PH CHEM, PLEASE HELP QUICK! NO LINKS/VIRUSES PLEASE! A solution is created by measuring 3.60 x 10-3 moles of NaOH and 5.95 x 10-

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PH CHEM, PLEASE HELP QUICK! NO LINKS/VIRUSES PLEASE!

A solution is created by measuring 3.60 x 10-3 moles of NaOH and 5.95 x 10-4 moles of HCl into a container and then water is added until the final volume is 1.00 L. What is the pH of this solution?

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Diễm Thu 5 years 2021-08-18T06:28:27+00:00 1 Answers 901 views 1

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  1. Sigrid
    -1
    2021-08-18T06:30:25+00:00
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    Answer:

    The pH of the solution is 11.48.

    Explanation:

    The reaction between NaOH and HCl is:

    NaOH  +  HCl  →  H₂O  +  NaCl

    From the reaction of 3.60×10⁻³ moles of NaOH and 5.95×10⁻⁴ moles of HCl we have that all the HCl will react and some of NaOH will be leftover:

    n_{NaOH}} = n_{i_{NaOH}} - n_{HCl} = 3.60 \cdot 10^{-3} moles - 5.95 \cdot 10^{-4} moles = 3.01 \cdot 10^{-3} moles

    Now, we need to find the concentration of the OH⁻ ions.

    [OH^{-}] = \frac{n_{NaOH}}{V}

    Where V is the volume of the solution = 1.00 L                

    [OH^{-}] = \frac{n_{NaOH}}{V} = \frac{3.01 \cdot 10^{-3} moles}{1.00 L} = 3.01 \cdot 10^{-3} mol/L

    Finally, we can calculate the pH of the solution as follows:

    pOH = -log([OH^{-}]) = -log(3.01 \cdot 10^{-3}) = 2.52

    pH + pOH = 14

    pH = 14 - pOH = 14 - 2.52 = 11.48

    Therefore, the pH of the solution is 11.48.

    I hope it helps you!

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