Which of the following statements is/are true for a 0.10 m solution of a weak acid ha? (a) the ph is 1.00 m (b) [h+ ] > > [a - ] (c) [h+ ] = [a -

c. [H+] = [A-]

The dissociation of weak acid in water occurs as shown by the equation;

HA → H+ + A-

The initial concentration of the weak acid is 0.10 M

Since you are dealing with a weak acid, all of it will not be dissociated to free H+.

Equal number of H+ and A- will be formed when HA dissociates. All the molecules will not be dissociated since it is a weak acid.

the ideal gas law equation is as follows

pv = nrt

where p - pressure

v - volume

n - number of moles

r - universal gas constant

t - temperature

so if the pressure, volume and temperature are already known

we are left with n and r

since r is the universal gas constant that has a known fixed value then r too is known

so we are left with 'n'

once we know temperature volume and pressure

we can find the number of moles of gas present using the ideal gas law equation

this is not my own answer, this is an answer for the same question by the user blahblahmali. i do not claim ownership of this account.

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