Period: Unit 8: Acids/Bases/Salts Addt'l Practice

Transcription

1 Unit 8: Acids/Bases/Salts Addt'l Practice Period: 1. A student tested a 0.1 M aqueous solution and made the following observations: conducts electricity -7^e cwo ^ turns blue litmus to red ^ c ^ f reacts with Zn(s) to produce gas bubbles ' ^ Which compound could be the solute in this solution? 6. According to the Arrhenius theory, a base reacts with an acid to produce cj^ t "1 K ( 1~1 1) ammonia and methane 2) ammonia and a salt 3) water and methane /4)^ater and a salt 1) CH3OH CvlceK^I (^)HBT o,ci <J 2) LiBr Voti^jt ^^^^ ^ 2. Which two compounds are electrolytes? \- ^ '^rsehuoe and CH3CH20lf^--cxV coko I 1) 2kC6Hi206 and HCl ^^M^aOH and HCl 4) NaOH and CH3CH2OH 3. As water is added to a 0.10 M NaCl aqueous solution, the conductivity of the resulting solution 1) decreases because the concentration of ions decreases 2) decreases, but the concentration of ions remains the same 3) increases because the concentration of ions decreases 4) increases, but the concentration of ions remains the same 7. When dissolved in water, an Arrhenius base yields 1) hydrogen ions (^^^ hydroxide ions / ^ 2) hydronium ions 4) oxide ions V t +^t>lt H are HNOfCaq) and CH3)S00H(aq} similar? 1) l^hey are Arrhenius acids and they turn blue litmus red. 2) They are Arrhenius acids and they turn red litmus blue. 3) They are Arrhenius bases and they turn blue litmus red. 4) They are Arrhenius bases and they turn red litmus blue. 9. According to the Arrhenius theory of acids, citric acid in oranges and acetic acid in vinegar are classified as ^ds because their aqueous solutions contain jliydrogen ions( 4'^ ^ 3) hydroxide ions (^OV\ 2) hydrogen atoms 4) hydroxide atoms ^c) ^ 4. What can be explained by the Arrhenius theory? ^^^he behavior of many acids and bases 2) the effect of stress on a phase equilibrium 3) the operation of an electrochemical cell 4) the spontaneous decay of some nuclei 54 Which compounds are classified as Arrhenius acids? 1) HCl and NaOH 3) NH3 and H2CO3 2) JIN03 and Na^l^^^^B^ and H2SO4 10. Which statement correctly describes a solution with aph of 9? 1) It has a higher concentration of H3O+ than OH" and causes litmus to turn blue. It has a higher concentration of OH" than H3O+ and causes litmus to turn blue. 3) It has a higher concentration of H3O+ than OH" and causes methyl orange to turn yellow. 4) It has a higher concentration of OH" than H30^ and causes methyl orange to turn red.

2 10/\ 11. Which ph change represents a hundredfold increase in the concentration of H3O+? 1) ph5toph7 2) ph BtopH 14 yppu 3 to ph 1 4) ph 4 to ph Red litmus will turn blue when placed in an aqueous solution of 1) KCl 3) CH3OH alcokdl ^^r^oh lo*^^^ 4) CH3COOH aciji 12. Which statement describes the characteristics of an Arrhenius base? 1) It changes blue litmus to red and has a ph less than 7. 2) It changes blue litmus to red and has a ph greater than 7. 3) It changes red litmus to blue and has a ph less lan 7. 4) It) changes red litmus to blue and has a ph greater than Given the reaction: H3,0Haq) +X-<aq), ac4^ 1 Based on the equation, HXwould be classified as 1) a base, because it donates a proton 2) a base, because it accepts a proton r^j}^ acid, because it donates a proton 4) an acid, because it accepts a proton 13. Given the following solutions: Solution.4: ph of 10 Solution B: ph of 7 Solution C: ph of 5 Which list has the solutions placed in order of increasing H+ concentration? \B, C 2) B, A, C 3) C, A, B 4) C B, A 14. Which indicator is blue in a solution that has a ph of romcresol green 3) methyl orange 2) bromthymol blue 4) thymol blue 18. Given the equation:, NH3(g) + H20( ) <-> NH4^(aq) + OHiaq) W \ \ The two acids, acting as proton donors are 1) NH3 and H2O (^^20 and NH4^ 2) NH3 and NH4+ 4) H2O and OH- 19. In the reaction: qda I 1 h^^^ fss + NH3<->NH4+ + HS- The two species that are considered bases are 1) NH3 andnh4+ C^^f^m and HS- 3) H2SandNH3 4) H2S and HS- 15. In which 0.01 M solution is phenolphthalein pink? avc o h) CH30H(aq) 3) CH3C00H(aq) ad^ bc$,^ ^^(0H)2(aq) 4) HN03(aq) ^^^-j^ 20. According to an alternative theory, an acid is any s^ies that can / Cil>^o"^te a proton 3) accept a proton 2) donate an electron 4) accept an electron

3 V 21. Which equation illustrates the amphiprotic properties of a reactant species? 1) NH2(aq) + UiOii) ^ NH4^(aq) + OH-(aq) C^^^iOii) + UiOii) H30+(aq) + OH-(aq) 3) HCl(aq) + HiOH) -> H30+(aq) + Cl-(aq) 4) 2H2(g) + 02(g) -> 2H20(^) 22. Which process is used to deterrnine^e rrninelhe ^ i concentration of an acid? ^ cl ^ 1) chromatography 2) distillation Jl^lectrolysis (^^tration Oh 23. Which volume of 0.10 M NaOH(aq) exactly neutrahzes 15.0 milliliters of 0.20 M HN03(aq)? 1) 1.5 ml 2) TJjnL. 3) 3.0 ml ^^>^0. u. ml mi.. / ^.10 GO',(oC;0) 24. How many milhliters of 2.5 M HCl are required to exactly neutralize 15 milliliters of 5.0 M NaOH? 1) 10. 2) 20. /5^30. 4) Which solution wilfbe e"5cactly neutralized by 1.0 liter of 1.OM NaOH? Ha H '^ 1) 1.0 liter of 0.50M HCl 2.^61 2) 1.0 liter of 2.0M HCl 2%^^^ 3) 0.50 liter of 0.50M HCl ' 1 /yxlil/^-^^ ^i*^^ of 2.0M HCl 26. A 16-milliliter sample of 0.50 M KOH will completely neutralize 32 milliliters of 1) 1.OMHNO3 2) 0.75 M HNO M HNO3 \0.25MHNO3 27. When HCl(aq) is exactly neutralized by NaOH(aq), the hydrogen ion concentration in the resulting mixture is ' ti^l 1) always less than the concentration of the hydroxide ions 2) always greater than the concentration of the ^ hydroxide ions (^^JJ^ways equal to the concentration of the hydroxide ions 4) sometimes greater and sometimes less than the concentration of the hydroxide ions 28. Sulfuric acid, H2S04(aq), can be used to neutralize barium hydroxide, Ba(0H)2(aq). What is the formula for the salt produced by this neutralization? 1) BaS 3) BaS03 2) BaS02 ^^^^as Which reactants form the salt CaS04(s) in a neutralization reaction? 1) H2S(g) and Ca(C104)2(s) 2) H2S03(aq) and Ca(N03)2(aq) 3l)H2S04(aq) and Ca(0H)2(aq) 4) S02(g) and CaO(s) 30. Which compound could serve as a reactant in a neutralization reaction?. ac I NaCl^-S^^^ ^ ^(->vud \ ^OH^boSe 3) CH3OH ' 4) CH3CHO 31. Which equation represents a neutralization reaction? 1) Na2C03 + CaCb ^ 2 NaCl + CaC03 2) Ni(N03)2 + H2S NiS + 2 HNO3 3) NaCl + AgN03 -> AgCl + NaN03 y<?rh2s04 + Mg(0H)2 -^MgS H2O a

4 Base your answers to questions 32 and 33 on the passage below. Acid rain is a problem in industrialized countries around the world. Oxides of sulfur and nitrogen are formed when various fuels are burned. These oxides dissolve in atmospheric water droplets that fall to earth as acid rain or acid snow. While normal rain has a ph between 5.0 and 6.0 due to the presence of dissolved carbon dioxide, acid rain often has a ph of 4.0 or lower. This level of acidity can damage trees and plants, leach minerals from the soil, and cause the death of aquatic animals and plants. If the ph of the soil is too low, then quicklime, CaO, can be added to the soil to increase the ph. Quicklime produces calcium hydroxide when it dissolves in water. 32. Samples of acid rain are brought to a laboratory for analysis. Several titrations are performed and it is ^ determined that a 20.0-milliliter sample of acid rain is4ieutrj;^ized with 6.50 milliliters of M NaOHTWhaMs the molarity of the ions in the acid rain?- 34. A student recorded the following buret readings during a titration of a base with an acid: Standard M HCl Unknown KOH Initial reading 9.08 ml 0.55 ml Final reading ml 5.56 ml a/calcuwe the molarity of the KOH. Show all work. Recom>your answer to the correctnumber of jigftiftcant figures. 0. oo(\o,o(^^x/'s-^a H A 33. A sample of wet soil has a ph of 4.0. After the. addition of quicklime, the H"^ ion concentration of of the original H"^ ion concentration of the soil. ai]\is the new ph of the soil sample? 10^ ' 1 lovlio 2 ow C ^anp^

5 /\n semp was usea to aetermme the unknown molar concentration of a solution of NaOH. A 1.2 M HCl solution was used as the titration standard. The following data were collected. Trial 1 Trial 2 Trial 3 Trial 4 Amount of HCl Standard Used Initial NaOH Buret Reading Final NaOH Buret Reading 10.0 ml 10.0 ml 10.0 ml 10.0 ml 0.0 ml 12.2 ml 23.2 ml 35.2 ml 12.2 ml 23.2 ml 35.2 ml 47.7 ml Explain why it is better to use the average data from multiple trials rather than the data from a single trial to calculate the results of the titration.