Name______________________________________________________period______IB chemistry Ch. 8: acid/bases 1. What is the difference between the Arrhenius and the Bronsted-Lowry definition of an acid? Arrhenious acids give H+ in water Bronsted-Lowry acids are proton donors 2. NH3(g) and HCl(g) react to form the ionic solid NH4Cl(s). Which substance is the bronsted-Lowry acid in this reaction? Which is the Bronsted-Lowry base? Acid- HCl; base-NH3 3. What is the difference between the Arrhenius and the Bronsted-Lowry definition of a base? Arrhenius bases give OH- in water Bronsted-Lowry bases are proton acceptors 4. Give the conjugate base of the following a. H2SO3 b. HC2H3O2 c. H2AsO4d. NH4+ e. H2O 2HSO3 C2H3O2 HAsO4 NH3 OH5. Give the conjugate acid of the following a. C7H5O2b. BrO2c. NH3 d. H2AsO4e. CO32HC7H5O2 HBrO2 NH4+ H3AsO4 HCO36. Identify the Bronsted-Lowry acid and the Bronsted-Lowry base in each reaction and the conjugate acid/base pair a. NH4+ + CN- HCN + NH3 acid base conjugate base conjugate acid b. (CH3)3N + H2O (CH3)3NH+ + OHbase c. HCHO2 + acid acid conjugate acid conjugate base PO43- CHO2- + HPO42- base conjugate base conjugate acid 7. a. HC2O4- is amphoteric. Write a balanced equation showing how it acts as an acid toward water and another equation showing how it acts as a base toward water. HC2O4- + H2O H2C2O4 + OHHC2O4- + H2O C2O42-+ H3O+ b. What is the conjugate acid of HC2O4- ? What is the conjugate base? H2C2O4; C2O428. For each of the following reactions, identify the Lewis acid and the Lewis base a. 4NH3 + Zn2+ [Zn(NH3)4]2+ base acid b. 2Cl- + BeCl2 [BeCl4]2base acid c. Mg2+ + 6H2O [Mg(H2O)6]2+ acid base 9. Which of the following could not act as a ligand in a complex ion of a transition metal? a. Clb. NCl3 c. PCl3 d. CH4 10. Prepare a table in which you compare the definitions of acids and bases according to the Lewis, Bronsted-Lowry, and Arrhenius theories. Which is the most general; that is, which includes the others within its scope? Explain. acid bases + Arrhenius produces H in water produces OH- in water Bronsted-Lowry proton donor proton acceptor Lewis electron pair acceptor electron pair donor Lewis is the most general 11. What color is litmus in an acid? In a base? Red; blue 12. What color is phenolphthalein in an acid? In a base? Clear; pink 13. Write equations for the following reactions a. sulfuric acid + copper(II) oxide H2SO4 + CuO CuSO4 + H2O b. nitric acid + sodium hydrogen carbonate HNO3 + NaHCO3 NaNO3 + H2O + CO2 c. phosphoric acid + potassium hydroxide H3PO4 + 3KOH K3PO4 + 3H2O d. ethanoic acid + aluminum 6CH3COOH + 2Al 2Al(CH3OO)3 + 3H2 e. hydrochloric acid + calcium hydroxide 2HCl + Ca(OH)2 CaCl2 + 2H2O f. hydrobromic acid + magnesium carbonate 2HBr + MgCO3 MgBr2 + CO2 + H2O 14. What are some properties of acids? Taste sour, turns red in litmus 15. What are some properties of bases? Taste bitter, turns blue in litmus, slippery 16. Why are strong acids also strong electrolytes (strong conductors or electricity)? completely ionize in water so there are a lot of ions to conduct electricity 17. Name each of the following and label them as a weak/strong acid or weak/strong base a. H3PO4 b. Ca(OH)2 c. Al(OH)3 d. HNO3 e. NH3 f. LiOH a.Phosphoric acid, weak b.calcium hydroxide, strong base c. aluminum hydroxide, weak base d. nitric acid, strong e. ammonia, weak base f. lithium hydroxide, strong base 18. Which of the following solutions will be the poorest conductor of electricity? a. HCl b. CH3COOH c. NaOH d. NaCl 19. Which of the following has the highest concentration of [H+]? 0.1 mol dm-3 HCl or 0.1 mol dm-3 HF 20. What is the [H+] in each? a. 0.5 mol dm-3 HCl b. 0.002 mol dm-3 HNO3 -3 0.5 mol dm 0.002 mol dm-3 21. What is the [OH ] in each? b. 0.03 mol dm-3 Ca(OH)2 b. 0.5 mol dm-3 NaOH -3 0.5 mol dm 0.06 mol dm-3 22. What is the pH of a 0.0034 M HNO3 solution? 2.5 23. What is the hydrogen ion concentration of a solution with a pH of 5? Is it an acid or a base? 1 x 10-5 mol dm-3; acid 24. Which of the following solutions would have the lowest pH? 0.10 M HCl, 0.009 M HNO3, 0.340 M HBr 25. Determine the pH of the following solutions and label if they are acidic or basic a. [H+] = 1 x 10 -6 b. [OH-] = 1 x 10 -3 c. [H+] = 2.3 x 10 -3 d. [OH-] = 3.4 x 10 -6 6 ; acidic 11; basic 2.64; acidic 8.5; basic + 26. determine the [H ] for the following solution and label if they are acidic or basic a. [OH-] = 1 x 10 -8 b. [OH-] = 2.3 x 10 -6 c. pH = 2 -6 1 x 10 , acidic 4 x 10 -9 , basic 1 x 10 -2, acidic d. pOH = 5 e. pH = 3.4 f. pOH = 4.2 1 x 10 -9, basic 4.0 x 10 -4, acidic 1.6 x 10 -10, basic 27. Determine the pH of the following solutions (label if they are acidic or basic) b. [H+] = 2.3 x 10 -3 c. [OH-] = 1.0 x 10 -11 a. [H+] = 1.0 x 10 -12 12; basic 2.6; acidic 3; acidic d. [OH-] = 6.7 x 10 -8 6.8; acidic g. 1 x 10 -2 mol dm-3 NaOH 12;basic b. 0.001 mol dm-3 HI 3; acidic e. 1 x 10 -2 mol dm-3 HNO3 f. 3.98 x 10 -4 mol dm-3 HCl 2; acidic 3.4; acidic -2 -3 + h. 8.9 x 10 mol dm Ba(OH)2 i. [H ] = 1 x 10 -7 13.2; basic 7; neutral 28. Which of the solutions in the previous problem is the most acidic? Most basic? E; h 29. Which of the solutions in #27 has the highest hydronium ion concentration? Highest hydroxide ion concentration? E; h 30. Determine the [H+] for each of the following a. [OH-] = 2.3 x 10 -4 b. pOH = 3.11 c. pH = 9 -11 -11 4.34 x 10 M 1.29 x 10 M 1 x 10 -9 M -3 d. 0.0001 mol dm KOH e. pOH = 2 f. 0.003 mol dm-3 HBr -10 -12 1 x 10 M 1 x 10 M 0.003 M Review 31. Write a balanced reaction when magnesium metal reacts with hydrobromic acid Mg + 2HBr MgBr2 + H2 b. How many moles of each product are produced if 5.4 mol of magnesium react? 5.4 mol of magnesium bromide and 5.4 mol of hydrogen 32. a. Write a balanced reaction when nitric acid react with aluminum hydroxide 3HNO3 + Al(OH)3 3H2O + Al(NO3)3 b. How many grams of nitric acid are needed to react with 2.3 mol of aluminum hydroxide? 430 g 33. Tell the shape of each, tell if they are polar or nonpolar, tell what intermolecular forces hold them together, and tell which one would have the lowest boiling point. a. H2O Bent Polar Hydrogen bond and LD b. NH3 c. CH4 trigonal pyramidal tetrahedral polar nonpolar hydrogen bond and LD London dispersion CH4 has the lowest boiling point 34. What is the difference between and exothermic and endothermic reaction? Exothermic releases energy and feels warm; endothermic absorbs energy and feels cold 35. H2 + F2 <-> 2HF ΔH -538 kJ b. Will raising the temperature cause the amount of product to increase? no c. How will the equilibrium shift if hydrogen is added to the reaction? right d. How will the equilibrium shift if HF is removed from the reaction? right e. What will happen to the amount of hydrogen if the temperature is decreased? decreases f. Will the temperature of the surroundings increase or decrease as the reaction moves forward? increases 36. How many cm3 of 0.340 M HBr would be needed to titrate 14.91 cm3 of 0.265 mol dm-3 Mg(OH)2? 23.2 cm3 37. What is the concentration of sulfuric acid solution if 34.1 cm3 of it is needed to reach the endpoint when titrated with 14.3 cm3 of 0.876 mol dm-3 aluminum hydroxide? 0.551 mol dm-3
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