8. What is the HiO concentration of a solution with a pH of 11.6 b) 10.6 M2.51 x 10-12 M e) 1.06 M a) 2.51 x 10-10 M d) 2.4 M 9. A 10.0 ml sample of an unknown concentration of acetic acid is titrated with 0.25 M solution of NaOH to the phenolphthalein end-point. The solution turned pink after adding 30.60 ml of the base. Calculate the concentration of acetic acid. a) 0.11 M. 50.08 M ) 7.7 M d) 77 M 10.0px 0.26m 30.60ml 10. The reaction below is at equilibrium. Use LeChatelier's principle to predict the effect of the following changes on the equilibrium. Answers: shifts to left; shifts to right, no effect. e) 0.77 M [H 304 PH= -11.6 log [30] 351102 timile PCI(g) + Ch(g) PCI(g) + 25 kcal a) Increases the temperature of the system? Shif to Left b) Decreasing the pressure on the system? Sok to Pight e) Adding Phosphorus Pentachloride gas to the system? A to left d) Removing Chlorine gas? S to fight M₂ VAIK = =0.08 M
8. What is the HiO concentration of a solution with a pH of 11.6 b) 10.6 M2.51 x 10-12 M e) 1.06 M a) 2.51 x 10-10 M d) 2.4 M 9. A 10.0 ml sample of an unknown concentration of acetic acid is titrated with 0.25 M solution of NaOH to the phenolphthalein end-point. The solution turned pink after adding 30.60 ml of the base. Calculate the concentration of acetic acid. a) 0.11 M. 50.08 M ) 7.7 M d) 77 M 10.0px 0.26m 30.60ml 10. The reaction below is at equilibrium. Use LeChatelier's principle to predict the effect of the following changes on the equilibrium. Answers: shifts to left; shifts to right, no effect. e) 0.77 M [H 304 PH= -11.6 log [30] 351102 timile PCI(g) + Ch(g) PCI(g) + 25 kcal a) Increases the temperature of the system? Shif to Left b) Decreasing the pressure on the system? Sok to Pight e) Adding Phosphorus Pentachloride gas to the system? A to left d) Removing Chlorine gas? S to fight M₂ VAIK = =0.08 M
Chapter13: Titrations In Analytical Chemistry
Section: Chapter Questions
Problem 13.28QAP
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I did the work I just woukd like to kniw if its correct and if not please tell me where i went wrong. Thank you.
![8. What is the H₁O concentration of a solution with a p
a pH of 11.6
a) 2.51 x 10-10 Mb) 10.6 M 2.51 x 10-12 M
d) 2.4 M
e) 1.06 M
9. A 10.0 ml sample of an unknown concentration of acetic acid is titrated with
0.25 M solution of NaOH to the phenolphthalein end-point. The solution turned.
pink after adding 30.60 ml of the base. Calculate the concentration of acetic acid.
a) 0.11 M
50.08 M c) 7.7 M
d) 77 M
e) 0.77 M
10.0px 0.26m
30.60ml
= 0.08 M
10. The reaction below is at equilibrium. Use LeChatelier's principle to predict the
effect of the following changes on the equilibrium. Answers: shifts to left; shifts
to right, no effect.
ml
PCI(g) + 25 kcal
11. Strong acids are completely
a) associated b) aqueous
to Left
a) Increases the temperature of the system? Shif
b) Decreasing the pressure on the system? Sot to Right
c) Adding Phosphorus Pentachloride gas to the system? ift to left
d) Removing Chlorine gas? St Right
a) 1.02 x 10-¹
d) 1.02 x 10-12
12. Calculate the hydronium ion concentration [H₂O*] of a solution that has a
hydroxide ion concentration [OH] of 9.85 x 10 M.
Zimme
PCI(g) + Cl2(g)
in water.
dissociated d) basic e) oxidized
69.85 x 10¹¹
a) Hydronium ion
d) hydroxide ion
PH=-log [A₂¹]
PH= -11.6 log
[H 30+]
[H30] =251×102
e) none of the above
13. If a proton (H') in added to a water molecule it creates a:
a) Hydrogen hydrate ion
d) a base
b) Hydroxide ion
Hydronium Ion
b>Water
c) 9.85 x 10¹7
14. In a neutralization reaction of an acid with a base a salt is produced. What is the
other product?
c) a metal
e) none of the above
[H0] [985-102
7982
= 9.15 × 10¹
c) Water hydride ion
M₂ VAK](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F31690de8-b08a-4f1b-9410-036c765b0e3a%2Fdc4ddb8a-6f0c-4bb9-902d-62bfd48291c3%2Fj0ii3bb_processed.jpeg&w=3840&q=75)
Transcribed Image Text:8. What is the H₁O concentration of a solution with a p
a pH of 11.6
a) 2.51 x 10-10 Mb) 10.6 M 2.51 x 10-12 M
d) 2.4 M
e) 1.06 M
9. A 10.0 ml sample of an unknown concentration of acetic acid is titrated with
0.25 M solution of NaOH to the phenolphthalein end-point. The solution turned.
pink after adding 30.60 ml of the base. Calculate the concentration of acetic acid.
a) 0.11 M
50.08 M c) 7.7 M
d) 77 M
e) 0.77 M
10.0px 0.26m
30.60ml
= 0.08 M
10. The reaction below is at equilibrium. Use LeChatelier's principle to predict the
effect of the following changes on the equilibrium. Answers: shifts to left; shifts
to right, no effect.
ml
PCI(g) + 25 kcal
11. Strong acids are completely
a) associated b) aqueous
to Left
a) Increases the temperature of the system? Shif
b) Decreasing the pressure on the system? Sot to Right
c) Adding Phosphorus Pentachloride gas to the system? ift to left
d) Removing Chlorine gas? St Right
a) 1.02 x 10-¹
d) 1.02 x 10-12
12. Calculate the hydronium ion concentration [H₂O*] of a solution that has a
hydroxide ion concentration [OH] of 9.85 x 10 M.
Zimme
PCI(g) + Cl2(g)
in water.
dissociated d) basic e) oxidized
69.85 x 10¹¹
a) Hydronium ion
d) hydroxide ion
PH=-log [A₂¹]
PH= -11.6 log
[H 30+]
[H30] =251×102
e) none of the above
13. If a proton (H') in added to a water molecule it creates a:
a) Hydrogen hydrate ion
d) a base
b) Hydroxide ion
Hydronium Ion
b>Water
c) 9.85 x 10¹7
14. In a neutralization reaction of an acid with a base a salt is produced. What is the
other product?
c) a metal
e) none of the above
[H0] [985-102
7982
= 9.15 × 10¹
c) Water hydride ion
M₂ VAK
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