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
Determine the Ka for an acid by constructing an ICE table and using this information to construct and solve the equilibrium constant expression. Complete Parts 1-2 before submitting your answer. NEXT > The pH for 0.0715 M solution of CCI3CO₂H is 1.40. Fill in the ICE table with the appropriate value for each involved species to determine the unknown concentrations of all reactants and products. Initial (M) Change (M) Equilibrium (M) -0.032 CCI3CO₂H(aq) 0 077 0.0715 + 1.40 H₂O(l) T -1.40 14 2 H3O+ (aq) 100 0.040 -0.040 + CCI3CO₂ (aq) 1 RESET 0.032
A certain weak base has a Kp of 8.60 x 10-7. what concentration of this base will produce a pH of 10.37? concentration: M
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)
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 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
We have 500.0 mL of a buffer solution which is 0.651 M in NH3 and 0.354 M in NH4Cl. 500.0 mL of a 0.224 M HCl solution are added. The final volume is 1.0000 L. The Kb value for NH3 is 1.8 x 10-5. What is the final pH of this solution?
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.).
5. Formic acid is an organic acid, found in the venom of ants and bees. The diagram shows a molecule of formic acid dissociating in water. || H H H H H H a) Determine the dissociation constant of a 0.100 mol L-' formic acid solution that has a pH of 2.38. b) Use the dissociation constant calculated in part (a) to identify the strength of this acid.
Determine the Ka for an acid by constructing an ICE table and using this information to construct and solve the equilibrium constant expression. Complete Parts 1-2 before submitting your answer. NEXT > 5 A solution of phenol (HC H₂O) is prepared by dissolving 0.385 g of phenol in 2.00 L of H₂O. The solution has a pH = 6.29. Fill in the ICE table with the appropriate value for each involved species o determine the unknown concentrations of all reactants and products. H_O*(aq) + Initial (M) Change (M) Equilibrium (M) 1 HC,H,O(aq) + 5 H₂O(1) 2 C_H,O(aq)
both parts please

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