PhysioEx Exercise 10 Activity 2
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PhysioEx Exercise 10 Activity 2
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PhysioEx Lab Report
Exercise 10: Acid-Base Balance
Activity 2: Rebreathing
Name: Jackie Chau
Date: 6 December 2023
Session ID: session-85c6a2fd-ba96-d43a-547f-28877800e189
Pre-lab Quiz Results
You scored 100% by answering 4 out of 4 questions correctly.
Experiment Results
Predict Question
Stop & Think Question
Experiment Data
Condition
Min. P
(mm Hg)
Max. P
(mm Hg)
Min. pH
Max. pH
Normal
40
40
7.42
7.42
In cases of acidosis, the pH of the blood is
You correctly answered:
less than 7.35.
1
Carbon dioxide and water form
You correctly answered:
carbonic acid (a weak acid).
2
Which of the following is true of respiratory acidosis?
You correctly answered:
The amount of carbon dioxide in the blood is greater than normal.
3
Rebreathing
You correctly answered:
is exemplified by breathing into a paper bag.
4
Predict Question: What do you think will happen to the pH and P
levels during
rebreathing?
Your answer:
pH will decrease and P
will increase.
1
CO
2
CO
2
Which of the following can cause respiratory acidosis?
You correctly answered:
airway obstruction.
1
CO
2
CO
2
12/6/23, 5:07 PM
PhysioEx Exercise 10 Activity 2
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Rebreathing
40
49.3
7.28
7.41
Post-lab Quiz Results
You scored 100% by answering 4 out of 4 questions correctly.
Normal Breathing
Rebreathing
Rebreathing simulates
You correctly answered:
hypoventilation and respiratory acidosis.
1
Hypoventilation results in
You correctly answered:
an accumulation of carbon dioxide in the blood.
2
The renal system can compensate for respiratory acidosis by
3
12/6/23, 5:07 PM
PhysioEx Exercise 10 Activity 2
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Review Sheet Results
You have not completed the Review Sheet.
You correctly answered:
excreting H
and retaining bicarbonate ion.
+
Respiratory acidosis can be caused by all of the following
except
You correctly answered:
an anxiety attack.
4
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Show What You Know: pH & pOH
What is the pOH of a solution with [H*] = 3.4 x 103 M? Show your work.
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Use the References to access important values if needed for this question.
A buffer solution contains 0.234 M C6H5NH3 Br and 0.315 M C6H5NH2 (aniline). Determine
the pH change when 0.090 mol HI is added to 1.00 L of the buffer. (Assume
Kb(C%HNH,)= 7.4 × 10-10.)
pH after addition - pH before addition
Submit Answer
4. Buffer + Strong Acid or Base (Henderson-Hasselbalch): This is group attempt 1 of 5
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The vapor pressure of Substance X is measured at several temperatures:
0
temperature vapor pressure
52. °C
News
63. °C
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74. °C
I Don't Know
0.0803 atm
0.124 atm
College information
0.188 atm
Use this information to calculate the enthalpy of vaporization of X.
Round your answer to 2 significant digits. Be sure your answer contains a correct unit symbol.
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Question 24
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Design a buffer that has a pH of 7.19 using one of the weak base/conjugate acid systems
Weak Base
CH3NH2
C6H1503N
C5H5N
$1
5
6. Prepare Buffers by Direct Addition: This is group attempt 1 of 5
Si
grams weak base
How many grams of the bromide salt of the conjugate acid must be combined with how many
grams of the weak base, to produce 1.00 L of a buffer that is 1.00 M in the weak base?
grams bromide salt of conjugate acid =
96
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F5
Kb
4.2×10-4
5.9x10-7
STE
Conjugate Acid Ka
CH3NH3 2.4×10-11
C6H1503NH+ 1.7×10-8
1.5x10-9 CsH5NH+ 6.7x10-6
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Spring 2021 Problem Set 3 Part I-21
Page 3 of 3
17.) Complete the following table:
[anion]
value of Q
unsaturated,
saturated, or
supersaturated
salt
[cation]
Kp expression
BaSO4
|1.1 x 10-10 2.20 x 10-6 5.00 x 105
Fe(CN);
8.0 x 10-16 9.66 x 10-5 5.12 x 10-7
Ag:CrO4
1.1 x 10-12 7.57 x 10+ 4.07 x 103
Mg;(PO4)2 2.0 x 10-2º | 2.53 x 10-5 | 4.00 x 10-
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Unknown Acid
Acid name
Acetic acid
Group #5
Group #6
Group #7
Mean
Standard Deviation
% Error
STATISTICAL ANALYSIS: Calculate mean values for molar mass, pKa, and Ka. Calculate % error and standard deviation:
Unknown acid # 1
Molar Mass of unknown acid (calculated), g/mol
Group #1
Group #2
Group #3
Group #4
Reaction
Initial conc. / M:
Change in conc. at
equilibrium / M:
Equilibrium conc. / M:
Acetic acid | Molar Mass, g/mol: 60.05 | pka = 4.76
Accepted Values
Molar mass, g/mol
60.05
Ka =
Part II
1. Using initial molarity of acid and measured pH of the acid before titration, build a RICE table and
calculate the Ka of the acid. You can use examples 1, 2 (pp. 3-4) from the Manual (posted on Canvas)
Initial Molarity of [HA], M
0.219
Initial pH of Acid
pka =
HA(aq) + H₂O(1)
[HA]
-X
58.8
57.4
60.4
61.0
58.4
59.2
59.7
59.3
1.13
0.01
[HA] + X
台
pH:
H3O+ (aq)
=
0
+X
2. Use the Henderson-Hasselbauch equation to perform the same calculation.
+X
pka
4.76
Ka =
pka
4.78
5.00
4.64
4.89
4.62
4.68
4.82…
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Part A
pH =
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A
a solution that is 0.13 M in NH3 and 0.17 M in NH4Cl (Kb (NH3) = 1.76 x 10-5)
Express your answer to one decimal place.
Submit
Asession.masteringchemistry.com
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C030
BY NC SA
S. Alvanipour, Y, Gedeon, G. Zoorob, CC BY-NC-SA 4.0
B. Determination of unknown acid concentration
Unknown Acid number
Volume of acid used
(ml)
Initial buret reading
(mL)
Final buret reading
(ml)
Volume of NaOH used
(ml)
Molarity of NaOH
Trial 1
Unknown
Quid
25.0ml
Ome
12.4ml
12.4ml
-10m
Calculated molarity of
HCI (M)
Show a sample calculation of HCI molarity
AVERAGE MOLARITY OF Unknown HCI
Show a sample calculation of NaOH molarity:
Trial 2
Unknown
25-am
omo
12.5ml
12.5ml
-lom
Trial 3
Unknown
af
20% ome
come
12.630
12.6ml
-tom
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pH
pH = 4.389
pH = 4.874
=
pH = 5.339
pKa
Answer Bank
Using the equation to calculate the quotient [A]/[HA] at three different pH values.
[A]
[HA]
+ log
[A-]
[HA]
[A]
[HA]
||
=
H
=
[A]
[HA]
1
0.3273
arrow_forward
pH
pH = 4.389
pH = 4.874
=
pH = 5.339
pKa
Answer Bank
Using the equation to calculate the quotient [AT]/[HA] at three different pH values.
[A]
[HA]
+ log
[A-]
[HA]
[A-]
[HA]
=
=
=
LA I
[HA]
1
0.3273
arrow_forward
Trial 1:
Initial pH= 3.92mL
Mass of KHP and Paper= 0.868g
Mass of paper= 0.357g
Mass of KHP= 0.511g
Trial 2:
Initial pH= 4.09ml
Mass of KHP and Paper= 0.870g
Mass of paper= 0.359g
Mass of KHP= 0.511g
1)Use Kb, the number of moles of C8H4O4^2- at the equivalence point, and the total volume at that point to calculate the pH for each sample at the equivalence point. Compare these calculated results with the experimental results.
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CHEM1407
A
Homework Ch 16, Sec 6A
Name:
# 3) A 2.5x10-³M of an unknown acid has a pH of 3.80 at 25C. What is the
hydronium ion concentration of the solution?
# 4) A 0.15M solution of cyanic acid (HCNO) has a Ka for the acid of 3.5x10-4.
What is pH for this acid?
# 5) The ionization constant of a very weak acid HA is 4.0x109. Calculate the
equilibrium concentrations of H3O+, A-, and HA in a 0.040M solution of the acid.
#6) Propoanoic acid, HC3H5O2, is an organic acid with a foul odor. The acid-
dissociation constant, Ka, for this acid is 1.4 x10-³M
a) write the dissociation equation for this acid
b) What is the pH and % dissociation for a 0.25M solution of this acid?
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QUESTION 9
Choose all acids:
ⒸH3PO4
Cu(NO3)2
☐ Ca3(PO4)2
NH3
KF
!
HCI
C₂H5OH
☐ H₂SO4
со
Li₂SO4
Click Save and Submit to save and submit. Click Save All Answers to save all answers.
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Direction: Explain the following scenarios why it resulted to increase or decrease the values
of pH, oxygen and Carbon dioxide.
Clinical Event
pH
02 co2
Rationale
1. Specimen was exposed to
air
2.Sealed specimen was left
at room temperature
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Answer
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Trial 1:
Initial pH= 3.92mL
Mass of KHP and Paper= 0.868g
Mass of paper= 0.357g
Mass of KHP= 0.511g
Trial 2:
Initial pH= 4.09ml
Mass of KHP and Paper= 0.870g
Mass of paper= 0.359g
Mass of KHP= 0.511g
1) find the volume at halfway point and the pH at halfway point of both trial
2) find the pKa of both trial and the mean pKa then use it to calculate Ka for KHP.
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weak ac
Calculate the percent dissoclation of acetic acid (CH,CO,H) In a 0.95 mM aqueous solutlon of the stuff. You may find some useful data In the ALEKS Data
resource.
Round your answer to 2 significant diglts.
x10
dlo
Explanation
Check
Privacy Accessibility
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esc
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"uonsanh stm
The hydroxide ion concentration of an aqueous solution of 0.532 M acetylsalicylic acid (aspirin), HC9H¬O4, is
[OH]=
M.
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Publisher:Cengage Learning
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ISBN:9780078021558
Author:Janice Gorzynski Smith Dr.
Publisher:McGraw-Hill Education
Chemistry: Principles and Reactions
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ISBN:9781305079373
Author:William L. Masterton, Cecile N. Hurley
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Elementary Principles of Chemical Processes, Bind...
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ISBN:9781118431221
Author:Richard M. Felder, Ronald W. Rousseau, Lisa G. Bullard
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