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2. How many milliliters of concentrated hydrochloric acid solution (36.0% HCl by mass, density = 1.18 g/mL) are required to produce 10.0 L of a solution that has a pH of 2.05?

2. How many milliliters of concentrated hydrochloric acid solution (36.0% HCl by mass, density = 1.18 g/mL) are required to produce 10.0 L of a solution that has a pH of 2.05?

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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### Problem 2: Calculation of Required Volume of Concentrated Hydrochloric Acid Solution **Question:** How many milliliters of concentrated hydrochloric acid solution (36.0% HCl by mass, density = 1.18 g/mL) are required to produce 10.0 L of a solution that has a pH of 2.05? **Explanation:** This problem involves finding the volume of a concentrated hydrochloric acid solution necessary to prepare a diluted solution with a specific pH. Given the concentration in terms of percentage by mass and its density, you need to calculate the necessary volume by understanding the relationship between molarity, volume, and pH. We begin by calculating the molarity (M) that corresponds to a pH of 2.05 using the formula: \[ \text{pH} = -\log[\text{H}^+] \] Given that the pH is 2.05: \[ [\text{H}^+] = 10^{-\text{pH}} = 10^{-2.05} \] Once the molarity of the hydrogen ions \(\text{H}^+\) in the solution is determined, the next step is to use the properties of concentrated hydrochloric acid (36.0% HCl by mass and density = 1.18 g/mL) to find the required volume. By expressing the concentration of the mixed solution in terms of molarity and using dilution principles (M1V1 = M2V2), we can solve for the unknown volume. In summary, the main steps involve: 1. Calculating the concentration of \(\text{H}^+\) ions. 2. Determining the molarity of the desired solution. 3. Using dilution principles along with the given properties of the concentrated acid to find the required volume. By following these steps, we will determine the number of milliliters of concentrated hydrochloric acid solution needed to achieve the desired final solution.
Transcribed Image Text:### Problem 2: Calculation of Required Volume of Concentrated Hydrochloric Acid Solution **Question:** How many milliliters of concentrated hydrochloric acid solution (36.0% HCl by mass, density = 1.18 g/mL) are required to produce 10.0 L of a solution that has a pH of 2.05? **Explanation:** This problem involves finding the volume of a concentrated hydrochloric acid solution necessary to prepare a diluted solution with a specific pH. Given the concentration in terms of percentage by mass and its density, you need to calculate the necessary volume by understanding the relationship between molarity, volume, and pH. We begin by calculating the molarity (M) that corresponds to a pH of 2.05 using the formula: \[ \text{pH} = -\log[\text{H}^+] \] Given that the pH is 2.05: \[ [\text{H}^+] = 10^{-\text{pH}} = 10^{-2.05} \] Once the molarity of the hydrogen ions \(\text{H}^+\) in the solution is determined, the next step is to use the properties of concentrated hydrochloric acid (36.0% HCl by mass and density = 1.18 g/mL) to find the required volume. By expressing the concentration of the mixed solution in terms of molarity and using dilution principles (M1V1 = M2V2), we can solve for the unknown volume. In summary, the main steps involve: 1. Calculating the concentration of \(\text{H}^+\) ions. 2. Determining the molarity of the desired solution. 3. Using dilution principles along with the given properties of the concentrated acid to find the required volume. By following these steps, we will determine the number of milliliters of concentrated hydrochloric acid solution needed to achieve the desired final solution.
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