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Solved: Making use of the assumptions we ordinarily make
Chapter , Problem 148(choose chapter or problem)
Making use of the assumptions we ordinarily make in calculating the pH of an aqueous solution of a weak acid, calculate the pH of a \(1.0 \times 10^{-6} M\) solution of hypobromous acid \(\left(\mathrm{HBrO}, K_{\mathrm{a}}=2 \times 10^{-9}\right)\). What is wrong with your answer? Why is it wrong? Without trying to solve the problem, tell what has to be included to solve the problem correctly.
Questions & Answers
QUESTION:
Making use of the assumptions we ordinarily make in calculating the pH of an aqueous solution of a weak acid, calculate the pH of a \(1.0 \times 10^{-6} M\) solution of hypobromous acid \(\left(\mathrm{HBrO}, K_{\mathrm{a}}=2 \times 10^{-9}\right)\). What is wrong with your answer? Why is it wrong? Without trying to solve the problem, tell what has to be included to solve the problem correctly.
ANSWER:Step 1 of 3
Hydronium ion is a fundamental species in aqueous chemistry and plays a crucial role in various chemical reactions. Hydronium ions are formed when acids, such as hydrochloric acid or sulfuric acid, dissociate in water, releasing hydrogen ions that quickly combine with water molecules to form hydronium ion.
Hydronium ions are important in defining the acidity of a solution, as their concentration determines the pH level. The more hydronium ions present, the lower the pH, indicating higher acidity. In neutral water, the concentration of hydronium ions is approximately 1 x 10^-7 moles per liter, corresponding to a pH of \(7\).