Domanda del libro di testo
Deuterium oxide 1D2O, where D is deuterium, the hydrogen-2 isotope) has an ion-product constant, Kw, of 8.9 * 10-16 at 20 °C. Calculate 3D+4 and 3OD-4 for pure (neutral) D2O at this temperature.
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Ch.16 - Acid-Base Equilibria
Brown15th EditionChemistry: The Central ScienceISBN: 9780137542970
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TOC.tableOfContents
- Ch.1 - Introduction: Matter, Energy, and Measurement146
- Ch.2 - Atoms, Molecules, and Ions200
- Ch.3 - Chemical Reactions and Reaction Stoichiometry176
- Ch.4 - Reactions in Aqueous Solution155
- Ch.5 - Thermochemistry126
- Ch.6 - Electronic Structure of Atoms131
- Ch.7 - Periodic Properties of the Elements126
- Ch.8 - Basic Concepts of Chemical Bonding123
- Ch.9 - Molecular Geometry and Bonding Theories143
- Ch.10 - Gases147
- Ch.11 - Liquids and Intermolecular Forces91
- Ch.12 - Solids and Modern Materials122
- Ch.13 - Properties of Solutions126
- Ch.14 - Chemical Kinetics174
- Ch.15 - Chemical Equilibrium101
- Ch.16 - Acid-Base Equilibria139
- Ch.17 - Additional Aspects of Aqueous Equilibria146
- Ch.18 - Chemistry of the Environment72
- Ch.19 - Chemical Thermodynamics129
- Ch.20 - Electrochemistry142
- Ch.21 - Nuclear Chemistry101
- Ch.22 - Chemistry of the Nonmetals68
- Ch.23 - Transition Metals and Coordination Chemistry66
- Ch.24 - The Chemistry of Life: Organic and Biological Chemistry10
Brown15th EditionChemistry: The Central ScienceISBN: 9780137542970Non è quello che usi tu?Cambia libro di testo
Capitolo 16, Problema 34b
Calculate 3OH-4 for each of the following solutions, and indicate whether the solution is acidic, basic, or neutral: (b) 3H+4 = 2.5 * 10-10 M
Guida verificata passo dopo passo1
Identify the given concentration: \([H^+] = 2.5 \times 10^{-10} \text{ M}\).
Use the relationship between \([H^+]\) and \([OH^-]\) in water: \([H^+][OH^-] = 1.0 \times 10^{-14}\).
Rearrange the equation to solve for \([OH^-]\): \([OH^-] = \frac{1.0 \times 10^{-14}}{[H^+]}\).
Substitute the given \([H^+]\) value into the equation to find \([OH^-]\).
Determine if the solution is acidic, basic, or neutral by comparing \([H^+]\) and \([OH^-]\): if \([H^+] > [OH^-]\), it's acidic; if \([H^+] < [OH^-]\), it's basic; if \([H^+] = [OH^-]\), it's neutral.
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pH and pOH
pH is a measure of the hydrogen ion concentration in a solution, while pOH measures the hydroxide ion concentration. The relationship between pH and pOH is defined by the equation pH + pOH = 14 at 25°C. Understanding this relationship is crucial for determining the acidity or basicity of a solution.
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Percorso guidato
02:09
pH and pOH Calculations
Acidic, Basic, and Neutral Solutions
A solution is considered acidic if its pH is less than 7, basic if its pH is greater than 7, and neutral if its pH is exactly 7. The concentration of hydrogen ions (H+) and hydroxide ions (OH-) determines these classifications. For example, a higher concentration of H+ indicates acidity, while a higher concentration of OH- indicates basicity.
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Percorso guidato
01:04Balancing Basic Redox Reactions
Calculating pOH from H+ Concentration
To find the pOH from the concentration of hydrogen ions (H+), first calculate the pH using the formula pH = -log[H+]. Then, use the relationship pOH = 14 - pH to find the pOH. This calculation is essential for determining the nature of the solution based on its hydroxide ion concentration.
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Percorso guidato
02:09pH and pOH Calculations
Pratica correlata
Domanda del libro di testo
Write the expression for the ion product constant for water, Kw.
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Domanda del libro di testo
Calculate 3OH-4 for each of the following solutions, and indicate whether the solution is acidic, basic, or neutral: (a) 3H+4 = 0.0505 M
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Domanda del libro di testo
By what factor does [H+] change for a pH change of (a) 2.00 units? (b) 0.50 units?
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Domanda del libro di testo
Calculate 3OH-4 for each of the following solutions, and indicate whether the solution is acidic, basic, or neutral: (c) a solution in which 3H+4 is 1000 times greater than 3OH-4.
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Domanda del libro di testo
Calculate [H+] for each of the following solutions, and indicate whether the solution is acidic, basic, or neutral: (a) [OH-] = 0.00045 M (b) [OH-] = 8.8 × 10-9 M (c) a solution in which [OH-] is 100 times greater than [H+].
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