Textbook Question
The solubility product for Zn1OH22 is 3.0 * 10-16. The formation constant for the hydroxo complex, Zn1OH242 - , is 4.6 * 1017. What concentration of OH- is required to dissolve 0.015 mol of Zn1OH22 in a liter of solution?
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Ch.17 - Additional Aspects of Aqueous Equilibria
Brown15th EditionChemistry: The Central ScienceISBN: 9780137542970
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Table of contents
- Ch.1 - Introduction: Matter, Energy, and Measurement111
- Ch.2 - Atoms, Molecules, and Ions166
- Ch.3 - Chemical Reactions and Reaction Stoichiometry138
- Ch.4 - Reactions in Aqueous Solution127
- Ch.5 - Thermochemistry104
- Ch.6 - Electronic Structure of Atoms109
- Ch.7 - Periodic Properties of the Elements107
- Ch.8 - Basic Concepts of Chemical Bonding102
- Ch.9 - Molecular Geometry and Bonding Theories120
- Ch.10 - Gases122
- Ch.11 - Liquids and Intermolecular Forces79
- Ch.12 - Solids and Modern Materials102
- Ch.13 - Properties of Solutions99
- Ch.14 - Chemical Kinetics153
- Ch.15 - Chemical Equilibrium83
- Ch.16 - Acid-Base Equilibria109
- Ch.17 - Additional Aspects of Aqueous Equilibria117
- Ch.18 - Chemistry of the Environment60
- Ch.19 - Chemical Thermodynamics109
- Ch.20 - Electrochemistry113
- Ch.21 - Nuclear Chemistry79
- Ch.22 - Chemistry of the Nonmetals52
- Ch.23 - Transition Metals and Coordination Chemistry57
- Ch.24 - The Chemistry of Life: Organic and Biological Chemistry7
Brown15th EditionChemistry: The Central ScienceISBN: 9780137542970Not the one you use?Change textbook
Chapter 17, Problem 111
A sample of 7.5 L of NH3 gas at 22 _x001F_C and 735 torr is bubbled into a 0.50-L solution of 0.40 M HCl. Assuming that all the NH3 dissolves and that the volume of the solution remains 0.50 L, calculate the pH of the resulting solution.
Verified step by step guidance1
Step 1: Convert the temperature from Celsius to Kelvin by adding 273.15 to the Celsius temperature. This will be used in the ideal gas law calculation.
Step 2: Use the ideal gas law, PV = nRT, to calculate the number of moles of NH3 gas. Convert the pressure from torr to atm by dividing by 760, and use the volume in liters, the temperature in Kelvin, and R = 0.0821 L·atm/mol·K.
Step 3: Calculate the initial moles of HCl in the solution using the concentration (0.40 M) and the volume of the solution (0.50 L).
Step 4: Determine the limiting reactant by comparing the moles of NH3 and HCl. NH3 reacts with HCl in a 1:1 molar ratio to form NH4Cl.
Step 5: Calculate the concentration of NH4+ in the solution after the reaction. Use this concentration to find the pH by considering the hydrolysis of NH4+ and using the expression for the equilibrium constant, Kb, of NH3.
Key Concepts
Here are the essential concepts you must grasp in order to answer the question correctly.
Ideal Gas Law
The Ideal Gas Law relates the pressure, volume, temperature, and number of moles of a gas through the equation PV = nRT. In this question, it is essential to calculate the number of moles of NH3 gas present in the sample before it reacts with HCl. Understanding this relationship allows for the conversion of gas conditions into moles, which is crucial for subsequent calculations.
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01:15
Ideal Gas Law Formula
Acid-Base Neutralization
Acid-base neutralization is a chemical reaction where an acid reacts with a base to produce water and a salt. In this scenario, NH3 acts as a weak base and HCl as a strong acid. The stoichiometry of the reaction will determine the amounts of NH3 and HCl that react, which is necessary to find the resulting concentrations of the products and the pH of the solution.
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05:04Lewis Acids and Bases
pH Calculation
pH is a measure of the acidity or basicity of a solution, calculated using the formula pH = -log[H+]. After determining the concentrations of the remaining acid or base in the solution post-reaction, the pH can be calculated. Understanding how to derive the concentration of hydrogen ions from the dissociation of acids and bases is critical for accurately determining the pH of the resulting solution.
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02:15pH Calculation Example
Related Practice
Textbook Question
Baking soda (sodium bicarbonate, NaHCO3) reacts with acids in foods to form carbonic acid (H2CO3), which in turn decomposes to water and carbon dioxide gas. In a cake batter, the CO2(g) forms bubbles and causes the cake to rise. (c) If 1/2 teaspoon of baking soda is indeed completely neutralized by the lactic acid in sour milk, calculate the volume of carbon dioxide gas that would be produced at 1 atm pressure, in an oven set to 350 F.
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Textbook Question
The value of Ksp for Cd(OH)2 is 2.5 × 10-14. (a) What is the molar solubility of Cd(OH)2?
Textbook Question
A concentration of 10–100 parts per billion (by mass) of Ag+ is an effective disinfectant in swimming pools. However, if the concentration exceeds this range, the Ag+ can cause adverse health effects. One way to maintain an appropriate concentration of Ag+ is to add a slightly soluble salt to the pool. Using Ksp values from Appendix D, calculate the equilibrium concentration of Ag+ in parts per billion that would exist in equilibrium with (b) AgBr (c) AgI.
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Textbook Question
(a) Write the net ionic equation for the reaction that occurs when a solution of hydrochloric acid (HCl) is mixed with a solution of sodium formate 1NaCHO22.
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