Chapter 9
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Chapter 09 Assignment
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Chapter 09 Assignment
Due: 12:00am on Tuesday, December 12, 2023
You will receive no credit for items you complete after the assignment is due. Grading Policy
Chapter 9 Reading Question 1
Part A
Identify the pair of substances that would be soluble and form a solution when mixed. Hint 1.
A solute and solvent having the same polarity will mix together: "like dissolves like." The attractions between the solute and solvent must be strong
enough to overcome the solute-solute attractions and the solvent-solvent attractions. See Section 9.1.
ANSWER:
Correct
Animation - Dissolution of NaCl in water
The process by which a substance dissolves in a solvent to form a solution is called dissolution
. When the specific solvent is water, dissolution may also be
referred to as hydration. For an ionic compound, the dissolution (dissolving in the solvent) takes place by forming the solvated ions.
Watch the animation showing NaCl dissolving in water
to learn about the dissolution of a salt, such as sodium chloride (
), in water.
is an ionic solid that has and ions held together by electrostatic forces of attraction known as ionic forces. When is added to water, the
and ions are surrounded by the polar water molecules as the attractive interactions with water molecules overcome the ionic forces of the crystal lattice.
These solvated ions are dispersed throughout the solution.
You may have heard of dipole-dipole interactions. There are also ion-dipole interactions. Ion-dipole interactions exist between the partial charge on a polar
molecule and the charge on an ion. Ion-dipole interactions are important for the hydrolysis of a salt, such as , whereas dipole-dipole interactions are
important to dissolve polar compounds such as acetone.
Part A
Identify the type of interactions involved in each of the following processes taking place as sodium chloride (
) dissolves in water.
Drag the appropriate items to their respective bins.
H
2
O solvent and I
2
solute H
2
O solvent and HCl solute H
2
O solvent and CCl
4
solute CCl
4
solvent and NaCl solute
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Chapter 09 Assignment
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Hint 1. The steps of the dissolution process
For an ionic solid like to dissolve in water, three processes must occur: 1. The water (solvent) molecules must be separated from one another to make room for the ions of .
2. The ions in the lattice (solute) must be separated from one another.
3. The forces of attraction between the ions of and the water molecules must be formed so that the ions are solvated.
Hint 2. Identify the different interactions involved
The process of dissolving the solute in the solvent water involves three main types of interactions: solute-solute interactions, solute-solvent
interactions, and solvent-solvent interactions.
Define each of the following interactions between the ions of and the molecules of water, .
Match the words in the left column to the appropriate blanks in the sentences on the right. Make certain each sentence is complete before
submitting your answer.
ANSWER:
Hint 3. Classify interactions by the type of intermolecular force
If you look at the molecular-level picture of events that occur when an ionic compound like is dissolved in a polar solvent like water, you can see
that intermolecular interactions between the ions of and those between water molecules must be broken, and intermolecular interactions
between and and water molecules must form. Given that is the solute and water is the solvent, classify the types of interactions that
occur according to the forces of attraction involved.
Drag the appropriate items to their respective bins.
ANSWER:
ANSWER:
Reset
Help
1. The
solute-solute
interaction is present between the ions of NaCl.
2. The
solvent-solvent
interaction is present between the water molecules.
3. The
solute-solvent
interaction is present between the ions of NaCl and the water molecules.
Reset
Help
solute-solvent interaction
solute-solute interaction
solvent-solvent interaction
Ion-dipole attraction
Ion-ion attraction
Dipole-dipole attraction
12/11/23, 11:52 PM
Chapter 09 Assignment
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3/23
Correct
The process of dissolution (a solute dissolving in a solvent) depends upon the separation of solute particles, the separation of solvent molecules, and
the formation of the attractive interaction between the solute particles and the solvent molecules.
Nature of a substance and its solubility in water
As a general rule, like dissolves like. There are stronger interactions between a solute and solvent if they have similar intermolecular forces.
For water, the intermolecular forces between the molecules are dipole-dipole forces and hydrogen bonding. For ionic compounds to dissolve in water, ion-dipole
interactions must occur, whereas for a polar covalent compound to dissolve in water, dipole-dipole interactions must occur between the molecules of the compound
and the water molecules. Compounds that cannot form ion-dipole or dipole-dipole interactions are generally insoluble in water. Such compounds have covalent
bonds and are nonpolar in nature.
Part B
Five different substances are given to you to be dissolved in water. Which substances are most likely to form a solution when placed in water?
Check all that apply.
Hint 1. How to approach the problem
To identify the substances that are most likely to to form a solution when placed in water, first determine which substances will have strong
intermolecular interactions with water.
Water is a polar compound, and the intermolecular forces that exist between water molecules are dipole-dipole forces and hydrogen bonding. Ionic
substances are most likely to form ion-dipole bonds with water, whereas polar compounds are most likely to form dipole-dipole or hydrogen bonds with
water.
Identify whether the different substances given to you are ionic, polar, or nonpolar. The ionic and polar substances have similar properties to those of
water and are likely to have strong solute-solvent interactions with water, resulting in solution formation.
Hint 2. Identify ionic substances
An ionic substance is formed between a positively charged cation and a negatively charged anion. Ionic substances are generally formed from metal
and nonmetal atoms, with the metal atoms forming the cations and the nonmetal atoms forming the anions.
Which of the given substances are ionic in nature?
Check all that apply.
ANSWER:
Reset
Help
interactions between the water
molecules
interactions involving dipole-dipole
attractions
interactions between the ions of
sodium chloride
interactions involving ion-ion
attractions
interactions formed between the
sodium ions and the oxygen atoms of
water molecules
interactions formed during hydration
Solvent-solvent interactions
Solute-solute interactions
Solute-solvent interactions
12/11/23, 11:52 PM
Chapter 09 Assignment
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Hint 3. Identify polar substances
Polar compound contain two atoms with different electronegativites. Electronegativity values in the periodic table generally increase from the left to right
and from the bottom to top of the periodic table.
Which of the given substances are polar in nature?
Check all that apply.
ANSWER:
ANSWER:
Correct
Solution formation is favored by an increase in disorder of the system. Unless solute-solute and solvent-solvent interaction are strong relative to
solute-solvent interactions, a solution will form when an ionic substance is added to water. For a nonpolar substance, the solute-solvent interactions
are weak relative to solute-solute and solvent-solvent interactions, and therefore it will not form a solution in water.
Solute-solvent interactions
Forces between two different molecules or substance can be analyzed similarly to forces between two of the same molecule or formula units of a compound. When
an ionic compound dissolves in water, there are ion-dipole forces between the positively charged ions and water, as well as the negatively charged ions and water.
A polar molecule may interact by dipole-dipole forces or hydrogen bonding with water. While two nonpolar substances may only interact through dispersion forces.
Part C
Classify the substances according to the strongest
solute-solvent interaction that will occur between the given substances and water as the solute dissolves.
Drag the appropriate items to their respective bins.
Hint 1. How to approach the problem
To determine the solute-solvent interactions that will occur, first determine whether each of the four substances given is polar or ionic. Then, classify the
interaction possible for those type of species.
potassium fluoride, toluene, hexane, propanol, sodium fluoride, sodium fluoride, toluene, hexane, propanol, potassium fluoride, sodium fluoride, potassium fluoride, hexane, propanol, toluene,
12/11/23, 11:52 PM
Chapter 09 Assignment
https://session.masteringchemistry.com/myct/assignmentPrintView?assignmentID=11885467
5/23
For example, to determine the solute-solvent interactions of the solute and the solvent water, you would first identify that is an ionic
compound. The and ions of can attract the dipoles of the water molecule. Therefore, the dominating intermolecular forces involved
when dissolves in water are the ion-dipole forces.
Hint 2. Define the different types of intermolecular forces
Define the following intermolecular forces of attraction.
Match the words in the left column to the appropriate blanks in the sentences on the right. Make certain each sentence is complete before
submitting your answer.
ANSWER:
Hint 3. Determine the relative strength of the intermolecular forces
Consider that dispersion forces are found in all the substances. Dipole-dipole forces add to dispersion forces in polar molecules. Polar molecules that
contain a hydrogen atom and an electronegative atom such as , , or show hydrogen bonding, a type of really strong dipole-dipole interaction.
These intermolecular forces are usually weaker than ionic or covalent bonds.
Given this information, arrange the intermolecular forces according to their strength.
Rank the intermolecular forces from strongest to weakest. To rank items as equivalent, overlap them.
ANSWER:
Reset
Help
1. The ion-dipole force
is the electrostatic force of attraction between a charged ion and a partially
charged species.
2. The dipole-dipole force
is the intermolecular force of attraction between permanent dipoles in
polar molecules.
3. Hydrogen bonding
is a special type of intermolecular force of attraction between a hydrogen
atom in a polar bond and an electronegative atom (usually an O, N, or F atom in another molecule).
4. The dispersion force
is the momentary electrostatic force of attraction present in all the
substances resulting from the induced momentary dipoles in their molecules.
Reset
Help
The correct ranking cannot be determined.
hydrogen bonding
dipole-dipole forces
dispersion forces
Weakest
Strongest
12/11/23, 11:52 PM
Chapter 09 Assignment
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6/23
Hint 4. Identify the substances that can form ion-dipole interactions with water
An ion-dipole interaction is the attractive force between ions and dipoles. Which of the following substances can form ion-dipole interactions with water
molecules?
Check all that apply.
ANSWER:
Hint 5. Identify the substances that can form hydrogen bonds with water
Which of the following substances can form hydrogen bonds with water molecules?
Check all that apply.
ANSWER:
ANSWER:
Correct
Chapter 9 Reading Question 2
Reset
Help
Ion-dipole forces
Hydrogen bonding
Dipole-dipole forces
Dispersion forces
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Related Questions
The following volumes of 0.000300 M SCN- are diluted to 15.00 mL. Determine the concentration of SCN- in each sample after dilution. These values will be used during the experiment.
Sample
0.000300 M SCN- (mL)
[SCN-] (M)
1
1.50
2
3.50
3
7.00
4
10.00
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Identify the type of error (systematic or random) for each of the following situations below and
defend your answer briefly:
The student forgot to obtain the mass of the filter paper before filtering the solution and
calculating the mass of the precipitate.
a.
b.
In the water analysis, trial 3 was analyzed 2 days after the analysis of trials 1 and 2.
Experiment #2 was conducted from 8:00 AM to 4:00 PM. The weather at the start of the
experiment was sunny then became rainy with thunderstorms after 12 NN.
C.
d.
The NaOH solution used by the students in the titration of vinegar was expired
arrow_forward
Consider the following reactions that take place in aqueous solution and related information.H2CO3 + HS- ⇋ H2S + HCO3-HSO4- + HCO3- ⇋ H2CO3 + SO4 2-H2CO3 (Ka1 = 4.2x10-7, Ka2 = 4.8x10-11) H2S (Ka1 = 1x10-7, Ka2 = 1x10-19) H2SO4 ( Ka1 = Very Large, Ka2 = 1.2x10-2)What is the strongest base in the reactions given?
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2
20
E
Solid silver fluoride is slowly added to 150 mL of a potassium chromate solution until the concentration of silver ion
is 0.0538 M. The maximum amount of chromate remaining in solution is
C
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A chemist tries to dissolve a solid ionic compound called "X" in water at 25°C. He adds 100 mL of water to
a beaker equipped with a stirrer on a balance. While slowly adding X to the beaker, he measures the mass of
X added and, at the same time, carefully watches to make sure that everything he adds dissolves. Suddenly,
when he has just added a total of 2 g of X, he sees that the mixture is no longer homogeneous (i.e. some of
the X remains on the bottom of the beaker and won't dissolve). He divides the 2 g of X by the 100 mL of
water and obtains the value 0.02 g X/mL water. This number répresents an important physical property of X.
What is it uniquely called?
A) the molarity of X in water at 25°C
B) the concentration of X in water at 25°C
C) the mass of X in water at 25°C
D) the density of X in water at 25°C
E) the solubility of X in water at 25°C
How would you describe the solution that the chemist prepared in Question#1?
A)…
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1- Perform the activity (Home Made Indicator) on page 138 of your textbook.
Activity
2- Prepare three cups one contains vinegar, the second contains salt solution and
the third contains clorox solution. Tabulate your observations.
Solution
Vinegar
Salt solution
Clorox solution
Color after adding indicator
3- To a cup containing chalk or egg shell add few ml of vinegar. Record your observation.
Observation
Reactants
Products
Word Equation
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Name
Chem
Section
Data Sheet
determination
23°C
23°C
25°C
temperature of filtered KHT
solution, °C
0.04m
concentration of NaOH solution,
mol L-
0.04 m
0.04m
KHT solution
14.9
49-5
final buret reading, mL
initial buret reading, mL
49.9
volume of KHT
used, mL
NaOH solution
28
final buret reading, mL
10
49.8
१.१
49.7
initial buret reading, mL
50
40mL
volume of NaOH
used, mL
number of moles of NaOH used
0014
0014
number of moles of HT titrated
.04
[HT] in KHT solution, mol L-
1.42
1.142
1.142
[K*] in KHT solution, mol L-1
solubility of KHT, mol L-1
average solubility of KHT,
mol L-
Ksp
average Ksp
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Heroin and morphine (shown below) are odorless solids. Drug-sniffing dogs can sometimes locate heroin that
has been exposed to the elements because of a strong odor that is present in small quantities. What compound
causes the odor and suggest what reaction is responsible for the compound's formation.
H3C.
но
reaction?
odor compound?
'N.
CHз
CHз
H3C
но
herion
morphine
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7. What mass of silver chloride will be recovered if excess sodium chloride is added to 500 mL
of solution containing 10.79 g of Ag*?
10.8 g
b. 21.6 g
28.6 g
d. 7.2 g
14.3 g
а.
е.
с.
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Pre-Lab Questions
1. Explain the benefit of letting the solutions of HCl(aq) and NaOH(aq) sit overnight.
2. When using the same graduated cylinder to measure the volumes of HCl(aq) and
NAOH(aq), it is important to rinse the cylinder with water and a small amount of the
second reactant before measuring the volume of the second reactant. Explain why this
is important for this investigation.
3. Describe how to perform each of the following safely:
• diluting a strong acid solution with water
• dissolving a solid base in water
• adding a solution of base to a solution of acid
4. If acid comes in contact with your skin, why must you flush the area with plenty of
cold water, rather than neutralizing the acid with a base?
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Suppose a pair of chemical compounds A and B can react in two different ways:
A+BC
Reaction 1 gives product C.
A+B D
Reaction 2 gives product D.
The following facts are known about the two reactions:
• Reaction 1 is endothermic and Reaction 2 is exothermic.
• If a reaction vessel is charged ("filled") with A and B, then at first D is produced faster than C.
Use these facts to sketch a qualitative reaction energy diagram for both reactions.
Note: because these sketches are only qualitative, the energies don't have to be exact. They only have to have the right relationship to each other. For example,
if one energy is less than another, that fact should be clear in your sketch.
Reaction 1
Reaction 2
energy
energy
A + B
A + B
reaction coordinate
reaction coordinate
Explanation
Check
2021 atcGre Educalion. All Rights feserved
earch
hp
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A student removes 25 mL of 3.0 M NaOH and dilutes it to final volume of 350 mL. What
is the concentration of the resulting solution.?
48.
А.
42 M
В.
0.024 M
С.
75 M
D.
0.10 M
E.
0.21 M
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CONCENTRATION DETERMINATION
Buret contains NaOH solution
*Sodium hydroxide solution: To 1 part reagent grade NaOH add 1 part distilled, carbon
dioxide-free water by weight
Erlenmeyer flask contains about 9ml of the acid and about 10 ml of distilled water
made recently free from CO2 by boiling.
DATA SHEET
II
Final Reading HCI
Initial Reading HCI
9.4
Final Reading NaOH
Initial Reading NaOH
10.65
10.55
1 ml HCI
1 mL NAOH
mL NAOH
mL NaOH
mL HCL
mL HCL
Mean Values:
1 ml HCI =
1 mL NaOH =
_mL NaOH
mL HCL
COMPUTATION:
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Two students are studying the Arrhenius
reaction below:
NAOH + Hz S04
acid
→ Na SOy
+ HzO
base
salt
water
Did the students identify the acid, base
and salt correctly? If not, provide the
correction.
arrow_forward
Which of the following substances has the highest concentration of hydroxide ion in balance with water?
H2O (Kw x 1.00 x 10-14)
HX (Ka x 2.2 x 10-8)
HY (Ka x 4.4 x 10-7)
HO2Y (Ka x 2.2 x 10-9)
TODAY (Ka x 4.4. x 10-10)
arrow_forward
Complete the following table, making sure to include your units!
Concentration of Concentration of
acetic acid
Water level on
measuring cylinder
before reaction
98 mL
91 mL
95 mL
0.5%
0.2%
0.1%
●
sodium
bicarbonate
0.5 M
0.5 M
0.5 M
From the results above, which reactant do you consider to be the limiting reagent? Why?
●
Water level on
measuring cylinder
after reaction
8 mL
49 mL
81 mL
Consider the reaction where the concentration of acetic acid was 0.5% and the concentration
of sodium bicarbonate was 0.5 M. Complete the table on page 5 to calculate the theoretical
yield of CO2 with these concentrations. The following bullet points may help:
You have already calculated the amount of sodium bicarbonate in 100 mL
In a 100 mL solution of acetic acid at 0.1% there will be 0.1 mL of acetic acid.
●
Volume of gas
produced
The density of acetic acid is 1.05 g/mL. You can use this value to calculate the mass of
acetic acid used in the reaction.
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7. A student weighs out exactly 1.562 grams of p-aminophenol and exactly 40 mL of water.
After dissolving p-aminophenol in HCI, 10 mL of acetic anhydride is added. The student
follows the procedure and acetaminophen is prepared. What is the maximum amount of
acetaminophen she could obtain from the reaction if the percentage yield is 76%? I
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Answered - Incorrect 1 attempt left
Resubmit
Question 6
Homework Unanswered
Determine the molar concentration of Cl lons in 2.59E-1 M CaCiz(aq).
Respond with the correct number of significant figures in scientific notation (Use E notation and only 1 digit before decimal eg 2.5ES for 2.5x 10)
Type your numeric answer and submit
1.
Submit
Unanswered 3 attempts left
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Report sheet for Titration of vinegar
Part I: Standardization of the NaOH solution with KHP
Trial 1 Trial 2 Trial 3
Mass of Erlenmeyer flask + KHP (g) 78.34 78.27 78.01
Mass of empty flask (g) 77.12 77.12 77.12
Mass of KHP (g) 1.22 1.15 0.89
Final buret reading (mL) 31.35 30.53 27.71
Initial buret reading (mL) 16.35 15.78 14.20
Vol NaOH solution delivered (mL)…
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4. A student performs the HCl tests on the three solid samples as described in Step 5 of Part B and gets the same result for the solid CaCO3 sample and the mixture. Which of the following statements is true concerning these results?
a. The results are to be expected.
b. The results are not expected and could have been caused by using contaminated HCl.
c. The results are not expected and could have been caused by using contaminated samples.
Explain your answer.
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1. Place a few crystals of bismuth trichloride in a test tube and add 3 ml of water.
Observations:
What change takes place?
Write the equation for the reaction.
Test the solution with litmus paper. What is the result?
What causes this change?
Add to the solution concentrated hydrochloric acid (CAUTION: CONCENTRATED
HYDROCHLORIC ACID IS CORROSIVE AND CAN BURN THE SKIN!) a drop at a time with
constant shaking until a change is observed.
Observations:
Give the effect of the following on the direction of the reversible reaction:
a) adding more water:
b) adding more HCl:
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Which process could not be an electrolytic reaction?
a.
2 PbSO4(s) + 4 H2O(l) Pb(s) + PbO2(s) + 2 H2SO4(aq)
b.
2H2O(l) 2H2(g) + O2(g)
c.
2Al2O3(l) 4Al(l) + 3O2(g)
d.
Na+(aq) + Cl−(aq) 2Na(l) + Cl2(g)
e.
2Fe(s) + 3O2(g) Fe2O3(s)
arrow_forward
If the initial volume reading for the second titration was 0.76 mL and the final volume reading was 11.73 mL, what volume of iodine solution was used in your second titration (in mL)? Include the unit and two decimal places in your answer.
arrow_forward
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Related Questions
- The following volumes of 0.000300 M SCN- are diluted to 15.00 mL. Determine the concentration of SCN- in each sample after dilution. These values will be used during the experiment. Sample 0.000300 M SCN- (mL) [SCN-] (M) 1 1.50 2 3.50 3 7.00 4 10.00arrow_forwardIdentify the type of error (systematic or random) for each of the following situations below and defend your answer briefly: The student forgot to obtain the mass of the filter paper before filtering the solution and calculating the mass of the precipitate. a. b. In the water analysis, trial 3 was analyzed 2 days after the analysis of trials 1 and 2. Experiment #2 was conducted from 8:00 AM to 4:00 PM. The weather at the start of the experiment was sunny then became rainy with thunderstorms after 12 NN. C. d. The NaOH solution used by the students in the titration of vinegar was expiredarrow_forwardConsider the following reactions that take place in aqueous solution and related information.H2CO3 + HS- ⇋ H2S + HCO3-HSO4- + HCO3- ⇋ H2CO3 + SO4 2-H2CO3 (Ka1 = 4.2x10-7, Ka2 = 4.8x10-11) H2S (Ka1 = 1x10-7, Ka2 = 1x10-19) H2SO4 ( Ka1 = Very Large, Ka2 = 1.2x10-2)What is the strongest base in the reactions given?arrow_forward
- 2 20 E Solid silver fluoride is slowly added to 150 mL of a potassium chromate solution until the concentration of silver ion is 0.0538 M. The maximum amount of chromate remaining in solution is C Submit Answer $ 4 R FI F V Retry Entire Group 8 more group attempts remaining % Use the References to access important values if needed for this question. 5 T Cengage Learning | Cengage Technical Support G ^ 6 B MacBook Pro Y H & N 20 7 U N ▶II * 00 8 J I M ( 9 K O V. ) O < L ✔ M. P A Previous Email Instructor + Next Save and Exit 21 ?arrow_forwardL.O Page View Read aloud V Draw A Highlight Erase A chemist tries to dissolve a solid ionic compound called "X" in water at 25°C. He adds 100 mL of water to a beaker equipped with a stirrer on a balance. While slowly adding X to the beaker, he measures the mass of X added and, at the same time, carefully watches to make sure that everything he adds dissolves. Suddenly, when he has just added a total of 2 g of X, he sees that the mixture is no longer homogeneous (i.e. some of the X remains on the bottom of the beaker and won't dissolve). He divides the 2 g of X by the 100 mL of water and obtains the value 0.02 g X/mL water. This number répresents an important physical property of X. What is it uniquely called? A) the molarity of X in water at 25°C B) the concentration of X in water at 25°C C) the mass of X in water at 25°C D) the density of X in water at 25°C E) the solubility of X in water at 25°C How would you describe the solution that the chemist prepared in Question#1? A)…arrow_forward1- Perform the activity (Home Made Indicator) on page 138 of your textbook. Activity 2- Prepare three cups one contains vinegar, the second contains salt solution and the third contains clorox solution. Tabulate your observations. Solution Vinegar Salt solution Clorox solution Color after adding indicator 3- To a cup containing chalk or egg shell add few ml of vinegar. Record your observation. Observation Reactants Products Word Equationarrow_forward
- Name Chem Section Data Sheet determination 23°C 23°C 25°C temperature of filtered KHT solution, °C 0.04m concentration of NaOH solution, mol L- 0.04 m 0.04m KHT solution 14.9 49-5 final buret reading, mL initial buret reading, mL 49.9 volume of KHT used, mL NaOH solution 28 final buret reading, mL 10 49.8 १.१ 49.7 initial buret reading, mL 50 40mL volume of NaOH used, mL number of moles of NaOH used 0014 0014 number of moles of HT titrated .04 [HT] in KHT solution, mol L- 1.42 1.142 1.142 [K*] in KHT solution, mol L-1 solubility of KHT, mol L-1 average solubility of KHT, mol L- Ksp average Ksparrow_forwardHeroin and morphine (shown below) are odorless solids. Drug-sniffing dogs can sometimes locate heroin that has been exposed to the elements because of a strong odor that is present in small quantities. What compound causes the odor and suggest what reaction is responsible for the compound's formation. H3C. но reaction? odor compound? 'N. CHз CHз H3C но herion morphinearrow_forward7. What mass of silver chloride will be recovered if excess sodium chloride is added to 500 mL of solution containing 10.79 g of Ag*? 10.8 g b. 21.6 g 28.6 g d. 7.2 g 14.3 g а. е. с.arrow_forward
- Pre-Lab Questions 1. Explain the benefit of letting the solutions of HCl(aq) and NaOH(aq) sit overnight. 2. When using the same graduated cylinder to measure the volumes of HCl(aq) and NAOH(aq), it is important to rinse the cylinder with water and a small amount of the second reactant before measuring the volume of the second reactant. Explain why this is important for this investigation. 3. Describe how to perform each of the following safely: • diluting a strong acid solution with water • dissolving a solid base in water • adding a solution of base to a solution of acid 4. If acid comes in contact with your skin, why must you flush the area with plenty of cold water, rather than neutralizing the acid with a base?arrow_forwardSuppose a pair of chemical compounds A and B can react in two different ways: A+BC Reaction 1 gives product C. A+B D Reaction 2 gives product D. The following facts are known about the two reactions: • Reaction 1 is endothermic and Reaction 2 is exothermic. • If a reaction vessel is charged ("filled") with A and B, then at first D is produced faster than C. Use these facts to sketch a qualitative reaction energy diagram for both reactions. Note: because these sketches are only qualitative, the energies don't have to be exact. They only have to have the right relationship to each other. For example, if one energy is less than another, that fact should be clear in your sketch. Reaction 1 Reaction 2 energy energy A + B A + B reaction coordinate reaction coordinate Explanation Check 2021 atcGre Educalion. All Rights feserved earch hparrow_forwardA student removes 25 mL of 3.0 M NaOH and dilutes it to final volume of 350 mL. What is the concentration of the resulting solution.? 48. А. 42 M В. 0.024 M С. 75 M D. 0.10 M E. 0.21 Marrow_forward
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