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- COHSOH(ag) + H2On + CeHsO (aq) + H3O*(a9) Ka= 1.12 x 10-10 (a) Phenol is a weak acid that partially dissociates in water according to the equation above. Write the equilibrium-constant expression for the dissociation of the acid in water. (b) What is the pH of a 0.75 M CaHsOH(ag) solution? (C) For a certain reaction involving CaHsOH(ag) to proceed at a significant rate, the phenol must be primarily in its deprotonated form, C3H5O (eg). In order to ensure that the CsHsOH(aq) is deprotonated, the reaction must be conducted in a buffered solution. On the number scale below, circle each pH for which more than 50 percent of the phenol molecules are in the deprotonated form (CoHsO (aq). Justify your answer. 1 2 3 4 5 6 7 8 9 10 11 12 13 14 Justification: (d) CeHsOH(ag) reacts with NaOH(ag). Write a net ionic equation representing this reaction (aka: invasion equation). (e) What is the pH of the resulting solution when 30 mL of 0.40 M CSH5OH(aq) is added to 25 mL of 0.60 M NAOH. Show all work…In which of the following does no reaction occur? K2CO3(aq) + Ca(NO3)2(aq) → HNO3(aq) + NaОНаq) - O Ni(s) + HC1(aq) → O Na,sO,(aq) + KOH(aq) →Which of the following reactions would occur to a measurable extent in water? Choose one or more: CIO (aq) + H₂O(1) →→→→→→ HCIO(aq) + OH¯ (aq) Br (aq) +H,O(l) →→→ HBr (aq) + OH¯¯ (aq) C104(aq) + H₂O(1) → HCIO (aq) + OH(aq) DNH(aq)+H,O(1) NH3 (aq) + H₂O¹ (aq) NO₂(aq) + H₂O(1) →→→→→ HNO₂ (aq) + OH¯(aq) Bro(aq) + H₂O(1) → HBrO (aq) + OH(aq) □K (aq) + 2H₂0 (1) →→KOH(aq) + H₂0¹ (aq) NO3 (aq) + H₂O(1) D_CT(aq)+H,O(1) OF (aq) +H₂O(1) → ->> HNO3(aq) + OH(aq) → HCl(aq) + OH(aq) → HF (aq) + OH (aq)
- Given the equilibrium reactions below and their equilibrium constants. H3O+ (aq) + A (aq) ⇒ HA(aq) + H₂O (1) Kc1 = 2.5 x 104 A™ + H₂O(1) OH- (aq) (aq) + HA(aq) 2.5 x 10-10 What is the value of Kc for the reaction 2 H₂O) H3O+ + OH (aq) (aq) 1.0 x 10¹4 6.3 x 10-6 1.0 x 10-14 none of the answers are correct Kc2 =Which of the following reactions is not product-favored? ONAOH(aq) → Na*(aq) + OH (aq) NH3(aq) + H2O() → NH4*(aq) + OH-(aq) HCIO4(aq) + H20() → H30*(aq) + CIO4-(aq) O HCI(aq) + H20() → H30*(aq) + CI-(aq) H2SO4(aq) + H20() → H3O*(aq) + HSO4-(aq)Calculate the K of A" given HA(aq) + H2O(l) = H₂O† (aq) + A¯¯(aq) K = 5.90×108
- A chemical system is set up by placing some solid ammonium chloride in an ammonia solution. The equilibrium established can be represented as follows: NH4*(aq) + H2O(e) 2 H30*(aq) + NH3(aq) The pH of the solution is taken, then a small amount of NaOH(aq) is added and the pH is taken again. What can be said about the change in pH for the solution? The pH significantly increases because a strong base has been added to the solution. The pH significantly decreases because a strong base has been added to the solution. There is very little change to the pH of the solution. If anything the pH of the solution decreases slightly. There is very little change to the pH of the solution. If anything the pH of the solution increases slightly.3 Co(s) + 2 NO 3- (aq) + 8 H+ (aq) = 3 Co 2+ (aq) + 2 NO (g) + 4 H2O (l) What would be the pH of the solution at standard conditions?( HINT: What are the concentrations of all aqueous species at standard conditions?)The balanced molecular equation for complete neutralization of H2SO4 by KOH in aqueous solution is: Group of answer choices 2H+ (aq) + 2OH- (aq) → 2H2O (l) H2SO4 (aq) + 2KOH (aq) → 2H2O (l) + K2SO4 (aq) H2SO4 (aq) + 2OH- (aq) → 2H2O (l) + SO42- (aq) H2SO4 (aq) + 2KOH (aq) → 2H2O (l) + K2SO4 (s) 2H+ (aq) + 2KOH (aq) → 2H2O (l) + 2K+ (aq)
- Calculate the equilibrium constant for the acid–base reaction between the reactants in each of the following pairs: (a) HCl + H2O (b) CH3COOH + H2O (c) CH3NH2 + H2O (d) CH3N+H3 + H2OWrite the equilibrium constant expression for this reaction: CH₂OH(aq) + Cl(aq) → CH₂Cl(aq)+OH (aq) X 8 ŚWhat is the correct equilibrium constant expression for the following reaction? NH3(aq) + H₂O(1) ⇒NH4*(aq) + OH¯(aq) O O (A) Ke (B) Kc (c) Ke (D) Kc (E) Kc - = = = [NH3] [H₂O] [NH4]+[OH]- [NH4+][OH-] [NH3] [NH4+] [OH [NH3] [H₂O] [NH3] [NH₂+] [OH-] 4 [NH₁+OH [NH3]