Acids and Bases Flashcards
Properties of acids:
- Molecular compounds with H+ dissolved in water
- pH is <7
- Reacts with bases
- Tastes sour
- Turns blue litmus paper red
- Electrolyte
- Ionizes
Properties of bases:
- Compounds with OH- when dissolved in water
- pH is >7
- Doesn’t react with metals
- Feels slippery
- Tastes bitter
- Turns red litmus paper blue
- Electrolyte
- Dissacociates
Aqueous hydrogen _ide =
hydro _ic acid
Aqueous hydrogen _ate =
_ic acid
Aqueous hydrogen _ite =
_ous acid
When do you use “ide”?
Group 17 elements (hydro _ic acid)
When do you use “ate”?
Polyatomic compounds (_ic acid)
When do you use “ite”?
Polyatomic compounds (_ous acid)
Hydro _ic acid =
Aqueous hydrogen _ide
_ic acid =
Aqueous hydrogen _ate
_ous acid =
Aqueous hydrogen _ite =
Neutralization:
Occurs between an acid and a base. Produces salt and water.
What is considered salt in regards to neutralization?
A neutral ionic compound.
Neutral molecular:
Doesn’t dissociate, non-electrolyte, no effect on litmus, pH = 7
Neutral ionic:
Dissociates into ions, electrolyte, no effect on litmus, pH = 7
Arrhenius Acid:
A substance that ionizes to produce H+
Arrhenius Base:
A substance that dissociates to produce OH-
Steps for writing modified Arrhenius equations for acids:
- Write the acid reacting with water to produce H30+(aq)
2. Determine the other product
Steps for writing modified Arrhenius equations for bases:
- If ionic, split it into its ions and use the negative one
- Write an equation showing the negative ion reacting with water to produce OH- ion
- Determine the other product
How do you show the equation of a weak acid/base?
With a double-sided arrow.
What does a double-sided arrow mean?
The reaction is occurring back and forth.
What are strong bases?
Include elements from groups 1 or 2, and an OH ion.
pH means:
Power of hydrogen
Explain the logarithms of the pH scale:
When the pH changes by 1, the concentration of hydrogen changes by 10 fold.
Sig digs for pH:
Whatever’s after the decimal
How do you calculate pH?
pH = -log [H30+(aq)]
How do you calculate [H3O+(aq)]?
[H3O+(aq)] = 10^(-pH)
How do you calculate pOH?
pOH = -log [OH-(aq)]
How do you calculate [OH-(aq)]?
[OH-(aq)] = 10^(-pOH)
What is the relationship between pH and pOH?
pH + pOH = 14
Titrant:
A continuous, progressive addition of a solution from the buret to a precisely measured volume of a solution.
Equivalence point:
Volume where the reaction is completed.
Endpoint:
The pH at which a reaction is complete.
Standard solution:
A solution with a known concentration that will not change.
What must be included in a drawn graph?
Title, labelled axis’ with units, scale, and important points that are labelled.
