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Title: What is the pH of a 0.005 M HCl solution? Assume complete dissociation. Post by: ppk on May 15, 2011 What is the pH of a 0.005 M HCl solution? Assume complete dissociation.
Title: Re: What is the pH of a 0.005 M HCl solution? Assume complete dissociation. Post by: Ali on May 17, 2011 -log[0.005]=2.3 (complete dissociation --> considered as H+ ion--> pH= -log[H+])
Title: Re: What is the pH of a 0.005 M HCl solution? Assume complete dissociation. Post by: ppk on May 17, 2011 -log[0.005]=2.3 (complete dissociation --> considered as H+ ion--> pH= -log[H+]) Thanks brother. Title: Re: What is the pH of a 0.005 M HCl solution? Assume complete dissociation. Post by: chemb on May 17, 2011 pH = 2.3. If pH = - log [H+] and HCl is a strong acid, we can assume complete dissociation will occur in solution.
Title: Re: What is the pH of a 0.005 M HCl solution? Assume complete dissociation. Post by: gage on Nov 13, 2018 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 |