Calculate the pH of a weak base solution (quadratic equation). Calculate the pH of a 0.0295 M aqueous solution of ethylamine (C₂H5NH₂, Kb = 4.3x10-4) and the equilibrium concentrations of the weak base and its conjugate acid. PH [C₂H5NH₂]equilibrium + [C₂H5NH3 Jequilibrium M M
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- COHSOH(ag) + H2On + CeHsO (aq) + H3O*(a9) Ka= 1.12 x 10-10 (a) Phenol is a weak acid that partially dissociates in water according to the equation above. Write the equilibrium-constant expression for the dissociation of the acid in water. (b) What is the pH of a 0.75 M CaHsOH(ag) solution? (C) For a certain reaction involving CaHsOH(ag) to proceed at a significant rate, the phenol must be primarily in its deprotonated form, C3H5O (eg). In order to ensure that the CsHsOH(aq) is deprotonated, the reaction must be conducted in a buffered solution. On the number scale below, circle each pH for which more than 50 percent of the phenol molecules are in the deprotonated form (CoHsO (aq). Justify your answer. 1 2 3 4 5 6 7 8 9 10 11 12 13 14 Justification: (d) CeHsOH(ag) reacts with NaOH(ag). Write a net ionic equation representing this reaction (aka: invasion equation). (e) What is the pH of the resulting solution when 30 mL of 0.40 M CSH5OH(aq) is added to 25 mL of 0.60 M NAOH. Show all work…Calculate the pH of a weak base solution ([B]o > 100 • Kp). Calculate the pH of a 0.104 M aqueous solution of triethanolamine (C,H1503N, K, = 5.8×10") and the equilibrium concentrations of the weak base and its conjugate acid. pH (C,H1503N]equilibeium (C,H15O3NH"]equilibrium Check & Submit Answer Show Approach Calculate the pH of a weak base solution (quadratic equation). Calculate the pH of a 0.0362 M aqueous solution of ethylamine (C,H;NH2. Kg – 4.3×10“) and the equilibrium concentrations of the weak base and its conjugate acid. pH (C,H;NH;lequilibrium M. (C,H,NH3" Jequilibrium M. Check & Submit Answer Show ApproachThe acid dissociation constant K, of alloxanic acid (HC,H;N,0,) is 2.24 x 10¬'. Calculate the pH of a 4.2 M solution of alloxanic acid. Round your answer to 1 decimal place. pH =
- Calculate the pH of a weak base solution (quadratic equation). Calculate the pH of a 0.0295 M aqueous solution of ethylamine (C₂H5NH₂, Kb = 4.3x10-4) and the equilibrium concentrations of the weak base and its conjugate acid. PH [C₂H5NH₂]equilibrium + [C₂H5NH3 Jequilibrium ΣΣThe amino acid asparagine has ionization constants Kal = 6.92 x 10-3 and K ₁2 = 6.92 x 10-3 and K₁2 = 1.86 x 10-9, which correspond to the carboxylic acid group and the amino group respectively. Calculate the pH of a 0.170 M asparagine (HN) solution. pH =Determine if the following salt is neutral, acidic or basic. If acidic or basic, write the appropriate equilibrium equation for the acid or base that exists when the salt is dissolved in aqueous solution. If neutral, simply write only NR. KC3H;O3 O4- 3- O2+ 3+ D 4+ 1 2 3 4 6. 7 8 9 1 3 4 6. 7 (s) (1) (g) ||(aq) + NR OH C H H30* H20 K Reset • x H20 Delete 1L LO 2. 2.
- 3. A 0.0560 g quantity of acetic acid is dissolved in enough water to make 50.0 mL of solution. Calculate the concentrations of H;O*, CH;COO and CH;COOH at equilibrium. What is the pH of the solution? (Ka = 1.8x10) CH;COOH(aq) = CH;COO (aq) + H;O* (aq) a) Calculate the initial concentration of CH;COOH. (C:12; H:1; 0:16) b) Calculate the concentration of CH;CoO (aq) and H;O* (aq) at equilibrium. c) Calculate pH of the solution.Calculate the pH and the equilibrium concentrations of HS and s2 in a 0.0805 M hydrosulfuric acid solution, H,S (aq). For H,S, Ka1 = 1.00×107 and K2 = 1.00x1019 pH = [HS') =Calculate the pH of a weak base solution ([B] > 100 K₂). Calculate the pH of a 0.247 M aqueous solution of hydroxylamine (NH₂OH, K₂ = 9.1×109) and the equilibrium concentrations of the weak base and its conjugate acid. pH [NH₂OH] equilibrium (NH3OH*]equilibrium ΣΣ
- According to Henry’s law the atmospheric partial pressure of CO2 dictates the concentration of aqueous CO2 according to the following equilibrium expression where k is the Henry’s law constant for CO2. CO2 (g) <-> CO2 (aq) k=1x10^-1.5 The acid dissociation constant Ka for carbonic acid applies to CO2 (aq). Given pKa1=6.35 and pKa2=10.33 and the fact that the partial pressure of CO2 in the atmosphere is 10^-3.5 atm, find the pH of water in equilibrium with the atmosphere.The acid dissociation constant K, of carbonic acid (H,CO,) is 4.5 × 10 '. Calculate the pH of a 4.0M solution of carbonic acid. Round your answer to 1 decimal place. pH ?What is the pH of a grapefruit that contains 0.007 M citric acid solution (CsH2O-)? CH;O;(aq) + H;O(2) = CH;0, (aq) + H3Oʻ(aq) K, = 7.5 x 104 Round your answer to 2 decimal places.