Consider the titration of a 26.1 −mL sample of 0.125 M RbOH with 0.110 M HCl. Determine each of the following. the initial pH

Question

Consider the titration of a 26.1 −mL sample of 0.125 M RbOH with 0.110 M HCl. Determine each of the following.

the initial pH
the volume of added acid required to reach the equivalence point
the pH at 6.0 mL of added acid
the pH at the equivalence point
the pH after adding 4.8 mL of acid beyond the equivalence point

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Bình An 17 hours 2021-07-22T04:20:19+00:00 1 Answers 0 views 0

Answers ( )

    0
    2021-07-22T04:21:31+00:00

    Answer:

    We’re asked to find the molar concentration of the

    NaCl

    solution given some titration data.

    Let’s first write the chemical equation for this reaction:

    NaOH

    (

    a

    q

    )

    +

    HCl

    (

    a

    q

    )

    NaCl

    (

    a

    q

    )

    +

    H

    2

    O

    (

    l

    )

    Using the molarity equation, we can find the number of moles of

    HCl

    that reacted:

    molarity

    =

    mol solute

    L soln

    mol solute

    =

    (

    molarity

    )

    (

    L soln

    )

    mol HCl

    =

    (

    0.105

    mol

    L

    )

    (

    0.0250

    L

    )

    =

    0.00263

    mol HCl

    (volume converted to liters)

    Now, using the coefficients of the chemical reaction, we can determine the number of moles of

    NaOH

    that reacted:

    0.00263

    mol HCl

    (

    1

    l

    mol NaOH

    1

    mol HCl

    )

    =

    0.00263

    mol NaOH

    Lastly, we’ll use the molarity equation (using given volume of

    NaOH soln

    ) again to determine the molarity of the sodium hydroxide solution:

    molarity

    =

    mol solute

    L soln

    M

    NaOH

    =

    0.00263

    l

    mol

    0.315

    l

    L

    =

    0.00833

    M

    (volume converted to liters)

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