Identify the correct equation for the equilibrium constant K, for the weak acid dissociation of acetic acid. HC,H;O, (aq) + H,0 (1) H;0* (aq) + C,H;O,¯ (aq) Select one: [H,O*|[C,H,0, [HC2H;O2|[H2O] HC,H,O,] [H,O"|C,H,0, K. K. [HC,H;O2|[H2O) [H;O*|[CH,O2 K = O Ka = [H,O*][C,H,O, ] HC;H3O2]
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- A weak acid, HA, is a monoprotic acid. A solution that is 0.140 Min HA has a pH of 1.800 at 25°C. HA(aq) + H,0(1) 2 H;0"(aq) + A (aq) What is the acid-ionization constant, K, for this acid? What is the degree of ionization of the acid in this solution? Ka- Degree of ionization =The lactate ion, C, H,O, (aq), reacts with water to form lactic acid and hydroxide ion. C;H,05 (aq) + H, O(1) = HC,H;O;(aq) + OH (aq) In a 0.378 M solution of sodium lactate, the [OH¯] = 5.2 × 10-6 M. Use the ICE table to determine the concentrations of OH¯ and HC, H,O,. You will use these values to calculate the Kp for HC,H,O3. C;H;O5 (aq) + H,O(1) = HC,H;O,(aq) + ОН (аq) initial 0.378 change +x +x equilibrium 0.378 – x What is the value for x in these expressions? Hint: you are given this value in the problem. x = MThe value of K for acetylsalicylic acid (aspirin) is 3.00x104. What is the value of Kp, for its conjugate base, CH,04? An error has been detected in your answer. Check for typos, miscalculations etc. before submitting your answer.
- The 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 =The dissociation of acetic acid, CH3COOH, has an equilibrium constant at 25 degrees celsius of 1.8 x 10-5. CH3COOH(aq) ⇋ CH3COO-(aq) + H+(aq) If the equilibrium concentration of CH3COOH is 0.46 moles in 0.500 L of water and that of CH3COO is 8.1 x 10-3 moles in the same 0.500 L, calculate the concentration of H + for the reaction.The dissociation of the weak acid acetic acid (CH3COOH) is represented by the equation below. Enter the equation including all formatting and physical states in the answer blank. CH,COOH(ag) + H,0() – H,0*(aq) +CH,Coo"(aq) x | x. Me -. 8. (agi.
- Nitrogen is discharged from wastewater treatment facilities into rivers and streams, usually as NH₃ and NH₄⁺: NH₃(aq)+H₂O(l) → NH₄⁺(aq)+OH⁻(aq) K(b)=1.76X10⁻⁵ One strategy for removing it is to raise the pH and “strip” the NH₃ from solution by bubbling air through the water. (a) AtpH 7.00, what fraction of the total nitrogen in solution is NH3,defined as [NH₃]/([NH₃] [NH₄⁺])? (b) What is the fraction at pH 10.00? (c) Explain the basis of ammonia stripping.Determine the pH of a 0.74 M aqueous solution of hydrocyanic acid (HCN) and the concentration of all species in solution. The K, of hydrocyanic acid is 4.9 x 1010. HCN (aq) + H20 (1) CN (aq) + H3o* (aq) The pH of the solution is (Select] The concentration of HCN at equilibrium is (Select ] The concentration of CN' at equilibrium is (Select] The concentration of H30O* at equilbrium is (Select] The concentration of OH` at equilbrium is (Select] The pOH of the solution is [Select ]Given the two reactions 1. H2 S(aq) = HS (aq) + H†(aq), K1 = 9.15×10-8, and 2. HS (aq) = S²-(aq) + H+(aq), K2 = 1.39×10-19, what is the equilibrium constant Kfinal for the following reaction? s2- (аq) + 2H* (аq) = H2S(aq) Enter your answer numerically.
- Methanoic acid is also called formic acid. It has the chemical formula HCOOH(l). It is a colourless fuming liquid that is mainly used as a preservative. It exhibits the following equilibrium in water:HCOOH(aq) + H2O(l) → HCOO–(aq) + H3O+(aq) 4) The concentration of the hydroxide ion, OH-(aq), in an aqueous solution is 2.5 x 10–3 mol/L. What is the pH of the solution? PLEASE HELP THIS IS VERY URGENTThe value of K, for phenol (a weak acid) is 1.00×10-10. What is the value of Kp, for its conjugate base, C,H5O"?The value of K, for phenol (a weak acid), C,H3OH , is 1.00×1010. Write the equation for the reaction that goes with this equilibrium constant. (Use H30* instead of H".)