Imagine you had HCl with a concentration of exactly 0.10 mol/dm3. If 0.023 dm3 of a sodium hydroxide solution, NaOH (aq), could exactly neut

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Imagine you had HCl with a concentration of exactly 0.10 mol/dm3. If 0.023 dm3 of a sodium hydroxide solution, NaOH (aq), could exactly neutralize 0.040 dm3 of the HCl solution, what is the concentration of the NaOH (aq)

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Thu Hương 3 years 2021-07-31T12:34:50+00:00 1 Answers 14 views 0

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  1. taiduc
    0
    2021-07-31T12:36:06+00:00
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    Answer:

    Explanation:

    Step 1: Calculate the amount of sodium hydroxide in moles

    Volume of sodium hydroxide solution = 25.0 ÷ 1,000 = 0.0250 dm3

    Rearrange:

    Concentration in mol/dm3 =

    Amount of solutein mol = concentration in mol/dm3 × volume in dm3

    Amount of sodium hydroxide = 0.100 × 0.0250

    = 0.00250 mol

    Step 2: Find the amount of hydrochloric acid in moles

    The balanced equation is: NaOH(aq) + HCl(aq) → NaCl(aq) + H2O(l)

    So the mole ratio NaOH:HCl is 1:1

    Therefore 0.00250 mol of NaOH reacts with 0.00250 mol of HCl

    Step 3: Calculate the concentration of hydrochloric acid in mol/dm3

    Volume of hydrochloric acid = 20.00 ÷ 1000 = 0.0200 dm3

    Concentration in mol/dm3 =

    Concentration in mol/dm3 =

    = 0.125 mol/dm3

    Step 4: Calculate the concentration of hydrochloric acid in g/dm3

    Relative formula mass of HCl = 1 + 35.5 = 36.5

    Mass = relative formula mass × amount

    Mass of HCl = 36.5 × 0.125

    = 4.56 g

    So concentration = 4.56 g/dm3

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