2. What volume of each of the following acids will react completely with ml of M NaOH? 1mol H + 1mol OH!
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1 Name Section Worksheet 5: Reactions in Solution Acid/Base and Redox 1. How many ml of a M NaOH solution is needed to neutralize ml of a M HCl solution? Molecular Rxn: HCl (aq) + NaOH (aq) NaCl (aq) + H 2 O (l) Net Ionic Rxn: H + (aq) + OH - (aq) H 2 O (l) 0.600mol HCl moles H + = L 1mol H + 1mol HCl = mol H + 1mol OH 1mol NaOH moles OH = mol H + " " = mol NaOH 1mol H + 1mol OH volume NaOH = mol NaOH volume NaOH = L NaOH 1000mL 0.800mol NaOH = L NaOH solution = 30.0mL NaOH solution 2. What volume of each of the following acids will react completely with ml of M NaOH? 0.100mol NaOH 1mol OH 1mol OH moles OH = L solution " " " = mol OH solution 1mol H + 1mol NaOH a M HCl moles H + = mol OH " 1mol H + 1mol HCl " 1mol OH 1mol H + volume HCl = mol HCl 0.100mol HCl = mol HCl = L HCl solution b M H 2 SO 3 (two acidic hydrogens) moles H + = mol OH " 1mol H + 1mol OH " 1mol H 2SO 3 = mol H 2mol H + 2 SO 3 volume H 2 SO 3 = mol H 2 SO mol H 2 SO = L H 2SO 3 solution 3 Page 1 of 7
2 c M PO 4 (three acidic hydrogens) moles H + = mol OH " 1mol H + 1mol OH " 1mol PO 4 3mol H + = mol PO 4 volume PO 4 = mol PO mol PO 4 = L PO 4 solution d M HNO 3 moles H + = mol OH " 1mol H + 1mol OH " 1mol HNO 3 = mol HNO 1mol H + 3 volume HNO 3 = mol HNO mol HNO = L HNO solution 3 3 e M HC 2 O 2 (one acidic hydrogen) moles H + = mol OH " 1mol H + 1mol OH " 1mol HC 2 O 2 1mol H + = mol HC 2 O 2 volume HC 2 O 2 = mol HC 2 O mol HC 2 O 2 = L HC 2 O 2 solution f M H 2 SO 4 (two acidic hydrogens) moles H + = mol OH " 1mol H + 1mol OH " 1mol H 2 SO 4 2mol H + = mol H 2 SO 4 volume H 2 SO 4 = mol H 2 SO mol H 2 SO 4 = L H 2 SO 4 solution 3. A ml solution of sodium hydroxide is titrated to the endpoint (the point where the acid and base have reacted to be completely neutralized) after the addition of ml of a M HCl solution. What is the molarity of the sodium hydroxide solution? Net Ionic Rxn: H + (aq) + OH - (aq) H 2 O (l) mol HCl moles H + = L 1mol H + 1mol HCl = "3 mol H + 1mol OH 1mol NaOH moles OH = " 10 3 mol H + " " = " 10 3 mol NaOH 1mol H + 1mol OH molarity NaOH = "3 mol NaOH 0.025L = M NaOH Page 2 of 7
3 4. An acid contains one acidic hydrogen per molecule (i.e., HA). A solution of the acid is made using g of the pure acid and distilled water. The acid is titrated to the endpoint with ml of a M NaOH solution. What is the molar mass of the acid? Net Ionic Rxn: H + (aq) + OH - (aq) H 2 O (l) mol NaOH moles OH = L " moles H + = "3 mol OH " 1mol H + molar mass HA = 1mol HA " 1mol OH 1mol H g HA = 397.1g mol HA "3 mol HA " 1mol OH 1mol NaOH = 7.251" 103 mol OH = "3 mol HA 5. Tell which of the following are oxidation-reduction reactions. For those that are, identify the oxidizing agent, the reducing agent, the substance being oxidized, and the substance being reduced. a. CH 4 (g) + 2O 2 (g) CO 2 (g) + 2H 2 O (g) oxidized: C (-4 to +4) oxidizing agent: O 2 reduced: O (0 to -2) reducing agent: CH 4 b. Zn (s) + 2HCl (aq) ZnCl 2 (aq) + H 2 (g) oxidized: Zn (0 to +2) oxidizing agent: HCl reduced: H (+1 to 0) reducing agent: Zn c. Cr 2 O 7- (aq) + 2OH - (aq) 2CrO 4 (aq) + H 2 O (l) No d. O 3 (g) + NO (g) O 2 (g) + NO 2 (g) oxidized: N (+2 to +4) oxidizing agent: O 3 reduced: O (0 to -2) reducing agent: NO e. 2H 2 O 2 (l) 2H 2 O (l) + O 2 (g) oxidized: O (-1 to 0) oxidizing agent: H 2 O 2 reduced: O (-1 to -2) reducing agent: H 2 O 2 Page 3 of 7
4 f. 2CuCl (aq) CuCl 2 (aq) + Cu (s) oxidized: Cu (+1 to +2) oxidizing agent: CuCl reduced: Cu (+1 to 0) reducing agent: CuCl g. HCl (g) + N (g) NH 4 Cl (s) No h. SiCl 4 (l) + 2H 2 O (l) 4HCl (aq) + SiO 2 (s) No i. SiCl 4 (l) + 2Mg (s) 2MgCl 2 (s) + Si (s) oxidized: Mg (0 to +2) oxidizing agent: SiCl 4 reduced: Si (+4 to 0) reducing agent: Mg 6. For each reaction, identify the atoms that undergo reduction or oxidation, list the oxidizing and reducing agents, and balance the reaction (in acidic solution, if needed). a. H 2 (g) + O 2 (g) H 2 O (g) oxidized: H (0 to +1) oxidizing agent: O 2 reduced: O (0 to -2) reducing agent: H 2 Balanced: 2H 2 (g) + O 2 (g) 2H 2 O (g) b. Zn (s) + Cu 2+ (aq) Zn 2+ (aq) + Cu (s) oxidized: Zn (0 to +2) oxidizing agent: Cu reduced: Cu (+2 to 0) reducing agent: Zn Balanced: Zn (s) + Cu 2+ (aq) Zn 2+ (aq) + Cu (s) c. AgCl (s) + H 2 (aq) 2Ag (s) + Cl - (aq) oxidized: H (0 to +1) oxidizing agent: AgCl reduced: Ag (+1 to 0) reducing agent: H 2 Balanced: 2AgCl (s) + H 2 (aq) 2H + (aq) + 2Ag (s) + 2Cl - (aq) d. MnO - 4 (aq) + C 2 O 4 (aq) Mn 2+ (aq) + CO 2 (g) - oxidized: C (+3 to +4) oxidizing agent: MnO 4 reduced: Mn (+7 to +2) reducing agent: C 2 O 4 Balanced: 2MnO - 4 (aq) + 16H + (aq) + 5C 2 O 4 (aq) 2Mn 2+ (aq) + 10CO 2 (g) + 8H 2 O (l) Page 4 of 7
5 7. Balance the following reactions using the oxidation states method. Step 1: Identify the atoms that undergo oxidation and reduction. Step 2: Draw tie-lines between atoms showing the changes in e -. Step 3: Find coefficients to equalize electron transfer. Step 4: Complete the balancing by inspection. a. C 6 H 12 O 6 (aq) + O 2 (g) CO 2 (g) + H 2 O (l) Assign oxidation states: C 6 H 12 O 6 (aq) + O 2 (g) CO 2 (g) + H 2 O (l) Find the electrons lost/gained: oxidized: C (0 to +4) x 6 C = 24 e - reduced: O (0 to -2) x 2 O = 4 e - Need 6 of these to balance Balanced: C 6 H 12 O 6 (aq) + 6O 2 (g) 6CO 2 (g) + 6H 2 O (l) b. N 2 H 4 (l) + N 2 O 4 (l) N 2 (g) + H 2 O (g) Assign oxidation states: N 2 H 4 (l) + N 2 O 4 (l) N 2 (g) + H 2 O (g) Find the electrons lost/gained: oxidized: N (-2 to 0) x 2 N = 4 e - Need 2 of these to balance reduced: N (+4 to 0) x 2 N = 8 e - Balanced: 2N 2 H 4 (l) + N 2 O 4 (l) 3N 2 (g) + 4H 2 O (g) 8. Balance the following reactions using the half reaction method in acidic solution, then in basic solution. Step 1: Identify and write equations for the half-reactions. Step 2: Balance each half-reaction. a) Balance all atoms that are neither oxygen nor hydrogen b) Balance oxygens by adding H 2 O c) Balance hydrogens by adding H + d) Balance charges by adding e - Step 3: Find coefficients to equalize electron transfer. Step 4: Add the two half reactions together. Step 5: For balancing in basic solution, add OH - to both sides to neutralize H +. Page 5 of 7
6 a. Cu (s) + HNO 3 (aq) Cu 2+ (aq) + NO (g) oxidation: Cu (s) Cu 2+ (aq) +2e - balanced reduction: HNO 3 (aq) NO (g) balance O with H 2 O HNO 3 (aq) NO (g) +2H 2 O (l) balance H with H + HNO 3 (aq) + 3H + (aq) NO (g) +2H 2 O (l) balance charges with e - HNO 3 (aq) + 3H + (aq) +3e - NO (g) +2H 2 O (l) Equalize electron transfer oxidation:3( Cu (s) Cu 2+ (aq) +2e - ) reduction:2(hno 3 (aq) + 3H + (aq) +3e - NO (g) +2H 2 O (l)) Total 3Cu (s) + 2HNO 3 (aq) + 6H + (aq) 3Cu 2+ (aq) + 2NO (g) + 4H 2 O (l) In basic solution, add OH - to neutralize H + 3Cu (s) + 2HNO 3 (aq) + 2H 2 O (l) 3Cu 2+ (aq) + 2NO (g) + 6OH - (aq) b. Cr 2 O 7 (aq) + NO (g) Cr 3+ (aq) + NO 3 - (aq) oxidation: NO (g) NO 3- (aq) reduction: Cr 2 O 7 (aq) Cr 3+ (aq) balance everything but O and H oxidation: NO (g) NO 3 - (aq) reduction: Cr 2 O 7 (aq) 2Cr 3+ (aq) balance O with H 2 O oxidation: NO (g) + 2H 2 O (l) NO 3- (aq) reduction: Cr 2 O 7 (aq) 2Cr 3+ (aq) + 7H 2 O (l) balance H with H + oxidation: NO (g) + 2H 2 O (l) NO 3 - (aq) + 4H + (aq) reduction: Cr 2 O 7 (aq) + 14H + (aq) 2Cr 3+ (aq) + 7H 2 O (l) balance charges with e - oxidation: NO (g) + 2H 2 O (l) NO 3 - (aq) + 4H + (aq) + 3e - reduction: Cr 2 O 7 (aq) + 14H + (aq) + 6e - 2Cr 3+ (aq) + 7H 2 O (l) Equalize electron transfer oxidation:2(no (g) + 2H 2 O (l) NO 3 - (aq) + 4H + (aq) + 3e - ) reduction: Cr 2 O 7 (aq) + 14H + (aq) + 6e - 2Cr 3+ (aq) + 7H 2 O (l) Page 6 of 7
7 Total 2NO (g) + Cr 2 O 7 (aq) + 6H + (aq) 2NO 3- (aq) + 2Cr 3+ (aq) + 3H 2 O (l) In basic solution, add OH - to neutralize H + 2NO (g) + Cr 2 O 7 (aq) + 3H 2 O (l) 2NO 3 - (aq) + 2Cr 3+ (aq) + 6OH - (aq) c. MnO 4 - (aq) + C 2 O 4 (aq) Mn 2+ (aq) + CO 2 (g) (aq) CO 2 (g) reduction: MnO 4 - (aq) Mn 2+ (aq) balance everything but O and H (aq) 2CO 2 (g) reduction: MnO 4 - (aq) Mn 2+ (aq) balance O with H 2 O (aq) 2CO 2 (g) reduction: MnO 4 - (aq) Mn 2+ (aq) + 4H 2 O (l) balance H with H + (aq) 2CO 2 (g) reduction: MnO 4- (aq) + 8H + (aq) Mn 2+ (aq) + 4H 2 O (l) balance charges with e - (aq) 2CO 2 (g) +2e - reduction: MnO 4 - (aq) + 8H + (aq) + 5e - Mn 2+ (aq) + 4H 2 O (l) Equalize electron transfer oxidation: 5(C 2 O 4 (aq) 2CO 2 (g) +2e - ) reduction: 2(MnO 4- (aq) + 8H + (aq) + 5e - Mn 2+ (aq) + 4H 2 O (l)) Total 5C 2 O 4 (aq) + 2MnO 4 - (aq) + 16H + (aq) 10CO 2 (g) + 2Mn 2+ (aq) + 8H 2 O (l) In basic solution, add OH - to neutralize H + 5C 2 O 4 (aq) + 2MnO 4 - (aq) + 8H 2 O (l) 10CO 2 (g) + 2Mn 2+ (aq) + 16OH - (aq) Page 7 of 7
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