Domanda del libro di testo
(a) By titration, 15.0 mL of 0.1008 M sodium hydroxide is needed to neutralize a 0.2053-g sample of a weak acid. What is the molar mass of the acid if it is monoprotic?
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Ch.4 - Reactions in Aqueous Solution
Brown15th EditionChemistry: The Central ScienceISBN: 9780137542970
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TOC.tableOfContents
- Ch.1 - Introduction: Matter, Energy, and Measurement146
- Ch.2 - Atoms, Molecules, and Ions200
- Ch.3 - Chemical Reactions and Reaction Stoichiometry176
- Ch.4 - Reactions in Aqueous Solution155
- Ch.5 - Thermochemistry126
- Ch.6 - Electronic Structure of Atoms131
- Ch.7 - Periodic Properties of the Elements126
- Ch.8 - Basic Concepts of Chemical Bonding123
- Ch.9 - Molecular Geometry and Bonding Theories143
- Ch.10 - Gases147
- Ch.11 - Liquids and Intermolecular Forces91
- Ch.12 - Solids and Modern Materials122
- Ch.13 - Properties of Solutions126
- Ch.14 - Chemical Kinetics174
- Ch.15 - Chemical Equilibrium101
- Ch.16 - Acid-Base Equilibria139
- Ch.17 - Additional Aspects of Aqueous Equilibria146
- Ch.18 - Chemistry of the Environment72
- Ch.19 - Chemical Thermodynamics129
- Ch.20 - Electrochemistry142
- Ch.21 - Nuclear Chemistry101
- Ch.22 - Chemistry of the Nonmetals68
- Ch.23 - Transition Metals and Coordination Chemistry66
- Ch.24 - The Chemistry of Life: Organic and Biological Chemistry10
Brown15th EditionChemistry: The Central ScienceISBN: 9780137542970Non è quello che usi tu?Cambia libro di testo
Capitolo 4, Problema 103b
(b) An elemental analysis of the acid indicates that it is composed of 5.89% H, 70.6% C, and 23.5% O by mass. What is its molecular formula?
Guida verificata passo dopo passo1
Step 1: Assume that you have 100 g of the compound. This means that you have 5.89 g of Hydrogen (H), 70.6 g of Carbon (C), and 23.5 g of Oxygen (O).
Step 2: Convert these masses into moles using the molar mass of each element. The molar mass of H is approximately 1 g/mol, the molar mass of C is approximately 12 g/mol, and the molar mass of O is approximately 16 g/mol.
Step 3: Divide each mole value by the smallest number of moles calculated. This will give you the mole ratio of H, C, and O in the compound.
Step 4: If the mole ratios are not whole numbers, multiply them by the smallest number that will convert them all to whole numbers. This will give you the empirical formula of the compound.
Step 5: To find the molecular formula, you need to know the molar mass of the compound. Divide the molar mass of the compound by the molar mass of the empirical formula. This will give you a whole number, which you multiply by the subscripts in the empirical formula to get the molecular formula.
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Empirical Formula
The empirical formula represents the simplest whole-number ratio of the elements in a compound. To determine the empirical formula from percentage composition, one converts the percentages to moles by dividing by the atomic masses of the elements. This ratio helps in identifying the basic composition of the compound before determining the molecular formula.
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02:26
Empirical vs Molecular Formula
Molecular Formula
The molecular formula indicates the actual number of atoms of each element in a molecule of a compound. It can be derived from the empirical formula by multiplying it by a whole number, which is determined by comparing the molar mass of the compound to the molar mass of the empirical formula. This formula provides more specific information about the compound's structure.
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02:08Determining Molecular Formulas
Molar Mass Calculation
Molar mass is the mass of one mole of a substance, typically expressed in grams per mole (g/mol). To find the molecular formula, one must first calculate the molar mass of the compound using the atomic masses of its constituent elements. This value is essential for determining the relationship between the empirical and molecular formulas.
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03:12Molar Mass Calculation Example
Pratica correlata
Domanda del libro di testo
A solid sample of Zn(OH)2 is added to 0.350 L of 0.500 M aqueous HBr. The solution that remains is still acidic. It is then titrated with 0.500 M NaOH solution, and it takes 88.5 mL of the NaOH solution to reach the equivalence point. What mass of Zn(OH)2 was added to the HBr solution?
Domanda del libro di testo
A sample of 7.75 g of Mg(OH)2 is added to 25.0 mL of 0.200 𝑀 HNO3. c. How many moles of Mg(OH)2,HNO3, and Mg(NO3)2 are present after the reaction is complete?
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Domanda del libro di testo
Suppose you have 5.00 g of powdered magnesium metal, 1.00 L of 2.00 M potassium nitrate solution, and 1.00 L of 2.00 M silver nitrate solution. d. What is the molarity of the Mg2+ ions in the resulting solution?
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Domanda del libro di testo
Suppose you have 5.00 g of powdered magnesium metal, 1.00 L of 2.00 M potassium nitrate solution, and 1.00 L of 2.00 M silver nitrate solution. a. Which one of the solutions will react with the magnesium powder?
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