Domanda del libro di testo
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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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 4, Problema 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.
Guida verificata passo dopo passo1
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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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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Percorso guidato
00:53
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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01:03Solution Dilution Process
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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00:50Ionic Salts
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