Quiz 1 - F05 Quiz 1 . September 8,2005 \ . I ‘ _ Name:...

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Unformatted text preview: F05 Quiz 1 . September 8,2005 \ . I ‘ _ Name: eID ,zU is air ‘ 1. The most important buffering system for maintaining proper blood pH is: S WW ; the charges on the surface of red blood cells he bicarbonate buffer system of C02, carbonic acid, and bicarbonate LL ' phosphate groups of serum phosphoproteins _ (My M. WLM~= «3 D) none of the above E) all of the above p ‘ firm] 1% m i ‘ a)»: QM“? My 2. Which of the following statements is true? }L A) Buffers work best when the pH is within 3 units of the pK. \zB) Buffers can be prepared using the Henderson—Hasselbalch equation. be) A buffer requires a combination of a weak acid and its conjugate base. A and B B and C 3. How many hydrogen bonds can a water molecule potentially take part in forming? A) one % B) two three four 9;. {3 . 20: E) none of the above 4. Rank the following in terms of strength, from greatest to lowest: a covalent bonds, hydrogen bonds, ionic interactions ovalent bonds, ionic interactions, hydrogen bonds C) ionic interactions, covalent bonds, hydrogen bonds D) hydrogen bonds, covalent bonds, ionic interactions E) none ofthe above —- ~ ' an”. mm.» A / _. 5. What is the final pH when iomeL of 0.1 M Hci'iEEEidéd to 909 mL ofwater? Q4 L) r" 2.0 L” ) 2.5 D) 3.0 E) 3.5 F) 7.0 G) none of the above "(J 1 --~-- --—~—w~—-«—-_i.,.._._..m......._w.__.---——-... 1...; “PM "Wham ,_ _ y 1h. 1 «loadiwdfi " 2.0 6. In a neutral aqueous solution the concentrations of H“ and OH' are each: A 55M 1x104M 1 IXIO'MM D) 5 mM E) none of the above 7. How does the hydrophobic effect influence the structures of large molecules? was.) nonpolar molecules are not easily solubilized in water and aggregate L43) polar groups are oriented on the surface, interacting with the water nonpolar molecules can mask the polar characteristics of the hydrophilic molecules AandB Version 1 Page 1 You want to prepare 1L of 0.1 M phosphate buffer at pH 7.8 Recall: H3PO4 <——-> H+ + H2PO4’<—-—> H+ + HPOd-Z Answer the following questions (hint: read all questions before answering!) 8. The relevant pKa for making this buffer is: n: 2.5 .s C) 12.5 D) none of the above h “A 9. The correct equation to determine the relative amounts of HP04'2 and H2PO4‘ to get to pH 7.8 is: A) 6.8: 7.8 + log [H2PO4']/[HP04'2] B) 6.8= 7.8 + log [HPO4‘2]/[H2PO4'] C 7.8: 6.8 + log [H2P04-]/[HPO4-z] _ h M! ,. @732 6.8 + log [HPO4'Z]/[H2PO4‘] "-2 Pkg)”. ‘7 none of the above ii A 10. The correct ratio of dissociated and undissociated for this pH is A) 2! l B) 3/1 - . -, Wang C) 1/1 ‘ . e T ‘53 whgw 3 to 5 i an“ 255/1“ \0 l i 0% M» mt'qvacmt.» IO m J, r ~ . m 1, my Kw I Mr W Cd Version 1 Page 2 F05 Quiz 1 September 8, 2005 Name: BID 2.- 1. In a neutral aqueous solution the concentrations of H+ and OH‘ are each: ; 55M @ x10'7M 1x10'”M D) 5 mM E) none of the above 2. How many hydrogen bonds can a water molecule potentially take part in forming? A) one B) two C three our E) none of the above 3. What is the final pH when 100 mL of 0.1 M HCl is added to 900 mL of water? - 1.5 .0 " 2.5 D) 3.0 E) 3.5 F) 7.0 G) none of the above 4. Which of the following statements is true? A) Buffers work best when the pH is within 3 units of the pK. VB) Buffers can be prepared using the Henderson—Hasselbalch equation. VC) A buffer requires a combination of a weak acid and its conjugate base. AandB B andC 5. The most important buffering system for maintaining proper blood pH is: L- the charges on the surface of red blood cells the bicarbonate buffer system of C02, carbonic acid, and bicarbonate phosphate groups of serum phosphoproteins D) none of the above E) all of the above 6. How does the hydrophobic effect influence the structures of large molecules? \/A) nonpolar molecules are not easily solubilized in water and aggregate VB) polar groups are oriented on the surface, interacting with the water C nonpolar molecules can mask the polar characteristics of the hydrophilic molecules A and B E) A and C 7. Rank the following in terms of strength, from greatest to lowest: covalent bonds, hydrogen bonds, ionic interactions ' \@ covalent bonds, ionic interactions, hydrogen bonds ionic interactions, covalent bonds, hydrogen bonds D) hydrogen bonds, covalent bonds, ionic interactions E) none of the above Version 2 Page 1 \JCF U-J uu U1..qu You want to prepare 1L of 0.1 M phosphate buffer at pH 7.8 Recall: I'IJPO4 <---> H+ + H2POA' <---> HJr + HPO-t'2 Answer the following questions (hint: read all questions before answering!) 8. The correct equation to determine the relative amounts of HPOr'2 and H2P04’ to get to pH 7.8 is: A) 6.8= 7.8 + log [H2P04‘]/[HP04'1] B) 6.8: 7.8 + log [HP04'2]/[H2PO4‘] C) 7.8= 6.8 + log [HzPOA']/[HPO4‘2] ® 7.3: 6.8 + log [HPO4’2].’[H2P04‘] none of the above 9. The correct ratio of dissociated and undissoeiated for this pH is A) 27'] B) 3/1 C) III D 5/1 éfitoi t 10. The relevant pKa for making this buffer is: 2.5 3 I 12.5 D) none of the above Version 2 Page 2 F05 Quiz 1 September 8, 2005 Name: eID 1. How does the hydrophobic effect influence the structures of large mo ules‘? \flgr) nonpolar molecules are not easily solubilized in water and aggregate VB) polar groups are oriented on the surface, interacting with the water C nonpolar molecules can mask the polar characteristics of the hydrophilic molecules A and B — A and C 2. In a neutral aqueous solution the concentrations of H+ and OH' are each: _.r.. 55M 6) 1 x 10‘7M I 1x 10"4M D) 5 mM E) none of the above 3. How many hydrogen bonds can a water molecule potentially take part in forming? A) one B) two C) three our none of the above 4. Rank the following in terms of strength, from greatest to lowest: g; covalent bonds, hydrogen bonds, ionic interactions ovalent bonds, ionic interactions, hydrogen bonds ionic interactions, covalent bonds, hydrogen bonds D) hydrogen bonds, covalent bonds, ionic interactions E) none of the above 5. What is the final pH when 100 mL of 0.1 M HCl is added to 900 mL of water? A 1.5 2.0 2.5 D) 3.0 E) 3.5 F) 7.0 G) none of the above 6. Which of the following statements is true? A) Buffers work best when the pH is within 3 units of the pK. VB) Buffers can be prepared using the HendersomHasselbalch equation. us?) A buffer requires a combination of a weak acid and its conjugate base. D A and B B and C 7. The most important buffering system for maintaining proper blood pH is: @the charges on the surface of red blood cells B the bicarbonate buffer system of C02, carbonic acid, and bicarbonate phosphate groups of serum phosphoproteins D) none of the above E) all of the above Version 3 Page 1 dc!” U-J U-J UL-uJLlU You want to prepare 1L of 0.1 M phosphate buffer at pH 7.8 Recall: H3P04 <---> H”r + H2P04'<---> H+ + HPOA‘2 Answer the following questions (hint: read all questions before answering!) 8. The relevant pKa for making this buffer is: 2.5 .s 12.5 D) none of the above 9. The correct equation to determine the relative amounts of HPOa‘2 and H2PO4' to get to pH 7.8 is: A) 6.8= 7.8 + log [H2PO4‘ ]/[HPO4-2] B) 6.8= 7.8 + log [HPO4'2]![H2PO4'] C 7.8= 6.8 + log [H2PO4‘]/[HPO4'2] @728: 6.8 + log [HPO4'2]/[H2PO4'] none of the above 10. The correct ratio of dissociated and undissociated for this pH is A) 2/1 B) 3/1 C) 1/1 D) 5!] 5mm Version 3 Page 2 F05 Quiz 1 September 8, 2005 Name: BID 1. How many hydrogen bonds can a water molecule potentially take part in forming? A) one B) two three four none of the above 2. What is the final pH when 100 mL of 0.1 M HCl is added to 900 ml. of water? 1.5 .0 2.5 D) 3.0 E) 3.5 F) 7.0 G) none of the above 3. The most important buffering system for maintaining proper blood pH is: ' the charges on the surface of red blood cells ' I e bicarbonate buffer system of C02, carbonic acid, and bicarbonate " phosphate groups of serum phosphoproteins D) none of the above E) all of the above 4. H w does the hydrophobic effect influence the structures of large molecules? X nonpolar molecules are not easily solubilized in water and aggregate LB) polar groups are oriented on the surface, interacting with the water nonpolar molecules can mask the polar characteristics of the hydrophilic molecules ( A and B ) A and C 5. Which of the following statements is true? )(A) Buffers work best when the pH is within 3 units of the pK. t/B) Buffers can be prepared using the Henderson—Hasselbalch equation. l)3) A buffer requires a combination of a weak acid and its conjugate base. AandB BandC 6. Rank the following in terms of strength, from greatest to lowest: covalent bonds, hydrogen bonds, ionic interactions covalent bonds, ionic interactions, hydrogen bonds C) ionic interactions, covalent bonds, hydrogen bonds D) hydrogen bonds, covalent bonds, ionic interactions E) none of the above 7. In a neutIal aqueous solution the concentrations of H+ and OH‘ are each: a 55 M x10‘7M C lx 10'14M D) 5 mM E) none of the above Version 4 Page 1 dc.” U-J U-J UL-uJ-JIU You want to prepare 1L of 0.1 M phosphate buffer at pH 7.8 Recall: H3P04 <—--> H+ + HQPOA‘ <---> H+ + HPOA'2 Answer the following questions (hint: read all questions before answering!) 8. The correct equation to determine the relative amounts of HP04'2 and H2P04' to get to pH 7.8 is: A) 6.8= 7.8 + log [H2P04']/[HPOa‘2] B) 6.8= 7.8 + log [HPO4'2]/[H2PO4'] 7.8: 6.3 + log [H2P04']/[HPO4‘2] 7.8= 6.8 + log [HPO4'2]/[H2P0.a‘] none of the above 9. The correct ratio of dissociated and undissociated for this pH is A) 2/1 E) 3/1 C) 1/1 D) 5/1 a») to i I 10. The relevant pKa for making this buffer is: A) 2.5 CW3 C 12.5 D) none of the above Version 4 Page 2 \JC'l-F UQJ UoJ ULQQJQJI‘I' F05 Quiz 1 September 8, 2005 Name: eID 1. Which of the following statements is true? Buffers work best when the pH is within 3 units of the pK. Buffers can be prepared using the Henderson—Hasselbalch equation. A buffer requires a combination of a weak acid and its conjugate base. A and B B and C 2. How does the hydrophobic effect influence the structures of large molecules? nonpolar molecules are not easily solubilized in water and aggregate B polar groups are oriented on the surface, interacting with the water 5 nonpolar molecules can mask the polar characteristics of the hydrophilic molecules A and B E) A and c 3. In a neutral aqueous solution the concentrations of H’ and OH' are each: A) 55 M 1x10‘7M ) 1x10’l4M D) SmM E) none of the above 4. How many hydrogen bonds can a water molecule potentially take part in forming? A) one B) two _ _ three ‘ A four " ' none of the above 5. The most important buffering system for maintaining proper blood pH is: the charges on the surface of red blood cells C? the bicarbonate buffer system of C02, carbonic acid, and bicarbonate phosphate groups of serum phosphoproteins D) none of the above E) all of the above 6. What is the final pH when 100 mL of 0.1 M HCl is added to 900 mL of water? a, 1.5 C) 2.5 D) 3.0 E) 3.5 F) 7.0 G) none of the above 7. Rank the following in terms of strength, from greatest to lowest: A covalent bonds, hydrogen bonds, ionic interactions @covalent bonds, ionic interactions, hydrogen bonds C) ionic interactions, covalent bonds, hydrogen bonds D) hydrogen bonds, covalent bonds, ionic interactions E) none of the above Version 5 Page 1 \JCI‘I’ UQJ U|J ULQQJQJI‘I' I”. 1U You want to prepare 1L of 0.1 M phosphate buffer at pH 7.8 Recall: H3P04 <---> H+ + H2P04'<---> H+ + HPO4'2 Answer the following questions (hint: read all questions before answering!) 8. The relevant pKa for making this buffer is: A 2.5 .8 ) 12.5 D) none of the above 9. The correct equation to determine the relative amounts of HPO4'2 and H2PO4' to get to pH 7.8 is: A) 6.8: 7.8 + log [H2P04']/[HPO4'2] B) 6.8: 7.8 + log [HPO4'2]i[H2PO4'] . .8= 6.8 + log [H2PO4']/[HPO4‘3] .8= 6.8 + log [HPO4‘2]/[H2_PO4‘] '7 ' none of the above 10. The correct ratio of dissociated and undissociated for this pH is A) 2/1 B) 3/1 C) 1/1 Version 5 Page 2 ...
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This note was uploaded on 12/30/2010 for the course CH 369 taught by Professor Kbrowning during the Spring '07 term at University of Texas at Austin.

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Quiz 1 - F05 Quiz 1 . September 8,2005 \ . I ‘ _ Name:...

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