Explain what would happen to a strong acidic solution as you slowly add a strong basic solution. In your answer, include the concept of equivalence. Explain what happens to the OH ions, H* ions, and the pH as the base is added.

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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 ОН HIO H₂O CH₂CICOO CH₂CICOOH CH₂O ΙΟ CH₂OH relative pH of 0.1 M aqueous solution 8 (highest) (Choose one) (Choose one) (Choose one) 1 (lowest) (Choose one) 7 2 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. species ОН IO C10₂ HCOOH HCIO₂ HIO HCOO relative pH of 0.1 M aqueous solution (Choose one) 7 (Choose one) 2 1 (lowest) (Choose one) (Choose one) X Ś olo 18 Ar

Question 34 of 35 A student was titrating a solution of HC H,O, with a Sr(OH), solution. Determine the pH at a particular point in the titration. To do this, construct an ICE table to the concentration of hydroxide in solution and then use this information to determine the pH (Part 2). Complete Parts 1-2 before submitting your answer. NEXT 40.0 mL of a 0.200 M HC H,O, solution was titrated with 100 mL of 0.100 M Sr(OH), (a strong base). Fill in the ICE table with the appropriate value for each involved species to determine the moles of reactant and product after the reaction of the acid and base. You can ignore the amount of water in the reaction. HC H,O,(aq) + OH (aq) H,O() CH,O,(aq) 1) [+] Before (mol) Change (mol) After (mol) 5 RESET 0.100 0.200 2.00 10 -2.00 10 8.00 10 8,00 x 10 1.00 x 10 -1.00 x 10 1.20 x 10 1.20 x 10 2.00 10 -2.00x 10 Question 34 of 35 A student was titrating a solution of HC H,O, with a Sr(OH), solution. Determine the pH at a particular point in the titration.…

A 0.658 g sample of a diprotic acid is dissolved in water and titrated with 0.130 M NAOH. What is the molar mass of the acid if 38.4 mL of the NaOH solution is required to neutralize the sample? Assume the volume of NaOH corresponds to the second equivalence point. 10 11 12 13 molar mass: g/mol 18 19 20 21 22 23 24

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 nom bases. 000 species NH₂ I Don't Know NH4 H₂O CH₂CH₂COOH F H₂0* CH₂CH₂COO HF Submit relative pH of 0.1 M aqueous solution 8 (highest) (Choose one) ▼ (Choose one) ▼ 3 6 1 (lowest) (Choose one) ▼ (Choose one) ▼ 4 X ? S Ar AL Send a

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 ΙΟ HF HIO F ОН NO₂ HNO₂ H₂O relative pH of 0.1 M aqueous solution (Choose one) (Choose one) 3 5 8 (highest) (Choose one) 2 (Choose one) 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. 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)

Calculate the pH of the solution that results from mixing 80.0 mL of 0.052 MHCN(aq) with 20.0 mL of 0.023 M NaCN(aq). The K, value for HCN is 4.9 × 10-10. pH = Calculate the pH of the solution that results from mixing 27.0 mL of 0.034 M HCN(aq) with 73.0 mL of 0.061 M NACN(aq). pH = Calculate the pH of the solution that results from mixing 49.0 mL of 0.115 M HCN(aq) with 49.0 mL of 0.115 M NaCN(aq). pH =