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HCl is a strong acid, so we assume that it completely breaks up into ions in solution.
HCl ----> H+ & Cl-
if we have 0.01m of HCl, it will give 0.01m of H+ and 0.01m Cl-
pH = -log [H+]
pH = -log 0.01
pH = 2
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Calculate the molarity of HCl of pH 5.7?
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What pH would you get from dilute hydrochloric acid?
It solely depends on H+ concentration: each HCl gives one H+ , to calculate use pH = -log[H+] So, at [HCl]=1.0 >> pH= 0.0 at [HCl]=0.5 >> pH= 0.7 at [HCl]=0.1 >> pH= 1.0 at [HCl]=1.0*10-5 >> pH= 5.0 but don't ever use this simplified 'acid pH' calculus method when the answer comes close to (or exceeds) 6.5, 7 or 8 etc.
How to calculate pH of 1N HCl solution?
pH = -log10[H+], where [H+] is the hydrogen ion concentration. So, in this case, pH = -log10[1], yielding pH = 0.
What is the pH of .25M HCl?
- log(0.25 M HCl) = 0.6 pH ------------
What is the pH of a 1.0x10-4m hcl solution?
- log(0.00450 M HCl)= 2.3 pH=======
Calculate the molarity of HCl of pH 5.7?
you have to learn chemistry
If pH is 3 what is the concentration of Hydrogen?
[H+]=10-pH=10-3=.001M
What pH would you get from dilute hydrochloric acid?
It solely depends on H+ concentration: each HCl gives one H+ , to calculate use pH = -log[H+] So, at [HCl]=1.0 >> pH= 0.0 at [HCl]=0.5 >> pH= 0.7 at [HCl]=0.1 >> pH= 1.0 at [HCl]=1.0*10-5 >> pH= 5.0 but don't ever use this simplified 'acid pH' calculus method when the answer comes close to (or exceeds) 6.5, 7 or 8 etc.
How to calculate pH of 1N HCl solution?
pH = -log10[H+], where [H+] is the hydrogen ion concentration. So, in this case, pH = -log10[1], yielding pH = 0.
How calculate pH for a solution?
HCl is a strong acid and dissociates completely. Therefore it can be found using the equation: ph= -log [H+]
What is the pH of .25M HCl?
- log(0.25 M HCl) = 0.6 pH ------------
What is the pH of a 1.0x10-4m hcl solution?
- log(0.00450 M HCl)= 2.3 pH=======
What is the pH of 260M HCl?
.260 M of HCL, not 260 More than likely correct, but, - log(0.260 M HCl) = 0.6 pH ----------- ( pH can be below 1 )
Is pH 2.0 HCl the same with 0.1 M HCl?
pH=-lg[H+][H+]=10-pHWith pH=2.0:Corrected:[H+]= 10-pH = 10-2.0 = 0.010 M HCL
What is the pH of 0.25 M HCl?
Since HCl is a strong acid it completely dissociates. Therefore [H+] = [HCl] and this case = 0.25 M. pH = -log [H+] = 0.602
What is pH value of 1N HCl?
In 0.01 M of HCl, the concentration of the Hydronium ions is 0.01M as well since HCl is monoprotic. pH = -log [H3O+] = -log 0.01 = -log10-2 = -(-2log10) = 2 Thus, the pH of 0.01 M HCl is 2.
What is pH of 0.1 N HCL?
0.1 M HCl =============
