Please help with 7a and 7b 7. Calculate the equilibrium concentration of each aqueous species (H2A, HA- A?-, H30*, and OH-)in the solution. Assume a temperature of 25°C. H2A: pKa1 = 2.05 and pk2 = 6.22а. 0.10 М Н,Аb. 0.10 M NazA

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Answered: 7. Calculate the equilibrium…

Chemistry: Principles and Reactions

8th Edition

ISBN:9781305079373

Author:William L. Masterton, Cecile N. Hurley

Publisher:William L. Masterton, Cecile N. Hurley

Chapter15: Complex Ion And Precipitation Equilibria

Section: Chapter Questions

Problem 76QAP

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9. We prepared a solution containing 1.0 mol.L' HF and 1.0 mol.L·' C,H3OH. The K, of hydrofluoric acid and phenol are 7.2 x 104 and 1.6 x 10-10 respectively. What is the pH of this solution? (Hint: find which acid is strongest and make the appropriate assumptions) b. What is the concentration of C,H;O¯ at equilibrium? а.
At 25°C, K = 3.40 x 10-3 S m-1 for 0.00100 M NH4OH. Values of Lo are: NH4C1 = 0.01497, NaOH = 0.02481, NaCl = 0.01265 S m2 mol-1. Find the dissociation constant of ammonium hydroxide.
8. Calculate the equilibrium concentration of each aqueous species (HzA, HA- A2, H3O*, and OH-) in the solution. Assume a temperature of 25°C. H2A: pKa1 = 2.05 and pKa = 6.22 a. 0.10 M HzA b. 0.10 M NazA
6. What are the equilibrium concentrations of a 0.80 M HCN solution for each species (in M to two decimal places)? HCN(aq) = H(aq) + CN¯(aq) Kc = 4.9 × 10-10 A: [HCN] = 0.80, [H] = 1.98×105, [CN] = 1.98×10 ghans
4. Determine the equilibrium concentrations of H2C4H4O5, HC4H4O5", C4H4O,2, and H* when 3.85 M H2C4H4O6 solution achieves equilibrium. Ka1 = 1.1 x 103 and Kaz = 4.6 x a 105
6. A buffer solution is formed by adding 0.500 mol of sodium acetate (CH3CO2NA) and 0.500 mol of acetic acid (CH3CO2H) to 1.00 L H,0. What is the pH of the solution at equilibrium? (K, = %3D 1.8 x 10°)
Part 3 - Put it all together. Calculate the concentrations of all species in a 0.690 M Na, So, (sodium sulfite) solution. The ionization constants for sulfurous acid are Ka = 1.4 x 102 and K = 6.3 x 108. !! [Na*] = 1.38 [SO] =| 0.690 [HSO,] = - TOOLS x10 [H,SO,] = [OH ] = M. %3D [H*] =
1. The ionization constant (K») of aniline (C6HSNH2) is 2.35 x 10-5, If 7.285 grams of aniline is dissolved in 100.0 mL of water, what are the equilibrium concentration of all species present? 2. A certain acidic vitamin is essential for all mammals since it plays a role in DNA repair and cell signaling. A 0.439 M solution of this acid is found to have a pH of 2.607. Based on the table below, what most likely is the identity of this unknown acid?
0.0500 M HF (Ka= 7.20 x 10–4) determine the equilibrium molar concentration of H3O+ and equilibrium molar concentration of HF (in 3 sig. figures).
1. The ionization constant (Kb) of aniline (C6H5NH2) is 2.35 x 10^-5. If 7.285 grams of aniline is dissolved in 100.0 mL of water, what are the equilibrium concentration of all species present?2. A certain acidic vitamin is essential for all mammals since it plays a role in DNA repair and cell signaling. A 0.439M solution of this acid is found to have a pH of 2.607. Based on the table below, what most likely is the identity of thisunknown acid?
Benzoic acid (C₂H5CO₂H), a weak acid, has a dissociation constant of K=6.3x10^-5. 1. Write the equilibrium equation of the solution. 2. Write the Ka expression of the equilibrium involved. 3. What is the equilibrium concentration of all species if the initial concentration is a.) 0.0315M, b) 0.315M² 4. What is the resulting pH and pOH for a) and b)? 5. What is the %ionization of benzoic acid in a) and b) solution?
Part 1 - Determining Kp by lon Concentration 9.92 4.03 9.3325 x 10 pH of solution: pOH = 14-pH: [OH] = 10: Complete the following ICE table (using x): Kup Table Mg(OH); (s): Molarity: initial concentration 1 Change Equilibrium concentration |-X 0.15589 MB (OH)2 Complete the following ICE table (now using actual concentrations): Mg(OH), (8) K, Table Molarity: initial concentration Change Equilibrium concentration Kip [Mg][OH]: Mg (aq) 4 X X + 2 OH(aq) 0 2x Mg² (aq) + 2x To find K, use the above ICE table to find the concentration of Mg" (you found the concentration of OH above using the pOH). Because there is a 1:2 stoichiometric ratio between Mg" and OH, [Mg] = [OH 1/2. Plug the values of [Mg] and [OH-] into the K, expression below: 2OH(aq)

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7. Calculate the equilibrium concentration of each aqueous species (H2A, HA- A²-, H30*, and OH-) in the solution. Assume a temperature of 25°C. H2A: pka1 = 2.05 and pK22 = 6.22 а. 0.10 М НА b. 0.10 M NazA