Question

TEACH ME how to do question 2 through your explanations.

Answer 1

Step-by-step explanation:

H20 has pH of 7

1st reaction [H30+] = 10^-7M

[OH-] = 10^-7M

1M HCl has pH of 0

2nd reaction [H3O+] = 1M

[Cl-] = 1M

given Ka = 4.6x10^-3 = [H3O+]x[NO2-] / [HNO2]

and [HNO2] + [NO2-] = 1M

each concentration can be solved

beaker D is a buffer solution n requires more info 2 solve

Answer 2

Step-by-step explanation:

The first two are easy:

H2O, H3O+ and OH- all exist in an equilibrium

[H3O+] = [OH-] = 10^-7 M

HCl is a strong acid so 1M of it will disassociate completely

[H3O+] = [Cl-] = 1 M

The third one is also an equilibrium as HNO2 is a weak acid. Ka is given so [HNO2] and [NO2-] can be calculated.

The fourth one is a buffer solution so its pH can be looked up to give the concentrations.