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Solubility Lesson 8 Titrations & Max Ion Concentration. Review Questions 1. Mg(OH) 2 will have the greatest solubility in: Mg(OH) 2 ⇌ Mg 2+ + 2OH - A. NaOH B. Mg(NO 3 ) 2 C. H 2 O . OH - lowers solubility. Mg 2+ lowers solubility. No effect solubility. D. AgNO 3.

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Presentation Transcript
slide1

Solubility

Lesson 8

Titrations &

Max Ion Concentration

slide2

Review Questions

1. Mg(OH)2 will have the greatest solubility in:

Mg(OH)2 ⇌ Mg2+ + 2OH-

A. NaOH

B. Mg(NO3)2

C. H2O

OH- lowers solubility

Mg2+ lowers solubility

No effect solubility

D. AgNO3

Ag+ increases solubility by reacting with OH-

slide3

Review Questions

2. Mg(OH)2 will have the lowest solubility in:

Mg(OH)2 ⇌ Mg2+ + 2OH-

A. 1.0 M NaNO3

B. 1.0 M NaOH

No effect

1.0 M OH- lowers solubility

C. 1.0 M Sr(OH)2

2.0 M OH- lowers solubility more

remember:Sr(OH)2  Sr2+ + 2OH-

1.0 M 1.0 M 2.0 M

slide4

Review Questions

3. PbCl2 will have the lowest solubility in:

PbCl2 ⇌ Pb2+ + 2Cl-

A. 1.0 M NaCl

B. 1.0 M MgCl2

C. 1.0 M AlCl3

1.0 M Cl-

2.0 M Cl-

3.0 M Cl-

D. 2.0 M CaCl2

4.0 M Cl-

slide5

Maximum Ion Concentration

0.100 M BrO3-

4. What is the maximum [Ag+]possible in a 0.100MNaBrO3 without forming a precipitate@ 25 0C.

[Ag+]

AgBrO3(s)⇌ Ag+ + BrO3-

0.100 M

Ksp = [Ag+][BrO3-]

What is the molarity of [Ag+] just before it precipitates?

5.3 x 10-5 = [Ag+][0.100]

[Ag+] =5.3 x 10-4 M

slide6

5. Calculate the maximumnumber of gramsof AgNO3 that will dissolve 100.0 mL of0.200M AlCl3without forming a precipitate @ 25 0C.

AgCl(s)⇌ Ag+ + Cl-

0.600 M

Ksp = [Ag+][Cl-]

1.8 x 10-10 = [Ag+][0.600]

[Ag+]= 3.0 x 10-10 M

0.1000 L AgNO3

x 3.0 x 10-10 moles

x 169.9 g

= 5.1 x 10-9 g

1 L

1 mole

slide7

6. In a titration 3.61 mLof0.0200MNaI is required to completely precipitate all of the lead II ions in 10.0 mLof saturatedPbCl2solution. Calculate the [Pb2+].

Pb2+ + 2I- PbI2

0.0100 L

0.00361 L

0.0200 M

? M

x 0.0200 mol

x 1 mol Pb2+

0.00361 L I-

2 mol I-

1L

[Pb2+] =

0.0100 L

=0.00361 M