Chemistry
Chemistry
10th Edition
ISBN: 9781305957404
Author: Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher: Cengage Learning
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Bronsted-Lowry base in inorganic chemistry is any chemical substance that can accept a proton from the other chemical substance it is reacting with.
Question

How do I write a balenced net ionic equation?

## Data Table: Part B1 | Salt Solution | Measured pH | |----------------|-------------| | 0.100 M NaHSO₄ | 2.20 | | 0.100 M Na₂CO₃ | 11.29 | | 0.100 M NH₃ | 10.87 | | 0.100 M NaCl | 7.67 | ### Instructions: For each solution having a pH less than 6 or greater than 8, write a balanced net ionic reaction that shows why the concentration of H₃O⁺ (if the solution is acidic) or OH⁻ (if the solution is basic) is greater in this solution than it would be in pure water alone. *Remember that net ionic reactions omit spectator ions.*
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Transcribed Image Text:## Data Table: Part B1 | Salt Solution | Measured pH | |----------------|-------------| | 0.100 M NaHSO₄ | 2.20 | | 0.100 M Na₂CO₃ | 11.29 | | 0.100 M NH₃ | 10.87 | | 0.100 M NaCl | 7.67 | ### Instructions: For each solution having a pH less than 6 or greater than 8, write a balanced net ionic reaction that shows why the concentration of H₃O⁺ (if the solution is acidic) or OH⁻ (if the solution is basic) is greater in this solution than it would be in pure water alone. *Remember that net ionic reactions omit spectator ions.*
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