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Home Q & A Board Science-Related Homework Help Chemistry (Moderator: Laser_3)
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ppk ppk
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13 years ago
What is the pH of a 0.005 M HCl solution? Assume complete dissociation.
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Ali
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#1
13 years ago
-log[0.005]=2.3 (complete dissociation Rightwards Arrow considered as H+ ion--> pH= -log[H+])
ppk Author
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#2
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13 years ago
Quote from: Ali (13 years ago)
-log[0.005]=2.3 (complete dissociation Rightwards Arrow considered as H+ ion--> pH= -log[H+])

Thanks brother.
wrote...
#3
13 years ago
pH = 2.3. If pH = - log [H+] and HCl is a strong acid, we can assume complete dissociation will occur in solution.
wrote...
#4
5 years ago
HCL + H20 <-> H30+ + CL-

you can also look at it like this

HCL <-> H+ + Cl-

HCL is a strong acid, therefore it dissociates completely. This means that for every molecule of HCL you have, you get a H+ ion and a Cl- ion. So a 0.005M solution of HCL gives a [H+] of 0.005M

pH can be expressed as the -log10([H+])

so, -log10(0.005) = 2.3

The pH of a 0.005M solution of HCl is 2.3
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