What should you do if you spill a chemical on your lab bench?
Clean it up using the spill kit
Leave it alone, it will evaporate
Leave it for the janitor to clean
Wipe it up with the towel
MgSO4 disappears when added to water and stirred. What describes the relationship between MgSO4 and water?
Insoluble
Soluble
Miscible
Immiscible
Adding mercury to water results in a solution consisting of two layers. What describes the relationship between mercury and water?
Souble
Miscible
Insoluble
Immiscible
What property is an example of a physical property?
A solid that dissolves in HNO3
A solid's ability to react with oxygen
A solid's melting point
A solid's ability to dissolve in water
Select the appropriate chemical formula that corresponds to a red brown solid.
Cu
CuO
CuSO4
Cu(OH)2
Select the appropriate chemical formula that corresponds to a black solid
CuSO4
CuO
Cu
Cu(OH)2
What is the mole to mole ratio between Cu(C2H3O2)2*H2O and NaC7H4SO3N*H2O
1:1
1:2
2:1
2:3
Spilling some of the sodium saccharinate while transferring solid to the beaker
Raises the actual yield
No effect
Lowers the actual yield
Washing the crystals with hot water
Lowers the actual yield
No effect
Raises the actual yield
Which definition corresponds to limiting reagent?
The reactant that is present as extra material when the reaction is complete
The reactant that is completely consumed during the reaction
A small portion of a chemical species
The amount of product that could be produced using a given amount of reactant
A chemical species that contains a metal ion that is coordinated to ligands
Which definition corresponds to theoretical yield?
The reactant that is present as extra material when the reaction is complete
The amount of product that could be produced using a given amount of reactant
The reactant that is completely consumed during the reaction
A small portion of a chemical species
A chemical species that contains a metal ion that is coordinated to ligands
Which definition corresponds to excess reagent?
A chemical species that contains a metal ion that is coordinated to ligands
The amount of product that could be produced using a given amount of reactant
The reactant that is present as extra material when the reaction is complete
The reactant that is completely consumed during the reaction
A small portion of a chemical species
What color is expected for the product, if NiCl2*6H2O is the limiting reagent?
Dark purple
White
Dark blue
Pink violet
Blue green
Lime green
Added an extra 5 ml of acetone in step 7 of Part II
Lowers the actual yield
No effect
Raises the actual yield
Left some product behind on the filter paper, not all on the watch glass
Raises the actual yield
Lowers the actual yield
No effect
Which definition corresponds to acid-base indicator?
The chemical species of interest
A chemical species that changes colors at different pH values
The chemical species being added in a titration
A chemical species that has a pH value < 7
Diluting the NaOH solution before filling the buret
No effect
Raises the value of mg citric acid/mL juice
Lowers the value of mg citric acid/mL juice
Under-titrating the end point
No effect
Lowers the value of mg citric acid/mL juice
Raises the value of mg citric acid/ml juice
You will conduct titrations again in Experiment 6. What will be used to measure the volume of titrant added to the solution?
Beral pipet
Buret
Drop counter
Graduate cylinder
In a different experiment, nitric acid (HNO3) is titrated with potassium hydroxide (KOH). What species are in solution at the equivalence point? What is the pH?
KNO3 and H2O only, pH = 7
KOH and H2O only, pH >7
KOH only, pH > 7
HNO3 only, pH <7
What will be the shape of the titration curve if oxalic acid, HO2C2O2H, is titrated with LiOH?
S-shaped with a vertical rapid rise and an initial pH > 7
S- shape with a vertical rapid rise and an initial pH < 7
Slanted S-shape with an initial pH > 7
Slanted S-shape with an initial pH < 7
How did you determine the equivalence point for each titration?
Mid point of rapid rise section of the plot
Divide the total volume of titrant added by 2
Color change from colorless to blue
Color change colorless to pink
(final pH - initial pH)/2
What is the conductivity classification for an unknown B that dissolves completely in water and dissociates completely into ions?
Weak electrolyte
Strong electrolyte
Nonelectrolyte
What is the conductivity classification for an unknown A that dissolves completely in water and partially dissociates into ions?
Nonelectrolyte
Strong electrolyte
Weak electrolyte
What is the conductivity classification for an unknown H that only partially ionizes in water?
Nonelectrolyte
Strong electrolyte
Weak electrolyte
Predict the conductivity of NaBr, a soluble, ionic compound
Nonelectrolyte
Weak electrolyte
Strong electrolyte
Predict the conductivity of HCOOH, a weak acid
Nonelectrolyte
Weak electrolyte
Strong electrolyte
Predict the conductivity of H2SO4
Nonelectrolyte
Weak electrolyte
Strong electrolyte
Predict the conductivity of H2O
Nonelectrolyte
Weak electrolyte
Strong electrolyte
Which statements explain the shape of the titration curve observed in lab?
Initially, the conductivity is zero since the reaction has not begun
During the reaction, the conductivity decreases due to the production of nonelectrolytes
During the reaction, the conductivity decreases due increase of ions
After the endpoint, the conductivity increases due to the excess titrant
Which statement about the spectrophotometric analysis of Red 40 dye is TRUE
The intensity of the color of the solution is indirectly proportional to concentration of the Red 40 dye
The calibration plot is a graph of concentration of Red 40 dye (y-axis) versus absorbance (x-axis)
If there is no Red 40 dye present in the solution, the absorbance will be zero
Absorbance = slope/concentration
Two future experiments, a dark red [Fe(SCN)6]3- solution is formed. Using the Color star, what color of wavelengths are being absorbed?
Red
Orange
Yellow
Green
Blue
Violet
The liquid above the solid in a mixture of solid and solution.
Precipitate
Supernate
Decantate
Centrifuge
The liquid that was carefully poured into a new container.
Precipitate
Supernate
Decantate
Centrifuge
CH3COOH and HC2H3O2 are different ways of writing the chemical formula of which chemical?
Acetic acid
Acetate ion
Peracetic acid
Acetone
You have two test tubes. One test tube contains Bi+3 and the other test tube contains Cu+2. Predict what will happen when NH3 is added to both test tubes.
Bi+3 will remain unchanged, Cu+2 will form a maroon precipitate, Cu2Fe(CN)6
Bi+3 will form a white precipitate, Bi(OH)3, Cu+2 will remain unchanged
Bi+3 will form a black solid, Bi, Cu+2 will remain unchanged
Bi+3 will form a white precipitate, Bi(OH)3 and Cu+2 will form a blue solution, [Cu(NH3)6]+2
Confirmation test for Bi+3
Black solid
Maroon solid
Blue solution
Pale yellow precipitate
Confirmation test for Cu+2
Maroon precipitate
Pale yellow precipitate
Gray white precipitate
Black precipitate
You have two test tubes. One test tube contains Pb+2 solution and the other test tube contains Cu+2. Predict what will happen when HCl is added to both test tubes.
Pb+2 will remain unchanged, Cu+2 will form a white precipitate, Cu2Fe(CN)6
Pb+2 will form a white precipitate, PbCl2, Cu+2 will remain unchanged
Pb+2 will form a yellow precipitate, PbCrO4, Cu+2 will remain unchanged
Pb+2 will remain unchanged, Cu+2 will form a blue solution, [Cu(NH3)6]+2
In step 1-B, the white precipitate completely dissolved when hot water was added and the solution was stirred.
Ag+ is confirmed as absent
Cu+2 is confirmed present
Fe+2 is confirmed present
Cr+3 is confirmed present
In step 1-C, after adding the CH3COOH and K2CrO4, the colorless solution turned yellow and a yellow precipitate formed
Pb+2 is confirmed absent
Pb+2 is confirmed present
Cu +2 is confirmed present
Ag+ is confirmed present
In step 1-A, after adding the 6M HCl to an unknown, a white precipitate formed with a colorless decantate
Ag+ and Pb+2 are indicated as possibly present
Cu+2 and Bi+3 are indicated as possibly present
Ag+ is absent
Pb+2 is absent
What reagent could you add to a mixture of PbCl2 and AgCl to seperate the two species?
SnCl2
Hot water
HCl
K4Fe(CN)6
K2CrO4
What reagent could you add to a mixture of Cu+2 and Bi+3 to seperate the two species?
SnCl2
NH3
HCl
K4Fe(CN)6
K2CrO4
Confirmation test for Mn+2
Yellow solution
Purple solution
White precipitate
Gray white precipitate
Confirmation test for Zn+2
Purple precipitate
Yellow precipitate
Gray white precipitate
Yellow solution
What reagent could you add to a mixture of Mn+2 and Zn+2 to seperate the two species?
NaOH
H2DMG
NaBiO3
BaCl2
K4Fe(CN)6
KSCN
What reagent could you add to a mixture of [Zn(OH)4]-2 and CrO4-2 to seperate the two species?
NaOH
H2DMG
NaBiO3
BaCl2
K4Fe(CN)6
In a certain reaction, a solid chemical dissolved in water. The temperature of the water sample dropped from 27.3 to 22.4
q system is a positive value
Q system is a negative value
Water is defined as the system
Water is defined as the surroundings
Heat was lost by the system
Heat was gained by the surroundings
The reaction is exothermic
The reaction is endothermic
Some of the NH4NO3 solid was spilled on the lab bench and not successfully added to the calorimeter
Increases the value of final temperature
Decreases the value of final temperature
No affect
Select all that apply to an exothermic reaction
The reaction releases heat to the surroundings
Heat is a reactant
The reaction absorbs heat from the surroundings
Adding heat will cause the equilibrium to shift towards products
Removing heat will cause the equilibrium to shift towards products
Select all the statements that are true concerning pH and buffers
As an acidic solution is diluted the pH decreases
As a basic solution is diluted the pH decreases
The smaller the concentrations of the buffer components, the greater its buffering capacity
A buffer works when either acids or bases are added
Select the redox terms that apply to Cu+2 in the half reaction. Cu+2 + e- --> Cu+
Species being reduced
Species being oxidized
Oxidizing agent
Reducing agent
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