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- What is the basis for referring to the hydrogen ion as a proton? (a) The Arrhenius definition of an acid. (b) The Brønsted-Lowry definition of an acid x (c) The Lewis definition of an acid. (d) H* exists as a bare proton. (e) None of these.Determine the pH of a 0.100 M solution of (NH4)2C2O4.The compound methylamine is a weak base like ammonia. A solution contains 0.199 M CH;NH3* and 0.117 M methylamine, CH3NH2. The pH of this solution is
- 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…calculate the pH of the following solution; (a)2.8 × 10–⁴M Ba (OH)2 (b) 5.2 × 10–⁴M HNO3·Predict whether aqueous solutions of the following substances are acidic, basic, or neutral and write hydrolysis equations for the acidic and basic solutions. (a) CsBr; (b) Al(NO3)3; (c) KCN; (d) CH3NH3Cl
- Ammonia, NH3, is amphoteric. (a) Give the formula for the conjugate acid of NH3. (b) Give the formula for the conjugate base of NH3.Carbon dioxide dissolves in water according to the equations:CO2( g) + H2O(l )<----->H2CO3(aq)H2CO3(aq) + H2O(l)<----->HCO3-(aq) + H3O+(aq)Carbon dioxide levels in the atmosphere have increased about 20% over the last century. Given that Earth’s oceans are exposed to atmospheric carbon dioxide, what effect might the increased CO2 be having on the pH of the world’s oceans? What effect might this change be having on the limestone structures (primarily CaCO3) of coral reefs and marine shells?24. A solution of volume 0.500 L contains 1.68 g NH3 and 4.05 g (NH4)2SO4. (a) What is the pH of this solution? (b) If 0.88 g NaOH is added to the solution, what will be the pH? (c) How many milliliters of 12 M HCl must be added to 0.500 L of the original solution to change its pH to 9.00?
