3rd

Which is a property of acids in aqueous solutions?
c
Which of these substances contributes to soap’s slippery texture?
b
Which compound plays an important role in leather processing and electroplating?
not d
Which is a characteristic of a strong base?
d
The main active components of bleach and many other household cleaners are
not c
Which pair of substances would most likely result in the production of a gas when reacting with an acid?
c
Look at the reaction below.

mc022-1.jpg

Which substance is the acid in the reaction?

not b
H2CO3 is used in soft drinks. What is the name of this compound?
b
Which of these acids occurs naturally in the body and performs important regulatory functions?
a
An acid is a substance that increases the concentration of H3O+ ions in solution. Look at the reaction below of phenol (C6H5OH) with water:

mc023-1.jpg

Which reactant acts as an acid by contributing a H+ ion to create H3O+ in the chemical equation?

a
When does phenolphthalein turn pink?
a
Look at the reaction below.

mc021-1.jpg

Which substance is the base in the reaction?

not c
What is a common use of bases?
not b
An unknown substance turns methyl orange solution red. This shows that the substance
c
Which of the following best defines an acid?
d
Ca(OH)2 is added to a large beaker of water. How is the solution different from the original water?
b
Which statement describes the Arrhenius interpretation of acids and bases?
d
What is the Arrhenius definition of an acid?
a
Consider the reaction below.

H2PO4- + H2O mc030-1.jpg H3O+ + HPO42-

Which of the following is a base-conjugate acid pair?

not c
What is the Bronsted-Lowry definition of an acid?
a
A substance is dissolved in water and produces hydronium ions. This occurs when hydrogen ions move from the substance to associate with water molecules. Which term best matches the behavior of this substance?
not a
Which characteristic best identifies an Arrhenius base?
c
A chemist lectures about the following definition for acids and bases.

The acid-base behavior is analyzed in terms of how electrons are transferred between compounds rather than in terms of how hydrogen ions are transferred.

What is the chemist defining?

What is the definition of a Lewis base?
b
Which of the following substances is an Arrhenius acid?
b
Which reaction displays an example of an Arrhenius base?
a
Which of these correctly defines the pH of a solution?
a
Which statement about the self-ionization of water is correct?
b
What is the pH of a solution with [H+] = 1.25 mc015-1.jpg 10-10 M?
Use mc015-2.jpg.
d
A solution containing HCl would likely have
b
The pOH of a solution is 10.75. What is the concentration of OH- ions in the solution?
Use mc013-1.jpg.
not c
Several substances are labeled on the pH scale below.

mc025-1.jpg

Which substance has the lowest [H+] concentration but is still considered an acid?

a
Pure water at 25°C
not a
A substance with a high pOH would likely have which of the following?
d
How can the pH of a solution be calculated if the pOH is known?
d
A solution of HCl has mc012-1.jpg = 0.01 M. What is the pH of this solution?
Use mc012-2.jpg.
d
Which description correctly characterizes the acidity or basicity of a solution?
b
A substance with a high [H+ ] would likely have which additional characteristics?
not d
Which of these equations correctly expresses the self-ionization of water?
not c
The pH of a solution decreases by 2.0. How does the hydronium ion concentration of the solution change?
b
Based on the definition of logarithms, what is the difference in hydrogen ion concentration between a substance with a pH of 2 and a substance with a pH of 3?
a
Which of these correctly defines the pOH of a solution?
d
What is the equilibrium constant of pure water at 25°C?
b
Which of these refers to the strength of an acid?
not c not d
What do strong acids and strong bases have in common?
b
An experimental procedure requires 10 ml of acid to be dissolved into a beaker of water. An additional 5 ml of acid is added to the solution. Which statement best describes the new solution?
c
Look at the diagram showing hydrochloric acid being added to water.

mc006-1.jpg

mc006-2.jpg

Which statement best explains what is taking place?

a
A base is added to water. What happens when the position of equilibrium lies to the left?
b
If the base-dissociation constant, Kb, for a substance is 4.3 mc021-1.jpg 10-10, what does this tell you about Ka?
Use mc021-2.jpg.
a
If hydrofluoric acid is a stronger acid than acetic acid, which statement is most likely true?
c
An acid has a molarity of 0.01 M. What does the 0.01 M refer to?
not a
Which is true of weak acids and bases?
a
Which statement correctly describes the Ka of a weak acid?
d
A weak base is added to water. Which information is required to find the strength of its conjugate acid?
not d
How does the value of mc019-1.jpg and mc019-2.jpg compare with the concentrations of hydronium ion and hydroxide ion?
not b not c
What does it mean for a strong acid to be in equilibrium?
a
A solution conducts an electric current more easily when the solution contains more ions. An acidic solution conducts an electric current very easily. What type of acid is in this solution?
b
Which of these accurately describes why an acid is strong?
d
Which statement best describes what makes a base weak?
not c
Which equations shows the complete dissociation of a strong base?
not c
A strong acid, HA, is added to water. Which statement about the solution is true?
not b
Look at the table of dissociation constants for some acids.

Acid

Ka

Acetic acid
mc024-1.jpg

Chlorous acid
mc024-2.jpg

Nitrous acid
mc024-3.jpg

Propionic acid
mc024-4.jpg

Which of these is the strongest acid?

b
Consider the total ionic equation below.

mc022-1.jpg

Which is the net ionic equation for the reaction?

not b
Which is the correctly balanced chemical equation for the reaction of KOH and H2SO4?
c
Consider the total ionic equation below.

mc018-1.jpg

What are the spectator ions in this equation?

not b not a
Consider the chemical equation below.

mc019-1.jpg

Which is the net ionic equation?

a
Which salt is produced when H2SO4 reacts with NaOH?
b
Which compound will conduct electricity when it is dissolved in water?
not a not c
Consider the incomplete reaction below.

NaOH + X mc005-1.jpg NaCH3COO + H2O

What is X in this reaction?

d
Use the following table to answer the question.

Strong acids Weak acids Weak bases Strong bases
HBr CH3COOH NH3 NaOH
hno3 HF NH4OH KOH
H2SO4 HCN Ca(OH)2

Which of these is a neutral salt?

a
The two products that are formed when a solution of HNO3 and a solution of NaOH react are water and
b
An acid (X) reacts with a base (Y) to produce Mg3(PO4)2. What are X and Y?
not c
Which salt is produced when NH4OH reacts with HNO3?
c
Consider the reaction below.

mc023-1.jpg

Which is the net ionic equation for the reaction?

not a not c
Which of the following is the correctly balanced chemical equation for the reaction of Ca(OH)2 and HNO3?
not c
Which value is most likely to be the pH of a salt that is formed by the reaction of a weak acid and a strong base?
not a
Consider the total ionic equation below.

mc029-1.jpg

What are the spectator ions in this equation?

c
Which statement is correct?
not a
Which are produced when HCl reacts with Ca(OH)2?
not b
Which statement best describes salts?
not b
The table below lists some acids and bases.

Strong acids Weak acids Weak bases Strong bases
HBr CH3COOH NH3 NaOH
HNO3 HCOOH NH4OH KOH
H2SO4 Ca(OH)2

Which salt has a pH < 7?

d
Which instrument is most often used to measure acid volume before a titration begins?
not a
Which is a disadvantage of using chemical indicators?
c
Which of these would most likely be one of the final steps when performing a strong acid-base titration?
d
Why is a chemical indicator added to the flask in which a titration will occur?
a
When are drops of indicator most likely added to the erlenmeyer flask?
d
Which of these is true about a pH meter?
not c not b
Which of the glassware shown below is an Erlenmeyer flask?
a
Which of the following would be the best reason to use titration for monitoring the effects of acid rain on drinking water?
not c
The equivalence point in a titration refers to the point when
c
Which will provide the most direct measure of pH by measuring the hydrogen ion concentration of a solution?
a
Which of the following is the main reason to use titration in chemistry?
d
Which of the following is the last step in performing a titration?
not a
Which step accurately describes how to measure the final burette volume?
not c
Terry, a student, performs a titration. He completes these steps as part of his titration procedure:

1. He cleans and rinses a burette with standardized base.
2. He fills the burette with standardized base solution.
3. He reads and records the initial burette volume.
4. He adds a base from the burette to an acid.
5. He observes a color change in the Erlenmeyer flask.
6. He stops the addition of base from the burette.
7. He reads and records the final burette volume.

Which steps will provide information needed to calculate the volume of base needed to reach the equivalence point?

b
A chemist is about to perform a titration by adding a base to an acid. What is the most important reason for using a base instead of water to rinse out the burette?
d
A base is added to an acid during a titration. A pH meter is used to monitor the reaction’s progress. When should the addition of base stop?
not a
Look at the diagram below.

mc003-1.jpg

Which best describes what is taking place in the diagram?

not b
Which is an advantage of using chemical indicators?
not d
Study the titration curve below.

mc007-1.jpg

Which statement correctly explains the nature of the solution at point A?

not b not d
An Erlenmeyer flask contains 30.00 mL of 0.450 M NaOH before a titration is begun. How many moles of hydroxide ions are present in the flask at this time?
not c
Which graph represents a titration between NaOH(aq) and HCl(aq)?
a
Which acid was most likely used for the titration graph below?
not b not c
The graph below is the curve for the titration of a strong acid with a strong base.
not d
At which of the four labeled points on the titration curve below do you expect to find the highest concentration of hydroxide ions?
not a
Students performed a titration experiment and plotted the following curve from the data that they collected.
b
At which point was neutralization complete for the acid that is being titrated below?
not a not c
Which pH corresponds to the equivalence point for the graph below?
not b not a
A group of students is comparing the graphs of strong acid-strong base and weak acid-strong base titration curves, where the base is the titrant. Which statement inaccurately describes a difference between the two curves?
not a not b
The Erlenmeyer flask that was used in the titration below contained 25.0 mL of 0.1 M HCl.

mc003-1.jpg

If 0.1 M NaOH solution was used in this titration, which statement correctly explains point B on the curve?

c
Consider the titration curve below.

mc002-1.jpg

If an Erlenmeyer flask that is used in this titration contains 40.0 mL of 0.10 M HCl, how many moles of hydrogen ions are present at the point that is labeled A on the graph?

b
Which titration curve represents 18.0 mL of 0.10 M NH3 titrated in a flask with 0.10 M HCl?
b
An Erlenmeyer flask contains 25.00 mL of 0.500 M HCl before a titration is begun. How many moles of hydrogen ions are present in the flask at this time?
not d
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