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Write the dissociation expression for the Ka of H2AsO4-.
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H3AsO4 + H2O ⇌ H3O+ + H2AsO4- |
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H2AsO4- + H2O ⇌ OH- + H3AsO4 |
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H2AsO4- + H2O ⇌ H3O+ + HAsO4-2 |
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HAsO4-2 + H2O ⇌ OH- + H2AsO4- |
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HAsO4-2 + H2O ⇌ H3O+ + AsO4-3 |
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- Formic acid dissociates reversibly according to the following equation. [ /20] HCOOH(aq) ⇌ HCOO-(aq) + H+(aq) Write the law of mass action for this equilibrium.K = Is the equilibrium constant in (a) a Ka? Briefly explain. If a solution is initially 0.20 mol/L HCOOH and the equilibrium constant in (a) is 1.8 × 10-4, what is the concentration of hydrogen ions at equilibrium? Show your work. Use the value obtained in (c) to find the solution’s pH and pOH at 25 °C. If you were unable to complete (c), you may assume a 0.0030 mol/L concentration of hydrogen ions. Would the addition of sodium formate (NaHCOO) to this solution increase pH? Explain.H3PO4 is a triprotic acid with the following acid dissociation constants: H3PO4 ⇌ H2PO4- + H+ Ka1 = 1.2 × 10-4 H2PO4- ⇌ HPO42- + H+ Ka2 = 4.3 × 10-9 HPO42- ⇌ PO43- + H+ Ka3 = 7.2 × 10-12 What is K for the following equilibrium: PO43- + 3H+ ⇌ H3PO4Write the equilibrium-constant expressions and obtain numerical values for each constant in the basic dissociation of aniline, C6H5NH2. the acidic dissociation of hypochlorous acid, HClO.
- What is the acid dissociation constant (Ka) expression for the following reaction? CH3COOH+H2O=CH3COO-+H3OFormic acid dissociates reversibly according to the following equation. HCOOH(aq) ⇌ HCOO-(aq) + H+(aq) Write the law of mass action for this equilibrium.K = Is the equilibrium constant in (a) a Ka? Briefly explain. If a solution is initially 0.20 mol/L HCOOH and the equilibrium constant in (a) is 1.8 × 10-4, what is the concentration of hydrogen ions at equilibrium? Show your work. sub parts to be solved Use the value obtained in (c) to find the solution’s pH and pOH at 25 °C. If you were unable to complete (c), you may assume a 0.0030 mol/L concentration of hydrogen ions. Would the addition of sodium formate (NaHCOO) to this solution increase pH? Explain.Formic acid dissociates reversibly according to the following equation. HCOOH(aq) ⇌ HCOO-(aq) + H+(aq) Write the law of mass action for this equilibrium.K = Is the equilibrium constant in (a) a Ka? Briefly explain. If a solution is initially 0.20 mol/L HCOOH and the equilibrium constant in (a) is 1.8 × 10-4, what is the concentration of hydrogen ions at equilibrium? Show your work. question 4, 5 need to be solved 4.Use the value obtained in (c) to find the solution’s pH and pOH at 25 °C. If you were unable to complete (c), you may assume a 0.0030 mol/L concentration of hydrogen ions. 5.Would the addition of sodium formate (NaHCOO) to this solution increase pH? Explain.
- Formic acid dissociates reversibly according to the following equation. HCOOH(aq) ⇌ HCOO-(aq) + H+(aq) Write the law of mass action for this equilibrium.K = Is the equilibrium constant in (a) a Ka? Briefly explain. If a solution is initially 0.20 mol/L HCOOH and the equilibrium constant in (a) is 1.8 × 10-4, what is the concentration of hydrogen ions at equilibrium? Show your work. 4.Use the value obtained in (c) to find the solution’s pH and pOH at 25 °C. If you were unable to complete (c), you may assume a 0.0030 mol/L concentration of hydrogen ions. 5.Would the addition of sodium formate (NaHCOO) to this solution increase pH? Explain.Formic acid dissociates reversibly according to the following equation. HCOOH(aq) ⇌ HCOO-(aq) + H+(aq) Write the law of mass action for this equilibrium.K = Is the equilibrium constant in (a) a Ka? Briefly explain. If a solution is initially 0.20 mol/L HCOOH and the equilibrium constant in (a) is 1.8 × 10-4, what is the concentration of hydrogen ions at equilibrium? Show your work.GivenKa of HClO = 2.9×10-8Kb of ClO- = 3.4×10-7Determine the value of K forHClO(aq) + H2O(ℓ) ⇌ H3O+(aq) + ClO-(aq) 3.4×10-7 2.9×10-8 3.4×107 2.9×106 0.084
- Write the equilibrium-constant expressions and obtain numerical values for each constant in the acidic dissociation of methyl ammonium hydrochloride, CH3NH3Cl. the dissociation of H3AsO3 to H3O+ and AsO33-Write equilibrium-constant expressions for each of the following: A) the base dissociation of ethyl-amine, CH3CH2NH2. B) the acid dissociation of hydrogen cyanide, HCN. C) the dissociation of H3AsO4 to H3O^+ and AsO4^3-. D) the reaction of CO3^2- with H2O to give H2CO3 and OH^-.For the following reaction, K< 1. Classify each of the reactants and products based on their strength as Bronsted-Lowry acids or bases. C18H21O3N + C,H;OH=C,H;0" + C18H21O3NH* Clear All C18H2103NH* Stronger Bronsted-Lowry acid Weaker Bronsted-Lowry C,H;O¯ acid C18H21O3N Stronger Bronsted-Lowry base Weaker Bronsted-Lowry C,H;OH base