In the laboratory, a general chemistry student measured the pH of a 0.313 M aqueous solution of acetylsalicylic acid (aspirin), HC9H7O4 to be 2.031. Use the information she obtained to determine the Ka for this acid.

for the acid is

Explanation:

   c             0             0

So dissociation constant will be:

Give c= 0.313 M and = 2.031

Also

[   

Putting in the values we get:

for the acid is

sodium (na), for example, has one electron in its valence shell. this is an unstable state because that valence shell needs eight electrons to be full. in order to fill its valence shell, find a way to add seven electrons to its valence shell

given:

mass of na = 115 g

excess cl2

to determine:

mass of nacl produced

explanation:

given reaction is-

2na(s) + cl2(g) → 2nacl(s)

since cl2 is in excess, na will be the limiting reagent

as per the reaction stoichiometry na: nacl = 1: 1

i.e. moles of na reacted = moles of nacl formed

now, # moles of na = mass of na/atomic mass

                                  = 115 g/23 g.mol-1 = 5 moles

therefore, moles of nacl = 5

molar mass of nacl = 58 g/mol

mass of nacl = 5 moles * 58 g.mol-1 = 290 g

ans: amount of nacl produced = 290 g