Determine the pH of a solution by constructinga BCA table, constructing an ICE table, writingthe equilibrium constant expression, and usingthis information to determine the pH. The valueof Kb for NH3 is 1.8 x 10-5. Complete Parts 1-4before submitting your answer.1234NEXTTwo solutions are mixed: 40.0 mL of 0.500 M NH3 and25.0 mL of 0.300 M HCI. Fill in the table with theappropriate value for each involved species to determinethe moles of reactant and product after the reaction ofthe acid and base.Before (mol)Change (mol)After (mol)NH3(aq)+H*(aq)->NH, (aq)RESET-040.00.50025.00.3000.300-x0.0075-0.00750.0100-0.01000.0125-0.01250.0200-0.0200

A BCA table is a tool used to track the amounts of the reactants and products involved in a chemical…

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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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Determine the number of grams of NH Br needed to prepare an aqueous solution at a specific pH by constructing an ICE table, writing the equilibrium constant expression, and using this information to determine the initial grams of NH Br required. The Kb of NH, is 1.8 × 10%. Complete Parts 1-3 before submitting your answer. 1 2 3 NEXT > An unknown quantity of NH Br is dissolved in 1.00 L of water to produce a solution with a pH = 5.16. Let x represent the original concentration of 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) NH,(aq) + H₂O(1) x -6.9 × 10€ x-6.9 × 10-6 = HO*(aq) 0 NH,(aq) 0 6.9 × 10-6 6.9 x 10 6.9 × 10-6 6.9 × 10€ RESET 0 1.00 5.16 1.8 x 10-5 x 2x 0.5x -x -2x -0.5x 6.9 × 10-0 -6.9 × 10* 0.709 -0.709 x+6.9 x 10-6 x-6.9 x 10-6 x +0.709 x-0.709 MacBook Air
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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
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Q3- The acid-dissociation constant for chlorous acid, HCIO,, at 25C is 1.0x10. Calcul the concentration of H+ if the initial concentration of acid is 0.100 M. d Q4- How many grams of sodium hydroxide (M.wi=58.5) can be added 0 2.5 liter of a solution mixture of 0.3M ammonia and 0.15M ammonium chloride without changi POH by more than lunit? Ky=1.8x 10°? w
A buffer solution is prepared by combining 0.848 moles of formic acid and 0.719 moles of sodium formate. What will the solution pH be if 0.126 moles of sodium hydroxide (NaOH) is added to the buffer solution? The K₂ of formic acid is 1.8 x 10-4. (Two decimal places) Type your answer...
The pH of a blood plasma is 7.36. Assuming the principle of buffer system is HCO3-/H2CO3, calculate the ratio HCO3-/H2CO3. Is this buffer solution more effective against an added acid or an added base? (Ka1= 4.2 x 10-7 and Ka2 = 4.8 x 10 -11) (Need to show your calculation.).

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