we calculate the molecular weight (MM) of NH₄Cl from the molar mass of N, H and Cl as follows:

    MM NH₄Cl = 14 g/mol + (4 x 1 g/mol) + 35.4 g/mol = 53.4 g/mol

    Now we have to calculate the number of moles of NH₄Cl we have in the solution. For this, we divide the mass (m) into the molecular weight of NH₄Cl (MM):

    moles NH₄Cl = m/MM = 7.4 g/53.4 g/mol = 0.138 moles

    The molarity of the solution is the number of moles of NH₄Cl in 1 liter of solution. So, we have to divide the number of moles of NH₄Cl into the volume in liters as follows:

    M = number of moles NH₄Cl/V = 0.138 moles/0.82 L = 0.169 mol/L ≅ 0.17 M
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