AP ChemistryAP ChemistryChapter 17 JeopardyChapter 17 Jeopardy

Jennie L. BordersJennie L. Borders

Round 1 – Chapter 17 Round 1 – Chapter 17

KKspsp BuffersBuffersStrong-Strong-Strong Strong

TitrationsTitrations

Strong-Strong-Weak Weak

TitrationsTitrationsSolubilitySolubility PrecipitatesPrecipitates

100 100 100 100 100 100

200 200 200 200 200 200

300 300 300 300 300 300

400 400 400 400 400 400

500 500 500 500 500 500

KKspsp 100 100

The molar solubility of PbBrThe molar solubility of PbBr22 at at

2525ooC is 1.0 x 10C is 1.0 x 10-2 -2 mol/L. Calculate mol/L. Calculate KKspsp..

4 x 104 x 10-6-6

KKspsp 200 200

If 0.0490g of AgIOIf 0.0490g of AgIO33 dissolves per dissolves per

liter of solution, calculate the liter of solution, calculate the solubility-product constant.solubility-product constant.

3.03 x 103.03 x 10-8-8

KKspsp 300 300

A 1L solution saturated at 25A 1L solution saturated at 25ooC with C with calcium oxalate contains 0.0061g calcium oxalate contains 0.0061g

calcium oxalate. Calculate the calcium oxalate. Calculate the solubility product constant for this solubility product constant for this

salt at 25salt at 25ooC.C.

2.28 x 102.28 x 10-9-9

KKspsp 400 400

Calculate the molar solubility of Calculate the molar solubility of AgBr in 0.1M NaBr solution. The AgBr in 0.1M NaBr solution. The

KKspsp for AgBr is 5.0 x 10 for AgBr is 5.0 x 10-13-13..

5 x 105 x 10-12-12MM

KKspsp 500 500

Calculate the solubility of Cu(OH)Calculate the solubility of Cu(OH)22

in grams per liter of solution. The in grams per liter of solution. The KKspsp for Cu(OH) for Cu(OH)22 is 4.8 x 10 is 4.8 x 10-20-20..

2.23 x 102.23 x 10-5-5 g/L g/L

Buffers 100Buffers 100

Calculate the pH of a buffer that is Calculate the pH of a buffer that is 0.105M in NaHCO0.105M in NaHCO33 and 0.125M in and 0.125M in

NaNa22COCO33. The K. The Kaa for HCO for HCO33-- is 5.6 x is 5.6 x

1010-11-11..

10.3310.33

Buffers 200Buffers 200

Calculate the pH of a solution Calculate the pH of a solution formed by mixing 65mL of 0.20M formed by mixing 65mL of 0.20M

NaHCONaHCO33 with 75mL of 0.15M with 75mL of 0.15M

NaNa22COCO33. The K. The Kaa for HCO for HCO33-- is 5.6 x is 5.6 x

1010-11-11..10.1810.18

Buffers 300Buffers 300

What is the ratio of HCOWhat is the ratio of HCO33-- to H to H22COCO33

in blood with a pH of 7.4? The Kin blood with a pH of 7.4? The Kaa

for Hfor H22COCO33 is 4.3 x 10 is 4.3 x 10-7-7..

10.8 10.8

Buffers 400Buffers 400

A buffer solution contains 0.1 mol A buffer solution contains 0.1 mol of Cof C22HH55COOH and 0.13 mol COOH and 0.13 mol

CC22HH55COONa in 1.50L. What is the COONa in 1.50L. What is the

pH of the buffer after the addition pH of the buffer after the addition of 0.10 mol of NaOH?of 0.10 mol of NaOH?

5.085.08

Buffers 500Buffers 500

A buffer solution contains 0.1 mol A buffer solution contains 0.1 mol of Cof C22HH55COOH and 0.13 mol COOH and 0.13 mol

CC22HH55COONa in 1.50L. What is COONa in 1.50L. What is

the pH of the buffer after the the pH of the buffer after the addition of 0.01 mol of HI? addition of 0.01 mol of HI?

(K(Kaa = 1.3 x 10 = 1.3 x 10-5-5))

4.934.93

Strong-Strong Titrations 100Strong-Strong Titrations 100

A 20mL sample of 0.200M HBr is A 20mL sample of 0.200M HBr is titrated with 0.200M NaOH titrated with 0.200M NaOH

solution. Calculate the pH of the solution. Calculate the pH of the solution after 15mL of base has solution after 15mL of base has

been added.been added.

1.541.54

Strong-Strong Titrations 200Strong-Strong Titrations 200

A 20mL sample of 0.200M HBr is A 20mL sample of 0.200M HBr is titrated with 0.200M NaOH solution. titrated with 0.200M NaOH solution. Calculate the pH of the solution after Calculate the pH of the solution after

19.9mL of base has been added.19.9mL of base has been added.

3.303.30

Strong-Strong Titrations 300Strong-Strong Titrations 300

A 20mL sample of 0.200M HBr is A 20mL sample of 0.200M HBr is titrated with 0.200M NaOH titrated with 0.200M NaOH

solution. Calculate the pH of the solution. Calculate the pH of the solution after 20.0mL of base has solution after 20.0mL of base has

been added.been added.

7.007.00

Strong-Strong Titrations 400Strong-Strong Titrations 400A 20mL sample of 0.200M HBr is A 20mL sample of 0.200M HBr is

titrated with 0.200M NaOH titrated with 0.200M NaOH solution. Calculate the pH of the solution. Calculate the pH of the

solution after 20.1mL of base has solution after 20.1mL of base has been added.been added.

10.7010.70

Strong-Strong Titrations 500Strong-Strong Titrations 500

A 20mL sample of 0.200M HBr is A 20mL sample of 0.200M HBr is titrated with 0.200M NaOH titrated with 0.200M NaOH

solution. Calculate the pH of the solution. Calculate the pH of the solution after 35.0mL of base has solution after 35.0mL of base has

been added.been added.

12.7412.74

Strong-Weak Titrations 100Strong-Weak Titrations 100

Consider the titration of 30.0mL Consider the titration of 30.0mL NHNH33with 0.025M HCl. Calculate the with 0.025M HCl. Calculate the

pH after 0mL of the titrant has been pH after 0mL of the titrant has been added. (Kadded. (Kbb = 1.8 x 10 = 1.8 x 10-5-5))

10.8710.87

Strong-Weak Titrations 200Strong-Weak Titrations 200

Consider the titration of 30.0mL Consider the titration of 30.0mL NHNH33with 0.025M HCl. Calculate the with 0.025M HCl. Calculate the

pH after 10.0mL of the titrant has pH after 10.0mL of the titrant has been added. (Kbeen added. (Kbb = 1.8 x 10 = 1.8 x 10-5-5))

9.679.67

Strong-Weak Titrations 300Strong-Weak Titrations 300

Consider the titration of 30.0mL Consider the titration of 30.0mL NHNH33with 0.025M HCl. Calculate the with 0.025M HCl. Calculate the

pH after 20.0mL of the titrant has pH after 20.0mL of the titrant has been added. (Kbeen added. (Kbb = 1.8 x 10 = 1.8 x 10-5-5))

9.169.16

Strong-Weak Titrations 400Strong-Weak Titrations 400

Consider the titration of 30.0mL Consider the titration of 30.0mL NHNH33with 0.025M HCl. Calculate the with 0.025M HCl. Calculate the

pH after 36.0mL of the titrant has pH after 36.0mL of the titrant has been added. (Kbeen added. (Kbb = 1.8 x 10 = 1.8 x 10-5-5))

5.555.55

Strong-Weak Titrations 500Strong-Weak Titrations 500

Consider the titration of 30.0mL of Consider the titration of 30.0mL of 0.030M NH0.030M NH33with 0.025M HCl. with 0.025M HCl.

Calculate the pH after 37.0mL of the Calculate the pH after 37.0mL of the titrant has been added. titrant has been added.

(K(Kbb = 1.8 x 10 = 1.8 x 10-5-5))

3.433.43

Solubility 100Solubility 100

Would MnS be more soluble in acidic Would MnS be more soluble in acidic solution than in pure water? Write solution than in pure water? Write

the equation.the equation.

YesYesMnS + 2HMnS + 2H++ Mn Mn2+2+ + H + H22SS

Solubility 200Solubility 200

Would PbFWould PbF22 be more soluble in be more soluble in

acidic solution than in pure water? acidic solution than in pure water? Write the equation.Write the equation.

YesYesPbFPbF22 + 2H + 2H++ Pb Pb2+2+ + 2HF + 2HF

Solubility 300Solubility 300

Would AuClWould AuCl33 be more soluble in be more soluble in

acidic solution than in pure water? acidic solution than in pure water? Write the equation.Write the equation.

NoNoAuClAuCl33 + 3H + 3H++ Au Au3+3+ + HCl + HCl

strong acidstrong acid

Solubility 400Solubility 400

Would HgWould Hg22CC22OO44 be more soluble in be more soluble in

acidic solution than in pure water? acidic solution than in pure water? Write the equation.Write the equation.

YesYesHgHg22CC22OO44 + 2H + 2H++ 2Hg 2Hg+ + + H+ H22CC22OO44

Solubility 500Solubility 500

Would CuBr be more soluble in acidic Would CuBr be more soluble in acidic solution than in pure water? Write solution than in pure water? Write

the equation.the equation.

NoNoCuBr + HCuBr + H++ Cu Cu++ + HBr + HBr

strong acidstrong acid

Precipitates 100Precipitates 100

Will Ca(OH)Will Ca(OH)22 precipitate from solution precipitate from solution

if the pH of a 0.05M solution of if the pH of a 0.05M solution of CaClCaCl22 is adjusted to 8.0? is adjusted to 8.0?

(K(Kspsp = 6.5 x 10 = 6.5 x 10-6-6))

Q < KQ < Kspsp so no Ca(OH) so no Ca(OH)22 will precipitate will precipitate

Precipitates 200Precipitates 200

Will AgWill Ag22SOSO44 precipitate with 100mL of precipitate with 100mL of

0.05M AgNO0.05M AgNO33 is mixed with 10mL is mixed with 10mL

of 5.0 x 10of 5.0 x 10-2-2M NaM Na22SOSO44 solution? solution?

(K(Kspsp = 1.5 x 10 = 1.5 x 10-5-5))

Q < KQ < Kspsp so no Ag so no Ag22SOSO44 will will

precipitateprecipitate

Precipitates 300Precipitates 300

Will Ca(OH)Will Ca(OH)22 precipitate from solution precipitate from solution

if the pH of a 0.02M solution of if the pH of a 0.02M solution of Co(NOCo(NO33))22 is adjusted to 8.5? is adjusted to 8.5?

(K(Kspsp = 1.3 x 10 = 1.3 x 10-15)-15)

Q > KQ > Kspsp so Co(OH) so Co(OH)22 will precipitate will precipitate

Precipitates 400Precipitates 400

Will AgIOWill AgIO33 precipitate when 20mL of precipitate when 20mL of

0.01M AgNO0.01M AgNO33 is mixed with 10mL is mixed with 10mL

of 0.015M NaIOof 0.015M NaIO33??

(K(Kspsp = 3.1 x 10 = 3.1 x 10-8-8))

Q > KQ > Kspsp so AgIO so AgIO33 will precipitate will precipitate

Precipitates 500Precipitates 500

A solution of NaA solution of Na22SOSO44 is added is added

dropwise to a solution that is dropwise to a solution that is 0.010M in Ba0.010M in Ba2+2+ (K (Kspsp = 1.1 x 10 = 1.1 x 10-10) -10)

and 0.01M Srand 0.01M Sr2+ 2+ (K(Kspsp = 3.2 x 10 = 3.2 x 10-7-7). ).

Which will precipitate first?Which will precipitate first?BaSOBaSO44 precipitates first precipitates first