Acids and Bases Flashcards
(27 cards)
What is a solution?
It is a completely perfect mixture of a solute and a solvent, where the particles of the solute are homogenous.
What is concentration?
It is the amount of solute that is dissolved in a given volume of a solution.
What is molarity?
It is the number of moles of solute per litre of solution.
What is an Arrhenius acid?
It is a substance that dissociates in water to produce H+ ions (protons).
What is an Arrhenius base?
It is a substance that dissociates in water to produce OH- ions (hydroxide).
What is a Bronsted Lowry acid?
It is a H+ ion (proton) donor.
What is a Bronsted Lowry base?
It is a H+ ion (proton) Accepter.
What is neutralisation?
It is the reaction between an acid and a base, forming a salt and water aqueous solution.
What is a conjugate acid?
A base that has accepted a H+ ion (proton).
What is a conjugate base?
A base that has donated a H+ ion (proton).
What is a conjugate pair?
An acid and a base that differ by a H+ ion (proton).
What is a primary standard?
It is a reagent that can be weighed easily, and which is so pure that its weight is truly representative of the number of moles of substance contained.
What is a titration?
It is a laboratory experiment where a measured volume of one solution is added to a known volume of another solution until the reaction is complete.
What is a base called when it donates 1 H+ ion (proton)? Give an example of one.
A monobasic acid; HCl
Notice there’s only one H
What is a base called when it donates 2 H+ ions (proton)? Give an example of one.
A dibasic acid; H2SO4
Notice there’s two H’s
What is a base called when it donates 3 H+ ions (proton)? Give an example of one.
A tribasic acid; H3PO4
Notice there’s three H’s
How do you classify acids?
Acids are classified as monobasic, dibasic, tribasic depending on the number of hydrogen atoms per molecule that are removed by a reaction with a base.
In 1887, Arrhenius designed a theory to explain how water allows acids to show their acidic properties.
Solve;
A.) HX —> ?
B.) HCl —> ?
C.) H2SO4 —> ?
A.) HX —> (H+) + (X-)
B.) HCl —> (H+) + (Cl-)
C.) H2SO4 —> (2H+) + (SO4^2-)
In 1887, Arrhenius designed a theory to explain how water allows bases to show their basic properties.
Solve;
NaOH —> ?
NaOH —> (Na+) + (OH-)
What did Arrehenius believe about dissociating acids and bases?
- In solution, weak acids and bases only slightly dissociate.
- In solution, strong acids and bases fully dissociate.
What are the two limitations to Arrhenius?
- It is limited to acid-base reactions that take place in water.
- It is also limited to bases that contain OH- ions.
What do these Bronsted Lowry acids and bases change to?
A.) HCl + H2O —> ?
B.) NH3 + H2O —> ?
C.) HCl + NH3 —> ?
A.) HCl + H2O —> (Cl-) + (H3O+)
B.) NH3 + H2O —> (NH4+) + (OH-)
C.) HCl + NH3 —> (Cl-) + (NH4+)
What is an amphoteric substance? Name an example.
It is a substance that can act as both an acid and a base.
For example, Water; (A: H2O —> OH-) (B: H2O —> H3O+
What conjugate base does a strong acid produce?
It produces a weak conjugate base.
