Determine the concentration of CH NH¸* in a buffer solution by constructing an ICE table, writing the equilibrium constant expression, and use this information to determine the concentration of CH NH+. The Kb for CH NH₂ is 3.8 × 10-10. Complete Parts 1-3 before submitting your answer. 2 1 2 3 NEXT > 2 A buffer solution contains dissolved CH NH and CH NH Cl. The initial concentration of CH NH2 is 0.50 M. The pH at equilibrium of the buffer is 4.20. Let x represent the original concentration of CH NH+ in the water. Fill in the ICE table with the appropriate value for each involved species to determine concentrations of all reactants and products. Initial (M) Change (M) Equilibrium (M) CH NH2(aq) + H₂O(I) = OH(aq) + C HẠNH, (aq) RESET 0 0.50 x 4.20 -4.20 6.3 x 10-5 -6.3 x 10-5 1.6 × 10-10 -1.6 × 10-10 3.8 × 10-10 -3.8 × 10-10 x +4.20 x-4.20 x + 6.3 x 10-5 x - 6.3 × 10-5 x + 1.6 × 10-10 x-1.6 × 10-10 x + 3.8 × 10-10 x - 3.8 × 10-10

Determine the concentration of CH NH¸* in a buffer solution by constructing an ICE table, writing the equilibrium constant expression, and use this information to determine the concentration of CH NH+. The Kb for CH NH₂ is 3.8 × 10-10. Complete Parts 1-3 before submitting your answer. 2 1 2 3 NEXT > 2 A buffer solution contains dissolved CH NH and CH NH Cl. The initial concentration of CH NH2 is 0.50 M. The pH at equilibrium of the buffer is 4.20. Let x represent the original concentration of CH NH+ in the water. Fill in the ICE table with the appropriate value for each involved species to determine concentrations of all reactants and products. Initial (M) Change (M) Equilibrium (M) CH NH2(aq) + H₂O(I) = OH(aq) + C HẠNH, (aq) RESET 0 0.50 x 4.20 -4.20 6.3 x 10-5 -6.3 x 10-5 1.6 × 10-10 -1.6 × 10-10 3.8 × 10-10 -3.8 × 10-10 x +4.20 x-4.20 x + 6.3 x 10-5 x - 6.3 × 10-5 x + 1.6 × 10-10 x-1.6 × 10-10 x + 3.8 × 10-10 x - 3.8 × 10-10

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

The equation is CH3COOH+H20 is in equilibrium with CH3COO^- + H30^+ How can I find the concentrations of the CH3COOH, CH3COO^-, H30^+ if I'm only given these: Initial concentration of CH3COOH = 1.00 M Final concentration of CH3COOH (with water) = 0.06666666667 M Fraction of CH3COOH ionized (labeled as a) = 0.01221 Fraction of CH3COOH ionized was calculated by dividing the molar conductivity of the sample divided by molar conductivity of solution in infinite dilution.
5 A buffer system is prepared by combining 0.569 moles of ammonium chloride (NH4Cl) and 0.586 moles of ammonia (NH3). What will the solution pH be if 0.158 moles of the nitric acid (HNO3) is added to the solution. Nitric acid is a strong acid. The K, of ammonia is 1.8 x 105. (Two decimal places) Type your answer..... Submit
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. The value of Ka for HCIO is 2.9 × 108. Complete Parts 1-4 before submitting your answer. 1 2 4 NEXT > 0.003 mol of solid NaOH is added to a 100.0 mL buffer containing 0.13 M HCIO and 0.37 M NaCIO. 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. HCIO(aq) + OH(aq) 0.013 0.003 Before (mol) Change (mol) -0.013 0.013 After (mol) 0.010 0.003 H₂O(I) + CIO (aq) 0.037 0.003 0.040 RESET 0 0.13 0.37 0.003 -0.003 0.013 -0.013 0.037 -0.037 0.010 -0.010 0.040 -0.040
A solution is prepared that is initially 0.27M in acetic acid (HCH3CO2) and 0.053M in potassium acetate (KCH3CO2). Complete the reaction table below, so that you could use it to calculate the pH of this solution. Use x to stand for the unknown change in [H₂O]. You can leave out the M symbol for molarity. [HCH2CO₂] cu_co, [H₂O*] initial change final
A patient presents itself to the emergency department in a critical condition. The patient’s blood was tested and the concentration of carbonic acid (H2CO3) was found to be 6.8 ×10-8 M and bicarbonate ion (HCO3-) 2.325 ×10-7 M Ka = 4.3 × 10-7 H2CO3(aq) ⇌ HCO3-(aq) + H+(aq) Show all calculations including equation(s) used. Calculate the pH of the patients’ blood. Based on your answer would you say the patient is suffering from Acidosis or Alkalosis?
4 A chemistry graduate student is given 100. mL of a 0.50M methylamine (CH,NH,) solution. Methylamine is a weak base with K,=4.4 × 10 *. What mass of CH,NH,Cl should the student dissolve in the CH, NH, solution to turn it into a buffer with pH = 10.93? You may assume that the volume of the solution doesn't change when the CH,NH, Cl is dissolved in it. Be sure your answer has a unit symbol, and round it to 2 significant digits. olo Ar x10
Consider the titration of 100.0 mL of 0.100 M NaOH with 1.00 M HBr. Find the pH at the following volumes of acid added. See the picture below. Kindly answer all the questions, thanks!
A pH buffer is a solution that resists changes in pH when acids or bases are added to it—typically, a solution of a weak acid and its conjugate base. What masses of dimethylamine and dimethylammonium chloride do you need to prepare 7.00 L of pH = 12.00 buffer if the total concentration of the two components is 0.500 M? Mass of dimethylamine = Mass of dimethylammonium chloride =