.ol Verizon LTE12:37 PMO 29% OQuestion 4 of 16SubmitDetermine concentration of OH- in a 0.724 Msolution of BrO" (Kb = 4.0 x 10-°).%3D123Based on your ICE table and definition of Kb, setup the expression for Kb in order to determine theunknown. Do not combine or simplify terms.Kp4.0 x 10-6%3D5 RESET[0][0.724][4.0 х 10-%][0.362][x][2x][2x]?[0.724 + x][0.724 - x][0.724 + 2x][0.724 - 2x][4.0 × 10-6 + x][4.0 x 10-6 - x][4.0 x 10-6 + 2x][4.0 x 10-6 - 2x] ll Verizon LTE12:36 PMO 29% OQuestion 4 of 16SubmitDetermine concentration of OH- in a 0.724 Msolution of BrO" (Kb = 4.0 x 10-6).%3D123Based on the given values, set up ICE table inorder to determine the unknown.BrO (aq) +H20(1)OH (aq) + HBrO(aq)Initial (M)Change (M)Equilibrium(M)5 RESET0.7244.0 x 10-e0.362+x-X+2x-2x0.724 + x0.724 - x0.724 + 2x0.724 - 2x4.0 × 10-6 + x4.0 × 10-6 - x4.0 x 10-6 + 2x| 4.0 × 10-6 - 2x

Given: Concentration of BrO- = 0.724 M Kb = 4.0 ×10−6 The reaction is,

Determine concentration of OH- in a 0.724 M solution of BrO" (Kb = 4.0 × 10-*). 1 2 3 > Based on your ICE table and definition of Kb, set up the expression for Kb in order to determine the unknown. Do not combine or simplify terms. Kb = 4.0 x 10-6

Determine concentration of OH- in a 0.724 M solution of BrO" (Kb = 4.0 × 10-*). 1 2 3 > Based on your ICE table and definition of Kb, set up the expression for Kb in order to determine the unknown. Do not combine or simplify terms. Kb = 4.0 x 10-6

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...

See similar textbooks

Similar questions

"Tonsanb stum. In the laboratory a student measures the percent ionization of a 0.532 M solution of acetylsalicylic acid (aspirin), HC,H,O1, to be 2.45 %. Calculate value of K, from this experimental data. K = Submit Answer Retry Entire Group 9 more group attempts remaining 6:39 PM 99+ 10/25/2020 prt sc end fo トI トト」 delete home po 40 & num 6. backspace lock 8. home H. J. K enter (3
Using the constant below, calculate the molar concentration (M) of acid H3O* in solution if the concentration of OH- is 3.4 x 10-5. Kw = 1.0 × 10-14 M²= [H3O*][OH]. %3D O a) 2.9 x 10-10 O b) 2.0 x 10-10 O) 3,4 x 109 d) 2.4 x 10-10 e) 3.4 x 109
You need to prepare a pH = 9.20 buffer solution containing NH3 and NH4Cl. If you start with 0.71 M NH4Cl solution, what concentration of NH3 l will you need to also start with? (Kb for NH3 is 1.8x10-5)
For a 5.55-102 M solution of H₂CHO calculate both the pH and the CH4O2 ion concentration. State symbols are not shown for water or the aqueous species in the reaction equations. HiệnHoDe+H2OHOHOH. Đó Ki-7,9×105 HC₂H₂O + H₂0H₂O + CH606² K₂21.6x10-12 pH = [CH₂O2)
Determine the pH at the point in the titration of 40.0 mL of 0.200 M H2NNH2 with 0.100 M HNO3 after 100.0 mL of the strong acid has been added. The value of Kb for H,NNH, is 3.0 × 10-6. ( PREV 1 Based on the result of the acid-base reaction, determine the pH of the solution. pH RESET 6.21 7.79 11.3 2.70 1.85 1.70 3.91 10.1 12.3 3.70 17.7
2. Acetic acid has a K₂ of 1.8 x 10-5. What is the concentration of H+ ions in a 0.20 M acetic acid solution? Remember that you'll need to use an ICE table and potentially the quadratic formula to solve this problem. There is a
The pH of blood is 7.4. What is the ratio (to one decimal place) of bicarbonate (conjugate base) to carbonic acid (weak acid) in the blood's buffering equilibrium? Note, the K₂ of carbonic acid is 4.27 x 10-7. Write your answer this way: # to 1 Done Clear Incorrect. The ratio is 10.7 to 1, indicating that there is 10 times more bicarbonate than carbonic acid. Enter the correct answer.
Determine 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. NEXT > 0.040 mol of solid NaOH is added to a 200.0 mL buffer containing 0.100 mol C6H5NH3Cl and 0.500 M C6H5NH₂. 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. You can ignore the amount of water in the reaction. Before (mol) Change (mol) After (mol) 0.060 Initial (M) Change (M) Equilibrium (M) 0 -X 0.700 - x 1 -0.060 C6H5NH3*(aq) + OH (aq) 0 1 0.040 0.140 0.500 + x CoHşNHz(aq) + 0.300 + x 2 0.500 0.500 - x -0.040 0.300 - x -0.140 Determine 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…
Assume that: • Acid 1 is a stronger acid that Acid 2. You prepare two separate solutions, using 1.0 mol of each acid and mixing it with 1.0 L of pure water. Determine which of the following statements is correct. Select all that apply. O Multiple answers: Multiple answers are accepted for this question Select one or more answers and submit. For keyboard navigation... SHOW MORE V a Acid 1 has a larger K value that Acid 2. b Acid 1 will generate a higher concentration of H,0* ions. The solution prepared using Acid 1 will have a lower pH. d. Acid 1 will generate a higher concentration of A- ions. e The concentration of unreacted "HA" at equilibrium for the Acid 1 solution will be lower. f The pK value for Acid 1 is lower than the pK value for Acid 2.
Calculate the pH after 0.032 mole of NaOH is added to 1.00 L of each of the following solutions. a. 0.145 M HONH, (K = 1.1 × 10-) pH = b. 0.145 M HONH, Cl pH = c. pure H₂O pH = d. a mixture containing 0.145 M HONH₂ and 0.145 M HỌNH3 C1 pH =
Part B Calculate the concentrations of HF, OH, and H₂O* in a 0.18 M KF solution (for which K. (HF) = 6.8 x 10-4). Express your answer in moles per liter to two significant figures. Enter your answers numerically separated by commas. 195] ΑΣΦ [HF). [OH], [H₂O*] = ? M >
Determine the resulting pH when 0.040 mol of solid NaOH is added to a 200.0 mL buffer containing 0.100 mol C6H5NH3CI and 0.500 M C6H5NH2. The value of Kb for C6H5NH2 is 4.3 x 101°. 1 2 3 4 NEXT Use the table below to determine the moles of reactant and product after the reaction of the acid and base. You can ignore the amount of liquid water in the reaction. C6H;NH3*(aq) Он (aq) H20(1) C6H;NH2(aq) + + Before (mol) Change (mol) After (mol) 5 RESET 0.040 -0.040 0.500 -0.500 0.100 -0.100 +x 0.040 + x 0.040 - x 0.100 + x 0.100 - x 0.060 -0.060 -x 0.140 -0.140 0.020 -0.020