Acid Bases Practice Test

Transcription

1 Name Acid Bases Practice Test Date 1. Which compounds are both classified as electrolytes? 1) NH4Cl and KCl 2) C6H12O6 and CH3OH 3) NH4Cl and C6H12O6 4) KCl and CH3OH 2. Which of the following 0.1 M solutions is the best conductor of electricity? 1) H2S(aq) 2) HCl(aq) 3) C6H12O6(aq) 4) C12H22O11(aq) 3. Given the reaction: NH3 + HCl NH4Cl In this reaction ammonia molecules (NH3) act as a base because they 1) accept hydrogen ions (H + ) 2) accept hydroxide ions (OH ) 3) donate hydrogen ions (H + ) 4) donate hydroxide ions (OH ) 4. Which compounds are classified as Arrhenius acids? 1) 2) 3) 4) 5. According to the Arrhenius theory, when a base is dissolved in water it produces a solution containing only one kind of negative ion. What is the name of this negative ion? 1) hydrogen carbonate ion 2) hydrogen sulfate ion 3) hydride ion 4) hydroxide ion 6. Which substance is an Arrhenius acid? 1) NH3 2) KOH 3) HC2H3O2 4) CH3OH 7. An aqueous solution of lithium hydroxide contains hydroxide ions as the only negative ion in the solution. Lithium hydroxide is classified as an 1) aldehyde 2) alcohol 3) Arrhenius acid 4) Arrhenius base 8. Which 0.1 M solution has a ph greater than 7? 1) C6H12O6 2) CH3COOH 3) KCl 4) KOH 9. Which 0.1 M solution contains the highest concentration of OH ions? 1) H2SO4 2) NH4Cl 3) KNO3 4) NaOH 10. Which ph indicates the highest concentration of H3O + ions? 1) 1 2) 7 3) 10 4) Which indicator would best distinguish between a solution with a ph of 3.5 and a solution with a ph of 5.5 1) bromthymol blue 2) bromcresol green 3) litmus 4) thymol blue 12. Which particle in a water solution of NaOH causes red litmus to turn blue? 1) Na + 2) H3O + 3) OH 4) H2O Page 1

2 13. What color is phenolphthalein in a basic solution? 1) blue 2) pink 3) yellow 4) colorless 14. The table below was compiled from experimental laboratory data. At what ph would all three indicators appear as yellow? 1) 1.9 2) 2.9 3) 4.7 4) In which solution will thymol blue indicator appear blue? 1) 0.1 M CH3COOH 2) 0.1 M KOH 3) 0.1 M HCl 4) 0.1 M H2SO4 16. Which compounds yield hydrogen ions as the only positive ions in an aqueous solution? 1) 2) 3) 4) 17. Given reactions A and B: (A) HCl + H2O Cl + H3O + (B) HCl + HS Cl + H2S In which of the reactions does HCl donate a proton and thus act as an acid? 1) A, only 2) B, only 3) both A and B 4) neither A nor B 18. In the reaction: NH2 + HOH NH3 + OH The two acids are 1) HOH and NH2 2) HOH and NH3 3) OH and HOH 4) OH and NH3 19. One acid-base theory defines a base as an 1) H + donor 2) H + acceptor 3) H donor 4) H acceptor 20. If HCl and H2O react together, in an acid-base reaction to form their Brönsted-Lowry conjugates, the products would be 1) HCl and H3O + 2) Cl and OH 3) Cl2 and H2 4) Cl and H3O + Page 2

3 21. In the reaction: H2O + H2O «H3O + + OH The water is 1) a proton donor, only 2) a proton acceptor, only 3) both a proton donor and a proton acceptor 4) neither a proton donor nor a proton acceptor 22. What is a conjugate acid-base pair in the reaction? H2O + HI «H3O + + I 1) H2O and HI + 2) H2O and I 3) HI and I 4) HI and HO What is the conjugate base of OH? 1) H2O 2) O 2 3) H3O + 4) H Which compound could serve as a reactant in a neutralization reaction? 1) NaCl 2) KOH 3) CH3OH 4) CH3CHO 25. An aqueous solution of an ionic compound turns red litmus blue, conducts electricity, and reacts with an acid to form a salt and water This compound could be 1) HCl 2) NaI 3) KNO3 4) LiOH 26. Which reaction occurs when equivalent quantities of H + (or H3O + ) and OH are mixed? 1) oxidation 2) reduction 3) hydrolysis 4) neutralization 27. What is the name of the salt produced by the reaction of calium hydroxide with sulfuric acid? 1) calcium thiosulfate 2) calcium sulfate 3) calcium sulfide 4) calcium sulfite 28. Which equation represents a neutralization reaction? 1) Na2CO3 + CaCl2 2 NaCl + CaCO3 2) Ni(NO3)2 + H2S NiS + 2 HNO3 3) NaCl + AgNO3 AgCl + NaNO3 4) H2SO4 + Mg(OH)2 MgSO4 + 2 H2O 29. Which element reacts spontaneously with 1.0 M HCl(aq) at room temperature? 1) copper 2) gold 3) silver 4) zinc 30. Given the balanced equation representing a reaction: H2SO4(aq) + 2KOH(aq) K2SO4(aq) + 2H2O( ) Which type of reaction is represented by this equation? 1) decomposition 2) neutralization 3) single replacement 4) synthesis 31. What are the products of a reaction between KOH(aq) and HCl(aq)? 1) H2 and KClO 2) H2O and KCl 3) KH and HClO 4) KOH and HCl Page 3

4 32. Base your answer to the following question on the information below. The diagram below shows typical ph values found in four parts of the human digestive system. In the small intestine, the enzyme lipase acts as a catalyst, increasing the rate of fat digestion. What is the color of thymol blue at the ph of the small intestine? 33. Base your answer to the following question 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. A sample of wet soil has a ph of 4.0. After the addition of quicklime, the H + ion concentration of the soil is of the original H + ion concentration of the soil. What is the new ph of the soil sample? 34. What is the ph of a solution that results from the complete neutralization of an HCl solution with a KOH solution? 1) 1 2) 7 3) 10 4) 4 Page 4

5 35. Which solution reacts with LiOH(aq) to produce a salt and water? 1) KCl(aq) 2) CaO(aq) 3) NaOH(aq) 4) H2SO4(aq) 36. If 50. milliliters of a 1.0 M NaOH solution is needed to exactly neutralize 10. milliliters of an HCl solution, the molarity of the HCl solution is 1) 1.0 M 2) 0.20 M 3) 5.0 M 4) 10. M 37. How many milliliters of M NaOH(aq) would be needed to completely neutralize 50.0 milliliters of M HCl(aq)? 1) 16.7 ml 2) 50.0 ml 3) 150. ml 4) 300. ml 38. A student completes a titration by adding 12.0 milliliters of NaOH(aq) of unknown concentration to 16.0 milliliters of 0.15 M HCl(aq). What is the molar concentration of the NaOH(aq)? 1) 0.11 M 2) 0.20 M 3) 1.1 M 4) 5.0 M 39. Information related to a titration experiment is given in the balanced equation and table below Based on the equation and the titration results, what is the concentration of the? 1) 2) 3) 4) 40. If 20. milliliters of 2.0 M KOH is exactly neutralized by 10. milliliters of HCl, the molarity of the HCl is 1) 1.0 M 2) 2.0 M 3) 3.0 M 4) 4.0 M 41. Base your answer to the following question on the information below. Some carbonated beverages are made by forcing carbon dioxide gas into a beverage solution. When a bottle of one kind of carbonated beverage is first opened, the beverage has a ph value of 3. State, in terms of the ph scale, why this beverage is classified as acidic. 42. A student recorded the following buret readings during a titration of a base with an acid: a Calculate the molarity of the KOH. Show all work. b Record your answer to the correct number of significant figures. Page 5

6 43. Base your answer to the following question on the information below and on your knowledge of chemistry. The gastric juice of the human stomach has a ph value of approximately 1.5. Hydrochloric acid in the gastric juice is necessary for the digestion process. However, excess hydrochloric acid may harm the stomach lining. One type of antacid uses to neutralize excess hydrochloric acid in the stomach. This neutralization is represented by the incomplete equation below. Describe the changes in both the hydrogen ion concentration and the ph of the gastric juice of a human after ingesting this type of antacid. Page 6

7 Answer Key Acids and bases practice yellow The beverage is acidic because its ph value is below 7. A ph of 3 is in the acid range on the ph scale. 42. a Example: V = Final - Initial Reading MAVA = MB VB b Hydrogen ion concentration: decreases/lower ph: Increases/higher Page 7