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Science Chemistry Chemistry: An Atoms-Focused Approach (Second Edition)

The p H and p O H of the solutions with the following hydrogen ion or hydroxide ion concentrations. Indicate which solutions are acidic, basic, or neutral O H - = 7.69 × 10 - 3 M O H - = 2.18 × 10 - 9 M H + = 4.0 × 10 - 8 M H + = 3.56 × 10 - 4 M Solution: p H = 11.89 ; p O H = 2.11 ; solution is basic. p H = 5.34 ; p O H = 8.66 ; solution is acidic. p H = 7.40 ; p O H = 6.60 ; solution is basic. p H = 3.45 ; p O H = 10.55 ; solution is acidic. Explanation: Concept: p H is the negative logarithm to the base ten of H + ion concentration, whereas p O H is the negative logarithm to the base ten of O H - ion concentration. The relation between p H and p O H is p H + p O H = 14 For an acidic solution, the value of p H is less than 7 and the value of p O H is greater than 7 . For a basic solution, the value of p H is greater than 7 and the value of p O H is less than 7 . For a neutral solution p H = p O H = 7 .00. Formulae: p H = - log ⁡ H + p O H = - log ⁡ O H - p H + p O H = 14 Given: O H - = 7.69 × 10 - 3 M O H - = 2.18 × 10 - 9 M H + = 4.0 × 10 - 8 M H + = 3.56 × 10 - 4 M Calculations: O H - = 7.69 × 10 - 3 M p O H = - log [ O H - ] p O H = - log ( 7.69 × 10 - 3 ) p O H = 2.11 p H = 14.00 - 2.11 p H = 11.89 p H > 7 , so the solution is basic. O H - = 2.18 × 10 - 9 M p O H = - log ⁡ O H - p O H = - l o g ⁡ ( 2.18 × 10 - 9 ) p O H = 8.66 p H = 14 - 8.66 p H = 5.34 p H < 7 , so the solution is acidic. H + = 4.0 × 10 - 8 M p H = - log [ H + ] p H = - log ( 4.0 × 10 - 8 ) p H = 7.40 p O H = 14 - 7.40 p O H = 6.60 p H > 7 , so the solution is basic. H + = 3.56 × 10 - 4 M p H = - log [ H + ] p H = - log ( 3.56 × 10 - 4 ) p H = 3.45 p O H = 14 - 3.45 p O H = 10.55 p H < 7 , so the solution is acidic. Conclusion: We calculated p H and p O H from the given concentrations and determined the acidity or basicity by using the p H scale.

The p H and p O H of the solutions with the following hydrogen ion or hydroxide ion concentrations. Indicate which solutions are acidic, basic, or neutral O H - = 7.69 × 10 - 3 M O H - = 2.18 × 10 - 9 M H + = 4.0 × 10 - 8 M H + = 3.56 × 10 - 4 M Solution: p H = 11.89 ; p O H = 2.11 ; solution is basic. p H = 5.34 ; p O H = 8.66 ; solution is acidic. p H = 7.40 ; p O H = 6.60 ; solution is basic. p H = 3.45 ; p O H = 10.55 ; solution is acidic. Explanation: Concept: p H is the negative logarithm to the base ten of H + ion concentration, whereas p O H is the negative logarithm to the base ten of O H - ion concentration. The relation between p H and p O H is p H + p O H = 14 For an acidic solution, the value of p H is less than 7 and the value of p O H is greater than 7 . For a basic solution, the value of p H is greater than 7 and the value of p O H is less than 7 . For a neutral solution p H = p O H = 7 .00. Formulae: p H = - log ⁡ H + p O H = - log ⁡ O H - p H + p O H = 14 Given: O H - = 7.69 × 10 - 3 M O H - = 2.18 × 10 - 9 M H + = 4.0 × 10 - 8 M H + = 3.56 × 10 - 4 M Calculations: O H - = 7.69 × 10 - 3 M p O H = - log [ O H - ] p O H = - log ( 7.69 × 10 - 3 ) p O H = 2.11 p H = 14.00 - 2.11 p H = 11.89 p H > 7 , so the solution is basic. O H - = 2.18 × 10 - 9 M p O H = - log ⁡ O H - p O H = - l o g ⁡ ( 2.18 × 10 - 9 ) p O H = 8.66 p H = 14 - 8.66 p H = 5.34 p H < 7 , so the solution is acidic. H + = 4.0 × 10 - 8 M p H = - log [ H + ] p H = - log ( 4.0 × 10 - 8 ) p H = 7.40 p O H = 14 - 7.40 p O H = 6.60 p H > 7 , so the solution is basic. H + = 3.56 × 10 - 4 M p H = - log [ H + ] p H = - log ( 3.56 × 10 - 4 ) p H = 3.45 p O H = 14 - 3.45 p O H = 10.55 p H < 7 , so the solution is acidic. Conclusion: We calculated p H and p O H from the given concentrations and determined the acidity or basicity by using the p H scale.

Solution Summary: The author explains the sum of pH and pOH in an aqueous solution is 14.00 at 25 °C.

Chemistry: An Atoms-Focused Approach (Second Edition)

Chemistry: An Atoms-Focused Approach (Second Edition)

2nd Edition

ISBN: 9780393614053

Author: Thomas R. Gilbert, Rein V. Kirss, Stacey Lowery Bretz, Natalie Foster

Publisher: W. W. Norton & Company

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