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**Titration of Acids and Bases (Pre-Lab Exercise)** Titration can be used to find the volume of solution that is needed to react with a measured or known amount of another substance. In this experiment, your goal is to carry out a titration reaction between an acid and a base. You will interpret the results to determine the concentration (molarity) of the original acid solution. 1. **You will be reacting HCl(aq) in the beaker with NaOH(aq) from the buret.** The following two sketches represent your system before the titration has started. (a) Draw a particle-level sketch of the beaker that contains the HCl(aq). Use 4 formula units of HCl in your sketch. Remember that unlike most molecular substances, HCl dissociates completely in aqueous solution to produce H⁺ and Cl⁻ ions. (b) Draw a particle-level sketch of the buret that contains the NaOH(aq). Use 8 formula units of NaOH in your sketch. The NaOH dissociates completely in aqueous solution to produce Na⁺ and OH⁻ ions. 2. **Now you will add the NaOH(aq) from the buret to the beaker with HCl(aq).** (a) Sketch a beaker where 2 formula units of NaOH have been added to the original 4 formula units of HCl. Clearly differentiate between ions dissolved in solution and circle the molecules formed during the reaction. This represents an early portion of the titration. (b) Sketch a beaker where 4 formula units of NaOH have been added to the original 4 formula units of HCl. Clearly differentiate between ions dissolved in solution and molecules formed during the reaction. This represents the equivalence point of the titration, where the mole amounts of added NaOH and HCl are equal. (c) Sketch a beaker where 6 formula units of NaOH have been added to the original 4 formula units of HCl. Clearly differentiate between ions dissolved in solution and molecules formed during the reaction. This represents a late portion of the titration (past the equivalence point). 3. Fill in the following table to acquire a particle-level understanding of the process of acid-base titration: | Composition of solution | 4 HCl (before titration) | 8 NaOH (before titration) | 4 HCl & 2 NaOH | 4 HCl & 4 NaOH | 4 HCl & 6 NaOH | |-------------------------|--------------------------|---------------------------|----------------|----------------|----------------| | number of free H⁺ ions | | | | | | | number of Cl⁻ ions | | | | | | | number of Na⁺ ions | | | | | | | number of free OH⁻ ions | | | | | |

**Titration of Acids and Bases (Pre-Lab Exercise)** Titration can be used to find the volume of solution that is needed to react with a measured or known amount of another substance. In this experiment, your goal is to carry out a titration reaction between an acid and a base. You will interpret the results to determine the concentration (molarity) of the original acid solution. 1. **You will be reacting HCl(aq) in the beaker with NaOH(aq) from the buret.** The following two sketches represent your system before the titration has started. (a) Draw a particle-level sketch of the beaker that contains the HCl(aq). Use 4 formula units of HCl in your sketch. Remember that unlike most molecular substances, HCl dissociates completely in aqueous solution to produce H⁺ and Cl⁻ ions. (b) Draw a particle-level sketch of the buret that contains the NaOH(aq). Use 8 formula units of NaOH in your sketch. The NaOH dissociates completely in aqueous solution to produce Na⁺ and OH⁻ ions. 2. **Now you will add the NaOH(aq) from the buret to the beaker with HCl(aq).** (a) Sketch a beaker where 2 formula units of NaOH have been added to the original 4 formula units of HCl. Clearly differentiate between ions dissolved in solution and circle the molecules formed during the reaction. This represents an early portion of the titration. (b) Sketch a beaker where 4 formula units of NaOH have been added to the original 4 formula units of HCl. Clearly differentiate between ions dissolved in solution and molecules formed during the reaction. This represents the equivalence point of the titration, where the mole amounts of added NaOH and HCl are equal. (c) Sketch a beaker where 6 formula units of NaOH have been added to the original 4 formula units of HCl. Clearly differentiate between ions dissolved in solution and molecules formed during the reaction. This represents a late portion of the titration (past the equivalence point). 3. Fill in the following table to acquire a particle-level understanding of the process of acid-base titration: | Composition of solution | 4 HCl (before titration) | 8 NaOH (before titration) | 4 HCl & 2 NaOH | 4 HCl & 4 NaOH | 4 HCl & 6 NaOH | |-------------------------|--------------------------|---------------------------|----------------|----------------|----------------| | number of free H⁺ ions | | | | | | | number of Cl⁻ ions | | | | | | | number of Na⁺ ions | | | | | | | number of free OH⁻ ions | | | | | |

Chemistry
Chemistry
10th Edition
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter1: Chemical Foundations
Section: Chapter Questions
Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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**Titration of Acids and Bases (Pre-Lab Exercise)** Titration can be used to find the volume of solution that is needed to react with a measured or known amount of another substance. In this experiment, your goal is to carry out a titration reaction between an acid and a base. You will interpret the results to determine the concentration (molarity) of the original acid solution. 1. **You will be reacting HCl(aq) in the beaker with NaOH(aq) from the buret.** The following two sketches represent your system before the titration has started. (a) Draw a particle-level sketch of the beaker that contains the HCl(aq). Use 4 formula units of HCl in your sketch. Remember that unlike most molecular substances, HCl dissociates completely in aqueous solution to produce H⁺ and Cl⁻ ions. (b) Draw a particle-level sketch of the buret that contains the NaOH(aq). Use 8 formula units of NaOH in your sketch. The NaOH dissociates completely in aqueous solution to produce Na⁺ and OH⁻ ions. 2. **Now you will add the NaOH(aq) from the buret to the beaker with HCl(aq).** (a) Sketch a beaker where 2 formula units of NaOH have been added to the original 4 formula units of HCl. Clearly differentiate between ions dissolved in solution and circle the molecules formed during the reaction. This represents an early portion of the titration.
Transcribed Image Text:**Titration of Acids and Bases (Pre-Lab Exercise)** Titration can be used to find the volume of solution that is needed to react with a measured or known amount of another substance. In this experiment, your goal is to carry out a titration reaction between an acid and a base. You will interpret the results to determine the concentration (molarity) of the original acid solution. 1. **You will be reacting HCl(aq) in the beaker with NaOH(aq) from the buret.** The following two sketches represent your system before the titration has started. (a) Draw a particle-level sketch of the beaker that contains the HCl(aq). Use 4 formula units of HCl in your sketch. Remember that unlike most molecular substances, HCl dissociates completely in aqueous solution to produce H⁺ and Cl⁻ ions. (b) Draw a particle-level sketch of the buret that contains the NaOH(aq). Use 8 formula units of NaOH in your sketch. The NaOH dissociates completely in aqueous solution to produce Na⁺ and OH⁻ ions. 2. **Now you will add the NaOH(aq) from the buret to the beaker with HCl(aq).** (a) Sketch a beaker where 2 formula units of NaOH have been added to the original 4 formula units of HCl. Clearly differentiate between ions dissolved in solution and circle the molecules formed during the reaction. This represents an early portion of the titration.
(b) Sketch a beaker where 4 formula units of NaOH have been added to the original 4 formula units of HCl. Clearly differentiate between ions dissolved in solution and molecules formed during the reaction. This represents the equivalence point of the titration, where the mole amounts of added NaOH and HCl are equal. (c) Sketch a beaker where 6 formula units of NaOH have been added to the original 4 formula units of HCl. Clearly differentiate between ions dissolved in solution and molecules formed during the reaction. This represents a late portion of the titration (past the equivalence point). 3. Fill in the following table to acquire a particle-level understanding of the process of acid-base titration: | Composition of solution | 4 HCl (before titration) | 8 NaOH (before titration) | 4 HCl & 2 NaOH | 4 HCl & 4 NaOH | 4 HCl & 6 NaOH | |-------------------------|--------------------------|---------------------------|----------------|----------------|----------------| | number of free H⁺ ions | | | | | | | number of Cl⁻ ions | | | | | | | number of Na⁺ ions | | | | | | | number of free OH⁻ ions | | | | | |
Transcribed Image Text:(b) Sketch a beaker where 4 formula units of NaOH have been added to the original 4 formula units of HCl. Clearly differentiate between ions dissolved in solution and molecules formed during the reaction. This represents the equivalence point of the titration, where the mole amounts of added NaOH and HCl are equal. (c) Sketch a beaker where 6 formula units of NaOH have been added to the original 4 formula units of HCl. Clearly differentiate between ions dissolved in solution and molecules formed during the reaction. This represents a late portion of the titration (past the equivalence point). 3. Fill in the following table to acquire a particle-level understanding of the process of acid-base titration: | Composition of solution | 4 HCl (before titration) | 8 NaOH (before titration) | 4 HCl & 2 NaOH | 4 HCl & 4 NaOH | 4 HCl & 6 NaOH | |-------------------------|--------------------------|---------------------------|----------------|----------------|----------------| | number of free H⁺ ions | | | | | | | number of Cl⁻ ions | | | | | | | number of Na⁺ ions | | | | | | | number of free OH⁻ ions | | | | | |
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