Question

a) What is the percent dissociation of a 0.45 M solution of nitrous acid?

b) What is the present dissociation of a 0.28 M solution of methylmine?

c)0.0950 M soution of acetic acid is 1.4% dissociated. Calculated concentration of three species present in this solution: hydronium ion, acetic acid, and acetate ion(not H2O or OH-):

d)what is present dissociation of a 0.35 M solution of hydrobromic acid?

Answer 1

a) Ka of nitrous acid is 4*10^(-4)

Molarity = 0.45 M

Calculate the [H+] concentration

4*10 ^ (-4) = [(x)(x)/0.45]

Calculate x, we get x as

x=1.34 * 10^(-2)

Divide the [H⁺] by the concentration, then multiply by 100

1.34*10^(-2)/0.45 = 2.98*10^(-2)

This multiplied by 100 gives us 2.98% dissociation.

b.) Ka for methylamine is 4.2 * 10^(-4)

The rest can be calculated in the exact same way as explained above

The answer to this is3.87%

c.) Need time to answer

d.) ka for hydrobromic acid is 10 ^ (9)

As per the procedure above the answer would be [5.28 * 10^(6)]%