What is the pH of a solution of 0.00001 M HCl?
Since HCl is a strong acid .00001M HCl will produce a .00001M hydrogen ion concentration. Therefore, the pH will be 5.
Molarity is the concentration of a solution, defined as moles per unit volume. Where, Molarity = moles / volume In this case the molarity of the HCl solution is 0.03 M The pH of this is calculated by the equation below pH = - log [H+] Where [H+] is the concentration of hydrogen ions/ protons present in the solution. As HCl only contains one hydrogen ion per molecule then the concentation of [H+] is 0.03…
What is the pH of a solution prepared by diluting 3.0 ml of 2.5 M HCl to a final volume of 100mL with water?
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
How does the pH level of a dilute solution of HCI compare with the pH level of concentrated solution of the same acid?
A solution of HCl is highly dissociated into ions, A 0.000001 M solution (1 x 10-6) has a pH of 6 ... close to neutral. A 0.001 M solution (1 x 10-3) has a pH of 3 ... more concenterated, but still not a really concentrated solution. A 0.1 M solution (1 x 10-1) has a pH of 1 ... even more concentrated. showing it is more acidic.
By definition [H+]=10-pH so pH = -log[H+]. So for 10 M HCl >>> pH = -log(10) = -1.0. This is only of theoretical importance because pH formula are for ideal solutions, which are only valid for diluted, not concentrated solutions. Also a pH-meter will not give relyable measurements at pH << 1.0 or below.
HCl is a strong acid, therefore we can assume that it ionises completely into H+ (or H3O+ if you prefer) and Cl- ions. Therefore an 0.10 M HCl solution will contain 0.10 moles/L of H+ ions. pH = -log10[H+] where [ ] denotes "concentration of" in moles/L Note that the formal definition of pH relies on the "activity" of H+ (which is the product of an activity coefficient and concentration), but for simple problems this…
pH = -log[H+] That is, the pH of a solution is the negative log of the concentration of hydrogen atoms. The concentration of hydrogen atoms must be in units of Molarity, or moles per liter. In order to determine the pH of a solution containing 1 mole of HCl, you must also know the volume of the solution. I am assuming the question is: What is the pH of 1M HCl, and not 1 mole…