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1 FIRST LETTER OF YOUR LAST NAME CHEMISTRY 118 EXAM II March 8, 014 Name Section Signature TA ID # PLEASE READ THE FOLLOWING INSTRUCTIONS Do NOT begin the exam until asked to do so. There are 8 numbered pages including a table of equilibrium constants for weak acids and their conjugate bases, a periodic table and equations page in this exam. Check to see that they are all here before you begin the exam. Return all these papers when you are finished. Write your name on every page. Use a pen with blue or black ink for the entire exam. Exams done in pencil, erasable ink, or where whiteout, liquid paper, etc. have been used are ineligible for regrades. Be sure to follow all directions. In working any numerical problem, you MUST SHOW ALL YOUR WORK. No credit will be given unless all work is clearly shown and the method of solution is logically correct. Pay attention to units and significant figures throughout. Do not write below this line Page Total Grader 1 / 6 / 18 3 / 10 4 / 1 5 / 3 6 / 14 7 / 7 8 / 0 Tot al Grade /150 Checked by
2 Chem 118, EXAM II March 8, 014 I. (54 points) A. (10 points) Consider the following six beakers. All have 100 ml of aqueous 0.1 M solutions of the following compounds. Beaker A has HI Beaker B has HNO Beaker C has NaOH Beaker D has Ba(OH) Beaker E NH 4 Cl Beaker F C H 5 NH Answer the questions below, using LT (for is less than), GT (for is greater than), EQ (for is equal to), or MI (for more information required) 1. The ph of beaker B the ph in beaker A.. The ph in beaker C the ph in beaker D. 3. The ph in beaker C the ph in beaker F. 4. The ph in beaker B the ph in beaker E. 5. Percent ionization in beaker A the % ionization in beaker C. B. (8 points) What is the ph of a solution obtained by diluting 15.0 ml of M solution of Sr(OH) to 85 ml of solution? C. (8 points) A 4.90 x 10 3 mol sample of a weak acid HY is dissolved in enough water. To form L of solution. If the ph of the solution is.65, what is K a for the weak acid? 1
3 Chem 118, EXAM II March 8, 014 D. (10 points) Ascorbic acid (HC 6 H 7 O 6, MM g/mol) is also known as vitamin C, and it is a weak acid. A solution of ascorbic acid is prepared by dissolving.00 g in enough water to make ml solution. If the K a of ascorbic acid is 7.6 x 10 5 calculate the following 1. The concentration of [H + ] in solution. The ph of the solution. E. (8 points) State whether a 1 M solution of the following salts in water will be acidic, basic, or neutral. 1. K 3 PO 4. NH 4 HCO 3 3. NaClO 4 4. LiH PO 4
4 Chem 118, EXAM II March 8, 014 F. (10 points) Thiamine hydrochloride (C 1 H 18 ON 4 SCl ) (MM g/mol) is a water soluble form of thiamine. Its acid dissociation constant is 3.37 X A solution of thiamine hydrochloride has a ph of How many grams of thiamine hydrochloride are needed in a ml solution to give the same ph? 3
5 Chem 118, EXAM II March 8, 014 II. (49 points) A. (1 points) Answer questions 1 4 below, using LT (for is less than), GT (for is greater than), EQ (for is equal to), or MI (for more information required) Beaker A has a weak acid (K a 1 x 10 5 ) Beaker B has HCl The volume and molarity of each acid in the beakers are the same. Both acids are to be titrated with a 0.1 M solutions of NaOH. 1. Before the titration starts, the ph of the solution is Beaker A is the ph of the solution in beaker B.. At half neutralization (halfway to the equivalence point), the ph of the solution in Beaker A the ph of the solution in beaker B. 3. When each solution has reached the equivalence point, the ph of the solution in Beaker A the ph of the solution in Beaker B. 4. At the equivalence point, the volume of NaOH used to titrate HCl in Beaker B the volume of NaOH used to titrate the weak acid in beaker A. Place your answer on the line provided. 5. A buffer may be prepared from a weak acid. Which of the acids below is best for the preparation of a buffer with a ph of 4.00? (A) sulfurous acid, H SO 3 ; K a 1.7 x 10 (B) hydrofluoric acid, HF; K a 6.9 x 10 4 (C) benzoic acid, HC 7 H 5 O ; K a 6.6 x 10 5 (D) dihydrogen phosphate ion, H PO 4 ; K a 6. x 10 8 (E) ammonium ion, NH 4 + ; K a 5.6 x All of the following statements are false for the titration of a strong base by a strong acid EXCEPT (A) the equivalence point occurs at ph 7. (B) there will be at least two equivalence points, one for the base and one for the acid. (C) the equivalence point and the end point are identical, regardless of what indicator is used. (D) equal masses of acid and base are required to neutralize the solution. (E) it is impossible to neutralize a strong acid with a strong base. 4
6 Chem 118, EXAM II March 8, 014 B. (8 points) If added to ml of 0.43 M HOCl, which of these would form a buffer? On the line provided write YES or NO mol NaOCl mol HNO mol KOH mol KOH C. (15 points) A buffer solution is prepared by dissolving g of sodium benzoate (NaC 7 H 5 O, MM ) in 45 ml of 0.49 M HC 7 H 5 O. Assume not volume change after NaC 7 H 5 O is dissolved. K a of HC 7 H 5 O 6.6 x Calculate the ph of this buffer.. Calculate the ph of the solution after moles HCl is added to this buffer. Assume no volume change. 5
7 Chem 118, EXAM II March 8, 014 D. (14 points) A 5.0 ml solution of lactic acid, HC 3 H 5 O 3, is titrated with ml of M Ba(OH). K a of lactic acid is 1.38 x Write a balanced net ionic equation. What are the species present at the equivalence point? 3. What is the molarity of the initial lactic solution? 4. What is the ph of the solution at the equivalence point? 6
8 Chem 118, EXAM II March 8, 014 III. (47 points) A. (8 points) Predict whether the forward or reverse reaction or no change will occur when the equilibrium is disturbed by PbCl (s) Pb + (aq) + Cl (aq) 1. addition of 1 M Pb(NO 3 ) solution. increase in temperature. 3. addition of Ag +, forming AgCl. 4. Addition of 1 M HCl. ΔH 3.4 kj B. (8 points) The solubility of an ionic compound M Y 3 is 3.6 x 10 7 g/l. What is the solubility product constant, K sp, for this compound? (MM of M Y g/mol) C. (6 points) What is the solubility of solid Ca 3 (PO 4 ) (K sp 1.3 x 10 3 ) in a 0.0 M Na 3 PO 4 solution. D. (5 points) A solution containing potassium bromide is mixed with a solution containing lead acetate to form a solution that is M in KBr and M in Pb(C H 3 O ). Will a precipitate form? K sp for PbBr is 4.0 x (SHOW YOUR CALCULATION) 7
9 Chem 118, EXAM II March 8, 014 E. (8 points) Consider the following equation: Cu(OH) (s) + 4NH 3 (aq) Cu(NH 3 ) + 4 (aq) + OH (aq) K sp for Cu(OH) x and K f for Cu(NH 3 ) 4 x What is the equilibrium constant, K, for the reaction given above?. What is [NH 3 ] at equilibrium when 1.68 g of copper(ii) hydroxide ( g/mol) are dissolved in ml of solution? F. (1 points) Solid Na CrO 4 is slowly added to a solution that is M in Pb + and M Ag +. K sp of PbCrO 4.0 x K sp of Ag CrO x Which compound will begin to precipitate first? Determine the concentration of CrO 4 to precipitate each cation? [CrO 4 ] to ppt Ag CrO 4 [CrO 4 ] to ppt PbCrO 4. What percentage of first cation precipitated when the second cation starts to precipitate? 8
10 Chem 118, EXAM II March 8, 014 Equilibrium Constants for Weak Acids and Their Conjugate Bases Acid K a Base K b Sulfurous acid H SO x 10 HSO x Hydrogen sulfate ion HSO x 10 SO x 10 1 Phosphoric acid H 3 PO x 10 3 H PO x 10 1 Hexaaquairon(III) ion Fe(H O) x 10 3 [Fe(H O) 5 OH] x 10 1 Hydrofluoric acid HF 6.9 x 10 4 F 1.4 x Nitrous acid HNO 6.0 x 10 4 NO Formic acid HCHO 1.9 x 10 4 CHO Lactic acid HC 3 H 5 O x 10 4 C 3 H 5 O 3 Benzoic acid HC 7 H 5 O 6.6 x 10 5 C 7 H 5 O Acetic acid HC H 3 O 1.8 x 10 5 C H 3 O 1.7 x x x x x Hexaaquaaluminum (III) ion Al(H O) x 10 5 [Al(H O) 5 OH] x Carbonic acid H CO x 10 7 HCO 3.3 x 10 8 Dihydrogen phosphate ion H PO 4 Hydrogen sulfite ion HSO 3 6. x 10 8 HPO x 10 8 SO x x 10 7 Hypochlorous acid HClO.8 x 10 8 ClO 3.6 x 10 7 Hydrocyanic acid HCN 5.8 x CN 1.7 x 10 5 Ammonium ion NH 4 + Tetraaquazinc (II) ion Zn(H O) x NH x x [Zn(H O) 3 OH] x 10 5 Hydrogen carbonate ion HCO 3 Hydrogen phosphate ion HPO x CO PO x x 10 9
11 mass moles molar mass u PA PV 3RT MM X A nrt 1 / PTOT mass m density TK t o + 73 C volume V rate A rate B 3RT E t N A 760 mm Hg MM MM 1 / B A 1 atm R R time time A B MM MM 8.31 J / mol L.atm 1 / A B K / mol.k hc 8 E υ λ c E hν c m / s λ h J s 3 18 N particles / mol R J H 1 E RH nlo 1 n hi En R H n Z C f X Y + q mc Τ q C Τ c H O 4.18J/ g C P H vap 1 1 P H ln OR vap T T1 P H ln OR vap 1 1 ln P1 R T1 T P1 R T1T P1 R T T1 T k m i T k m i b b f f k b π i M R T (H O) 0.5 C / m (H O) 1.86 C / m ln E a 1 1 k lnk1 R T1 T OR k Ea 1 1 ln k1 R T1 T k f ln H 1 1 K lnk1 R T1 T OR K H 1 1 ln K1 R T1 T [A] 0 [ A] 0 [A] kt t1 / k [A] ln kt t1 / [A] k kt t 1/ y mx + b [A] [A] k[a] 0 K w 1.0 x K a x K b 1.0 x [HB] nhb [ H ] K a K a [B ] n 0 B x 1, b± b 4ac a
12 Periodic Table of the Elements H He Li Be B C N O F Ne Na.99 1 Mg Al Si P S Cl Ar K Ca Sc Ti V Cr Mn Fe Co Ni Cu Zn Ga Ge As Se Br Kr Rb Sr Y Zr Nb Mo Tc (98) 44 Ru Rh Pd Ag Cd In Sn Sb Te I Xe Cs Ba Lu Hf Ta W Re Os Ir Pt Au Hg Tl Pb Bi Po (10) 85 At (10) 86 Rn (0) 87 Fr (3) 88 Ra Lr (6) 104 Rf (61) 105 Db (6) 106 Sg (66) 107 Bh (64) 108 Hs (77) 109 Mt (68) 110 Ds (81) 111 Rg (7) 11 Cp (85) 114 ( ) 116 ( ) 118 ( ) 57 La Ce Pr Nd Pm (145) 6 Sm Eu Gd Tb Dy Ho Er Tm Yb Ac Th Pa U Np Pu (44) 95 Am (43) 96 Cm (47) 97 Bk (47) 98 Cf (51) 99 Es (5) 100 Fm (57) 101 Md (56) 10 No (59)
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