Posted by Mary Ann on Thursday, March 21, 2013 at 1:37am.
(HBr) diluted = 0.000625 x (146.6/860) = about 1.08E-4
pH = -log(H^+) = -log(HBr) since HBr is a strong acid and ionizes 100%.
Then pH + pOH = pKw = 14. You know pH and pKw solve for pOH.
Related Questions
Chemistry - Calculate the pH and the pOH of an aqueous solution that is 0.025 M ...
Chemistry - a 25.0 mL sample of .050 M solution of aqueous trimethylamine is ...
Chemistry - A 2.00 ml sample of an aqueous solution of hydrogen peroxide, H2O2 (...
Chemistry - A 16.6 mL portion of an HBr solution of unknown strength is diluted ...
college chemistry - Calculate the pH of a solution prepared by mixing 150.mL of ...
chemistry - A 0.0875 M solution of aqueous ammonia was titrated with a solution ...
Chemistry - An aqueous solution with a density of 0.998 g/ml at 20 degrees ...
College Chemistry - Calculate the pH of a solution prepared by mixing 250.mL of ...
chemistry - When 25.0 mL of 1.0 M H2SO4 is added to 50.0 mL of 1.0 M NaOH at 25....
Chemistry - Which one of the following pairs of 0.100 mol L-1 solutions, when ...
For Further Reading
