Determine the pH of a 500 mL solution that is 0.250 M HNO2. ( Ka= 4.6 x 10^-4).

Question

Determine the pH of a 500 mL solution that is 0.250 M HNO2. ( Ka= 4.6 x 10^-4). Show work.
Determine the pH of 500 mL buffer solution that is 0.250 M HNO2 and 0.250. M KNO2. ( Ka = 4.6 x 10^-4)
What is the pH after adding 0.0122 moles NaOH. Same Ka as above. Using an Ice table Determine the pH of a 500 mL solution that is 0.250 M HNO2. ( Ka= 4.6 x 10^-4). Show work.
Determine the pH of 500 mL buffer solution that is 0.250 M HNO2 and 0.250. M KNO2. ( Ka = 4.6 x 10^-4)
What is the pH after adding 0.0122 moles NaOH. Same Ka as above. Using an Ice table
Determine the pH of 500 mL buffer solution that is 0.250 M HNO2 and 0.250. M KNO2. ( Ka = 4.6 x 10^-4)
What is the pH after adding 0.0122 moles NaOH. Same Ka as above. Using an Ice table

Explanation / Answer

pH of weakacid = 1/2(pka-logC)

pka = -logka = -log(4.6*10^-4) = 3.37

c = concentration of acid = 0.25 M

pH = 1/2(3.37-log0.25)

   = 1.986

pH of buffer = pka + log(salt/acid)

    = 3.37+log(0.25/0.25)

pH f buffer = 3.37

after adding 0.0122 moles NaOH

pH = pka + log(salt+base/acid-base)

   =3.37+log((0.25+0.0122)/(0.25-0.0122))

   = 3.412

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