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Q: ********* H H H OH
A: Given,The molecule is:
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- Write the basic equilibrium equation for IO⁻. Be sure to include the proper phases for all species within the reaction.Consider the following acidic equilibrium: H₂CO₃(aq) + H₂O(l) ⇌ HCO₃⁻(aq) + H₃O⁺(aq). If you add NaHCO₃ to this solution, which of the following will occur? A) The reaction quotient will decrease. B) The reaction will shift in the reverse direction. C) The equilibrium constant will increase. D) No changes to the equilibrium positions will take place.Write the basic equilibrium equation for HS⁻. Be sure to include the proper phases for all species within the reaction.
- What is the concentration of H3O+ in a solution that is 0.0600 M Hypochlorous acid (HClO)? What is the pH? To solve this problem: Write the acid dissociation equilibrium for HClO Set up an ICE chart ( with x = the concentration of H3O+ at equilibrium) Write the expression for Ka. Fill this in with the concentrations of H3O+, ClO- and HClO at equilibrium, in terms of x. Decide if x can be neglected. You may neglect x if the initial concentration of the HClO is greater than 100 times the Ka. You will need the value of Ka. Look it up on the chart (p 4 of packet) Solve for x Find the pH The pH of a 0.0200 M solution of an unknown acid is 2.56. What is the Ka of this acid? To solve this problem: Write the acid dissociation equilibrium for the generic aicd “HA” Set up an ICE chart ( with x = the concentration of H3O+ at equilibrium) Write the expression for Ka. Fill this in with the concentrations of H3O+, A- and HA at equilibrium, in terms of x. What is x? Can you find it…Write the balanced reaction of carbonate ions accepting protons to form carbonic acid.Predict the position of equilibrium and calculate the equilibrium constant, Keq, for each acid-base reaction
- For the following reaction, the products are favored at equilibrium. Classify each of the reactants and products based on their strength as Bronsted-Lowry acids or bases. C3H10N4O2 + HCIO=HC3H1,N4O2* + CIO" Clear All Stronger Bronsted-Lowry acid HCIO Weaker Bronsted-Lowry HC3H1,N4O2* acid Stronger Bronsted-Lowry base C3H10N402 Weaker Bronsted-Lowry base CIOFormic 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. 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.What is standardization in acid-base chemistry? What constitutes a standard in analytical chemistry? Give types and examples.
- Calculate the hydrogen-ion concentration and the pH of a solution of 0.0001M H2CO3, and also calculate what fraction of the H2CO3 has been dissociated. Compare this fraction with the fraction dissociated when the concentration is 0.01M (given that the pH is 4.2 in a 0.01M solution). What generalization can you make regarding the effect of dilution on the degree of dissociation?Write the acidic equilibrium equation for HC₆H₅CO₂. Be sure to include the proper phases for all species within the reaction.12. Draw the general structures of a Brønsted acid and a Lewis acid.
