Solubility & Ksp Flashcards
(25 cards)
point at which equal amounts of sample and titrant are present
equivalence point
Ksp
an equilibrium constant for slightly soluble ionic compounds
small Ksp = compound is less soluble
large Ksp = compound is more soluble
the point at which an indicator changes colour
endpoint
unsaturate soln
could dissolve more solute
anion of a strong acid combined with the cation of a strong base
neutral salt
Does common ion affect Ksp
no
a chemical that changes colour with a change in pH
indicator
strong acid & weak base
a salt and an acidic solution
molar solubility
the amount in moles of solute in 1.0L of a saturated solution
a proton donor in equilibrium with its conjugate base
weak acid
cream of tarter?
potassium hydrogen tartrate
~ allows cake to rise and prevents them from deflating
~ used in baking, cleaning, natural remedy
How does temp affect Ksp
if its endothermic
~ increasing temp = increasing Ksp
~ favours forward rxn
if its exothermic;
~ increasing temp = decreasing Ksp
~ shifts to the left
weak acid & strong base
produces a weakly basic solution
common ion effect
adding a compound that contains an ion already present in a solution (a “common ion”) to an existing equilibrium results in a decrease in the solubility of a slightly soluble salt
ex:
- If you add a soluble salt like sodium chloride (NaCl) to a saturated solution of lead(II) chloride (PbCl₂), the chloride ion (Cl⁻) is a common ion.
- Adding NaCl increases the concentration of Cl⁻ ions, causing the equilibrium to shift towards the solid state of PbCl₂, resulting in a decrease in the solubility of PbCl₂.
proton acceptor
strong base
Qsp & Ksp
- if Qsp < Ksp, the solution is unsaturated, no precipitate
- if Qsp = Ksp, the solution is SATURATED, no change/precipitate
- if Qsp > Ksp, a precipitate forms until the solution is saturated
saturated soln
contains max amount of dissolve solute
the solution in the erlenmeyer
sample
precipitate
an insoluble product that forms from a reaction between 2 soluble ionic compounds
is Ksp temperature dependent
yes; normal temp for it is 25 degrees
drop by drop neutralization of an acid by a base to determine the conc of an unknown solution
titration
standardized solution you put in a buret
titrant
solubility
the max amount of solute that can dissolve in a given quantity of solvent at a particular temperature
weak acid in equilibrium with its salt that can resist a change in PH
buffer
