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Science Chemistry CHEM:ATOM FOC 2E CL (TEXT)

The p H and p O H of the solutions with the following hydrogen ions or hydroxide ion concentrations. Indicate which solutions are acidic, basic, or neutral. H + = 3.45 × 10 - 8 M H + = 2.0 × 10 - 5 M H + = 7.0 × 10 - 8 M O H - = 8.56 × 10 - 4 M Solution: p H = 7.46 ; p O H = 6.54 ; solution is basic. p H = 4.70 ; p O H = 9.30 ; solution is acidic. p H = 7.15 ; p O H = 6.85 ; solution is basic. p H = 10.93 ; p O H = 3.07 ; solution is basic. 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 sum of p H and p O H for any aqueous solution is always 14.00 at 25 C . 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 . Formula: p H = - log ⁡ H + p O H = - log ⁡ O H - p H + p O H = 14.00 Given: H + = 3.45 × 10 - 8 M H + = 2.0 × 10 - 5 M H + = 7.0 × 10 - 8 M O H - = 8.56 × 10 - 4 M Calculations: H + = 3.45 × 10 - 8 M Calculate the p H : p H = - log ⁡ H + p H = - log ⁡ ( 3.45 × 10 - 8 M ) p H = 7.46 Calculate p O H : p H + p O H = 14 p O H = 14 - 7.46 p O H = 6.54 Since the value of p H = 7.46 > 7 , the solution is basic. H + = 2.0 × 10 - 5 M Calculate the p H : p H = - log ⁡ ( 2.0 × 10 - 5 ) p H = 4.70 Calculate p O H : p O H = 14 - 4.70 p O H = 9.30 Since the value of = 4.70 < 7 , the solution is acidic. H + = 7.0 × 10 - 8 M Calculate the p H : p H = - log ⁡ ( 7.0 × 10 - 8 ) p H = 7.15 Calculate the p O H : p O H = 14 - 7.15 p O H = 6.85 Since the value of p H = 7.15 > 7 , the solution is basic. O H - = 8.56 × 10 - 4 M Calculate the p O H : p O H = - log ⁡ O H - p O H = - log ⁡ 8.56 × 10 - 4 p O H = 3.07 Calculate the p H : p H + p O H = 14 p H = 14 - 3.07 p H = 10.93 Since the value of p H = 10.93 > 7 , the solution is basic. Conclusion: For an acidic solution, p H < 7 , for a basic solution p H > 7 and for a neutral solution p H = 7.00 .

The p H and p O H of the solutions with the following hydrogen ions or hydroxide ion concentrations. Indicate which solutions are acidic, basic, or neutral. H + = 3.45 × 10 - 8 M H + = 2.0 × 10 - 5 M H + = 7.0 × 10 - 8 M O H - = 8.56 × 10 - 4 M Solution: p H = 7.46 ; p O H = 6.54 ; solution is basic. p H = 4.70 ; p O H = 9.30 ; solution is acidic. p H = 7.15 ; p O H = 6.85 ; solution is basic. p H = 10.93 ; p O H = 3.07 ; solution is basic. 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 sum of p H and p O H for any aqueous solution is always 14.00 at 25 C . 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 . Formula: p H = - log ⁡ H + p O H = - log ⁡ O H - p H + p O H = 14.00 Given: H + = 3.45 × 10 - 8 M H + = 2.0 × 10 - 5 M H + = 7.0 × 10 - 8 M O H - = 8.56 × 10 - 4 M Calculations: H + = 3.45 × 10 - 8 M Calculate the p H : p H = - log ⁡ H + p H = - log ⁡ ( 3.45 × 10 - 8 M ) p H = 7.46 Calculate p O H : p H + p O H = 14 p O H = 14 - 7.46 p O H = 6.54 Since the value of p H = 7.46 > 7 , the solution is basic. H + = 2.0 × 10 - 5 M Calculate the p H : p H = - log ⁡ ( 2.0 × 10 - 5 ) p H = 4.70 Calculate p O H : p O H = 14 - 4.70 p O H = 9.30 Since the value of = 4.70 < 7 , the solution is acidic. H + = 7.0 × 10 - 8 M Calculate the p H : p H = - log ⁡ ( 7.0 × 10 - 8 ) p H = 7.15 Calculate the p O H : p O H = 14 - 7.15 p O H = 6.85 Since the value of p H = 7.15 > 7 , the solution is basic. O H - = 8.56 × 10 - 4 M Calculate the p O H : p O H = - log ⁡ O H - p O H = - log ⁡ 8.56 × 10 - 4 p O H = 3.07 Calculate the p H : p H + p O H = 14 p H = 14 - 3.07 p H = 10.93 Since the value of p H = 10.93 > 7 , the solution is basic. Conclusion: For an acidic solution, p H < 7 , for a basic solution p H > 7 and for a neutral solution p H = 7.00 .

Solution Summary: The author explains the relationship between pH and pOH for any aqueous solution, which is always 14.00 at 25 °C.

CHEM:ATOM FOC 2E CL (TEXT)

CHEM:ATOM FOC 2E CL (TEXT)

2nd Edition

ISBN: 9780393284218

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

Publisher: WW Norton & Co

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CHEM:ATOM FOC 2E CL (TEXT)

Ch. 15 - Prob. 15.1VP Ch. 15 - Prob. 15.2VP Ch. 15 - Prob. 15.3VP Ch. 15 - Prob. 15.4VP Ch. 15 - Prob. 15.5VP Ch. 15 - Prob. 15.6VP Ch. 15 - Prob. 15.7VP Ch. 15 - Prob. 15.8VP Ch. 15 - Prob. 15.9VP Ch. 15 - Prob. 15.10VP

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