In a titration, a few drops of an indicator are added to a flask containing 35.0 milliiters of HNO3(aq) of unknown concentration. After 30.0

Question

In a titration, a few drops of an indicator are added to a flask containing 35.0 milliiters of HNO3(aq) of unknown concentration. After 30.0 millliters of 0.15 M NaOH(aq) solution is slowly added o the flask, the indicator changes color, showing the acid is neutralized. Which choice is a correct numerical setup for calculating the concentration of the HNO3(aq) solution

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Khánh Gia 6 months 2021-07-29T00:45:26+00:00 1 Answers 7 views 0

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    2021-07-29T00:46:46+00:00

    Answer:

    0.13M HNO3 is the concentration of the unknown

    Explanation:

    Nitric acid, HNO3, reacts with NaOH as follows:

    HNO3 + NaOH  → H2O + NaNO3

    Where 1mol HNO3 reacts with 1mol NaOH

    To find the concentration of HNO3 we must find, as first, the moles NaOH added = Moles HNO3 in the solution:

    30mL * (1L / 1000mL) * (0.15mol / 1L) = 0.0045 moles HNO3

    In 35.0mL = 0.035L:

    0.0045 moles HNO3 / 0.035L =

    0.13M HNO3 is the concentration of the unknown

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