exam 2 key - Chem t3 See-tater zeta Exam 2 Name _ . I Show...

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Unformatted text preview: Chem t3 See-tater zeta Exam 2 Name _ . I Show your work (“it indicates no work showa m no credit} and indicate your results here and on Scanner}. Question t Identify the conjugate base of HPO42‘ in the reaction H003" + HPO42‘ =-_-r*'-—~« H2C03 + PO43" A) H20 B) H003" . C) H2003 ..__.;@Po:- E) None of these. _ Question 2* Calculate the H+ ion concentration in a 8.8 x ‘10“!1 M Ca(OH)2 solution. 2mm CG—(Otii "7' 352* 90” H mm it #7 22 WOW M ‘ _______.>®5.7x10"”M ZHUflQfi-j ._—,. /p*’4 4., 20”” .. LQ—fl XhHZ‘ fill7éwflfj Qoestion 3* Calculate the pH of a 0.10 M HCN solution that is 0.0070% ionized. A100 .-===- 4' F 3; 0.00070 H C n} “"1" H +C/U j, c 3.15 4' #— M545 719m : £5.3- x/oo 4‘" 7:0 X09 1" E) 7.00 D [New]; 4L V '5 0290-4, 3&4] Questioe a Diet cola drinks have a pH of about 3.0, while milk has a pH of about 7.0. How many times greater is the H30+ concentration in diet cola than in milk? A) 2.3 times higher in diet cola than in milk B) 400 times higher in diet cola than in milk C) 0.43 times higher in diet cola than in milk D 1,000 times higher in diet cola than in milk 0.000 times higher in diet cola than in milk Question 5 Which solution will have the lowest pH? A) 0.10 M HCN __.——9® 0.10 M HNO3 C) 0.10 M NaCl D) 0.10 M H2C03 I E) 0.10 M NaOH Question 6 Acid strength decreases in the series Hi > HSO4‘ > HF > HCN. Which of these anions is the weakest base? [APE r _ B) sof C) F— D) CN" Questteo 7 Arrange the acids HOCI. HCIOg, and HCIOZ in order of increasing acid strength. A HOCI < Holo3 < Holo2 HOCI < HCIo2 < HCl03 ' C) I—ICIo2 < HOCl < HCl03 0) H003 < HOCI < I—ICIo2 E) HCl03< HCio2 < HOCI Question 3 Predict the direction in which the equilibrium will lie for the reaction H2003 + F" “wfi H003“ + HF. Ka1( H2003) = 4.2 x 10—7; K3(HF) = 7.1 x 10"” A) to the right We the left - C) in the middle D) none of the above Question 9“" Calculate the pH of a 0.021 M NaCN solution. [K3(HCN) = 4.9 x 10-10] I 0 ~ "i A)1.68 C01; 0"“ C + H- Q =3 w... B) 3.13 A) H; 7 H M a b 79TH) “9 C) 5.49 ._ 0 _. K x I! .. (a 4 o : “W _____._..—- 10.82 . 1L 2 i Y .5— -.-.-.. 2 D MD '5- /— ML. 'v . (0 021-40 A 0492‘ 2 ‘(QWDJ “I .. I ¥ .1: - ‘3— D Q‘Vg ....,_ ‘ Kr - . Qaestion i9 - )5 é fl 0 L] *=- Which of the following solutions can not act as a buffer? (homework problem 16.10) A) KCN/HCN B) N32804IN3HSO4 C NH3/NH4N03 Nal/HI Qoesiion ii In which one of the following solutions will acetic acid have the greatest percent ionization? _..,—>.@0.1 M CH3COOH B) 0.1 M CH3COOH dissolved in 1.0 M HCl C) 0.1 M CH3COOH plus 0.1 M CH3COONa D) 0.1 M CH3COOH plus 0.2 M CH3COONa Question if“ Calculate the pH of a buffer solution that contains 025 M benzoic acid (C6H5C02H) and 0.15M sodium benzoate (C6H5C00Na). [Kat = 6.5 x 10‘5 for benzoic acid] -—-——- P Ra .__.. 1L B) 4.33 (I'M? C) 4.19 D) 3.40 _. _ ( “:- as? Quostion “£3 What is the net ionic equation for the reaction that occurs when small amounts of hydrochloric acid are added to a HOCl/NaOCl buffer solution? A) 11* + H20 —> H3o+ N H+ + ocr ——> HOCl C) HOCl —> H+ + 001"" D) H+ + ECO] o'HZOCF E) HCl + HOCI —> H20 + c12 Question M Acid dissociation constants for phosphoric acid are given below. A buffer with a pH = 7.4 can best be made by using A) H3P04 and N3H2P04. [fl NaH2P04 and NaZHPOr C) N32HPO4 and N33PO4. D) only NEH2P04. E) only N32HPO4_ Question i5 The pH at the equivalence point of a titration may differ from 7.0 due to A) the initial concentration of the standard solution. B) the indicator used. C) the self-ionization of H20. D) the initial pH of the unknown. figfilydrolysis of the salt fonned. Question t5* Calculate the concentration of fluoride ions in a saturated barium fluoride (KSP = 1.7 x 10—6) solution. *2 ..- A) 7.6 x10'3M :7 X F a @15 X10_2 M Ea E £30, +1 C) 3.4 x 10:: M 5‘ 2 5 D) 1.7 X 10 M 2 E) 3.4 X 10*3 M [(59 : jefi'zjgj Question i? What is the pH at the equivalence point in the titration of 100 mL of 0.10 M HCl with 0.10 M NaOH? A) 1.0 B; 6.0 D) 3.0 E) 13.0 Question 18* The solubility product for chromiumflll) fluoride is K313 = 6.6 X 10"“. What is the molar solubility of chromiumflll) fluoride? fl + A)1.6><10‘3M CrBEC‘ 5*3F aghll ><10'3 M C) 2.2 ><10_3 M 0 5 33 D)1.6><1045M t .. 3 E) 6.6x10““M : ng-Jc-ajzi: :i P ' ‘I’ :: 3(3553 5' 3'75 .4) 6 1% ‘f (5.? : MLQWD : (9‘41; {(0 Question t9”? 5' L75- moi-3 Will a precipitate of magnesium fluoride [KSp = 6.9 x 10—9] form when 200. mL of 1.9 x 10“3 M _2 ur- _MgC12 are added to 300. mL of1.4>< 10 MNa: E- 1; Sea”? 2 F e I 3 V1 a _. J _. :72 ‘7‘?K10*3M *4’ 3?”:5632: 2: a J 0 C) g'Q : '7 éK/0 M C)NO:Q=KSD I D < "' I ' '- fl Egggqufléj. [F 1.. o 39 r mm» /‘1 .,_ c5 4. no N (9.52 ' & :[H3*37[F02 :(‘Zé-ZC/OF 5'3; #0“? > Kl}; If “ Question 26* Find the concentration of calcium ions in a solution made by adding 3.50 g of calcium fluoride to _ —11 __ ‘ 750.mLof0.125MNaF. [For CaF2,KSp—3.95 x 10 .] F is Commmk I0“ A)3.16><10"10M C =:. C: +2 F” aging >< 10"”9M F; '7' *2 C)4.29><10‘4M 5 0 0 0125'" D) 6.32 x10_10M Zr +5 +25 E) 2.15 x104M r—-—- M n 6 (0 12€+25) k5? $31.95* ’0 = S'Eo lag-+25): asstkm: O \25‘ :- 25 "It: 0J2? :1 5 0.12 9' a - ’74 -- 5m“) g -:- Q 537:“? I” " Qaesttoa 2'? {extra credit) The pH of a 0.30 M solution of a weak base is 10.66. What is the Kb of the base? ? '5‘- miéé ...
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exam 2 key - Chem t3 See-tater zeta Exam 2 Name _ . I Show...

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