CHEM 230L _ exp 2. Recrystallization
docx
School
Chapman University *
*We aren’t endorsed by this school
Course
230L
Subject
Chemistry
Date
Jan 9, 2024
Type
docx
Pages
7
Uploaded by ProfMorningMouse32
CHEM 230L: Organic Chemistry I Lab
Chapman University
Experiment 2:
Purification of Organic Compounds Using
Recrystallization and ID by Melting Point
Intended Learning Outcomes
By completing this lab, we will:
Understand the relationship between compound structure, solubility, and temperature
and the role they play in recrystallization.
Learn how to purify impure solid organic compounds by the method recrystallization.
Be able to determine the purity of organic compounds and the identity of unknown
organic compounds by using melting point.
Introduction
Organic compounds that we use every day such as medicines, materials, food products,
and fuels are either synthesized in a lab or isolated from nature. When synthesized in the lab,
desired organic compounds are often mixed with impurities from side reactions or unreacted
starting material. Similarly, when organic compounds are isolated from nature they are often
found in complex mixtures.
To make optimal use of organic compounds, we need to be able to
isolate and purify them
There are many methods for purifying organic compounds and one of
the best ways to purify solid organic compounds is by using recrystallization.
Recrystallization utilizes solubility, which you explored in some detail during our first
experiment. In addition, recrystallization employs the fact that different compounds have
different degrees of solubility in the same solvent at different temperatures. An impure solid can
be dissolved in a solvent at high temperature while also dissolving the impurities present. To
successfully recrystallize an impure solid, the recrystallization solvent needs to be chosen
carefully. The desired organic compound must be insoluble at low temperatures and soluble at
high temperatures.
If the desired compound is too soluble at room or low temperature,
recrystallization may be very difficult and percent recovery will be low. Ideally, most impurities
will dissolve and stay in solution even at low temperatures. If the proper solvent is chosen, the
desired organic compound can be crystallized and recovered while leaving the impurity behind
in solution upon cooling down.
Pre-Lab Reading
The reading below needs to be completed before the start of lab.
1.
Lab textbook (Pavia, 6
th
edition): Technique 11 – Crystallization: Purification of Solids
Part A (Theory) - page 696-699
Part B (Semimicroscale Crystallization) - page 699-704
2.
Lab textbook (Pavia, 6
th
edition): Technique 9 – Physical Constants of Solids: The
Melting Point
Section 9.1 to 9.4 - page 678-680
CHEM 230L: Organic Chemistry I Lab
Chapman University
Pre-Lab Assignment (15 points)
Answer the following questions:
1.
If the solubility of a solid in acetone is 125 mg/mL, how many mL of acetone is needed to
dissolve 300 mg of the solid? (3 pts.)
300 mg
1 mL
=
2.4 mL
125 mg
2.
If 250 mg of impure solid is purified by recrystallization and 100 mg of the pure solid
crystals are recovered after cooling in an ice bath, what is the % recovery for this
recrystallization if the impure sample was 15% impurity by mass? (4 pts.)
100 - 15% impurity = 85% pure solid of 250 mg
0.85*250 mg = 212.5 mg
100mg/212.5mg = 0.471*100 = 47.1%
47.1%
3.
A student dissolves 124 mg of sulfanilamide in 95% ethanol/water by directly adding 25
mL of 95% ethanol/water to the sulfanilamide. The student then boils the solution until all
solid dissolves, cools the solution to room temperature, and then places the flask in an
ice bath for 20 minutes.
Upon removing the flask from the ice bath, they notice that no
crystals have formed.
What did the student do that resulted in no crystals forming?
Explain how this mistake caused the recrystallization to fail and describe how they might
be able to correct this mistake? (HINT: check the solubility of sulfanilamide at 0
o
C in 95%
ethanol/water). (4pts.)
At 0 C, the solubility of sulfanilamide in 95% ethanol/water is 14mg/mL. Given that the
student dissolves 124 mg of sulfanilamide, this means that he only needed about 9 mL of
95% ethanol/water (124 mg/14 mg = 8.86 mL). Since the student added an excessive
amount of 95% ethanol/water of 25 mL, it may have made it difficult for crystals to form.
To correct this mistake, they can restart the crystallization by adding a minimal initial
amount of solvent (1 mL) and adding minimal amounts throughout the dissolving process
until the solute has completely dissolved.
4.
Explain why the slow cooling of the hot solution with all of the sample dissolved is
necessary to increase the purity of the final crystals that are isolated. (4 pts.)
The slow cooling of the hot solution with all of the sample dissolved is necessary
because it disables the impurities from being included with the resulting crystals and
gives us a higher chance of obtaining pure crystals. It also gives the crystals more time
to collide with each other to give a higher yield of larger crystals and a greater purity.
Procedure
Purification of Organic Compounds Using Recrystallization
CHEM 230L: Organic Chemistry I Lab
Chapman University
A. Recrystallization of an impure organic compound.
1. Choose an impure sulfanilamide sample and add 300 mg of the impure sulfanilamide sample
into a 10 mL Erlenmeyer flask. It is if you cannot measure out exactly 300 mg so long as you are
close. Record the actual mass used for the recrystallization as well as a description of the
appearance of the impure sample (color, granule shape, etc.)
2. Add 1.00 mL of 95% ethanol to the Erlenmeyer flask and begin to heat the Erlenmeyer flask
slowly on a hot plate while swirling the flask periodically until the solution begins to boil gently.
3. Check to see if all the sulfanilamide has dissolved.
If solid sulfanilamide is still present, slowly
add more 95% ethanol (5-10 drops at time) to the solution while still swirling and heating until all
of it dissolves.
Make sure to swirl and wait 1-2 minutes before adding subsequent aliquots of
solvent (using minimal solvent will increase recovery).
4. Once all the sulfanilamide has dissolved, move the flask off the hotplate and onto the
benchtop and let it cool down to room temperature. Cover the flask to prevent particles in the air
from falling into the flask.
While waiting, prepare an ice bath in a small beaker.
5. After the flask has cooled to room temperature, add it to the ice bath carefully. Secure the
flask with a clamp to ensure that it does not fall into the bath.
Leave the flask in the ice bath for
a minimum of 20 minutes (leaving the flask for longer will slightly increase the amount of crystals
formed).
B.
Recovery of purified crystals.
1. Connect a vacuum flask to the vacuum in the fume hood using a thick vacuum hose.
Add a
Hirsch funnel fitted with a gray rubber filter adapter to the vacuum flask and turn on the vacuum
line. Pour the contents of the Erlenmeyer flask onto the Hirsch funnel and wash the crystals with
2 small aliquots of cold 95% ethanol in water. Note the color of the solution that is now in the
vacuum flask.
2. Cover the Hirsch funnel with a clean beaker to prevent particles in the air from getting onto
the crystals. Keep the crystals under vacuum for a minimum of 15 minutes to ensure that all
solvent has been removed from the crystals.
3. After the crystals are sufficiently dried, tare an empty weigh boat, and transfer all the crystals
from the Hirsch funnel onto the weigh boat. Record the mass of the recovered crystals and a
description of the crystals (color, shape, etc.).
C. Determining crystal purity by melting point.
1. Pack some of the isolated crystals into a small capillary tube by poking the open end of the
capillary tube into the crystals.
Drop the capillary tube through a hollow plastic pipette with the
closed end down to pack the precipitate tightly.
2. Follow the MelTemp procedure posted near the MelTemp machine to obtain the melting point
of your crystals. Record the melting point of your crystals.
Your preview ends here
Eager to read complete document? Join bartleby learn and gain access to the full version
- Access to all documents
- Unlimited textbook solutions
- 24/7 expert homework help
CHEM 230L: Organic Chemistry I Lab
Chapman University
Identification of an Unknown Organic Compound by Melting Point
1. Obtain an unknown sample and determine the melting point of this pure sample by using the
MelTemp machine. Record your unknown sample number and the observed melting point.
2. The unknown compound is either Benzoic Acid, Bezoin, Acetylsalicylic Acid, Succinimide, or
o-Toluic Acid.
Compare the melting point of your unknown compound with the literature melting
points of these five compounds on page 27 of the lab textbook (you may also look these values
up online).
3. Mix 25 mg of your unknown sample with 25 mg of the compound that has the closest melting
point to the experimentally determined melting point of your unknown.
4.Determine the melting point of the mixture and record this value
. If the melting point of this
mixture and that of your unknown is the same, then the unknown compound is the same as the
compound it was mixed with. If the melting point of the mixture decreases significantly (more
than 5
o
C) then try another compound to mix with your unknown with until the melting point
remains the same. Record the melting point of all tested mixtures
.
Post-Lab Assignment (40 points)
Data Analysis - Recrystallization
1.
Enter the mass of your impure Sulfanilamide sample used (1pt.) __________
2.
Describe the physical appearance of the impure sulfanilamide sample (2 pts.)
3.
What was the color of the solution that ended up in the vacuum flask (1 pt.)
4.
Enter the mass of your purified Sulfanilamide crystals (1 pt.) ________
5.
Describe the physical appearance of your purified sulfanilamide crystals (2 pts.)
CHEM 230L: Organic Chemistry I Lab
Chapman University
6.
Calculate the % recovery of pure Sulfanilamide from the impure sample that you used.
Assume that the impure sample had 10% impurity by mass. Show your calculations. (5
pts.)
% recovery ____________
7.
Enter the melting point range of your purified Sulfanilamide crystals (2 pt.) ________
8.
Based off your experimental melting point and the literature value for the melting point of
sulfanilamide, how pure do you think your Sulfanilamide crystals are? (3 pts.)
9.
Comment on the overall success of your recrystallization (did you have a good %
recovery, high purity, etc.). (3 pts.)
Data Analysis – Melting Points of an Unknown Compound
1.
Enter the ID of your unknown sample used. (1pt.) __________
2.
What is the melting point of your unknown sample? (2 pts.) __________
CHEM 230L: Organic Chemistry I Lab
Chapman University
3.
What was the first compound that you mixed unknown with to check for its identity and
why did you choose this compound? (3pts.)
4.
Enter the melting point of the mixture? (2 pts.) _________
5.
Did you mix your unknown with any other compounds? If so, what did you mix it with and
what was the melting point? (2 pts.)
6.
What was the identity of your unknown? Explain how you came to this determination. (3
pts.)
Additional Conceptual Question:
1. Suppose you wanted to recrystallize an impure sample of anthracene (shown below).
If you
could choose water, 95% ethanol (CH
3
CH
2
OH), or acetone as a recrystallization solvent, which
would you choose? Explain your answer. (4 pts.)
Anthracene
2. A student is attempting to recrystallize caffeine, but accidently add too much solvent. How can
the student remedy this situation if adding more caffeine is not an option? (3 pts)
Your preview ends here
Eager to read complete document? Join bartleby learn and gain access to the full version
- Access to all documents
- Unlimited textbook solutions
- 24/7 expert homework help
CHEM 230L: Organic Chemistry I Lab
Chapman University
Related Documents
Related Questions
LEARNING COMPETENCY:
Describe some simple reactions of organic compounds; combustion of organic fuels,
addition, condensation, and saponification of fats. (STEM_GC110Cllg-j-9).
SITUATION: You are a Grade 12 research student in your school and you are researching
on the potential of a certain plant that can be an additive in making a hand soap. Your task
is to write the Methodology of the Research by indicating the step-by-step procedure of
preparing a hand soap.
TASK: Research for a procedure in the preparation of hand soap. Write the materials and
procedures and answer the guide questions below.
GUIDE QUESTIONS:
1. What are other oils, besides coconut, that are used to make bath soaps?
2. Based on your research, why is potassium hydroxide used instead of sodium
hydroxide to make certain kinds of soaps?
3. Based on your research, what is a micelle?
4.
What is the chemical name of the most common fatty-acid molecule found in
coconut oil?
5. Describe the process of saponification of…
arrow_forward
Table 1. Physical Properties of Selected Compounds
Density
(g/mL)
Melting
point (°C)
Boiling
point (°C)
Substance
Acetanilide
1.22
114
304
Acetone
0.79
-95
56
Benzophenone
Bromoform
1.15
48
306
150
2.89
0.98
0.79
2.46
8
-2.4
2,3-Butanedione
t-Butyl alcohol
Cadmium nitrate 4H;O
Chloroform
Cyclohexane
p-Dibromobenzene
p-Dichlorobenzene
Diphenyl
Diphenylamine
Diphenylnethane
Ether, ethyl propyl
88
83
25
59
132
1.49
0.78
1.83
-63.5
6.5
86.9
61
81.4
219
1.46
53
70
53
27
174
0.99
255
1.16
302
265
1.00
1.37
-79
64
Hexane
0.66
69
Isopropyl alcohol
Lauric acid
0.79
0.88
1.63
-98
83
225
330
43
Magnesium nitrate 6H2O
Methyl alcohol
Methylene chloride
Naphthalene
a-Naphthol
Phenyl benzoate
Propionaldehyde
Sodium acetate 3H2O
Stearic acid
Thymol
Toluene
p-Toluidine
Zinc chloride
89
79
1.34
-98
-97
65
40.1
1.15
1.10
80
218
94
288
1.23
71
314
0.81
1.45
0.85
0.97
-81
58
48.8
123
70
291
232
52
0.87
0.97
2.91
-95
111
45
200
283
732
MAR
...
arrow_forward
1. Consider the solubility and boiling point of the following pair of compounds: n-butyl alcohol and diethyl ether. The boiling points for the compounds are 118 °C and 35 °C respectively. The solubility for both compounds is the same (8g/100g water). Explain this observation for (i) boiling point disparity; (ii) solubility similarity
a. H-bonds form in diethyl ether; n-butyl alcohol forms H-bonds in water
b. H-bonds form in n-butyl alcohol; diethyl ether forms H-bonds in water
c. H-bonds in n-butyl alcohol; Both compounds form H-bonds in water
d. Both compounds form H-bonds; Both compounds form H-bonds in water
2. Account for the bond angle differences between (i) H-C-H (109.5°) in methane and H-S-H (90°); H-C-H (109.5°) and H-O-H (107.5°) in water.
a. The H-S-H has two lone pairs; The H-O-H has two lone pairs
b. The H-S-H has no hybridization at p-orbitals; The H-O-H has two lone pairs
c. The H-S-H has two lone pairs; The H-O-H has no hybridization…
arrow_forward
Pls help ASAP on the whole questions and pls include all steps and calculations
arrow_forward
Please help me how to solve this question. Thank you very much
arrow_forward
When setting up an organic reaction for the first time, a concentration of reactants in tens to hundreds of micromolar range (mM) is often required. How much solvent (DCM) is required to prepare a solution that has a reactant concentration of 200mM?
a) 0.126mL
b) 1.26mL
c) 12.60mL
d) 126mL
e) None of the options is correct.
arrow_forward
Can you fill the rest of the chart please
arrow_forward
The disinfection of drinking water to control microbial contaminants can form
chemical disinfection byproducts. These compounds result from the reaction of chlorine
with naturally occurring organic matter (the dissolved molecules that give natural water the
yellow-greenish color). One class of disinfection byproducts is the malodorous and
unpalatable chlorophenols. 2,4-dichlorophenol is one compound of this class.
a) Calculate the vapor pressure p*L of 2,4-dichlorophenol at 60 °C using Tb and structural
information only
OH
.CI
M, = 163.0 g/mol
Tm = 43.7 °C
Tp = 213.0°C
%3D
%3D
%3D
arrow_forward
PAP Chemistry-2903012-42100P-1/ Le Chatelier's Principle/ Lesson 128
2. Zinc (Zn) granules react slowly with dilute hydrochloric acid (HCI), but much faster if the acid is concentrated.
Zn(s)
2HCI(aq)ZnCl2(aq) + H2(g)
Zinc + Hydrochloric Acid Zinc Chloride + Hydrogen
What causes the reaction to proceed faster with concentrated acid?
The concentrated hydrochloric acid causes more hydrogen gas to be produced.
The pressure of hydrogen gas molecules increases as concentration increases.
The concentrated hydrochloric acid molecules move faster than in dilute acid.
There are more collisions between the zinc and concentrated hydrochloric acid.
PREVIOU
arrow_forward
Justify the solubility of the samples in the corresponding solvent based on their structure.
Sample
water
5% NaHCO3
5% HCl
5%NaOH
Conc. H2SO4
ether
Aniline
n-butyl amine
Acetic acid
Phenol
cyclohexanol
2-Propanol
Benzoic acid
bromobenzene
Ethylene glycol
arrow_forward
26) Organic chemistry subject, please provide the correct solution for the following.
arrow_forward
REAGENT AMOUNTS In this section, you must record the actual amounts and volumes of reagens use
in the lab.
090
ml
Volume of methyl benzoate:
mmol
Equivalent to a molar amount of:
30 1.0
ml
Volume of concentrated Nitric acid (16 M = 16 mol/L):
Equivalent to a molar amount of :
mmol
Volume of concentrated Sulfurie acid acid (18 M = 18 mol/L):
3.0
ml
Equivalent to a molar amount of:
mmol
0.90 mL IL
=0.0009 L
lo0omL
arrow_forward
Please help me check if the information below is correct for both the types of reactions and the special rules or laws to predict predominant products for alcohols. If not please insert the correct information. Please make the information in jot notes.
TYPES OF REACTIONS ALCOHOL:
Dehydration: This is a reaction where an alcohol loses a water molecule to form an alkene. For example, when ethanol is treated with an acidic catalyst, such as sulfuric acid, it undergoes dehydration to form ethene (CH2=CH2) and water.
Oxidation: In this reaction, an alcohol is converted to either a carbonyl compound or a carboxylic acid. For example, primary alcohols can be oxidized to aldehydes or carboxylic acids, while secondary alcohols can be oxidized to ketones. Tertiary alcohols are not oxidized under normal conditions.
Esterification: This reaction involves the formation of an ester from an alcohol and a carboxylic acid in the presence of an acid catalyst. For example, when ethanol is…
arrow_forward
please answer all parts
arrow_forward
BASIC
PURE SUBSTANCE
MIXTURE
UNIT
DESCRIPTION
(color; physical state; transparent/translucent/opaque;
shiny/dull malleable/ductile, shape and size of particles
for solids; odor for organic series only)
SAMPLE OF
Соmpound
(for Pure
substances
Element
MATTER
only)
Homo-
Hetero-
atom,
molecule, or
formula unit
Metal
Nonmetal
Ionic
Covalent
Series 8. ORGANIC CHEMICALS
C,H14(1)
Нехane
HC,H3O2(aq)
C4H3O2(1)
ethyl acetate
C;H60(1)
Acetone
CH,O(1)
ethyl alcohol (ethanol)
C10H3O(s)
1-naphthol
C;H,O(1)
Benzaldehyde
C3H3O2(1)
methyl benzoate
C,H§O(I)
trans-cinnamaldehyde
arrow_forward
Draw structural formulas for organic products A and B in the window below.
Mg
H20
A
H3CC=CH2
ether
Br
• Draw only products having the organic portion of the original alkyl halide.
• Draw carbon-lithium bonds using the single bond tool. If a structure has a copper-lithium bond, do not draw the lithium.
• Separate products from different steps using the → sign from the drop-down menu.
arrow_forward
Hello can I get help with this question soon please?!? I am very confused and do not know where to start. An explanation leading to the correct answer would be helpful. Thank you!
arrow_forward
Oo.105.
Subject :- Chemistry
arrow_forward
Classify the compounds as either more soluble in water or more soluble in nonpolar organic solvent.
More soluble in water
CH, (CH₂),COO K+
(CH₂)₂CHCH₂CH₂
Answer Bank
CH,CON(CH,CH;)
More soluble in organic solvent
CH₂CH₂CH₂COOCH₂CH₂CH₂
CH₂CH₂CONHCH,
arrow_forward
▼
T
G
Part B
butylpropylamine
Express your answer as a condensed structural formula. Do not include bonds between atoms.
1.
6
H
= | ΑΣΦ
A chemical reaction does not occur for this question.
P Pearson
#1
|
Copyright © 2023 Pearson Education Inc. All rights reserved. Terms of Use Privacy Policy |
Permissions Contact Us
&
U
J
8
C
K
9
O
?
L
P
3
f12
{
+
+
79°F Mostly cloudy
ins
prt sc
delete
backspace
home
num
lock
ENG
8:21 PM
4/14/2023
end
7
home
pa
8
arrow_forward
SEE MORE QUESTIONS
Recommended textbooks for you

Macroscale and Microscale Organic Experiments
Chemistry
ISBN:9781305577190
Author:Kenneth L. Williamson, Katherine M. Masters
Publisher:Brooks Cole
Related Questions
- LEARNING COMPETENCY: Describe some simple reactions of organic compounds; combustion of organic fuels, addition, condensation, and saponification of fats. (STEM_GC110Cllg-j-9). SITUATION: You are a Grade 12 research student in your school and you are researching on the potential of a certain plant that can be an additive in making a hand soap. Your task is to write the Methodology of the Research by indicating the step-by-step procedure of preparing a hand soap. TASK: Research for a procedure in the preparation of hand soap. Write the materials and procedures and answer the guide questions below. GUIDE QUESTIONS: 1. What are other oils, besides coconut, that are used to make bath soaps? 2. Based on your research, why is potassium hydroxide used instead of sodium hydroxide to make certain kinds of soaps? 3. Based on your research, what is a micelle? 4. What is the chemical name of the most common fatty-acid molecule found in coconut oil? 5. Describe the process of saponification of…arrow_forwardTable 1. Physical Properties of Selected Compounds Density (g/mL) Melting point (°C) Boiling point (°C) Substance Acetanilide 1.22 114 304 Acetone 0.79 -95 56 Benzophenone Bromoform 1.15 48 306 150 2.89 0.98 0.79 2.46 8 -2.4 2,3-Butanedione t-Butyl alcohol Cadmium nitrate 4H;O Chloroform Cyclohexane p-Dibromobenzene p-Dichlorobenzene Diphenyl Diphenylamine Diphenylnethane Ether, ethyl propyl 88 83 25 59 132 1.49 0.78 1.83 -63.5 6.5 86.9 61 81.4 219 1.46 53 70 53 27 174 0.99 255 1.16 302 265 1.00 1.37 -79 64 Hexane 0.66 69 Isopropyl alcohol Lauric acid 0.79 0.88 1.63 -98 83 225 330 43 Magnesium nitrate 6H2O Methyl alcohol Methylene chloride Naphthalene a-Naphthol Phenyl benzoate Propionaldehyde Sodium acetate 3H2O Stearic acid Thymol Toluene p-Toluidine Zinc chloride 89 79 1.34 -98 -97 65 40.1 1.15 1.10 80 218 94 288 1.23 71 314 0.81 1.45 0.85 0.97 -81 58 48.8 123 70 291 232 52 0.87 0.97 2.91 -95 111 45 200 283 732 MAR ...arrow_forward1. Consider the solubility and boiling point of the following pair of compounds: n-butyl alcohol and diethyl ether. The boiling points for the compounds are 118 °C and 35 °C respectively. The solubility for both compounds is the same (8g/100g water). Explain this observation for (i) boiling point disparity; (ii) solubility similarity a. H-bonds form in diethyl ether; n-butyl alcohol forms H-bonds in water b. H-bonds form in n-butyl alcohol; diethyl ether forms H-bonds in water c. H-bonds in n-butyl alcohol; Both compounds form H-bonds in water d. Both compounds form H-bonds; Both compounds form H-bonds in water 2. Account for the bond angle differences between (i) H-C-H (109.5°) in methane and H-S-H (90°); H-C-H (109.5°) and H-O-H (107.5°) in water. a. The H-S-H has two lone pairs; The H-O-H has two lone pairs b. The H-S-H has no hybridization at p-orbitals; The H-O-H has two lone pairs c. The H-S-H has two lone pairs; The H-O-H has no hybridization…arrow_forward
- Pls help ASAP on the whole questions and pls include all steps and calculationsarrow_forwardPlease help me how to solve this question. Thank you very mucharrow_forwardWhen setting up an organic reaction for the first time, a concentration of reactants in tens to hundreds of micromolar range (mM) is often required. How much solvent (DCM) is required to prepare a solution that has a reactant concentration of 200mM? a) 0.126mL b) 1.26mL c) 12.60mL d) 126mL e) None of the options is correct.arrow_forward
- Can you fill the rest of the chart pleasearrow_forwardThe disinfection of drinking water to control microbial contaminants can form chemical disinfection byproducts. These compounds result from the reaction of chlorine with naturally occurring organic matter (the dissolved molecules that give natural water the yellow-greenish color). One class of disinfection byproducts is the malodorous and unpalatable chlorophenols. 2,4-dichlorophenol is one compound of this class. a) Calculate the vapor pressure p*L of 2,4-dichlorophenol at 60 °C using Tb and structural information only OH .CI M, = 163.0 g/mol Tm = 43.7 °C Tp = 213.0°C %3D %3D %3Darrow_forwardPAP Chemistry-2903012-42100P-1/ Le Chatelier's Principle/ Lesson 128 2. Zinc (Zn) granules react slowly with dilute hydrochloric acid (HCI), but much faster if the acid is concentrated. Zn(s) 2HCI(aq)ZnCl2(aq) + H2(g) Zinc + Hydrochloric Acid Zinc Chloride + Hydrogen What causes the reaction to proceed faster with concentrated acid? The concentrated hydrochloric acid causes more hydrogen gas to be produced. The pressure of hydrogen gas molecules increases as concentration increases. The concentrated hydrochloric acid molecules move faster than in dilute acid. There are more collisions between the zinc and concentrated hydrochloric acid. PREVIOUarrow_forward
- Justify the solubility of the samples in the corresponding solvent based on their structure. Sample water 5% NaHCO3 5% HCl 5%NaOH Conc. H2SO4 ether Aniline n-butyl amine Acetic acid Phenol cyclohexanol 2-Propanol Benzoic acid bromobenzene Ethylene glycolarrow_forward26) Organic chemistry subject, please provide the correct solution for the following.arrow_forwardREAGENT AMOUNTS In this section, you must record the actual amounts and volumes of reagens use in the lab. 090 ml Volume of methyl benzoate: mmol Equivalent to a molar amount of: 30 1.0 ml Volume of concentrated Nitric acid (16 M = 16 mol/L): Equivalent to a molar amount of : mmol Volume of concentrated Sulfurie acid acid (18 M = 18 mol/L): 3.0 ml Equivalent to a molar amount of: mmol 0.90 mL IL =0.0009 L lo0omLarrow_forward
arrow_back_ios
SEE MORE QUESTIONS
arrow_forward_ios
Recommended textbooks for you
- Macroscale and Microscale Organic ExperimentsChemistryISBN:9781305577190Author:Kenneth L. Williamson, Katherine M. MastersPublisher:Brooks Cole

Macroscale and Microscale Organic Experiments
Chemistry
ISBN:9781305577190
Author:Kenneth L. Williamson, Katherine M. Masters
Publisher:Brooks Cole