**Adjusting pH in an Unbuffered Solution**A 0.1-L unbuffered solution needs the pH adjusted from 3.5 to 2. How many microliters of a 12 molar HCl solution need to be added to adjust the pH?**Instructions:**- Report your answer to four decimal places.- Assume the volume of HCl being added is negligible and the total volume of the solution does not change.- The volume of the solution is *not* 1 L as it was in the practice pools.- The question requests your answer be reported in μL (microliters).**Media Resource:**- **Name:** CalculatingChangeInpH (04:33)- **Duration:** 04:33- **Added:** 15 Jan 2018 04:04 PMA media resource is available for further explanation. Watch the video for more detailed guidance on calculating the change in pH.

pH is used to determine the concentration of hydronium ion. Assume; volume of NaOH solution = x The calculation of moles is shown below: moles = molarity ×volume= 12 ×x1000= 0.012 x The calculation of desired pH is shown below: pH = 3.5 -2= 1.5 The calculation of concentration of hydronium ion is shown below: H+ = 10-pH= 10-1.5=0.032 M So; the 0.032 concentration of hydronium ion have to be added. Assume; volume remains constant. when moles of hydronium ion that have to be added. moles = change in concentration ×volume = 0.032 ×0.1 = 0.0032 The calculation of value of x is shown below: 0.012 x = 0.0032x= 0.27 Lx =2.7 ×105 μLAnswer: 2.7×105 microliters should be added.

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A 0.1-L unbuffered solution needs the pH adjusted from 3.5 to 2. How many microliters of a 12 molar HCI solution need to be added to adjust the pH? Report your answer to four decimal places.

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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