IntroAcids - Group Report Template
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Acids, Bases, and pH Group Report Include your name and your lab partner’s name and submit the same file to both partners’ Canvas accounts if and only if both of you collaborated on this report. Do not modify or remove the question text. Do not use bold font in your answers. Do not use red text in your answers. Module 1 Acid Strength 1.
Include a copy of the plot of log(conductivity) vs. pH. Table 1. Log(conductivity) vs. pH. 2.
Describe the trend your data shows between log(conductivity) and pH does your data show. The data shows a downward trend between log(conductivity) and pH. As pH increases, log(conductivity) decreases. 3.
Which of the acids in this module are strong acids? You can look up a list of common strong acids in almost any chemistry resource
. Sulfuric acid, Nitric acid, HC. 4.
Explain why you should expect most strong acids to give the same pH as each other if they are prepared at the same concentration.
If the strong acids have the same molarity, they will have the same concentration of H
+
ions, therefore, the same pH.
5.
Your measurement sulfuric acid in water should have a slightly lower pH than other strong acids. What is different about sulfuric acid that would explain this? (
Hint: Look at the molecular formula of sulfuric acid.) Unlike many of the other acids, sulfuric acid has two ionizable hydrogens for every molecule, giving it a low pH. Module 2 Acids, Bases, and Salts 6.
Compare the indicated pH of each species in module 2 to that of water and indicate for each of the first 12 species, which are acidic, basic, and neutral compared to water. The acidic species are HC
2
H
3
O
2
, Fe(NO
3
)
3
, HNO
3
, and Al(NO
3
), the basic species are NaOH, NaC
2
H
3
O
2
, Na
2
CO
3
, NaHCO
3
, Na
3
PO
4
, and NH
4
OH, the neutral species are H
2
O and NaCl. Similarly, some bases are easily identified by the presence of the hydroxide ion directly in their formula. 7.
Many acidic compounds have a loosely bound hydrogen atom that can be easily donated as an H
+
ion. a.
Which of the Module II compounds fit(s) this description? Some of the module II compounds that fit this description are HNO
3
and Al(NO
3
)
3
. Both compounds are strong acids and will easily donate H+ ions. On the other hand, other acidic compounds such as HC
2
H
3
O
2
are weak acids, or acidic salts such as Fe(NO
3
)
3 and Al(NO
3
)
3 are acidic salts and do not give up H+ ions as easily. b.
Write a chemical reaction for one of these compounds showing how it can lower the pH of water. HNO
3 (g) + H
2
O (l) →
H
3
O
+
(aq) + NO
3
-
(aq)
8.
Many basic compounds have a hydroxide ion (OH
−
) as part of the formula, which becomes dissociated and part of the water solution when the compound is dissolved in water. a.
Which of the Module II compounds fit(s) this description? Some of the Module II compounds that fit this description are NaOH, NaC
2
H
3
O
2
, Na
2
CO
3
, and NaHCO
3
. b.
Write a chemical reaction for one of these compounds showing how it can raise the pH of water. NaHCO
3
_ (s) + H
2
O (l) → Na
+ (aq) + HCO
3
- (aq)
9.
Some compounds can lower the pH of water even without having a hydrogen in the formula. a.
Which of the Module II compound(s) fit(s) this description? NaCl would fit this description.
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An aqueous solution contains 0.393 M hydrofluoric acid.
Calculate the pH of the solution after the addition of 2.07x102 moles of sodium hydroxide to 150 mL of this solution.
(Assume that the volume does not change upon adding sodium hydroxide).
pH =
Use the References to access important values if needed for this question.
Submit Answer
Retry Entire Group 8 more group attempts remaining
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Question 10
Classify the given compound/ ion by writing: A (if acid), B (if base), or C (if amphoteric)
(Note: case & space sensitive)
H30*
A Moving to another question will save this response.
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SHOW WORK. Perform the following calculations &
determinations for this solution.
8.99 x 10-7 M OH-
Calculate the molarity of H*. Enter the value in the first blank (with proper sig figs) and
the exponent with proper sign in the second blank.
pH:
x 10
Calculate the pH for this solution and report the result to 2 decimal places.
M
Relative acidity:
Is this solution acidic, basic, or neutral? Enter the term that applies.
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Which product contains a strong base that would most likely completely dissolve in water?
O drain cleaner
ammonia
baking soda
antacid
Next
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Correction: pH=-log[H+] *
Chemistry. The pH of a solution is a measure of the molar concentration of hydrogen
ions, H* in moles per liter, in the solution, which means that it is a measure of the acidity
or basicity of the solution.
The letters pH stand for "power of hydrogen", and the numerical value as defined as
pH =
Very acid corresponds to pH values near 1,
Neutral corresponds to a pH near 7 (pure water), and
Very basic corresponds to values near 14.
If the wine has an approximate hydrogen ion concentration of 5.01×104 , calculate its
pH value.
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Use the change of base formula with base 2 to evaluate the expression. Answer as integer. log_(64)(8)
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SHOW WORK. Perform the following calculations & determinations for this solution.
6.84 x 10 2 M OH
Calculate the molarity of H. Enter the value in the first blank (with proper sig figs) and the exponent with proper sign in the second blank.
x 10
M.
Calculate the pH for this solution and report the result 5 2 decimal places.
pH:
Is this solution acidic, basic, or neutral? Enter the term that applies.
Relative acidity:
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I
Part 2 Procedure, Data & Analysis:
Recall: The amount of ionization or dissociation of ions
determines the strength of an acid or base. The
concentration of [H3O+], hydronium ion and [OH].
hydroxide ion, can be used to calculate pH and pOH as
shown on the diagram here:
Note: we use [H3O+] and [H*] interchangeably.
1. Click on Water Solution, Graph View, Probe Tool.
Insert the
probe in the
water.
Notice that
given before
2. Fill in the
hydronium
the
the pH.
3. Use the
the pOH.
Equilibrium Concentration (mol/L)
10²
10¹
10⁰
10¹
10
10ª
104
10%
10⁰
107
10⁰
pH: 7.00
2 H₂O H3O+ + OH-
H
1L
4
[H₂O*]
or [H*]
pH
(OH)-1x10¹4
H
(H)-1x10-¹4
-LOUISE
POH-14-PH
pH-14-POH
Show work:
[OH]
LIO - امي
the initial concentration of the solution is
any ionization or dissociation takes place.
4. Did your answer to # 2 match the pH given in the simulation?
5. Is the answer to #3 equal to: (14 - pH)?
6. Is the solution an acid, a base or neutral, based upon the calculated pH?
Attach notebook paper to show…
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- Part A
State whether each of the following is acidic, basic, or neutral.
Drag the appropriate items to their respective bins.
Reset Help
fruit punch, pH 3.27
bile, pH 7.96
orange juice, pH 3.5
saltine crackers, pH 7.9
bleach, pH 11.9
pineapples, pH 3.6
Acidic
Basic
Neutral
Submit
Request Answer
Provide Feedback
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page-General Chemistry x
6 Pearson MyLab and Mastering x
I Course Home
Acid and Base lonization Const X
envellum.ecollege.com/course.html?courseld3D17238291&OpenVellumHMAC=b5d99ca5abc343615f7c3fe5e11934a4#10001
Beta
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Please plot this in excel as a smooth line scatter chart with the Volume on the X axis and the pH on the Y
title it Volume vs pH
title the both axis
Volume of sodium hydroxide
pH
0.00
5.00
1.00
5.96
2.00
6.26
3.00
6.41
4.00
6.64
5.00
6.77
6.00
6.88
7.00
6.97
8.00
7.07
9.00
7.16
10.00
7.25
11.00
7.35
12.00
7.43
13.00
7.54
14.00
7.65
15.00
7.77
16.00
7.91
17.10
8.12
17.20
8.15
17.30
8.17
17.40
8.20
17.50
8.23
17.60
8.26
17.70
8.28
17.8
8.31
17.9
8.34
18.0
8.38
18.1
8.45
18.2
8.48
18.3
8.53
18.4
8.60
18.5
8.66
18.6
8.76
18.7
8.88
18.8
9.03
18.9
9.22
19.0
9.39
19.1
9.58
19.2
9.70
19.3
10.00
19.4
10.22
19.5
10.46
19.6
10.60
19.7
10.72
19.8
10.81
19.9
10.91
20.9
11.42
21.9
11.63
22.9
11.77
23.9
11.88
24.9
11.97
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The pH of a 0.1 M weak acid HA is 3.4.
a. What is the percent dissociation?
b. Solve for the acid dissociation constant.
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A student at CHEM 146 lab found that a 0.486 M unknown weak base is 15.46% ionized. What is the Kb value of this weak base?
Report your answer with four decimals. Enter numbers only; do not enter units.
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Question 12
Determine the reaction of the salt in aqueous soln. Write A (if acidic),_B (if basic).or C (if neutral)
(Note: case & space sensitive)
AIBT3
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. ACIDITY AND ALKALINITY
Place 4 pieces each of blue and red litmus papers on a dry watch glass. Moisten the tip of the stirring rod with the solutions below using only one solution at a time. Rinse the stirring rod before touching the next solution. Touch the litmus paper with the stirring rod.
based on the expirement above, Classify each specified below, if it is as strong acid , weak acid, strong base or weak base based on the degree of the change in color of the litmus paper.
dilute HCl
dilute acetic acid
dilute NH4Cl
aniline
Give a general statement as to the difference in the degree of acidity and alkalinity between organic and inorganic compounds.
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Complete the table below. Be sure each of your answer entries has the correct number of significant digits. You may assume the temperature is 25 °C.
conjugate acid
conjugate base
formula
K.
formula
HCN
-10
49 x 10
NH,
-5
1.8 x 10,
CH, NH,
-4
4.4 x 10
Fxplanation
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True or False. Write TRUE if the statement is correct and FALSE if it is incorrect.
___________1. The acidity of the solution is higher with higher pH.
___________2. pH is the measure of the alkalinity of solution.
___________3. The strength of acids and bases depends on their ionization constant. ___________4. The higher Ka or Kb, the stronger is the acid or base.
___________5. Given HA yields H+ + A-, its = [??] /[?+][?−]
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True or False. Write TRUE if the statement is correct and FALSE if it is incorrect.
___________1. The acidity of the solution is higher with higher pH.
___________2. pH is the measure of the alkalinity of solution.
___________3. The strength of acids and bases depends on their ionization constant.
___________4. The higher Ka or Kb, the stronger is the acid or base.
___________5. Given HA yields H+ + A-, its .
___________6. pH = log [H+]
___________7. The addition of common ion in a solution decreases solubility.
___________8. In determining pH, the [H-] is used.
___________9. Given pOH = -log [OH-], [OH-] = 10pOH.
___________10. The sum of the acidity and alkalinity of a solution is equal to zero.
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Complete the table below. Be sure each of your answer entries has the correct number of significant digits. You may assume the temperature is 25 °C.
conjugate acid
conjugate base
K.
K,
formula
formula
H,BO,
5.8 x 10 10
HSO,
0.012
HONH,
1.1 x 10
aplanation
Check
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Learning Goal:
Another way to express acid strength is by using pk
To understand the relation between the strength of
an acid or a base and its pK, and pK, values.
The degree to which a weak acid dissociates in
solution is given by its acid-ionization constant, K.
For the generic weak acid. HA.
pk. =
log K.
Another way to express base strength is by using pk
log K
HA(ag) A (aq) + H'(aq)
and the acid-ionization constant is given by
Part A
IA H
HA
K.
Similarty, the degree to which a weak base reacts
with HO in solution is given by its base-ionization
constant, K. For the generic weak base, B.
A new potential heart medicine, code named X-281, is being tested by a pharmaceutical company.
Pharma pill. As a research technician at Pharma-pil you are told that X-281 is a monoprotic weak acid, but
because of security concerns, the actual chemical formula must remain top secret. The company is
Interested in the drug's K, value because only the dissociated form of the chemical is active in…
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Use the References to access important values if needed for this question.
An aqueous solution contains 0.374 M nitrous acid.
Calculate the pH of the solution after the addition of 2.75x10-2 moles of potassium hydroxide to 225 mL of this
solution.
(Assume that the volume does not change upon adding potassium hydroxide).
pH =
Submit Answer
Retry Entire Group 6 more group attempts remaining
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An aqueous solution contains 0.306 M nitrous acid.
Calculate the pH of the solution after the addition of 1.80x10-2 moles of potassium hydroxide to 155 mL of this
solution.
(Assume that the volume does not change upon adding potassium hydroxide)
pH =
Submit Answer
[Review Topies]
(References)
Use the References to access important values if needed for this question.
Submit Answer
Retry Entire Group 9 more group attempts remaining
An aqueous solution contains 0.386 M hypochlorous acid.
Calculate the pH of the solution after the addition of 2.40x102 moles of sodium hydroxide to 125 mL of this
solution.
(Assume that the volume does not change upon adding sodium hydroxide)
pH =
Retry Entire Group 9 more group attempts remaining
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[References]
This question has multiple parts. Work all the parts to get the most points.
Use the References to access important values if needed for this question.
The pK of a solution is defined by the equation:
eq
pK, = =log K,
Where:
K = acid dissociation constant
req
NOTE: Write Ka as Ka for the answers below.
req
a Use the rules for logarithms and exponents to solve for K. in terms of pK.
K =
2req
Submit
2req
2req
Submit Answer
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[Review Topics]
[References]
Use the References to access important values if needed for this question.
1. The formula for the conjugate base of HNO2 is
2. The formula for the conjugate acid of CH3COO is
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Table 2. pH Measurement of various substances using paper indicators and pH meter and the corresponding [H], pOH & [OH-].
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1. Consider Lewis structure for methane (CH4).
a. If methane were to behave as an acid (if possible), draw the Lewis structure of its
resulting conjugate base.
b. Reflecting on your answer for Part A and using the three acid-base models above,
would you predict the conjugate base would form? (Does this situtation make
sense)?
c. If methane were to behave as a base (if possible), draw the Lewis structure of its
resulting conjugate acid.
d. Reflecting on your answer for Part A and using the three acid-base models above,
would you predict the conjugate acid would form? (Does this situtation make
sense)?
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Related Questions
- An aqueous solution contains 0.393 M hydrofluoric acid. Calculate the pH of the solution after the addition of 2.07x102 moles of sodium hydroxide to 150 mL of this solution. (Assume that the volume does not change upon adding sodium hydroxide). pH = Use the References to access important values if needed for this question. Submit Answer Retry Entire Group 8 more group attempts remaining Previous Email Instructor Next Save andarrow_forwardA session.masteringchemistry.com/myct/itemView?assignmentProblemID=1557285948&offset=nextarrow_forwardForce Completion This test can be saved and resumed later. Your answers are saved automatically. Question Completion Status: A Moving to another question will save this response. Question 10 Classify the given compound/ ion by writing: A (if acid), B (if base), or C (if amphoteric) (Note: case & space sensitive) H30* A Moving to another question will save this response.arrow_forwardSHOW WORK. Perform the following calculations & determinations for this solution. 8.99 x 10-7 M OH- Calculate the molarity of H*. Enter the value in the first blank (with proper sig figs) and the exponent with proper sign in the second blank. pH: x 10 Calculate the pH for this solution and report the result to 2 decimal places. M Relative acidity: Is this solution acidic, basic, or neutral? Enter the term that applies.arrow_forwardWhich product contains a strong base that would most likely completely dissolve in water? O drain cleaner ammonia baking soda antacid Next Save and Exit Mark this and return .com/ContentViewers/AssessmentViewer/Activit.arrow_forwardCorrection: pH=-log[H+] * Chemistry. The pH of a solution is a measure of the molar concentration of hydrogen ions, H* in moles per liter, in the solution, which means that it is a measure of the acidity or basicity of the solution. The letters pH stand for "power of hydrogen", and the numerical value as defined as pH = Very acid corresponds to pH values near 1, Neutral corresponds to a pH near 7 (pure water), and Very basic corresponds to values near 14. If the wine has an approximate hydrogen ion concentration of 5.01×104 , calculate its pH value.arrow_forwardUse the change of base formula with base 2 to evaluate the expression. Answer as integer. log_(64)(8)arrow_forwardSHOW WORK. Perform the following calculations & determinations for this solution. 6.84 x 10 2 M OH Calculate the molarity of H. Enter the value in the first blank (with proper sig figs) and the exponent with proper sign in the second blank. x 10 M. Calculate the pH for this solution and report the result 5 2 decimal places. pH: Is this solution acidic, basic, or neutral? Enter the term that applies. Relative acidity:arrow_forwardI Part 2 Procedure, Data & Analysis: Recall: The amount of ionization or dissociation of ions determines the strength of an acid or base. The concentration of [H3O+], hydronium ion and [OH]. hydroxide ion, can be used to calculate pH and pOH as shown on the diagram here: Note: we use [H3O+] and [H*] interchangeably. 1. Click on Water Solution, Graph View, Probe Tool. Insert the probe in the water. Notice that given before 2. Fill in the hydronium the the pH. 3. Use the the pOH. Equilibrium Concentration (mol/L) 10² 10¹ 10⁰ 10¹ 10 10ª 104 10% 10⁰ 107 10⁰ pH: 7.00 2 H₂O H3O+ + OH- H 1L 4 [H₂O*] or [H*] pH (OH)-1x10¹4 H (H)-1x10-¹4 -LOUISE POH-14-PH pH-14-POH Show work: [OH] LIO - امي the initial concentration of the solution is any ionization or dissociation takes place. 4. Did your answer to # 2 match the pH given in the simulation? 5. Is the answer to #3 equal to: (14 - pH)? 6. Is the solution an acid, a base or neutral, based upon the calculated pH? Attach notebook paper to show…arrow_forward- Part A State whether each of the following is acidic, basic, or neutral. Drag the appropriate items to their respective bins. Reset Help fruit punch, pH 3.27 bile, pH 7.96 orange juice, pH 3.5 saltine crackers, pH 7.9 bleach, pH 11.9 pineapples, pH 3.6 Acidic Basic Neutral Submit Request Answer Provide Feedback P Pearson Copyright © 2021 Pearson Education Inc. All rights reserved. | Terms of Use | Privacy Policy | Permissions | Contact Us | MacBook Air DI DD 80 888 F8 F9 F10 F11 F5 F6 F7 F3 F4 & #3 2$ 3 6. 7 8. { E R Y U K ... ーの エarrow_forwardEdit History Bookmarks Profiles Tab Window Help View page-General Chemistry x 6 Pearson MyLab and Mastering x I Course Home Acid and Base lonization Const X envellum.ecollege.com/course.html?courseld3D17238291&OpenVellumHMAC=b5d99ca5abc343615f7c3fe5e11934a4#10001 Betaarrow_forwardPlease plot this in excel as a smooth line scatter chart with the Volume on the X axis and the pH on the Y title it Volume vs pH title the both axis Volume of sodium hydroxide pH 0.00 5.00 1.00 5.96 2.00 6.26 3.00 6.41 4.00 6.64 5.00 6.77 6.00 6.88 7.00 6.97 8.00 7.07 9.00 7.16 10.00 7.25 11.00 7.35 12.00 7.43 13.00 7.54 14.00 7.65 15.00 7.77 16.00 7.91 17.10 8.12 17.20 8.15 17.30 8.17 17.40 8.20 17.50 8.23 17.60 8.26 17.70 8.28 17.8 8.31 17.9 8.34 18.0 8.38 18.1 8.45 18.2 8.48 18.3 8.53 18.4 8.60 18.5 8.66 18.6 8.76 18.7 8.88 18.8 9.03 18.9 9.22 19.0 9.39 19.1 9.58 19.2 9.70 19.3 10.00 19.4 10.22 19.5 10.46 19.6 10.60 19.7 10.72 19.8 10.81 19.9 10.91 20.9 11.42 21.9 11.63 22.9 11.77 23.9 11.88 24.9 11.97arrow_forwardarrow_back_iosSEE MORE QUESTIONSarrow_forward_ios
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