HBr is a strong acid.
[H+] = [HBr] = 0.036 M
pH = -log[H+] = -log(0.036) = -(-1.44) = 1.44
pOH = pKw - pH = 14.00 - 1.44 = 12.56
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 0.020 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 0.050 M in HCl(aq) and 0.060 M in HBr(aq) at 25℃.
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 0.030 M in HCl(aq) and 0.095 M in HBr(aq) at 25 C Thank you in advance
Determine eacg of the following for a 0.130 M HBr solution: a) [H3O+] b) pH c)pOH d) write the balanced equation for the reaction with LiOH e) calulate the volume in milliliters, of HBr solution required to nuetralize 35 mL of a .340 M LiOH solution
calculate the pH & POH of a mixture containing 20.0 mL of 0.150 m HBr mixed W/ 40.0 mL of water.
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.
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 POH . [+] , and (OH) for a solution of 0.36 M HCI Question 27 5 pts Calculate the pH pОН [H] and (OH) for a solution of O. of 0.37 MHF