An analytical chemist is titrating 245.6 mL of a 0.6400 M solution of ethylamine (C2H_NH,) with a 0.9000 M solution of HNO3. The pK, of ethylamine is 3.19. Calculate the pH of the base solution after the chemist has added 17.7 mL of the HNO3 solution to it.
Note for advanced students: you may assume the final volume equals the initial volume of the solution plus the volume of HNO, solution added.
Round your answer to 2 decimal places.
pH ?

explanation:

metals have excess of electrons whereas non-metals have deficiency of electrons. thus, in order to gain stability metals easily donate their electrons to the non-metals.

for example, electronic configuration of sodium is and electronic configuration of phosphorous is .

when a phosphorous atom and sodium atom combine together then sodium will donate is extra one electron to the phosphorous atom. as a result there will be formation of ionic bond between sodium and phosphorous.

the reaction will be as follows.

there, are three sodium sodium atoms and each of them will donate its one extra electron to phosphorous atom. thus, the sub-shell of phosphorous gets completely filled.  

thus, we can conclude that electrons are transferred from atoms of sodium to atoms of phosphorous. this transfer makes the sodium atoms donate one electron and the phosphorous atoms to gain one electron. as a result, the sodium and phosphorus atoms strongly attract each other.

can you list the answers so i can answer

fe 55.85 g/mol and h2o 18.02 g/mol.

it is stable as it is in group 0 which have full outer shells of electrons