Acids and Bases
A solution with a pH less than 7, where [H+] is greater than [OH–].
What is an acidic solution?
Like HBr, this type of acid dissociates or ionizes completely.
What is a strong acid?
The pH of a neutral solution.
What is 7?
The products of a neutralization reaction.
What are salt and water?
A solution with a weak acid and its conjugate base that resists change in pH.
What is a buffer?
Also known as a proton, this is the component by which a conjugate acid-base pair differ.
What is H+?
Like HC2H3O2, this type of acid dissociates or ionizes partially.
What is a weak acid?
–log[H+]
What is pH?
The reactants in a neutralization reaction, a special type of double replacement reaction.
What are an acid and a base?
This type of solution results when you have a salt that was produced from a weak acid.
What is basic?
Like HCl, a producer of H+ in solution.
What is an Arrhenius acid?
This portion of a chemical indicates that it is a strong base.
What is OH- or hydroxide?
10–pH
What is [H+]?
A lab procedure used to determine the concentration of an unknown.
What is a titration?
The chemical that helps produced a buffer in your bloodstream, keeping your blood pH buffered around 7.4.
What is CO2?
Like NH3, this accepts H+ in solution.
What is a Bronsted-Lowry base?
This equals [H+][A–]/[HA].
What is the acid equilibrium constant, Ka?
The sum of pH and pOH.
What is 14?
A chemical whose color is pH dependent.
What is an indicator?
The ability or measurement of just how much acid or base a buffer can tolerate before being destroyed.
What is buffer capacity?
Like FeCl3, this is an electron pair acceptor.
What is a Lewis acid?
Occurring in solutions of weak acids, a state of reaction where the forward and backward rates are equal.
What is equilibrium?
The equation used to solved for pH when [OH–] is provided.
What is 14 - (-log[OH-])?
When moles of acid [H+] equals moles of base [OH–].
What is the equivalence point?
The Henderson-Hasselbalch equation.
What is pH = pKa + log ([A–]/[HA])?