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14 February, 14:54

A 17.85 mL volume of nitric acid neutralizes 25.00 mL of 0.150 mol/L sodium hydroxide. What is the concentration of the nitric acid when the pH is exactly 7.0?

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Answers (2)
  1. 14 February, 15:01
    0
    0.005 M

    Explanation:

    Nitric acid is a strong acid, so it's concentration is equal to the amount of [H+] ions in solution. NaOH is also a strong base, meaning the same thing but with it's [OH-] ions. In order for a base to be neutralized, the number [H+] ions inserted must be equal to the number of [OH-] ions present.

    Sodium Hydroxide Volume: 25 mL / 1000 = 0.025 L

    Sodium Hydroxide Molarity: 0.15 mol/L * 0.025 L = 0.00375 M.

    Now we can use M1V1=M2V2 to find the concentration of the nitric acid:

    (0.025) (0.00375) = (17.85/1000) (X)

    X = 0.005M
  2. 14 February, 17:58
    0
    0.210 mol/L

    Explanation:

    NaOH (aq) + HNO3 (aq) = HOH + NaNO3 (aq)

    25ml 17.85ml

    6.150mol/L

    NaOH = CxV = 0.150mol/L x 25 = 3.75mmol x 1/1 = 3.75mmol HNO3

    C=n/V = 3.75mmol/17.85ml = 0.210 mol/L
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