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when 0.05 mol of propionic acid (C2H5CO2H) is dissolved in 0.5L of water, proton transfer occurs:...
When 0.607 mol of CH3COCOOH is dissolved in 0.358 L of water, proton transfer occurs. CH3COCOOH + H2O ⇄CH3COCOO- + H3O+ The equilibrium concentration of H3O+ ions is 0.0640 M. Evaluate Keq. Chapter 14, Question 33 Parameterization When 0.607 mol of CH3COCOOH is dissolved in 0.358 L of water, proton transfer occurs. CH3COCOOH H20 CH3C0COO + H30+ The equilibrium concentration of H30+ ions is 0.0640 M. Evaluate Kea the tolerance is +/-2%
When 0.950 mol of HCOOH is dissolved in 0.891 L of water, proton transfer occurs. HCOOH + H2O ⇄HCOO- + H3O+ The equilibrium concentration of H3O+ ions is 0.0137 M. Evaluate Keq.
When 0.070 mol of propionic acid, C2H5CO2H, is dissolved in 450 mL of water, the equilibrium concentration of H3O+ ions is measured to be 2.19 x 10−3 M. What is Ka for this acid?
When 0.070 mol of propionic acid, C2H5CO2H, is dissolved in 300 mL of water, the equilibrium concentration of H3O+ ions is measured to be 2.01 x 10−3 M. What is Ka for this acid?
1) When 0.519 mol of HCOOH is dissolved in 0.409 L of water, proton transfer occurs. HCOOH + H2O ⇄HCOO- + H3O+ The equilibrium concentration of H3O+ ions is 0.0149 M. Evaluate Keq.
8) An acid (1.5pts) produces hydroxide ions when dissolved in water. donates protons in a proton transfer reaction. does none of the above. donates electrons in an electron transfer reaction. changes the color of phenolphthalein indicator from colorless to pink. 9) A base (1.5pts) produces hydrogen ions in solution. donates a proton in a proton transfer reaction. causes phenolphthalein indicator to change from colorless to pink. accepts electrons in an electron transfer reaction. does none of the above. 10) Which,...
Writing Proton-Transfer Equations for Acid-Base Reactions •PROBLEM: Write balanced total and net ionic equations for the following reactions and use curved arrows to show how the proton transfer occurs. –(a) hydriodic acid (aq) + calcium hydroxide (aq) → Give the name and formula of the salt present when the water evaporates. –(b) potassium hydroxide (aq) + propionic acid (aq) → Note that propionic acid is a weak acid. Be sure to identify the spectator ions in this reaction.
1. A certain amount if nitrous acid is dissolved in water at 25 celcius. At equilibrium, the pH of the solution is 2.33. What is the concentration of H3O+ and NO2-? 2. Calculate the valye if the equilibriym constant at 25 celcisus for the reaction: HNO2+OH- -> H2O + NO2-
1.0 mol of ethanol and 1.0 mol of acetic acid are dissolved in water and kept at 100? degrees C. The volume of the solution is 250 mL. At equilibrium, 0.25 mol of acetic acid has been consumed in producing ethyl acetate. Calculate Kc? at 100 degrees C for the reaction: C2H5OH?(aq) + CH3CO2H(aq) CH3CO2C2H5(aq) + H2O?(l)
4. When 0.100 mol ammonia is dissolved in water to make a 500 mL solution, the following equilibrium is established NH3(aq) + H2O(0) - NH. (aq) + OH(aq) K = 1.8 x 10-5 a. Find the concentration of OH' and the pH of the solution at equilibrium. Remember: pOH = -log(OH) and pH + pOH = 14 b. Consider the following reaction: 2H2O(1) 2 H,0*(aq) + OH(aq) K = 1.0 x 10-14 Write the equilibrium expression and find the value...