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?,

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)

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.

Question 9