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The ka of acetic acid (hc2h3o2) is 1. 8 × 10-5. What is the ph at 25. 0 °c of an aqueous solution that is 0. 100 m in acetic acid?

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The pH at 25.0 °c of an aqueous solution that is 0. 100 m in acetic acid is 5.744.

What is ka expression?

The acid dissociation constant is the equilibrium constant of an acid's dissociation reaction.

The ka is given [tex]1. 8 \times 10^-^5[/tex]

From the equation pf ka for weak acid

[tex]\rm H^+ = \sqrt{Ka \times C}[/tex]

Putting the values in the equation

[tex]\rm H^+ = \sqrt{ 1. 8 \times 10^-^5 \times 0.100 } = 0.0000018[/tex]

Now, the [tex]\rm pH = -log[H^+][/tex]

[tex]\rm pH = -log[0.0000018] = 5.744[/tex]

Thus, the pH of acetic acid is 5.744

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