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Calculate the concentration of an aqueous solution of Ca1OH22 that has a pH of 10.05.
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Ch.16 - Acid-Base Equilibria
Brown14th EditionChemistry: The Central ScienceISBN: 9780134414232
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TOC.tableOfContents
- Ch.1 - Introduction: Matter, Energy, and Measurement177
- Ch.2 - Atoms, Molecules, and Ions231
- Ch.3 - Chemical Reactions and Reaction Stoichiometry216
- Ch.4 - Reactions in Aqueous Solution189
- Ch.5 - Thermochemistry175
- Ch.6 - Electronic Structure of Atoms168
- Ch.7 - Periodic Properties of the Elements150
- Ch.8 - Basic Concepts of Chemical Bonding177
- Ch.9 - Molecular Geometry and Bonding Theories200
- Ch.10 - Gases179
- Ch.11 - Liquids and Intermolecular Forces113
- Ch.12 - Solids and Modern Materials154
- Ch.13 - Properties of Solutions157
- Ch.14 - Chemical Kinetics199
- Ch.15 - Chemical Equilibrium128
- Ch.16 - Acid-Base Equilibria164
- Ch.17 - Additional Aspects of Aqueous Equilibria163
- Ch.18 - Chemistry of the Environment105
- Ch.19 - Chemical Thermodynamics164
- Ch.20 - Electrochemistry171
- Ch.21 - Nuclear Chemistry122
- Ch.22 - Chemistry of the Nonmetals82
- Ch.23 - Transition Metals and Coordination Chemistry79
- Ch.24 - The Chemistry of Life: Organic and Biological Chemistry16
Brown14th EditionChemistry: The Central ScienceISBN: 9780134414232Non è quello che usi tu?Cambia libro di testo
Capitolo 16, Problema 46c
Calculate [OH-] and pH for each of the following strong base solutions: (c) 10.0 mL of 0.0105 M Ca(OH)2 diluted to 500.0 mL
Guida verificata passo dopo passo1
Step 1: Identify the base in the solution. In this case, the base is Ca(OH)2. It's a strong base, which means it will dissociate completely in water to form Ca2+ and 2OH- ions.
Step 2: Calculate the initial concentration of OH- ions. Since each Ca(OH)2 molecule produces 2 OH- ions, the initial concentration of OH- ions is twice the concentration of Ca(OH)2. In this case, the initial concentration of OH- ions is 2 * 0.0105 M = 0.021 M.
Step 3: Calculate the final concentration of OH- ions after dilution. The formula for dilution is M1V1 = M2V2, where M1 and V1 are the initial molarity and volume, and M2 and V2 are the final molarity and volume. In this case, M1 = 0.021 M, V1 = 10.0 mL, and V2 = 500.0 mL. Solve for M2 to find the final concentration of OH- ions.
Step 4: Calculate pOH using the formula pOH = -log[OH-]. Use the final concentration of OH- ions from step 3.
Step 5: Calculate pH using the formula pH = 14 - pOH. Use the pOH value from step 4.
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Strong Bases
Strong bases are substances that completely dissociate in water to produce hydroxide ions (OH-). Common examples include alkali metal hydroxides and alkaline earth metal hydroxides, such as calcium hydroxide (Ca(OH)2). Understanding the dissociation of strong bases is crucial for calculating hydroxide ion concentration in solution.
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01:09
Strong Acid-Strong Base Titration
Dilution
Dilution is the process of reducing the concentration of a solute in a solution, typically by adding more solvent. The dilution equation, C1V1 = C2V2, relates the initial concentration and volume to the final concentration and volume. This concept is essential for determining the new concentration of hydroxide ions after the solution is diluted to a specific volume.
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00:58Dilution Equation
pH and pOH Calculations
pH and pOH are measures of the acidity and basicity of a solution, respectively. The pH scale ranges from 0 to 14, with lower values indicating higher acidity and higher values indicating higher basicity. The relationship between pH and pOH is given by the equation pH + pOH = 14. For strong bases, calculating pOH from the hydroxide ion concentration allows for the determination of pH.
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02:09pH and pOH Calculations