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What is the pH of a 0.01 M solution of sulfuric acid (H2SO4)?
What is the pH of a 0.01 M solution of sulfuric acid (H2SO4)?
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What is the pH of a 0.01 M solution of sulfuric acid (H2SO4)?
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H2SO4 is a strong acid and dissociates completely, so pH = -log(0.01) = 2.
Questions & Step-by-step Solutions
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Q: What is the pH of a 0.01 M solution of sulfuric acid (H2SO4)?
Solution:
H2SO4 is a strong acid and dissociates completely, so pH = -log(0.01) = 2.
Steps: 7
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Step 1: Understand that sulfuric acid (H2SO4) is a strong acid, which means it completely breaks apart in water.
Step 2: Recognize that a 0.01 M solution means there are 0.01 moles of H2SO4 in one liter of water.
Step 3: Since H2SO4 dissociates completely, it produces 0.01 moles of H+ ions for every mole of H2SO4.
Step 4: Therefore, the concentration of H+ ions in the solution is also 0.01 M.
Step 5: To find the pH, use the formula pH = -log[H+]. Here, [H+] is 0.01.
Step 6: Calculate the pH: pH = -log(0.01).
Step 7: The result of -log(0.01) is 2, so the pH of the solution is 2.
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