Write the equilibrium constant expression, K, for the following reaction taking place in dilute aqueous solution. CH3COOH(aq) + H₂O(1) H3O+ (aq) + CH3COO(aq) K=
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- Ascorbic acid (H₂C,H,O) is a diprotic acid. The acid dissocation constants for H₂C,H,O, are Kal = 8.00 x 10-5 and K₁2 = 1.60 x 10-12 Determine the pH of a 0.117 M solution of ascorbic acid. pH = Determine the equilibrium concentrations of all species in the solution. [H₂C,H,O,] = [HC,H,O,]= [C,H,O2] = M M MTopics References] Obtain the equilibrium constant for the reaction HCN(aq) = H*(aq) + CN¯(aq) From the following: HCN(aq) + OH (aq) = CN (aq) + H2O(1), K1 = 4.9 x 104 H2 O(1) = H* (aq) + OH (aq), K2 = 1.0 × 10 14 Equilibrium constant =Write the equilibrium constant expression, K, for the following reaction taking place in dilute aqueous solution.ClO- (aq) + H2O (l)HClO (aq) + OH- (aq)
- For each of the equilibrium reactions, give the products, balance the equation, and add the states (solid, liquid, gas, aqueous). Equilibrium Equation: Na2CO3 + AgNO3 ⇌ Equilibrium Equation: Ag2CO3 + HNO3 ⇌ Equilibrium Equation: AgNO3 + HCl ⇌ Equilibrium Equation: AgCl + NH3 ⇌ Equilibrium Equation: Ag(NH3)2+ + HNO3 + Cl- ⇌ Equilibrium Equation: AgCl + NH3 ⇌ Equilibrium Equation: Ag(NH3)2+ + Cl- + KI ⇌When the reversible reaction HC2H;O2 (aq) E> H(aq) + C2H3O2 (aq) is at equilibrium at room temperature, pH of the reaction mixture is 5. What will be the change in pH when you add a large amount of NaOH (aq) to the reaction mixture? a) pH will not change because NaOH is not a part of the reaction equation. b) pH will not change because acetic acid and NaOH form a buffer. c) pH will increase because NaOH will completely neutralize acetic acid. d) pH will decrease because NaOH will completely neutralize acetic acid. In the reversible reaction A (aq) + B(aq) E > C(aq), reactant A is very expensive. What are two ways to get it to react as fully as possible to form as much C as possible? a) remove C as it forms, and use an excess of A b) add another reactant that will form a precipitate with B c) remove C as it forms, and use an excess of B d) add another reactant that will form a precipitate with ACalculate the equilibrium constant for the following reaction: CH3COOH(aq) + F¯ (aq)=CH₂COO (aq) + HF (aq) Be sure your answer has the correct number of significant digits. Note: Reference the K of acids at 25 °C table for additional information. a x10 x S
- You are on one of Saturn's many moons and discover a substance, Y2O that undergoes autoionization just like water on Earth. Y2O + Y2O ⇌ Y3O+ + OY– Through a series of experiments, you determine the equilibrium constant (Keq) for this autoionization reaction at various temperatures. The value of Keq at 28.7ºC is 7.6 x 10-14. What is the pY of the pure substance at this temperature? Report your answer to the hundreths placeFor the reaction of hydrazine (N2H4) in water, H,NNH, (ag) + H20(1) = H,NNH,+(aq) + OH¯(@ag) K, is 3.0 x 10-. Calculate the concentrations of all species and the pH of a 1.6-M solution of hydrazine in water. [H,NNH,] =| %3D [H,NNH, !3! JOH |= %3D [H*]=[ ]M pH= %3DGiven the equilibrium reactions below and their equilibrium constants. H3O+ (aq) + A (aq) ⇒ HA(aq) + H₂O (1) Kc1 = 2.5 x 104 A™ + H₂O(1) OH- (aq) (aq) + HA(aq) 2.5 x 10-10 What is the value of Kc for the reaction 2 H₂O) H3O+ + OH (aq) (aq) 1.0 x 10¹4 6.3 x 10-6 1.0 x 10-14 none of the answers are correct Kc2 =
- A 0.050 M solution of the salt NaA has a pH of 9.00. Determine the [OH] and the pH of a 0.010 M solution of the acid HA. Show your work in the question parts below. Determine the equilibrium concentration of H3O* using the acid ionization equation. Recall that [OH] = 1.0 x 10-5. Consider the ionization equation described below.. HA(aq) + H20(1) =H;O*(aq) + A (aq) 1 Based on the given information, set up the ICE table in order to determine the unknown equilibrium concentration of all reactants and products. НА(ag) H20(1) H;O*(aq) А (ag) + Initial () Change () Equilibrium () 5 RESET 0.010 0.050 +x -2х +2x -x 0.010 + x 0.010 - x 0.050 + x 0.050 - x 0.010 + 2x 0.010 - 2x 0.050 + 2x 0.050 - 2x3. 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.The following reaction is in equilibrium: NO2- (aq) + H2O (l) = HNO2 (aq) + OH- (aq). Kb (NO2-) = 2.2 x 10-11. Which of the following statement is correct if we pump HCl (g) into the above solution? Note that the solution volume stays the same after HCl (g) is pumped into the above solution. Choose one option only. Options: a. The reaction will shift to right to re-establish equilibrium and the pH of the solution will decrease. b. There is no effect to pump HCl (g) into the solution. c. The reaction will shift to the left to re-establish equilibrium and the pH of the solution will increase. d. The reaction will shift to the right to re-establish equilibrium and the pH of the solution will increase. e. The reaction will shift to left to re-establish equilibrium and the pH of the solution will decrease.