Chem 2 Test 2

Front 1

Calculate the pH for an aqueous solution of pyridine that contains 2.15x10^-4 M hydroxide ion.

Back 1

10.33

Front 2

Calculate the pH of a solution formed by mixing 100.0 mL of 0.20 M HClO with 200.0 mL of 0.30 M KClO. The Ka for HClO is 2.9 × 10-8.

Back 2

8.01

Front 3

Which of the following is a polyprotic acid?

Back 3

H2SO4

Front 4

Determine the Ka of an acid whose 0.294 M solution has a pH of 2.80

Back 4

8.5x10^-6

Front 5

Which of the following acids will have the strongest conjugate base?

Back 5

HCN

Front 6

Calculate the pOH of a solution that contains 2.4 × 10-5 M H3O+ at 25°C

Back 6

9.38

Front 7

Calculate the pOH of a solution that contains 7.8 x 10-6 M OH- at 25°C

Back 7

5.11

Front 8

Which of the following is a triprotic acid

Back 8

H3PO4

Front 9

Identify the weak diprotic acid

Back 9

H2SO3

Front 10

The pH of an aqueous solution at 25.0°C is 10.66. What is the molarity of H+ in this solution

Back 10

2.2x10^-11

Front 11

Which of the following acids is the WEAKEST? The acid is followed by its Ka value

Back 11

HCN, 4.9 × 10^-10

Front 12

What is the hydronium ion concentration of a 0.500 M acetic acid solution with Ka = 1.8 × 10-5? The equation for the dissociation of acetic acid is:

Back 12

3.0x10^-3

Front 13

Determine the pH of a 0.023 M HNO3 solution

Back 13

1.64

Front 14

Identify the weak diprotic acid

Back 14

H2CO3

Front 15

Calculate the pH of a solution that contains 3.9 x 10-5 M H3O+ at 25°C

Back 15

4.41

Front 16

What is the hydronium ion concentration of a 0.150 M hypochlorous acid solution with Ka= 3.5x10^-8. The equation for the dissociation of hypochlorous acid is

Back 16

7.2x10^-5

Front 17

Place the following in order of increasing acid strength.HBrO2 HBrO3 HBrO HBrO4

Back 17

HBrO < HBrO2 < HBrO3 < HBrO4

Front 18

Determine the pOH of a 0.00598 M HClO4 solution

Back 18

11.777

Front 19

Determine the [OH-] concentration of a 0.123 M Sr(OH)2 solution at 25°C

Back 19

.246 M

Front 20

Calculate the concentration of H3O+ in a solution that contains 5.5 × 10-5 M OH- at 25°C. Identify the solution as acidic, basic, or neutral

Back 20

1.8 × 10-10 M, basic

Front 21

Calculate the molarity of hydroxide ion in an aqueous solution that has a pOH of 5.00

Back 21

1.0x10^-5

Front 22

Calculate the hydronium ion concentration in an aqueous solution that contains 2.50 × 10-6 M in hydroxide ion

Back 22

4.00 × 10^-9 M

Front 23

Calculate the pOH in an aqueous solution with a pH of 7.85 at 25°C

Back 23

6.15

Front 24

Calculate the hydroxide ion concentration in an aqueous solution with a pH of 9.85 at 25°C

Back 24

7.1x10^-5 M

Front 25

A 7.0 × 10-3 M aqueous solution of Ca(OH)2 at 25.0°C has a pH of

Back 25

12.15

Front 26

Identify the weakest acid

Back 26

HF

Front 27

Calculate the hydroxide ion concentration in an aqueous solution that contains 3.50 × 10-4 M in hydronium ion

Back 27

2.86x10^-11 M

Front 28

A 100.0 mL sample of 0.20 M HF is titrated with 0.10 M KOH. Determine the pH of the solution after the addition of 200.0 mL of KOH. The Ka of HF is 3.5 × 10-4

Back 28

h

Front 29

If the pKa of HCHO2 is 3.74 and the pH of an HCHO2/NaCHO2 solution is 3.11, which of the following is TRUE

Back 29

h

Front 30

The molar solubility of Ag2S is 1.26 × 10-16 M in pure water. Calculate the Ksp for Ag2S

Back 30

h

Front 31

Calculate the pH of a buffer that is 0.225 M HC2H3O2 and 0.162 M KC2H3O2. The Ka for HC2H3O2 is 1.8 × 10-5

Back 31

4.60

Front 32

Determine the molar solubility of BaF2 in a solution containing 0.0750 M LiF. Ksp (BaF2) = 1.7 × 10-6

Back 32

h

Front 33

Calculate the pH of a buffer that is 0.158 M HClO and 0.099 M NaClO. The Ka for HClO is 2.9 × 10-8

Back 33

7.33

Front 34

Calculate the pH of a buffer that is 0.040 M HF and 0.020 M LiF. The Ka for HF is 3.5 × 10-4

Back 34

3.16

Front 35

A 1.00 L buffer solution is 0.250 M in HF and 0.250 M in LiF. Calculate the pH of the solution after the addition of 0.150 moles of solid LiOH. Assume no volume change upon the addition of base. The Ka for HF is 3.5 × 10-4

Back 35

4.06

Front 36

Consider a reaction that has a negative ΔH and a negative ΔS. Which of the following statements is TRUE

Back 36

h

Front 37

A buffer solution is 0.100 M in both HC7H5O2 and LiC7H5O2 and has a pH of 4.19. Which of the following pH values would you expect from the addition of a small amount of a dilute solution of a strong base

Back 37

h

Front 38

A 100.0 mL sample of 0.10 M Ca(OH)2 is titrated with 0.10 M HBr. Determine the pH of the solution after the addition of 400.0 mL HBr

Back 38

h

Front 39

You wish to prepare an HC2H3O2 buffer with a pH of 4.24. If the pKa of is 4.74, what ratio of C2H3O2-/HC2H3O2 must you use

Back 39

.32

Front 40

A 100.0 mL sample of 0.180 M HClO4 is titrated with 0.270 M LiOH. Determine the pH of the solution after the addition of 75.0 mL of LiOH

Back 40

h

Front 41

A 100.0 mL sample of 0.18 M HClO4 is titrated with 0.27 M LiOH. Determine the pH of the solution after the addition of 30.0 mL of LiOH

Back 41

h

Front 42

A 1.50 L buffer solution is 0.250 M in HF and 0.250 M in NaF. Calculate the pH of the solution after the addition of 0.0500 moles of solid NaOH. Assume no volume change upon the addition of base. The Ka for HF is 3.5 × 10-4

Back 42

h

Front 43

A 100.0 mL sample of 0.18 M HClO4 is titrated with 0.27 M LiOH. Determine the pH of the solution after the addition of 100.0 mL of LiOH

Back 43

h

Front 44

Determine the molar solubility of Fe(OH)2 in pure water. Ksp for Fe(OH)2)= 4.87 × 10-17

Back 44

h

Front 45

Calculate the pH of a solution formed by mixing 150.0 mL of 0.10 M HC7H5O2 with 100.0 mL of 0.30 M NaC7H5O2. The Ka for HC7H5O2 is 6.5 × 10-5

Back 45

h

Front 46

A 100.0 mL sample of 0.18 M HClO4 is titrated with 0.27 M LiOH. Determine the pH of the solution after the addition of 66.67 mL of LiOH (this is the equivalence point)

Back 46

h

Front 47

Calculate the pH of a solution formed by mixing 250.0 mL of 0.15 M HCHO2 with 100.0 mL of 0.20 M LiCHO2. The Ka for HCHO2 is 1.8 × 10-4

Back 47

h

Front 48

Calculate the pH of a buffer that is 0.058 M HF and 0.058 M LiF. The Ka for HF is 3.5 × 10-4

Back 48

3.46

Front 49

Calculate the pH of a buffer that is 0.105 M HC2H3O2 and 0.146 M KC2H3O2. The Ka for HC2H3O2 is 1.8 × 10-5

Back 49

4.89

Front 50

A 1.0 L buffer solution is 0.250 M HC2H3O2 and 0.050 M LiC2H3O2. Which of the following actions will destroy the buffer?

Back 50

h