Textbook Question
Identify the stronger base in each of the following pairs.
Explain your reasoning.
(c) HS- or OH-
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Ch.16 - Aqueous Equilibria: Acids & Bases
McMurry8th EditionChemistryISBN: 9781292336145
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Table of contents
- Ch.1 - Chemical Tools: Experimentation & Measurement143
- Ch.2 - Atoms, Molecules & Ions134
- Ch.3 - Mass Relationships in Chemical Reactions149
- Ch.4 - Reactions in Aqueous Solution157
- Ch.5 - Periodicity & Electronic Structure of Atoms92
- Ch.6 - Ionic Compounds: Periodic Trends and Bonding Theory73
- Ch.7 - Covalent Bonding and Electron-Dot Structures47
- Ch.8 - Covalent Compounds: Bonding Theories and Molecular Structure51
- Ch.9 - Thermochemistry: Chemical Energy104
- Ch.10 - Gases: Their Properties & Behavior138
- Ch.11 - Liquids & Phase Changes43
- Ch.12 - Solids and Solid-State Materials56
- Ch.13 - Solutions & Their Properties98
- Ch.14 - Chemical Kinetics79
- Ch.15 - Chemical Equilibrium107
- Ch.16 - Aqueous Equilibria: Acids & Bases94
- Ch.17 - Applications of Aqueous Equilibria125
- Ch.18 - Thermodynamics: Entropy, Free Energy & Equilibrium66
- Ch.19 - Electrochemistry130
- Ch.20 - Nuclear Chemistry73
- Ch.21 - Transition Elements and Coordination Chemistry122
- Ch.22 - The Main Group Elements155
- Ch.23 - Organic and Biological Chemistry43
Chapter 16, Problem 76d
Calculate the H3O+ concentration to the correct number of significant figures for solutions with the following pH values. (d) 14.25
Verified step by step guidance1
Understand that pH is a measure of the acidity of a solution, defined as the negative logarithm (base 10) of the hydronium ion concentration: \( \text{pH} = -\log[\text{H}_3\text{O}^+] \).
To find the \([\text{H}_3\text{O}^+]\) concentration from a given pH, use the inverse of the logarithm function: \([\text{H}_3\text{O}^+] = 10^{-\text{pH}}\).
Substitute the given pH value into the equation: \([\text{H}_3\text{O}^+] = 10^{-14.25}\).
Calculate the power of 10 using the given pH value to find the \([\text{H}_3\text{O}^+]\) concentration.
Ensure that the final answer is expressed with the correct number of significant figures, which should match the number of decimal places in the given pH value.
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Key Concepts
Here are the essential concepts you must grasp in order to answer the question correctly.
pH Scale
The pH scale measures the acidity or basicity of a solution, ranging from 0 to 14. A pH of 7 is considered neutral, while values below 7 indicate acidity and values above 7 indicate basicity. The scale is logarithmic, meaning each whole number change represents a tenfold change in hydrogen ion concentration.
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The pH Scale
Hydronium Ion Concentration
The concentration of hydronium ions (H3O+) in a solution is directly related to its pH. The formula to calculate H3O+ concentration from pH is [H3O+] = 10^(-pH). This relationship allows for the conversion of pH values into molarity of hydronium ions, which is essential for understanding the solution's acidity.
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06:25Hydronium Ion Concentration Example
Significant Figures
Significant figures are the digits in a number that contribute to its precision. When performing calculations, especially in chemistry, it is crucial to report results with the correct number of significant figures based on the precision of the measurements involved. This ensures that the reported concentration accurately reflects the reliability of the data.
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Related Practice
Textbook Question
Which of the following species behave as strong acids or asstrong bases in aqueous solution?(a) HNO2 (b) HNO3(c) NH4+ (d) Cl-
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Textbook Question
Which of the indicators given in Figure 16.5, methyl violet, bromcresol green, phenol red, or thymolphthalein, would be most appropriate to detect a pH change from: (b) 8 to 10?
359
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Textbook Question
Identify the stronger base in each of the following pairs.
Explain your reasoning.
(d) HS- or Br-
115
views