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Would this reaction have more products or reactants at equilibrium?
H2PO4- + NH3 ⇌ NH4+ + HPO42-
7.2 36 9.8 12.3 - (pka)
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- Lactic acid, CH3CH(OH)COOH, is a weak monoprotic acid with a melting point of 53 C. It exists as two enantiomers (Sec. 7-2f) that have slightly different Ka values. The D form has a Ka of 1.5 104 and the L form has a Ka of 1.6 104. The D form is synthesized by some bacteria. The L form is produced in muscle cells during anaerobic metabolism in which glucose molecules are broken down into lactic acid and molecules of adenosine triphosphate (ATP) are formed. When lactic acid builds up too rapidly in muscle tissue, severe pain results. (a) Which form of lactic acid (D or L) is the stronger acid? Explain your answer. (b) Determine the pKa that would be measured for a 50:50 mixture of the two forms of lactic acid in aqueous solution, pKa = log Ka (c) A solution of D-lactic acid is prepared. Use HL as a general formula for lactic acid, and write the equation for the ionization of lactic acid in water. (d) If 0.100-M solutions of these two acids (D and L) were prepared, calculate what the pH of each solution would be. (e) Before any lactic acid dissolves in the water, what reaction determines the pH? (f) Calculate the pH of a solution made by dissolving 4.46 g D-lactic acid in 500. mL of water. (g) Calculate the volume (mL) of 1.15-M NaOH(aq) required to completely neutralize 4.46 g of pure lactic acid. (h) Calculate the pH of the solution when exactly enough NaOH was added to neutralize all of the lactic acid for (i) the D form; (ii) the L form; and (iii) a 50:50 mixture of the two forms.Draw an energy diagram for a reaction with keq = 1. What is the value of ∆G° in this reaction?Use pKa values to predict which of the following equilibria will favor the reactants. B C O + OH₂ + SH Br NH₂ Multiple answers: Multiple answers are accepted for this question H OH + LOH Yo HBr e NH
- 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 0.084G GR Carbonic anhydrase, an enzyme that converts carbon dioxide and water to carbonic acid as shown below, functions in the blood at an optimum pH of 7.0-7.5. Which of the following will lower the rate of carbonic anhydrase-catalyzed reaction? Carbonic anhydrase CO2+H2O Houdy O running the reaction at 4 °C O adding more carbonic anhydrase O increasing the concentration of carbon dioxide O carrying out the reaction at pH 7.2 Search ma omiWhich of the following equilibrium equations have the smallest equilibrium constant? a) CH₂CH₂O`Na + -OH 0 CHOON b) (CH3)₂CHCO Na + H₂O c) NaOH + -OH CI d) More information is needed
- What are the concentrations of OH-(aq), (CH3)2NH2+(aq), and (CH3)2NH in a 0.450M solution of dimethylamine? Kb = 7.40 x 10-4 (CH3)2NH + H2O ↔ (CH3)2NH2+ + OH I 0.450 0 0 C -x +x +x E 0.450 - xGiven the reactionsHF(aq) ⇌ H+(aq) + F-(aq) Kc = 6.9 x 10-4H2C2O4(aq) ⇌ 2 H+(aq) + C2O42 - (aq) Kc = 3.8x 10-6 Determine the value of Kc for the reaction2 HF(aq) + C2O42 - (aq) ⇌ 2 F-(aq) + H2C2O4(aq)Oxacarbazepine ( C15H12N2O) is used to treat epilepsy. What would happen to the equilibrium of oxacarbazepine in water when more oxacarbazepine is added to the system? a.) Ratef < Rateb and the equilibrium would shift to reactants (to the left) b.) Ratef > Rateb and the equilibrium would shift to reactants (to the left) c.) Ratef < Rateb and the equilibrium would shift to products (to the right) d.) Ratef > Rateb and the equilibrium would shift to products (to the right)
- The Keq for the reaction: A + B <--> AB is 3.013 What is the Keq for 3 + AB <--> 3 A + 3 BThe following reactions all have K > 1.1) HF (aq) + C6H5O- (aq) F- (aq) + C6H5OH (aq)2) CH3COOH (aq) + C6H5O- (aq) C6H5OH (aq) + CH3COO- (aq)3) HF (aq) + CH3COO- (aq) F- (aq) + CH3COOH (aq)Arrange the substances based on their relative acid strength. Strongest acid, intermediate acid, weak acid, not a Bronsted-Lowry acid. CH3COOH HF C6H5OH CH3COO- F- C6H5O-Co(H2O)6+2 +2 + 4 Cl- <----> CoCl4-2 + 6 H2O Based on the above equation, explain where the equilibrium shifted when the following reagents were added: H2O HCl AgNO3