Acid base titration problem. Need Help

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To adjust the pH of a solution from 7.17 to 5.85, one must calculate the molar concentration of H3O+ ions at both pH levels. A pH of 7.17 corresponds to a concentration of approximately 6.76 x 10^-8 M, while a pH of 5.85 yields a concentration of about 1.41 x 10^-6 M. The difference in these concentrations indicates the amount of H3O+ needed, which is approximately 1.34 x 10^-6 moles for one liter of solution. Understanding the relationship between pH and molar concentration is crucial for solving such titration problems. This process highlights the importance of precise calculations in acid-base chemistry.
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How many moles of H3O+ must be added to one liter of a solution to adjust the pH from 7.17 to 5.85?

Correct answer 1.34E-6 (1.34 * 10-6)

The correct answer is given, however I would like to know how to do this problem.
 
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See definition of pH - http://www.chembuddy.com/?left=pH-calculation&right=pH-definition

The pH is related to the molar concentration.

pH = 7.17 yields a molar concentration of 10-7.17 = 6.76 x 10-8 M, or moles/liter

Now try to find the number of moles in one liter for pH = 5.85.

Take the difference which gives the number of moles of H+ or H3O+ one needs to add to one liter.
 
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