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10 February, 19:26

Volume of 0.150 M NaOH solution required to neutralize 25mL of a 0.055 M HCl solution?

Equation of the reaction: NaOH (aq) + HCl (aq) - --> H2O (l) + NaCl (aq)

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  1. 10 February, 21:48
    0
    9.17 mL

    Explanation:

    In this question we are given;

    Molarity of NaOH as 0.150 M Molarity of the acid, HCl as 0.055 M Volume of the acid, HCl as 25 mL Equation for the reaction as;

    NaOH (aq) + HCl (aq) → H2O (l) + NaCl (aq)

    We are required to determine the volume of the alkali, NaOH used;

    Step 1: Determine the moles of the acid, HCl

    Molarity = Number of moles : Volume

    Thus, rearranging the formula;

    Moles = Molarity * volume

    = 0.055 M * 0.025 L

    = 0.001375 moles

    Step 2: Moles of the alkali, NaOH From the reaction; 1 mole of HCl reacts with 1 mole of NaOH

    Therefore;

    Moles of HCl = Moles of NaOH

    Hence; Moles of NaOH = 0.001375 moles

    Step 3: Determine the volume of the alkali, NaOH From the previous equation;

    Molarity = Moles : Volume

    Rearranging the equation;

    Volume = Moles : Molarity

    Therefore;

    Volume of NaOH = 0.001375 moles : 0.150 M

    = 0.00917 L, but, 1 L = 1000 mL

    = 9.17 mL

    Therefore, the volume of NaOH required is 9.17 mL
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