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Lab Report #4-2-1: 0.1 M NH4CI solution, using the given pH data, calculate: [H*], [OH"]: O [H*] = 3.2 x 10-5 M, [OH"]= 3.2 x 10-10 M O [H*] = 2.2 x 10-9 M, [OH¯]= 4.5 x 10-6 M O [H*] = 3.2 x 10-10 M, [OH"]= 3.2 x 10-5 M %3D [H*] = 1.0 x 10-7 M, [OH"]= 1.0 x 10-7 M

Lab Report #4-2-1: 0.1 M NH4CI solution, using the given pH data, calculate: [H*], [OH"]: O [H*] = 3.2 x 10-5 M, [OH"]= 3.2 x 10-10 M O [H*] = 2.2 x 10-9 M, [OH¯]= 4.5 x 10-6 M O [H*] = 3.2 x 10-10 M, [OH"]= 3.2 x 10-5 M %3D [H*] = 1.0 x 10-7 M, [OH"]= 1.0 x 10-7 M

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Chemistry
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ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter1: Chemical Foundations
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**Lab Report #4-2-1:** **Task:** Using a 0.1 M NH₄Cl solution and the given pH data, calculate the concentration of \([H^+]\) and \([OH^-]\). **Options:** - ⃝ \([H^+]\) = \(3.2 \times 10^{-5}\) M, \([OH^-]\) = \(3.2 \times 10^{-10}\) M - ⃝ \([H^+]\) = \(2.2 \times 10^{-9}\) M, \([OH^-]\) = \(4.5 \times 10^{-6}\) M - ⃝ \([H^+]\) = \(3.2 \times 10^{-10}\) M, \([OH^-]\) = \(3.2 \times 10^{-5}\) M - ⃝ \([H^+]\) = \(1.0 \times 10^{-7}\) M, \([OH^-]\) = \(1.0 \times 10^{-7}\) M
Transcribed Image Text:**Lab Report #4-2-1:** **Task:** Using a 0.1 M NH₄Cl solution and the given pH data, calculate the concentration of \([H^+]\) and \([OH^-]\). **Options:** - ⃝ \([H^+]\) = \(3.2 \times 10^{-5}\) M, \([OH^-]\) = \(3.2 \times 10^{-10}\) M - ⃝ \([H^+]\) = \(2.2 \times 10^{-9}\) M, \([OH^-]\) = \(4.5 \times 10^{-6}\) M - ⃝ \([H^+]\) = \(3.2 \times 10^{-10}\) M, \([OH^-]\) = \(3.2 \times 10^{-5}\) M - ⃝ \([H^+]\) = \(1.0 \times 10^{-7}\) M, \([OH^-]\) = \(1.0 \times 10^{-7}\) M
### Table of pH Values for Various Solutions The following table presents the pH values of different solutions, both before and after specific treatments such as boiling. | Solutions | pH Values | |-------------------|-----------| | H₂O (unboiled) | 3.5 | | H₂O (boiled) | 7.0 | | NaCl | 7.0 | | NaC₂H₃O₂ | 9.1 | | NH₄Cl | 4.5 | | NaHCO₃ | 9.5 | | Na₃PO₄ | 11.9 | | Na₂CO₃ | 11.0 | #### Explanation of the Table: - **H₂O (unboiled)**: This is water that has not undergone the boiling process, with a pH of 3.5, indicating it is slightly acidic. - **H₂O (boiled)**: Water that has been boiled shows a neutral pH of 7.0. - **NaCl (Sodium Chloride)**: This solution has a neutral pH of 7.0. - **NaC₂H₃O₂ (Sodium Acetate)**: This solution is slightly basic with a pH of 9.1. - **NH₄Cl (Ammonium Chloride)**: This solution has a pH of 4.5, showing it is mildly acidic. - **NaHCO₃ (Sodium Bicarbonate)**: This solution has a basic pH of 9.5. - **Na₃PO₄ (Trisodium Phosphate)**: This solution is strongly basic with a pH of 11.9. - **Na₂CO₃ (Sodium Carbonate)**: This solution also shows a strong basicity with a pH of 11.0. Use this table to understand the acidity or basicity of common solutions, which is critical in various applications, including industrial processes, cooking, and scientific research.
Transcribed Image Text:### Table of pH Values for Various Solutions The following table presents the pH values of different solutions, both before and after specific treatments such as boiling. | Solutions | pH Values | |-------------------|-----------| | H₂O (unboiled) | 3.5 | | H₂O (boiled) | 7.0 | | NaCl | 7.0 | | NaC₂H₃O₂ | 9.1 | | NH₄Cl | 4.5 | | NaHCO₃ | 9.5 | | Na₃PO₄ | 11.9 | | Na₂CO₃ | 11.0 | #### Explanation of the Table: - **H₂O (unboiled)**: This is water that has not undergone the boiling process, with a pH of 3.5, indicating it is slightly acidic. - **H₂O (boiled)**: Water that has been boiled shows a neutral pH of 7.0. - **NaCl (Sodium Chloride)**: This solution has a neutral pH of 7.0. - **NaC₂H₃O₂ (Sodium Acetate)**: This solution is slightly basic with a pH of 9.1. - **NH₄Cl (Ammonium Chloride)**: This solution has a pH of 4.5, showing it is mildly acidic. - **NaHCO₃ (Sodium Bicarbonate)**: This solution has a basic pH of 9.5. - **Na₃PO₄ (Trisodium Phosphate)**: This solution is strongly basic with a pH of 11.9. - **Na₂CO₃ (Sodium Carbonate)**: This solution also shows a strong basicity with a pH of 11.0. Use this table to understand the acidity or basicity of common solutions, which is critical in various applications, including industrial processes, cooking, and scientific research.
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