Textbook Question
Indicate the concentration of each ion present in the solution formed by mixing: (b) 44.0 mL of 0.100 M Na2SO4 with 25.0 mL of 0.150 M KCl
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Ch.4 - Reactions in Aqueous Solution
Brown14th EditionChemistry: The Central ScienceISBN: 9780134414232
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Table of contents
- Ch.1 - Introduction: Matter, Energy, and Measurement140
- Ch.2 - Atoms, Molecules, and Ions192
- Ch.3 - Chemical Reactions and Reaction Stoichiometry172
- Ch.4 - Reactions in Aqueous Solution156
- Ch.5 - Thermochemistry151
- Ch.6 - Electronic Structure of Atoms137
- Ch.7 - Periodic Properties of the Elements127
- Ch.8 - Basic Concepts of Chemical Bonding143
- Ch.9 - Molecular Geometry and Bonding Theories167
- Ch.10 - Gases147
- Ch.11 - Liquids and Intermolecular Forces97
- Ch.12 - Solids and Modern Materials129
- Ch.13 - Properties of Solutions126
- Ch.14 - Chemical Kinetics175
- Ch.15 - Chemical Equilibrium107
- Ch.16 - Acid-Base Equilibria127
- Ch.17 - Additional Aspects of Aqueous Equilibria133
- Ch.18 - Chemistry of the Environment88
- Ch.19 - Chemical Thermodynamics140
- Ch.20 - Electrochemistry137
- Ch.21 - Nuclear Chemistry99
- Ch.22 - Chemistry of the Nonmetals66
- Ch.23 - Transition Metals and Coordination Chemistry69
- Ch.24 - The Chemistry of Life: Organic and Biological Chemistry11
Brown14th EditionChemistry: The Central ScienceISBN: 9780134414232Not the one you use?Change textbook
Chapter 4, Problem 71d
Ignoring protolysis reactions, indicate the concentration of each ion or molecule present in the following solutions: (d) a mixture of 45.0 mL of 0.272 M NaCl and 65.0 mL of 0.0247 M (NH4)2CO3. Assume that the volumes are additive.
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Calculate the total volume of the solution by adding the volumes of the NaCl and (NH4)2CO3 solutions. This is done by adding 45.0 mL and 65.0 mL.
Calculate the moles of NaCl initially present using its concentration and the volume of the NaCl solution. Use the formula: moles = concentration (M) imes volume (L).
Calculate the moles of (NH4)2CO3 initially present using its concentration and the volume of the (NH4)2CO3 solution. Use the same formula as in step 2.
Determine the concentration of each ion in the final solution. For NaCl, which dissociates into Na+ and Cl-, the concentration of each ion is equal to the total moles of NaCl divided by the total volume of the solution. For (NH4)2CO3, which dissociates into 2NH4+ and CO32-, the concentration of NH4+ is twice the moles of (NH4)2CO3 divided by the total volume, and the concentration of CO32- is equal to the moles of (NH4)2CO3 divided by the total volume.
Summarize the concentrations of Na+, Cl-, NH4+, and CO32- in the final solution.
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Key Concepts
Here are the essential concepts you must grasp in order to answer the question correctly.
Concentration and Molarity
Concentration refers to the amount of solute present in a given volume of solution, commonly expressed in molarity (M), which is moles of solute per liter of solution. Understanding how to calculate molarity is essential for determining the concentration of ions or molecules in a mixture.
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Molarity Concept
Dilution and Mixing Solutions
When two solutions are mixed, the total volume increases, and the concentrations of the solutes change. The final concentration can be calculated using the formula C1V1 + C2V2 = CfinalVfinal, where C is concentration and V is volume. This principle is crucial for accurately determining the concentrations of ions in the resulting solution.
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Ionic Dissociation
Ionic compounds, such as NaCl, dissociate into their constituent ions when dissolved in water. For example, NaCl dissociates into Na⁺ and Cl⁻ ions. Understanding how different compounds dissociate is vital for calculating the concentrations of individual ions in a mixed solution.
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Related Practice
Textbook Question
(a) Which will have the highest concentration of potassium ions: 0.20 M KCl, 0.15 M K2CrO4, or 0.080 M K3PO4?
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Textbook Question
Indicate the concentration of each ion present in the solution formed by mixing: (c) 3.60 g KCl in 75.0 mL of 0.250 M CaCl2 solution. Assume that the volumes are additive.
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Textbook Question
Indicate the concentration of each ion or molecule present in the following solutions: (a) 0.35 M K3PO4 (b) 1.3×10−2 M MgSO4 (c) 0.0184 M CH3CH2OH
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Textbook Question
Indicate the concentration of each ion present in the solution formed by mixing: (a) 42.0 mL of 0.170 M NaOH with 37.6 mL of 0.400 M NaOH.
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