Domanda del libro di testo
(a) How many milliliters of 0.120 M HCl are needed to completely neutralize 50.0 mL of 0.101 M Ba(OH)2 solution?
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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 81b
(b) What volume of HCl is needed to neutralize 2.87 g of Mg(OH)2?
Guida verificata passo dopo passo1
Identify the balanced chemical equation for the reaction: \[ \text{Mg(OH)}_2 + 2\text{HCl} \rightarrow \text{MgCl}_2 + 2\text{H}_2\text{O} \]
Calculate the molar mass of \( \text{Mg(OH)}_2 \) using the periodic table: \( \text{Mg} = 24.31 \text{ g/mol}, \text{O} = 16.00 \text{ g/mol}, \text{H} = 1.01 \text{ g/mol} \).
Convert the mass of \( \text{Mg(OH)}_2 \) to moles using its molar mass: \[ \text{moles of Mg(OH)}_2 = \frac{2.87 \text{ g}}{\text{molar mass of Mg(OH)}_2} \]
Use the stoichiometry from the balanced equation to find the moles of \( \text{HCl} \) needed: \[ \text{moles of HCl} = 2 \times \text{moles of Mg(OH)}_2 \]
Calculate the volume of \( \text{HCl} \) solution required using its concentration: \[ \text{Volume of HCl} = \frac{\text{moles of HCl}}{\text{concentration of HCl}} \]
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Neutralization Reaction
A neutralization reaction occurs when an acid reacts with a base to produce water and a salt. In this case, hydrochloric acid (HCl) reacts with magnesium hydroxide (Mg(OH)2) to form magnesium chloride (MgCl2) and water. Understanding this reaction is crucial for determining the stoichiometry involved in calculating the required volume of HCl.
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Percorso guidato
05:56
Lewis Dot Structures: Neutral Compounds
Stoichiometry
Stoichiometry is the calculation of reactants and products in chemical reactions based on balanced chemical equations. It allows us to determine the mole ratios of the substances involved. For this question, knowing the molar mass of Mg(OH)2 and the balanced equation for its reaction with HCl will enable us to find out how much HCl is needed to neutralize a specific mass of Mg(OH)2.
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01:16Stoichiometry Concept
Molarity
Molarity is a measure of concentration defined as the number of moles of solute per liter of solution. It is essential for calculating the volume of HCl required for neutralization. By knowing the molarity of the HCl solution, we can use the stoichiometric relationships from the balanced equation to find the exact volume needed to react with the given mass of Mg(OH)2.
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Percorso guidato
01:13Molarity
Pratica correlata
Domanda del libro di testo
(d) If 45.3 mL of a 0.108 M HCl solution is needed to neutralize a solution of KOH, how many grams of KOH must be present in the solution?
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Domanda del libro di testo
(c) If 25.8 mL of an AgNO3 solution is needed to precipitate all the Cl- ions in a 785-mg sample of KCl (forming AgCl), what is the molarity of the AgNO3 solution?
Domanda del libro di testo
(a) What volume of 0.115 M HClO4 solution is needed to neutralize 50.00 mL of 0.0875 M NaOH?
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