Definitions
Acid definition (Brønsted-Lowry)
What is proton donor?
Formula for pH
What is -log[H⁺]?
This is a strong acid including Cl
What is HCl?
This is what Ka measures
What is acid strength?
This is the point where moles acid = moles base
What is equivalence point?
Base definition (Brønsted-Lowry)
What is proton acceptor?
This is the result of adding pH and pOH
What is 14?
Weak acids only partially do this
What is dissociate?
This is the relationship between Ka and Kb
What is Kw = Ka x kb?
This is close to where the indicator changes color
What is the equivalence point?
This is what strong acids do in water
What is completely dissociate?
This is the pH of a neutral solution at 25°C
What is 7?
This includes Group 1 hydroxides
What are strong bases?
This is the formula for pKa
What is -log(Ka)?
This is what is contained in a buffer
What is a weak acid and conjugate base?
Substance that can act as acid or base
What is amphoteric?
This means the solution is more acidic
What is a lower pH?
This leads to small Ka values
What are weak acids?
This results in larger Ka
What is a stronger acid?
This is the equation used for buffer calculations
What is the Henderson-Hasselbalch equation?
What is one proton?
This is relationship between [H⁺] and [OH⁻]
What is Kw = 1.0 × 10⁻¹⁴?
This leads to lower pKa
What are strong acids?
This is the relationship between conjugate base and acid strength
What is inverse?
This is what the pH equals at the half-equivalence point
What is pKa?