The question has two part please answer both Determine the pH of a solution of HCIO₂ by constructing an ICE table, writing the equilibrium constantexpression, and using this information to determine the pH. The Ka of HCIO₂ is 1.2 x 102. Complete Parts1-3 before submitting your answer.[0]PREVBased on your ICE table and the definition of Ka, set up the expression for Ka in order to determine the unknown. Each reactionparticipant must be represented by one tile. Do not combine terms.[0.020 -x][0.020][0.020 + 2x]Question 11 of 17K₂ =[1.2 x 10-¹]2[0.010][1.2 x 10-x][1.2 x 10+ x)[0.020 - 2x]= 1.2 x 10-²[2x][2x]²[1.2 x 10+ 2x] [1.2 x 10-² - 2x]RESET[0.020 + x]NEXT> Initial (M)Change (M)Equilibrium (M)pull up for additional resourcesDetermine the pH of a solution of HCIO₂ by constructing an ICE table, writing the equilibrium constantexpression, and using this information to determine the pH. The Ka of HCIO, is 1.2 x 102. Complete Parts1-3 before submitting your answer.NEXT >A 0.020 Maqueous solution of HCIO₂ is prepared. Fill in the ICE table with the appropriate value for each involved species todetermine concentrations of all reactants and products..HCIO₂(aq)1.2 x 10-2x00.020+xQuestion 11 of 170.0200.020-x1.2 x 10-²H₂O(l)0.020 + 2x0.0100.020 - 2x+x1.2 x 10-2 + xH,O*(aq)WEEEEEERESET+2x1.2 x 10+2x+CIO₂ (aq)

Given, Molarity of HClO2 = 0.020 MKa of HClO2 = 1.2 x 10-2

Initial (M) Change (M) Equilibrium (M) Determine the pH of a solution of HCIO, by constructing an ICE table, writing the equilibrium constant expression, and using this information to determine the pH. The Ka of HCIO, is 1.2 x 102. Complete Parts 1-3 before submitting your answer. 2 NEXT > A 0.020 Maqueous solution of HCIO₂ is prepared. Fill in the ICE table with the appropriate value for each involved species to determine concentrations of all reactants and products.. -2x HCIO₂(aq) 1.2 x 10-2x 0 0.020 + x Question 11 of 17 + 0.020 0.020-x G 1.2 x 10-² H₂O(l) 0.020 + 2x 0.010 +x 0.020 - 2x 1.2 x 10+x H,O^(aq) 1.2 x 10-x RESET +2x 1.2 x 10+ 2x CIO, (aq)

Initial (M) Change (M) Equilibrium (M) Determine the pH of a solution of HCIO, by constructing an ICE table, writing the equilibrium constant expression, and using this information to determine the pH. The Ka of HCIO, is 1.2 x 102. Complete Parts 1-3 before submitting your answer. 2 NEXT > A 0.020 Maqueous solution of HCIO₂ is prepared. Fill in the ICE table with the appropriate value for each involved species to determine concentrations of all reactants and products.. -2x HCIO₂(aq) 1.2 x 10-2x 0 0.020 + x Question 11 of 17 + 0.020 0.020-x G 1.2 x 10-² H₂O(l) 0.020 + 2x 0.010 +x 0.020 - 2x 1.2 x 10+x H,O^(aq) 1.2 x 10-x RESET +2x 1.2 x 10+ 2x CIO, (aq)

Chemistry: An Atoms First Approach

2nd Edition

ISBN:9781305079243

Author:Steven S. Zumdahl, Susan A. Zumdahl

Publisher:Steven S. Zumdahl, Susan A. Zumdahl

Chapter13: Acids And Bases

Section: Chapter Questions

Problem 164CWP: Consider a 0.60-M solution of HC3H5O3, lactic acid (Ka = 1.4 104). a. Which of the following are...

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Consider a 0.60-M solution of HC3H5O3, lactic acid (Ka = 1.4 104). a. Which of the following are major species in the solution? i. HC3H5O3 ii. C3H5O3 iii. H+ iv. H2O v. OH b. Complete the following ICE table in terms of x, the amount (mol/L) of lactic acid that dissociates to reach equilibrium. c. What is the equilibrium concentration for C3H3O3? d. Calculate the pH of the solution.
ermine the pH of a solution by constructing a BCA table, constructing an ICE table, writing the equilibrium constant expression, and using this information to determine the pH. Complete Parts 1-4 before submitting your answer. 2 NEXT > Two solutions are mixed: 40.0 mL of 0.500 M NH, and 25.0 mL of 0.300 M HCI. Fill in the 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.. NH3(aq) NH, (aq) (be),H Before (mol) Change (mol) After (mol) 5 RESET 40.0 0.500 25.0 0.300 0.300 -x 0.0075 -0.0075 0.0100 -0.0100 0.0125 -0.0125 0.0200 -0.0200 Based on the result of the acid-base reaction (Part 1), set up the ICE table in order to determine the unknown concentrations of all reactants and products. NH3(aq) H,O(1) OH (aq) NH, (aq) Initial (M) Change (M) Equilibrium (M) 5 RESET 0.500 0.300 0.192 0.313 0.115 0.500 -x 0.300 -x 0.192 +* 0.192 -x 0.500 + x 0.300 +x 0.313 + x 0.313 -x 0.115 +x 0.115-x
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