0
Want this question answered?
Be notified when an answer is posted
Add your answer:
Earn +20 pts
What is the pH of an aqueous solution of HCl with a concentration of 42m?
the pH is .377 the pH is .377
The pH of a 0.1 molar aqueous solution of HCl would equal -?
1
What is the pH of a solution whose hydrogen ion concentration is 0.000001?
The answer is 4 - .0001 equals 1X10 -4 which equals a pH of 4
Explain why a 0.10 HCL solution is assumed to have a pH value 1?
HCl is a strong acid. Therefore, it can be expected to fully dissociate in aqueous solution, yielding one hydrogen ion and one chloride ion per molecule. The concentration of the hydrogen ion should thus be the same as the initial concentration of the HCl. Therefore, a 0.10M HCl solution has an H+ concentration of 0.10M. By the equation pH=-log[H+], the pH of this solution is 1.
What is the pH of an aqueous solution C6H12O6?
The solution is neutral.
What has a pH of 1 and completely ionizes in aqueous solution?
HCl
What is the pH of an aqueous solution of HCl with a concentration of 42m?
the pH is .377 the pH is .377
How many liters of water must be added to 1 liter of an aqueous solution of hcl with a pH of 1 to create an aqueous solution with pH of 2?
9
The pH of a 0.1 molar aqueous solution of HCl would equal -?
1
What is the pH of a solution whose hydrogen ion concentration is 0.000001?
The answer is 4 - .0001 equals 1X10 -4 which equals a pH of 4
How much muriatic acid to lower pH of a gallon of water 1ppm?
1 ppm HCl in aqueous solution would have a pH of around 6.
Explain why a 0.10 HCL solution is assumed to have a pH value 1?
HCl is a strong acid. Therefore, it can be expected to fully dissociate in aqueous solution, yielding one hydrogen ion and one chloride ion per molecule. The concentration of the hydrogen ion should thus be the same as the initial concentration of the HCl. Therefore, a 0.10M HCl solution has an H+ concentration of 0.10M. By the equation pH=-log[H+], the pH of this solution is 1.
What is the pH of an aqueous solution C6H12O6?
The solution is neutral.
How do you standardise 0.1M HCl?
Titrate the HCl with an aqueous solution containing a known mass of laboratory grade base, like KOH, and measure the pH after each drop with a computer-based probe.
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
Is pH value only for liquids?
That is correct, only an aqueous solution has a pH value. There are certainly chemicals in either a solid or gaseous state which will have an effect on the pH of an aqueous solution if they dissolve in that solution, but until they do, they do not have a pH.
The pH in aqueous solution of hcl at 25c is 4 hcl0.003 moles was added to 1l of this solution calculate the new pH in the solution assume complete dissociation of hcl?
if its complete dissociation, then the products would be a salt and water, which means the pH is 7 or neutral. OMG, if the pH is currently 4 then [H+] = 1.0 e-4 M (pH = -log[H+]) if you add 0.003 moles then 1.0e-4 M +.003 M = .0031 M (Since the strong acid HCL completely dissociates in aq solution) pH = -log [.0031M] = 2.51
