Chapter 11_Solutions_examples

# Chapter 11_Solutions_examples - 2 2 2 29 29 M 0.1378 L...

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CHM 11200 Spring 10 Chapter 11 Worked Lecture Examples

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Example 1 (Practice Problem 10.1, p 380) 2 When a solution of lead(II) nitrate is mixed with a solution of potassium chromate, a yellow precipitate forms according to the equation Pb(NO 3 ) 2 (aq) + K 2 CrO 4 (aq) PbCrO 4 (s) + 2 KNO 3 (aq) What volume of 0.105 M lead(II) nitrate is required to react with 100.0 mL of 0.120 M potassium chromate? What mass of PbCrO 4 solid forms? ( 29 ( 29 ( 29 L 0.114 mol 0.105 L 1 ) Pb(NO mol 0.01200 ) Pb(NO mol 0.01200 CrO K mol 1 ) Pb(NO mol 1 CrO K mol 0.01200 CrO K mol 0.01200 L 1 mol 0.120 CrO K L 0.1000 2 3 2 3 4 2 2 3 4 2 4 2 4 2 = = =
Example 2 (Practice Problem 10.2, p 382) 3 We need 28.28 mL of 0.2437 M HCl solution to completely titrate 25.00 mL of Ba(OH) 2 solution of unknown concentration. What is the molarity of the barium hydroxide solution? “Completely titrate” can be read as “completely react with”. . . First, write a balanced equation (this is an acid/base neutralization):

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Unformatted text preview: 2 2 2 ( 29 ( 29 M 0.1378 L 0.02500 Ba(OH) mol 0.003446 Ba(OH) mol 0.003446 HCl mol 2 Ba(OH) mol 1 HCl mol 0.006892 HCl mol 0.006892 L 1 mol 0.2437 HCl L 0.02828 2 2 2 = = = Example 3 (Practice Problem 10.4, p 387) 4 What is the freezing point for a 1.5 m solution of sucrose in water? (K f for water = 1.86°C/ m ) ( 29 C 2.8 -C 2.8 -C 0.0 T C 2.8 m C 1.86 m 1.5 ΔT f = = = = Example 4 (Practice Problem 10.9, p 396) 5 Which of the following aqueous solutions is expected to have the lowest freezing point? 0.5 m CH 3 CH 2 OH, 0.5 m Ca(NO 3 ) 2 , 0.5 m KBr 0.50 m particles 1.5 m particles 1.0 m particles lowest freezing point...
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Chapter 11_Solutions_examples - 2 2 2 29 29 M 0.1378 L...

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