Show your calculations for each of the questions below and on the following page. 1. Find the pH of a solution whose hydrogen ion concentration is: a. 2.0 x 10-7 M b. 0.052 М с. 8.0 M 2. A solution of a weak acid was tested with the indicators used in this experiment. The colors observed were: Methyl violet: violet Congo red: violet Bromocresol green: yellow Thymol blue: yellow What is the approximate pH of the solution?,

Show your calculations for each of the questions below and on the following page. 1. Find the pH of a solution whose hydrogen ion concentration is: a. 2.0 x 10-7 M b. 0.052 М с. 8.0 M 2. A solution of a weak acid was tested with the indicators used in this experiment. The colors observed were: Methyl violet: violet Congo red: violet Bromocresol green: yellow Thymol blue: yellow What is the approximate pH of the solution?,

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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Order these chemical species by increasing pH of an 0.1 M aqueous solution of each. That is, imagine making an 0.1 M solution of each species. Select 1 next to the species that makes the solution with the lowest pH. Select 2 next to the species that makes the solution with the next higher pH, and so on. Notice that some of the rankings have been filled in for you already. Also notice that water is on the list. For that particular case, just compare the pH of pure water to the pH of the other solutions. Note for advanced students: for all charged species, you may assume the necessary counterions act as neither acids nor bases. species relative pH of 0.1 M aqueous solution + C6H5NH3 HCOOH 3 2 HCOO (Choose one) H₂O HONH3 5 + (Choose one) C6H5NH2 (Choose one) H₂O+ (Choose one) HONH2 8 (highest)
I'm taking a practice test and I'm having some trouble and was hoping you could help. This is not graded I just need help See attached:
Order these chemical species by increasing pH of an 0.1 M aqueous solution of each. That is, imagine making an 0.1 M solution of each species. Select 1 next to the species that makes the solution with the lowest pH. Select 2 next to the species that makes the solution with the next higher pH, and so on. Notice that some of the rankings have been filled in for you already. Also notice that water is on the list. For that particular case, just compare the pH of pure water to the pH of the other solutions. Note for advanced students: for all charged species, you may assume the necessary counterions act as neither acids nor bases. relative pH of 0.1 M aqueous solution species ? 103 |(Choose one) ▼ OH |(Choose one) ▼ H,0 4 HC,04 6. HIO, 1 (lowest) NO2 |(Choose one)
Substance to be tested Tap water Vinegar/acetic acid Milk of magnesia (Mg(OH)2) Coffee (make liquid solution) Green tea (make liquid solution) Liquid soap pH 0 Estimated pH based on color from Is this substance an acid, a base, or universal indicator paper pH-neutral? pH Scale for Part A: Add the tested substances to the pH scale below. Orange juice is provided as an example. Orange juice pH 3.9 pH 7 2 818440005473 Prepared by: Patricia Mejabi, M.Sc., M.HSA and Daniel Czerny, PhD 2 June 2023 pH 14
Order these chemical species by increasing pH of an 0.1 M aqueous solution of each. That is, imagine making an 0.1 M solution of each species. Select 1 next to the species that makes the solution with the lowest pH. Select 2 next to the species that makes the solution with the next higher pH, and so on. Notice that some of the rankings have been filled in for you already. Also notice that water is on the list. For that particular case, just compare the pH of pure water to the pH of the other solutions. Note for advanced students: for all charged species, you may assume the necessary counterions act as neither acids nor bases. species HS H₂O HCOOH H₂S HCOO + CH₂NH3 CH,NH, + H₂O* relative pH of 0.1 M aqueous solution 8 (highest) (Choose one) (Choose one) (Choose one) 6 3 (Choose one) 1 (lowest) X Ś
Order these chemical species by increasing pH of an 0.1 M aqueous solution of each. That is, imagine making an 0.1 M solution of each species. Select 1 next to the species that makes the solution with the lowest pH. Select 2 next to the species that makes the solution with the next higher pH, and so on. Notice that some of the rankings have been filled in for you already. Also notice that water is on the list. For that particular case, just compare the pH of pure water to the pH of the other solutions. Note for advanced students: for all charged species, you may assume the necessary counterions act as neither acids nor bases. relative pH of species 0.1 M aqueous solution HC₂04 7 + H₂O* 1 (lowest) H₂PO4 (Choose one) H₂PO4 4 103 (Choose one) HIO₂ H₂C₂O4 (Choose one) H₂O (Choose one)
Determine the Ka value Solution 1 3.98 X 10-3 M Solution 2 6.03 X 10-4 M Solution 3 1.07 X 10-5 M Solution 4 1.05 X 10-5 M Solution 5 4.68 X 10-10 M
2. A solution of HClO is mixed and found to have a pH of 4.7. Find what the initial concentration of HClO was for this solution. Ka = 3.00 × 10−8 for HClO. Answer in units of mol/L.
the solution has to be acidified before testing for Ag+ ions. To make sure that the solution is acidic, what should be done? Apply a drop of the solution to red litmus paper to see if it turns blue. Apply a drop of the solution to blue litmus paper to see if it turns red. Apply a drop of the solution to pH paper to see if the pH is above 7. Apply a drop of the solution to your tongue to see if it tastes sour.
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