All High School Chemistry Resources
Example Questions
Example Question #11 : Acid Base Chemistry
What is a triprotic acid?
An acid that donates an electron pair
An acid with one ionizable hydrogen
An acid with three ionizable hydrogens
An acid with two ionizable hydrogens
An acid that accepts an electron pair
An acid with three ionizable hydrogens
Acids have hydrogen ions and balanced charges. "Tri" tells us that the acid has three potential hydrogen ions. Once ionized, a hydrogen turns into a proton, hence, protic. An example of a triprotic acid is phosphoric acid
Example Question #12 : Acid Base Chemistry
What is a monoprotic acid?
Any acid with more than 2 ionizable hydrogens
An acid with three ionizable hydrogens
An acid with two ionizable hydrogens
A really weak base
An acid with one ionizable hydrogen
An acid with one ionizable hydrogen
Acids have hydrogens that can dissociate into solution. In this case, the word "mono" tells us that there is only one potential hydrogen ion in that acid; so only one hydrogen ion can be ionized from that acid. A diprotic acid, such as has two ionizable hydrogens.
Example Question #13 : Acid Base Chemistry
What is a polyprotic acid?
An acid that increases the concentration of hydrogen ions in a solution
An acid with one ionizable hydrogen
An acid with two ionizable hydrogens
An acid with three ionizable hydrogens
Any acid with more than two ionizable hydrogens
Any acid with more than two ionizable hydrogens
By definition, a polyprotic acid is one that has more than two ionizable hydrogens.
Example Question #14 : Acid Base Chemistry
Which of the following substances are amphoteric?
Remember: amphoteric means that the substance can act as either an acid or a base. Using the Bronsted-Lowry definition of acids and bases (acids donate hydrogens and bases accept hydrogens) we find that is the only compound that can give up a hydrogen (and be left with ), or accept a hydrogen (and become ).
Example Question #15 : Acid Base Chemistry
According to the Arrhenius definition __________.
bases increase the concentration of hydroxide ions in a solution
bases accept electron pairs
acids are hydroxide donors
acids increase the concentration of hydroxide ions in a solution
acids accept electron pairs
bases increase the concentration of hydroxide ions in a solution
According to the Arrhenius definition, bases increase the concentration of hydroxide ions in a solution.
Example Question #16 : Acid Base Chemistry
According to the Arrhenius definition, acids __________.
Acids are proton acceptors
Acids are hydrogen donors
Acids are hydroxide donors
Acids increase the concentration of hydroxide ions in a solution
Acids increase the concentration of hydrogen ions in a solution
Acids increase the concentration of hydrogen ions in a solution
According to the Arrhenius definition, acids increase the concentration of hydrogen ions in a solution.
Example Question #14 : Acid Base Chemistry
What is the Bronsted-Lowry definition of acids?
Acids are electron pair donors
Acids are electron pair acceptors
Acids are hydrogen donors
Acids are hydrogen acceptors
Acids are amphoteric
Acids are hydrogen donors
According to the Bronsted-Lowry definition, acids are hydrogen donors.
Example Question #422 : High School Chemistry
What is the definition of a Bronsted-Lowry base?
Electron pair acceptors
Hydrogen donors
Electron pair donors
Hydrogen acceptors
Increases the concentration of hydrogen ions in a solution
Hydrogen acceptors
According to the Bronsted-Lowry definition, bases are hydrogen acceptors.