Textbook Question
(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?
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 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: 9780134414232Not the one you use?Change textbook
Chapter 4, Problem 105d
Suppose you have 3.00 g of powdered zinc metal, 3.00g of powdered silver metal and 500.0 mL of a 0.2 M copper(II) nitrate solution. (d) What is the molarity of Cu2+ ions in the resulting solution?
Verified step by step guidance1
insert step 1> Calculate the moles of copper(II) nitrate in the solution using the formula: moles = molarity \(\times\) volume. Remember to convert the volume from mL to L.
insert step 2> Write the balanced chemical equations for the reactions of zinc and silver with copper(II) nitrate.
insert step 3> Determine the limiting reactant by calculating the moles of zinc and silver and comparing them to the stoichiometry of the reactions.
insert step 4> Calculate the moles of Cu^{2+} ions that react based on the limiting reactant and the stoichiometry of the reaction.
insert step 5> Subtract the moles of Cu^{2+} ions that reacted from the initial moles of Cu^{2+} ions to find the moles of Cu^{2+} ions remaining. Then, calculate the molarity of Cu^{2+} ions in the resulting solution by dividing the remaining moles by the total volume of the solution in liters.
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Key Concepts
Here are the essential concepts you must grasp in order to answer the question correctly.
Molarity
Molarity is a measure of concentration defined as the number of moles of solute per liter of solution. It is expressed in moles per liter (M). To calculate molarity, one must know the amount of solute in grams, convert it to moles using the molar mass, and then divide by the volume of the solution in liters.
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Molarity
Stoichiometry
Stoichiometry involves the calculation of reactants and products in chemical reactions. It is based on the balanced chemical equation, which shows the ratio of moles of each substance involved. Understanding stoichiometry is essential for determining how much of each reactant is consumed and how much product is formed, which is crucial for calculating concentrations after a reaction.
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Copper(II) Nitrate Dissociation
Copper(II) nitrate (Cu(NO3)2) dissociates in solution to release Cu2+ ions and nitrate ions (NO3-). The dissociation is complete in a strong electrolyte like copper(II) nitrate, meaning that the concentration of Cu2+ ions in the solution will be equal to the initial molarity of the copper(II) nitrate solution, assuming no other reactions consume the Cu2+ ions.
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Related Practice
Textbook Question
The discovery of hafnium, element number 72, provideda controversial episode in chemistry. G. Urbain, a Frenchchemist, claimed in 1911 to have isolated an elementnumber 72 from a sample of rare earth (elements 58–71)compounds. However, Niels Bohr believed that hafniumwas more likely to be found along with zirconium thanwith the rare earths. D. Coster and G. von Hevesy, workingin Bohr's laboratory in Copenhagen, showed in 1922 thatelement 72 was present in a sample of Norwegian zircon,an ore of zirconium. (The name hafnium comes from theLatin name for Copenhagen, Hafnia). (c) Solid zirconiumdioxide, ZrO2, reacts with chlorine gas in the presenceof carbon. The products of the reaction are ZrCl4 and twogases, CO2 and CO in the ratio 1:2. Write a balanced chemicalequation for the reaction.
Textbook Question
Suppose you have 3.00 g of powdered zinc metal, 3.00g of powdered silver metal and 500.0 mL of a 0.2 M copper(II) nitrate solution. (b) What is the net ionic equation that describes this reaction?
Textbook Question
(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?
Textbook Question
Suppose you have 3.00 g of powdered zinc metal, 3.00g of powdered silver metal and 500.0 mL of a 0.2 M copper(II) nitrate solution. (a) Which metal will react with the copper(II) nitrate solution?
Textbook Question
(c) If 18.65 mLof the caesium hydroxide solution was needed to neutralize a42.3 mL aliquot of the hydroiodic acid solution, what is theconcentration (molarity) of the acid?