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
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.
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.
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.
The pH of a 6M HCl solution is 0.
The pH scale is a convenient method for expressing the hydronium ion concentration of a solution. pH = log(1/[H+]) = -log [H+]. [H+] is the hydronium ion concentration in M (molarity), which is the number of moles of solute per liter of 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 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.
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.
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.
The pH of a 6M HCl solution is 0.
The pH scale is a convenient method for expressing the hydronium ion concentration of a solution. pH = log(1/[H+]) = -log [H+]. [H+] is the hydronium ion concentration in M (molarity), which is the number of moles of solute per liter of solution.
The pH of a solution containing 6M HCl is 0.
- log(0.00450 M HCl)= 2.3 pH=======
The pH of a 42m HCl solution would be approximately -log(42) = -1.62. This solution is strongly acidic.
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.
its PH is 3
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.