Acid & Base Definitions
Acids and bases can be defined in different ways. We have covered these definitions in class today and you are now expected to pass the quiz that will cover that topic in the next class. The test below is designed to give you a scoop of what is expected of you. Give it a try and polish up on what you fail to answer.
- 1.
What is the definition of an Arrhenius base?
- A.
Any substance that can donate a proton
- B.
Any species that can accept electron pairs
- C.
Any substance that can accept a proton
- D.
A substance that when dissolved in water produces OH- ions, it is an OH- donor
- E.
A substance that when dissolved in water dissociates to form H+ ions
Correct Answer
D. A substance that when dissolved in water produces OH- ions, it is an OH- donorExplanation
An Arrhenius base is defined as a substance that, when dissolved in water, produces hydroxide ions (OH-) and acts as an OH- donor. This definition distinguishes Arrhenius bases from other options such as substances that can donate a proton or accept electron pairs. Arrhenius bases specifically produce OH- ions when dissolved in water, allowing them to increase the concentration of hydroxide ions in a solution.Rate this question:
-
- 2.
Which of the following is a good Lewis base?
- A.
Any species with lone pairs on the central atom
- B.
H3O+
- C.
Any species that can accept electron pairs
- D.
Any substance that can accept an H+ ion
- E.
Any substance that can donate an H+ ion
Correct Answer
A. Any species with lone pairs on the central atomExplanation
A Lewis base is a species that can donate a pair of electrons. In the given options, the only choice that fits this definition is "any species with lone pairs on the central atom." This is because species with lone pairs on the central atom have the ability to donate those electrons, making them good Lewis bases. The other options, such as H3O+, refer to species that can accept electrons or donate or accept H+ ions, which do not fit the definition of a Lewis base.Rate this question:
-
- 3.
Which of the following defines an acid as a species that can accept electron pairs?
- A.
Bronsted-Lowry
- B.
Arrhenius
- C.
Lewis
- D.
Svante
Correct Answer
C. LewisExplanation
The correct answer is Lewis. Lewis acid-base theory defines an acid as a species that can accept electron pairs. This theory focuses on the transfer of electrons during acid-base reactions, with the acid being the electron acceptor and the base being the electron donor. Unlike the Arrhenius and Bronsted-Lowry definitions, which focus on the presence of hydrogen ions in acids, the Lewis definition is broader and includes species that can accept electron pairs regardless of the presence of hydrogen ions. Svante is not a recognized acid-base theory, so it is not the correct answer.Rate this question:
-
- 4.
Which of the following defines an base as any substance that can accept an H+ ion?
- A.
Arrhenius
- B.
Lewis
- C.
Bronsted-Lowry
Correct Answer
C. Bronsted-LowryExplanation
The Bronsted-Lowry definition of a base states that it is any substance that can accept a hydrogen ion (H+). This definition is different from the Arrhenius definition, which defines a base as a substance that produces hydroxide ions (OH-) in water, and the Lewis definition, which defines a base as any electron pair donor. The Bronsted-Lowry definition is more inclusive as it allows for bases that do not necessarily need to be in water or produce hydroxide ions.Rate this question:
-
- 5.
What is an arrhenius acid?
- A.
Any substance that can donate an H+ ion
- B.
A substance that when dissolved in water dissociates to form hydrogen ions
- C.
Any substance that can accept an H+ ion
- D.
Any species that can accept electron pairs
Correct Answer
B. A substance that when dissolved in water dissociates to form hydrogen ionsExplanation
An Arrhenius acid is defined as a substance that, when dissolved in water, dissociates to form hydrogen ions. This means that it releases H+ ions into the solution. This is in contrast to an Arrhenius base, which would instead release hydroxide ions (OH-) when dissolved in water. Therefore, the correct answer is "a substance that when dissolved in water dissociates to form hydrogen ions."Rate this question:
-
- 6.
Which of the following is the definition of a Bronsted-Lowry base?
- A.
Any substances that can donate H+ ions
- B.
A substance when dissolved in water produces OH- ions
- C.
Any substance that can accept H+ ions (proton)
- D.
A substance that when dissolved in water dissociates to form hydrogen ions
Correct Answer
C. Any substance that can accept H+ ions (proton)Explanation
A Bronsted-Lowry base is defined as any substance that can accept H+ ions (protons). This means that when a Bronsted-Lowry base reacts with an acid, it accepts a proton from the acid, forming a new compound. The base acts as a proton acceptor in the reaction. This definition is different from the other options because it focuses on the ability of a substance to accept protons, rather than donate or produce them.Rate this question:
-
Quiz Review Timeline +
Our quizzes are rigorously reviewed, monitored and continuously updated by our expert board to maintain accuracy, relevance, and timeliness.
-
Current Version
-
Mar 20, 2023Quiz Edited by
ProProfs Editorial Team -
Oct 28, 2009Quiz Created by
Msorensen
Back to top