12:04Question 4 of 9SubmitA buffer solution contains dissolved C6H5NH2and C6H;NH;CI. The initial concentration ofC6HŞNH2 is 0.50 M and the pH of the buffer is4.20. Determine the concentration ofC6HŞNH3* in the solution. The value of Kb forC6H;NH2 is 3.8 × 10-1º.123Let x represent the original concentration ofC6H,NH,* in the water. Based on the givenvalues, set up the ICE table in order todetermine the unknown.C6H5NH2(at H20(1) = OH-(aq) +C6H5NH3*(aInitial (M)Change (M)Equilibrium(M)5 RESET0.50-4.20-4.206.3 x 10-5-6.3 x 10-51.6 x 10-10-1.6 x 10-103.8 x 10-10-3.8 x 10-10x + 4.20x - 4.20x + 6.3 x 10-5х - 6.3 х 10-6x + 1.6 x 10-10x - 1.6 x 10-10x + 3.8 x 10-10x - 3.8 x 10-10Tap here or pull up for additional resources

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A buffer solution contains dissolved C6HsNH2 and CsHsNH3CI. The initial concentration of CeHŞNH2 is 0.50 M and the pH of the buffer is 4.20. Determine the concentration of CeHŞNH3* in the solution. The value of Kb for C6H;NH2 is 3.8 × 10-1°. 3 Let x represent the original concentration of C6H,NH3* in the water. Based on the given values, set up the ICE table in order to determine the unknown. C6HŞNH2(at H2O(1) = OH-(aq) C6H5NH3*(a Initial (M) Change (M) Equilibrium (M)

A buffer solution contains dissolved C6HsNH2 and CsHsNH3CI. The initial concentration of CeHŞNH2 is 0.50 M and the pH of the buffer is 4.20. Determine the concentration of CeHŞNH3* in the solution. The value of Kb for C6H;NH2 is 3.8 × 10-1°. 3 Let x represent the original concentration of C6H,NH3* in the water. Based on the given values, set up the ICE table in order to determine the unknown. C6HŞNH2(at H2O(1) = OH-(aq) C6H5NH3*(a Initial (M) Change (M) Equilibrium (M)

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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