Q: it refers to the amount of acid or base which a buffer can consume before noticeable pH changes occur
A: capacity

Q: conjugate acid
A: a base with an attached proton

Q: a commonly used precipitating anion
A: sulfide

Q: titration
A: adding an acid and base together in measured quantities

Q: the pH of a buffer containing equal molar concentrations of a weak acid and its salt
A: pka

Q: hydrochloric is this type of acid
A: binary

Q: the relationship between the concentrations of molecular and ion forms of an indicator when the intermediate color is reached
A: equal

Q: common ion effect
A: when an ion from an added salt alters the solubility equilibrium of a slightly soluble salt

Q: the name for HClO
A: hypochlorous acid

Q: his theory explains the acidity of some solutions which contain metal ions
A: Lewis

Q: a commonly used simplifying mathematical procedure with dissociation constants are very small
A: approximation

Q: an ion formed from a simple ion and a molecule or other ions
A: complex ion

Q: it is weak in a strong acid
A: conjugate base

Q: sulfuric acid is this type of acid
A: diprotic

Q: when anions of these are present low solubility systems often alter solubility via pH changes
A: weak acids

Q: the presence of this element often indicates the substance is a base
A: nitrogen

Q: phenolphthalein
A: a commonly used indicator in acid - base titrations

Q: the character of a weak acid , strong base titration at the endpoint
A: basic

Q: perchloric acid is one of these
A: strong acid

Q: a bond in which only one atom provides the bonding pair of electrons
A: coordinate covalent

Q: these acid names end in ic or ous
A: oxyacids

Q: most acids and bases are of this type
A: weak

Q: acetic acid dissolved in a sodium acetate solution
A: buffer

Q: the sum of pH and pOH
A: fourteen