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21 February, 16:01

What is the concentration of a solution of HCl in which a 10.0 mL sample of acid required 50.0 mL of 0.150 M NaOH for neutralization? What is the concentration of a solution of HCl in which a 10.0 mL sample of acid required 50.0 mL of 0.150 M NaOH for neutralization? 0.600 M 0.0300 M 0.750 M 0.150 M 7.50 M

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  1. 21 February, 17:13
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    The answer is 0.75M HCl

    Explanation:

    To calculate the concentration of 10 ml of HCl that would be required to neutralize 50.0 mL of 0.150 M NaOH, we use the formula:

    To calculate the concentration of 10 ml of HCl that would be required to neutralize 50.0 mL of 0.150 M NaOH, we use the formula:

    C1V1 = C2V2

    C1 = concentration of acid

    C2 = concentration of base

    V1 = volume of acid

    V2 = volume of base

    From the information supplied in the question:

    concentration of acid (HCl) is the unknown

    volume of acid (HCl) = 10ml

    concentration of base (NaOH) = 0.15M

    volume of base (NaOH) = 50ml

    C1 x 10ml = 0.15M x 50ml

    C1 x 10 = 7.5

    divide both side by 10

    C1 = 0.75M

    concentration of acid (HCl) is 0.75M
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