What is the pH of a solution when 4.9 g of ammonium bromide, NH4BR (M=98) , is used to make 200 mL of solution?NH4*(aq) + H20(1) →H30*(aq) + NH3(aq)The equilibrium constant Kc= 5.6 x 10-10O a. 12.22O b. 9.07O c. 1.77O d. 7O e. 4.92

Mass of NH4Br = 4.9 g Volume of solution = 200 mL K = 5.6E-10 pH =?

What is the pH of a solution when 4.9 g of ammonium bromide, NH,Br (M=98) , is used to make 200 mL of solution? NH4*(aq) + H2O(1) →H3O*(aq) + NH3(aq) The equilibrium constant Kc= 5.6 x 10-10 O a. 12.22 O b. 9.07 О с. 1.77 O d. 7 О е.4.92

What is the pH of a solution when 4.9 g of ammonium bromide, NH,Br (M=98) , is used to make 200 mL of solution? NH4(aq) + H2O(1) →H3O(aq) + NH3(aq) The equilibrium constant Kc= 5.6 x 10-10 O a. 12.22 O b. 9.07 О с. 1.77 O d. 7 О е.4.92

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

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Acid Base Titration

An acid-base titration is the method of quantitative analysis for determining the concentration of an acid and base by exactly neutralizing it with a standard solution of base or acid having known concentration.

Question

What is the pH of a solution when 4.9 g of ammonium bromide, NH4BR (M=98) , is used to make 200 mL of solution?
NH4*(aq) + H20(1) →H30*(aq) + NH3(aq)
The equilibrium constant Kc= 5.6 x 10-10
O a. 12.22
O b. 9.07
O c. 1.77
O d. 7
O e. 4.92

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