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Using the expression Ka=[H+][A−][HA] , explain how to determine which solution has the lower pH , 0.10MHF(aq) or 0.10MHC2H3O2(aq) . Do not perform any numerical calculations.

Sagot :

ajeigbeibraheem

Answer:

0.10MHF(aq)

Explanation:

Given that:

[tex]K_a = \dfrac{[H^+][A^-]}{HA}[/tex] , to find the solution with a lower pH between 0.10MHF(aq) or 0.10MHC2H3O2(aq).

Recall that:

The higher the Ka value, the higher the ionization, hence more formation of protons in the solution. Also, higher H⁺ in solution results in a lower pH value.

Since HF have a higher Ka value, then HF solution will have a lower pH.

The acidity and alkalinity measure of a substance based on hydroxyl or hydrogen ion released is called pH. It is measured based on the pH scale that tells about the acidity and basicity of the substance.

0.10 M [tex]\rm HF[/tex] (aq) has lower pH.

The pH can be explained as:

The acid dissociation constant ([tex]\rm K_{a}[/tex]) is given by,

[tex]\rm K_{a} = \dfrac{[H^{+}][A^{-}]}{[HA]}[/tex]

  • The value [tex]\rm K_{a}[/tex] of can be used for determining the lower and higher pH.

  • When the [tex]\rm K_{a}[/tex] value is high then the ionization of the substance will be higher resulting in the release of more protons in the solution.

  • When [tex]\rm H^{+}[/tex] is high then the pH will be lower and the solution will be more acidic.

  • The [tex]\rm K_{a}[/tex] value of [tex]\rm HF[/tex] is more compared to the [tex]\rm HC_{2}H_{3}O_{2}[/tex] resulting in lower pH and more acidity.

Therefore, 0.10 M [tex]\rm HF[/tex] (aq) has lower pH.

Learn more about pH and acid dissociation here:

https://brainly.com/question/12729588

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