Determine the pH of a solution by constructing an ICE table, writing the equilibrium constant expression, and using this information to determine the pH. Complete Parts 1-3 before submitting your answer. 1 3 A solution is prepared with 0.075 M (CH3)3N and 0.10 M (CH3)2NHCI. 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) 5.2 x 10-4 -2x (CH3)3N (aq) + +X 0.075 + x H₂O (1) = 0.075 OH (aq) + (CHs)sNH*(aq 0.075 - x NEXT > RESET 0.10 +2x 0.075 + 2x

Determine the pH of a solution by constructing an ICE table, writing the equilibrium constant expression, and using this information to determine the pH. Complete Parts 1-3 before submitting your answer. 1 3 A solution is prepared with 0.075 M (CH3)3N and 0.10 M (CH3)2NHCI. 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) 5.2 x 10-4 -2x (CH3)3N (aq) + +X 0.075 + x H₂O (1) = 0.075 OH (aq) + (CHs)sNH*(aq 0.075 - x NEXT > RESET 0.10 +2x 0.075 + 2x

Chemistry for Engineering Students

4th Edition

ISBN:9781337398909

Author:Lawrence S. Brown, Tom Holme

Publisher:Lawrence S. Brown, Tom Holme

Chapter12: Chemical Equilibrium

Section: Chapter Questions

Problem 12.66PAE

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Determine the pH of a buffer solution by constructing an ICE table, writing the equilibrium constant expression, and using this information to determine the pH. Complete Parts 1-3 before submitting your answer. 3 > A solution is prepared with 0.55 M HNO2 and 0.75 M KNO2. 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) -2x 0.75 -2x 0 1 HNO₂(aq) 0.55 + x 0.55 -X 0.55-x 0.55 0.55 - x 0.75 2 H₂O(l) III 0.55 + 2x 6.8 x 104 0.55 - 2x 1L +x H3O+(aq) 0.75 + x +x -X 0.75-x + NO₂ (aq) RESET +2x NEXT 0.75 + 2x +x
Based on your ICE table (Part 1) and the definition of Kb, set up the expression for Kb in order to determine the unknown. Each reaction participant must be represented by one tile. Do not combine terms. Kb = = 5.2 × 10-4 RESET [0] [0.075] [0.10] [5.2 × 10] [x] [2x] [2x]² [0.075 + x] [0.075 - x] [0.075 + 2x] [0.075 - 2x] [0.10+x] [0.10 - x] [0.10 + 2x] [0.10 -2x] < PREV 2 3 Based on your ICE table (Part 1) and the equilibrium expression for Kb (Part 2), determine the pH of the solution. pH = RESET 0 7.86 6.14 0.075 3.9 × 10 3.41 10.59 1.12
Determine the pH of a buffer solution by constructing an ICE table, writing the equilibrium constant expression, and using this information to determine the pH. Complete Parts 1-3 before submitting your answer. NEXT > The buffer was prepared by dissolving 21.5 g HC,H,O₂ and 37.7 g of NaC,H,O₂ in 200.0 mL of solution. 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) 0.178 0.880-x [0] [0.888] [1.31 + x) 0 0 0.888 1.31 + x HC₂H5O₂(aq) + [21.5] [x] Ka = 4.2 x 10-² 21.5 0.178 + x +x [37.7] [2x] 1 [0.178+x][0.888 + x] 37.7 -x 0.888 + x Determine the pH of a buffer solution by constructing an ICE table, writing the equilibrium constant expression, and using this information to determine the pH. Complete Parts 1-3 before submitting your answer. 6.23 The Ka for HC₂H5O₂ is 6.3 x 10-5. Based on your ICE table (Part 1) and the definition of Ka, set up the expression for Ka…
Determine the pH of a buffer solution by constructing an ICE table, writing the equilibrium constant expression, and using this information to determine the pH. Complete Parts 1-3 before submitting your answer. 3 NEXT > The buffer was prepared by dissolving 21.5 g HC7H5O2 and 37.7 g of NaC7H5O₂ in 200.0 mL of solution. 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) 0.178 0.880 - x 0 0.888 1 HC7H5O₂(aq) + 1.31 + x 21.5 +X 0.178 + x 37.7 -X H₂O(1) 0.888 + x 0.176 21.5-x H3O+ (aq) 0.261 37.7 + x + 0.880 0.176 - x C7H5O₂ (aq) RESET 1.31 0.261 + x
A solution is prepared that is initially 0.30M in hydrofluoric acid (HF) and 0.13M in potassium fluoride (KF). 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 [H3O+]. You can leave out the M symbol for molarity. [HF] [F] [H,O] initial 0 0 change 0 final 0 0 ㅁ 1 G
A solution is prepared that is initially 0.078M in propanoic acid (HC,H,CO,) and 0.38M in potassium propanoate (KC,H,CO,). 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 H30" |. You can leave out the M symbol for molarity. [HC,H,Co,] [c,,co] [1,0] initial change final
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. Initial (M) Change (M) Equilibrium (M) 0.022 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. 0 1 CCI CO₂H(aq) + 0.0715 1.40 2 -1.40 H₂O(1) 2 H3O+ (aq) + CCI3CO₂ (aq) NEXT > 0.040 -0.040 RESET 0.032 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. Initial (M) Change (M) Equilibrium (M) 0.000 The pH for 0.0715 M solution of CCI.COH 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. 0 1 CCI.COH(aq) + H₂O(l)…
A solution is prepared that is initially 0.29.M in hydrofluoric acid (HF) and 0.40 Afin sodium fluoride (NAF). 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 [H0] You can leave out the M symbol for molarity. initial change finali 0 0 0 [r] 0 0 0 [1,01] 0 0 0 DO
ACID-BASE EQUILIBRIA Doc Jill wants to determine the Ao of a weak acid she isolated called Xcitingpartic acid (HXp). She prepared a solution of the weak acid by diluting 2.7 ml of 0.20 M HXp with 19.3 mlL of water. Upon measuring the conductivity of the solution and a blank, she obtained 205.0 µS/cm and 2.0 uS/cm, respectively. She also measured the pH of the solution and got a pH of 3.49. Help her find the following: 1. Concentration of the weak acid (HXp) after dilution 2. Corrected conductivity 3. Molar conductivity of the solution 4. Equilibrium concentration of H30, and Xp 5. a 6. Equilibrium concentration of the weak acid (HXp) 7. K, 8. Ao
A student was titrating a solution of hydrazine (H,NNH,) with a nitric acid solution. Determine the pH at a particular point in the titration. Do this by constructing a BCA table, constructing an ICE table, writing the equilibrium constant expression, and use this information to determine the pH. Complete Parts 1-4 before submitting your answer. NEXT > A 40.0 mL of 0.200 M H,NNH, was titrated with 10 mL of 0.100 M HNO, (a strong acid). Fill in the ICE 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 liquid water in the reaction. H,NNH,(aq) H'(aq) H,NNH, (aq) Before (mol) Change (mol) After (mol) S RESET 0.200 0.100 1.00 x 10 -1.00 x 10 2.00 x 10 -2.00 x 10° 7.00 x 10° -7.00 x 10 8.00 x 10° -8.00 x 10 6.00 x 10° -6.00 x 10*
ACID-BASE EQUILIBRIA Doc Jill wants to determine the A, of a weak acid she isolated called Xcitingpartic acid (HXp). She prepared a solution of the weak acid by diluting 2.7 mL of 0.20 M HXp with 19.3 mL of water. Upon measuring the conductivity of the solution and a blank, she obtained 205.0 µS/cm and 2.0 µS/cm, respectively. She also measured the pH of the solution and got a pH of 3.49. Help her find the following: 1. Concentration of the weak acid (HXp) after dilution 2. Corrected conductivity 3. Molar conductivity of the solution 4. Equilibrium concentration of H30*, and Xp" 5. a 6. Equilibrium concentration of the weak acid (HXp) 7. Ka 8. Ao
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 HC₂H₂O₂ is 1.8 × 105. Complete Parts 1-4 before submitting your answer. 2 3 2 NEXT > 2 Two solutions are mixed: 20.0 mL of 0.20 M HC₂H₂O₂ and 20.0 mL of 0.10 M NaOH. 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. Before (mol) Change (mol) After (mol) -2.0 × 10-³ 0 3.0 × 10-³ 1 HC,H,O,(aq) 20.0 -3.0 × 10-³ 2 0.20 OH(aq) 4.0 × 10-³ 0.10 3 -4.0 × 10-³ H₂O(1) 1.0 × 10-³ 4 -1.0 × 10³ C,H,O,(aq) RESET 2.0 × 10-³

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