A student titrates a 25 ml of an unknown concentration of hcl with 35 ml of a 0.890 m solution of koh to reach the equivalence point. what is the ph of the hcl solution? 1.2 -0.10

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07-04-2018
Chemistry

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A student titrates a 25 ml of an unknown concentration of hcl with 35 ml of a 0.890 m solution of koh to reach the equivalence point. what is the ph of the hcl solution? 1.2 -0.10

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mixter17 mixter17 · Answer 1 · 2018-04-21T02:10:59+02:00

Hello!

The chemical equation for the neutralization of HCl with KOH is the following:

HCl(aq) + KOH(aq) → KCl(aq) + H₂O(l)

To calculate the concentration of the unknown solution, we can apply the following equation for the equivalence point:

[tex]moles HCl=molesKOH \\ \\ cHCl*vHCl=cKOH*vKOH \\ \\ cHCl= \frac{cKOH*vKOH}{vHCl}= \frac{0,890M*35mL}{25 mL}=1,246 M [/tex]

So, the concentration of the HCl solution is 1,246 M

Have a nice day!