교과서 질문
Determine whether each of the following statements concerning the titrations in Problem 17.35 is true or false. (a) The pH at the beginning of the two titrations will be the same.
Ch.17 - Additional Aspects of Aqueous Equilibria
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
17장, 문제 35a
The samples of nitric and acetic acids shown here are both titrated with a 0.100 M solution of NaOH(aq).
Determine whether each of the following statements concerning these titrations is true or false. (a) A larger volume of NaOH1aq2 is needed to reach the equivalence point in the titration of HNO3.
검증된 단계별 안내1
Step 1: Identify the acids in the beakers. The first beaker contains 30.0 mL of 0.50 M chloric acid (HClO3), and the second beaker contains 30.0 mL of 0.50 M formic acid (HCOOH).
Step 2: Write the balanced chemical equations for the titration reactions. For chloric acid: HClO3 + NaOH -> NaClO3 + H2O. For formic acid: HCOOH + NaOH -> HCOONa + H2O.
Step 3: Calculate the moles of each acid present. Use the formula: moles = molarity * volume (in liters).
Step 4: Determine the moles of NaOH required to reach the equivalence point for each titration. Since both reactions are 1:1 stoichiometry, the moles of NaOH needed will be equal to the moles of each acid.
Step 5: Compare the volumes of 0.100 M NaOH needed to reach the equivalence point for each acid. Use the formula: volume (L) = moles / molarity.
비슷한 문제에 대한 검증된 영상 답변:
이 영상 해법은 위 문제에 도움이 된다고 튜터들이 추천한 것입니다.
영상 길이:
2m주요 개념
질문에 올바르게 답하기 위해 반드시 이해해야 하는 핵심 개념들은 다음과 같습니다.
Titration
Titration is a quantitative analytical technique used to determine the concentration of a solute in a solution. It involves the gradual addition of a titrant, a solution of known concentration, to a sample until the reaction reaches its equivalence point, where the amount of titrant equals the amount of substance in the sample. The endpoint is often indicated by a color change due to an indicator.
추천 영상:
가이드 코스
03:04
Acid-Base Titration
Equivalence Point
The equivalence point in a titration is the stage at which the amount of titrant added is stoichiometrically equivalent to the amount of substance present in the sample. At this point, the reaction between the acid and base is complete, and the pH of the solution changes significantly. Understanding the equivalence point is crucial for determining the volume of titrant needed for complete neutralization.
추천 영상:
가이드 코스
01:07At the Equivalence Point
Acid Strength and Concentration
The strength of an acid refers to its ability to dissociate in solution, with strong acids like nitric acid (HNO3) completely ionizing, while weak acids like formic acid (HCOOH) only partially ionize. The concentration of an acid, measured in molarity (M), indicates the amount of acid present in a given volume of solution. The combination of strength and concentration affects the volume of titrant required to reach the equivalence point in a titration.
추천 영상:
가이드 코스
03:51Binary Acid Strengths
관련 실천
교과서 질문
Predict whether the equivalence point of each of the following titrations is below, above, or at pH 7: (a) NaHCO3 titrated with NaOH (c) KOH titrated with HBr.
교과서 질문
The accompanying graph shows the titration curves for two monoprotic acids. (d) Estimate the pKa of the weak acid.
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교과서 질문
Compare the titration of a strong, monoprotic acid with a strong base to the titration of a weak, monoprotic acid with a strong base. Assume the strong and weak acid solutions initially have the same concentrations. Indicate whether the following statements are true or false. (a) More base is required to reach the equivalence point for the strong acid than the weak acid.
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교과서 질문
Determine whether each of the following statements concerning the titrations in Problem 17.35 is true or false. (b) The titration curves will both be essentially the same after passing the equivalence point.
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