Solutions are classified into acid or base based on the pH value. If pH value is less than 7, the solution is acidic and if pH is greater than 7, the solution is basic. pH of a solution can be determined by identifying the concentration of in the solution.
…… (1)
pH is the measure of hydrogen ion present in a solution. It is the negative logarithm of the H+ concentration to the base 10. It gives the acidic strength of the solution.
…… (2)
pOH is the measure of the hydroxide ion present in a solution.
It is the negative logarithm of the concentration to the base 10. It gives the basic strength of the solution.
Ionic product for water:
…… (3)
…… (4)
The pH and pOH of the aqueous solution is
Calculate the pH and the pOH of an aqueous solution that is 0.050 M in HCl(aq)...
Calculate the pH and the pOH of an aqueous solution that is 0.050 M in HCl(aq) and 0.085 M in HBr(aq) at 25 °C. pH = pOH =
Calculate the pH and the pOH of an aqueous solution that is 0.050 M in HCl(aq) and 0.070 M in HBr(aq) at 25°C
Calculate the pH and the pOH of an aqueous solution that is 0.020 M in HCl(aq) and 0.055 Min HBr(aq) at 25°C. pH = pOH = Question Source: MRG - General Chemistry Publisher: University Science
Calculate the pH and the pOH of an aqueous solution that is 0.030 M in HCl(aq) and 0.095 M in HBr(aq) at 25 C Thank you in advance
Calculate the pH and the pOH of an aqueous solution that is 0.040M in HCl(aq)and 0.075M in HBr(aq)at 25 °C. pH= pOH
Calculate the pH and pOH of 1.2 x 10-3 M HCl solution. Calculate pH, pOH and [OH-] of 0.1 M HNO3 solution. If a solution X has pH = 5, which of the following is true: Solution X is neutral. H3O+ ion concentration is higher than OH- concentration. c. OH- ion concentration is higher than H3O+ concentration.
(a) The hydroxide ion concentration in an aqueous solution of HCl is 2.6x10-13 M. Calculate [H3O+], pH, and pOH for this solution. [H30*]=1 M pH= pOH = (b) The pH of an aqueous solution of HNO3 is 2.50. Calculate [H3O+], [OH"), and pOH for this solution. [H3O+]= M [OH]= M pOH =
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