0
pH=-lg[H+]
[H+]=10-pH
With pH=2.0:
Corrected:
[H+]= 10-pH = 10-2.0 = 0.010 M HCL
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∙ 13y ago
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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 best describes solutions of equal concentrations of HCL and CH3COOH?
Do not have the same 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 )
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 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 best describes solutions of equal concentrations of HCL and CH3COOH?
Do not have the same 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 )
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 =============
Why does pH of HCl increase as HCl is diluted?
The pH increases because the HCl is becoming less acidic. A pH of 7 is neutral. A pH falls below 7, acidity increases. As pH rises above 7, basicity increases. Diluting HCl means that the HCl becomes less concentrated, and therefore, less acidic. As it becomes less acidic, the pH will become more basic, and thus increase.
The pH of a 0.01 M solution of HCl in water would be?
pH = - log[H+] so a 0.01 M solution of HCl has, pH= 2
What is the pH of the solution formed when 100 milliliter of hcl is mixed with 100 milliliter of NaOH?
I think it'd be pH 7. Same amount of both, providing they are the same molarity!
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.
What is the pH of a 0.001 M of HCl solution?
its PH is 3
