0
The answer depends on several unspecified variables, most importantly the final molarity of the solution, which depends on the final volume.
You can calculate the value yourself using the formula:
pH = -log[H+]
where [H+] is the final concentration of H+ ions in solution. For HCl, [H+] is equal to molarity.
So, for example, if you add 50.0 ml of 1.0M HCl to 950 ml of deionized water, your final concentation is:
(50.0 ml/1000 ml) * (1.0M) = 0.05M
Therefore:
pH = -log[0.05] = 1.3
If your question was something like this: 100.mL of 0.200M HCl is titrated with 0.250M NaOH.
A) What is the pH of the solution after 50.0mL of base has been added?
B)What is the pH of the solution at the equivalence point?
A) moles HCl = 100 x 0.2 /1000 = 0.02
Moles NaOH = 50 x 0.250 / 1000 = 0.0125
moles HCl in excess = 0.02 - 0.0125 = 0.0075
Total volume = 150 mL = 0.150 L
[H+] = 0.0075 / 0.150 = 0.05 M
pH = - log 0.05 = 1.30
B) at equivalence point [OH-] = [H+] so pH = 7
.003 L HCL * 2.5 moles HCL/1L = .0075 moles HCL
.0075 moles HCL/ .1 L HCL = .075 M HCL = .075 M H3O+
pH = -log[H3O+]
pH = -log[.075] = 1.12
this of course is not adjusted for activities of the ions in solution, but it would be very close to this value.
The pH of a solution made by mixing 40.00 mL of 0.10 M HCl with 25.00 mL of 0.10 M KOH:
Here the molarity of base and acid are same but the volume of acid is more than the volume of base so the resultant solution is acidic.
The concentration of OH- in solution = (molarity of base * volume of base - molarity of acid * volume of acid) / total volume
= (40 mL*0.1M - 25 mL *0.1 M ) / (40 mL +25mL)/ 1000)
= 0.021428571 M
pH = -log(0.021428571) = 1.669
The pH of a 0.100 M HCl solution is 1. The strong acid, HCl, ionizes completely in water to produce H+ ions, resulting in a highly acidic solution with a low pH value.
It should be some where around .10. But this is a conjecture as the correspondent has not had Chemistry for many years and the answers provided on the net are not very clear.
Add your answer:
Earn +20 pts
The pH of a 0.1 molar aqueous solution of HCl would equal -?
The pH of a 0.1 molar aqueous solution of HCl would be 1. This is because HCl is a strong acid that completely dissociates in water to produce H+ ions, resulting in a high concentration of H+ ions in solution, leading to a low pH value.
What is the pH of a 0.00001 molar HCl solution A 1 B 9 C 5 D 4?
The pH of a 0.00001 molar HCl solution is 5. HCl is a strong acid, and at this concentration, it would dissociate almost completely in water to produce H+ ions, resulting in a pH of 5.
How can you prepare several different pH solutions from a 1 Molar stock solution of HCl?
To prepare several different pH solutions from a 1 Molar stock solution of HCl, you can dilute the stock solution with water to achieve the desired pH. You can use a pH meter to measure and adjust the pH as needed by adding either more stock solution or more water. Make sure to handle HCl with caution as it is a strong acid.
How is the pH of the solution calculated?
The pH of a solution is calculated using the formula pH = -log[H+], where [H+] is the concentration of hydrogen ions in the solution. Lower pH values indicate acidic solutions, while higher pH values indicate basic solutions.
What is the pH of a 1.0x10-4m hcl solution?
The pH of a 1.0x10^-4 M HCl solution is 4. This is because HCl dissociates completely in water to form H+ ions, resulting in an acidic solution.
What is the pH of a 0.280 molar HCl solution?
The pH of a 0.280 M HCl solution is approximately 0.55. This is because HCl is a strong acid that dissociates completely in solution to produce H+ ions, leading to a low pH value.
The pH of a 0.1 molar aqueous solution of HCl would equal -?
The pH of a 0.1 molar aqueous solution of HCl would be 1. This is because HCl is a strong acid that completely dissociates in water to produce H+ ions, resulting in a high concentration of H+ ions in solution, leading to a low pH value.
What is the pH of a 0.00001 molar HCl solution A 1 B 9 C 5 D 4?
The pH of a 0.00001 molar HCl solution is 5. HCl is a strong acid, and at this concentration, it would dissociate almost completely in water to produce H+ ions, resulting in a pH of 5.
How can you prepare several different pH solutions from a 1 Molar stock solution of HCl?
To prepare several different pH solutions from a 1 Molar stock solution of HCl, you can dilute the stock solution with water to achieve the desired pH. You can use a pH meter to measure and adjust the pH as needed by adding either more stock solution or more water. Make sure to handle HCl with caution as it is a strong acid.
How is the pH of the solution calculated?
The pH of a solution is calculated using the formula pH = -log[H+], where [H+] is the concentration of hydrogen ions in the solution. Lower pH values indicate acidic solutions, while higher pH values indicate basic solutions.
What is the pH of a 1.0x10-4m hcl solution?
The pH of a 1.0x10^-4 M HCl solution is 4. This is because HCl dissociates completely in water to form H+ ions, resulting in an acidic solution.
What is the pH of an aqueous solution of HCl with a concentration of 42m?
The pH of a 42m HCl solution would be approximately -log(42) = -1.62. This solution is strongly acidic.
What is the pH of 0.0001M aqueous solution of hcl?
The pH of a 0.0001M aqueous solution of HCl is 4. The pH of a solution is calculated using the formula pH = -log[H+], where [H+] is the concentration of hydrogen ions in the solution. Since HCl is a strong acid that dissociates completely in water, the concentration of H+ ions in a 0.0001M solution of HCl is also 0.0001M.
Can an aqueous solution have a pH of zero?
No. pH is a log scale. You can't have a pH of zero. ---- Above answer left in to correct a misconception. Yes, you certainly can have a pH of zero. A 1 molar solution of a strong acid has a pH of zero, and stock HCl (roughly 12 molar) has a pH of about -1.1 or so. pH is the negative log of the hydrogen/hydronium ion concentration, which for a strong acid is approximately the same as the acid concentration. The log of 1 is zero, therefore the pH of a 1 molar solution of a strong acid is zero. The log of 10 is 1, therefore the pH of a 10 molar solution of a strong acid is -1.
What is the pH of a 0.001 M of HCl solution?
its PH is 3
What is the pH of a solution of 0.010 M HCl?
The pH of a 0.010 M HCl solution is approximately 2. This is because HCl is a strong acid that completely dissociates in water to form H+ ions, resulting in an acidic solution.
What is the pH of 10.0L of 0.0020 M HCL?
The pH of a 0.0020 M HCl solution is around 2.70. This is because HCl is a strong acid and dissociates completely in water to form H+ ions, resulting in a low pH.
