Theories
This acid-base theory defines acids as proton donors and bases as proton acceptors.
What is the Bronsted-Lowry theory?
The pH of a neutral solution at 25°C is ___.
What is 7?
A buffer is composed of a __________ acid and its __________ base.
What is a weak acid and its conjugate base?
The equivalence point in a strong acid-strong base titration occurs at pH ____.
What is 7?
The color change of an indicator largely depends on its ____.
What is the pKa?
In the Lewis definition, acids are electron pair ___________, and bases are electron pair __________.
What are acceptors and donors?
The ion-product constant of water (Kw) at 25°C is ___.
What is 1.0 × 10⁻¹⁴?
The equation used to calculate the pH of a buffer solution is called the _______________.
What is the Henderson-Hasselbalch equation?
What is the purpose of an indicator in a titration?
What is to signal the endpoint of the reaction?
What mathematical method do you need to use to determine how much of a weak acid will dissociate into hydrogen ions and the conjugate base?
What is an ICE Table?
Name a substance that is amphoteric (can act as both an acid and a base).
What is water? (or another amphoteric molecule)
If a solution has a [H⁺] of 1.0 × 10⁻⁵ M, what is its pH?
What is 5?
If a buffer system has equal concentrations of weak acid and its conjugate base, the pH is equal to the __________ of the acid.
What is the pKa?
In a titration, what is the term for the sample with the unknown concentration?
What is the analyte?
How do you determine the Kb of a weak base if you only know the Ka of the conjugate acid?
What is use Kw = Ka*Kb?
What two definitions of acids are essentially the same?
What are Arrhenius and Bronsted-Lowery definitions of acids?
If a solution has a pH of 3, what is its pOH?
What is 11?
What happens to the pH of a buffer when a small amount of strong acid is added?
What is it changes slightly? (but stay near the buffered pH)
In a weak acid-strong base titration, the pH at the equivalence point is ______ than 7.
What is greater than 7?
Which part of the indicator system exists in a higher concentration if the pH of a solution is much lower than its pKa?
What is the acidic form of the indicator?
Name the definition of acids and bases that requires the presence of water.
What is the Arrhenius definition?
What is the pH of a 0.025 M solution of HNO₃?
What is 1.60?
A buffer is prepared using the same concentration of acetic acid and sodium acetate. If the Ka of acetic acid is 1.8 × 10⁻⁵, what is the pH for this buffer?
What is 4.74?
In a titration, what is the name of the solution that has a known concentration used to determine the sample's concentration?
What is the titrant?
pH is a measure of _____________ while pOH is a measure of __________. (Don't think ions.)
What is acidity and basicity?