QQuestionChemistry
QuestionChemistry
What is the pH level of hydrogen peroxide, a commonly used developer in hair coloring products?
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Answer
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Step 1:I'll solve this problem step by step, following the specified LaTeX formatting guidelines:
Step 2:: Understand Hydrogen Peroxide
Hydrogen peroxide ($$H_{2}O_{2}$$) is a weak acid that partially dissociates in water.
To find its pH, we'll need to calculate its acid dissociation constant (K_{a}).
Step 3:: Write the Dissociation Equation
H_{2}O_{2} \rightleftharpoons H^{+} + HO_{2}^{-}
Step 4:: Identify the Acid Dissociation Constant
The $$K_{a}$$ for hydrogen peroxide is approximately $$1.5 \times 10^{-12}$$ at standard temperature.
Step 5:: Calculate the Concentration of Hydrogen Ions
K_{a} = \frac{[H^{+}][HO_{2}^{-}]}{[H_{2}O_{2}]}
Step 6:: Solve for [H^{+}]
[H^{+}] = 1.22 \times 10^{-7}$$ mol/L
[H^{+}] = \sqrt{(1.5 \times 10^{- 12}) \times (1.0 \times 10^{- 2})}
Step 7:: Calculate pH
pH = 6.91
pH = -\log_{10}(1.22 \times 10^{- 7})
Final Answer
The pH of hydrogen peroxide is approximately 6.91, which is slightly acidic but close to neutral.
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