Consider the following equilibrium:
HF + H2O(l) H3O+ + F -
Under what circumstances will this system behave as a buffer?
A.
when [F -] is equal to Ka
B.
when [F -] is equal to [HF]
C.
when [F -] is equal to [H2O]
D.
when [F -] is equal to [H3O]

B.

Explanation:

Buffer has equal concentrations of A- and HA.

B. when [F -] is equal to [HF]

see explanataion

Explanation:

Buffer solutions are defined as solutions containing a weak electrolyte (wk acid or wk base) and the salt of the weak electrolyte.

Given HF(aq) + H₂O(l) ⇄ H₃O(l) + F⁻, a buffer solution would result from a solution composition when  [F -] is equal to [HF]. Such is commonly referred to as a 50/50 buffer as the acid and salt are in equal concentrations. However, a buffer solution still will exist even if the concentrations of acid and salt are not equal. The presence of the weak acid or weak base and the salt of the electrolytes is the only requirement.

the answer would be b i believe

answer is: naturally occurring solid, inorganic compound or element is mineral.

minerals usually have crystalline form, that means than crystal constituents (atoms, molecules or ions) are arranged in a highly ordered microscopic structure, forming a crystal lattice that extends in all directions.

for example magnetite is a mineral of iron oxide (fe₂o₃).

calcite is a carbonate mineral and the most stable polymorph of calcium carbonate (caco₃).

dolomite is an   carbonate mineral composed of calcium magnesium carbonate (camg(co₃)₂).