Calculate the pH of 1.00 L of a buffer solution which contains 0.120 mole of nitrous...

Question

Question

science chemistry

Answer 1

Answer #1

It is case of acidic buffer

v=1L ne 0.120 mol HNO2 [HH] n 0-120 = 0.120M Nano n=0.105 mol (Naną] - 0.105 0.105M pkq af HNO It is = 3.39 Case of Aridic Bu

Answer 2

Similar Homework Help Questions

A buffer solution contains 0.120 mole of propionic acid, and 0.110 mole of potassium propionate. the...

A buffer solution contains 0.120 mole of propionic acid, and 0.110 mole of potassium propionate. the buffer solution has a total volume of 1.00 L a) Find the pH of this buffer solution. b) Find the pH of this buffer solution after the addition of 10.0 mL of 0.400 M KOH solution.
A 1.00 L solution contains 22.52 g of nitrous acid, HNO2. What mass of sodium nitrite,...

A 1.00 L solution contains 22.52 g of nitrous acid, HNO2. What mass of sodium nitrite, NaNO2, should be added to it to make a buffer with a pH of 2.96? Ka (HNO2) = 4.0 × 10–4.
A 1.00 L solution contains 23.52 g of nitrous acid, HNO2. What mass of sodium nitrite,...

A 1.00 L solution contains 23.52 g of nitrous acid, HNO2. What mass of sodium nitrite, NaNO2, should be added to it to make a buffer with a pH of 2.36? Ka (HNO2) = 4.0 × 10–4.

A 1.00 L solution contains 15.52 g of nitrous acid, HNO2. What mass of sodium nitrite,...

A 1.00 L solution contains 15.52 g of nitrous acid, HNO2. What mass of sodium nitrite, NaNO2, should be added to it to make a buffer with a pH of 2.66? Ka (HNO2) = 4.0 × 10–4.
A 1.00 L solution contains 20.52 g of nitrous acid, HNO2.What mass of sodium nitrite, NaNO2, should...

A 1.00 L solution contains 20.52 g of nitrous acid, HNO2.What mass of sodium nitrite, NaNO2, should be added to it to make a buffer with a pH of 3.56? Ka (HNO2) = 4.0 × 10–4.
1.) A 1.00 L solution contains 18.52 g of nitrous acid, HNO2.What mass of sodium nitrite, NaNO2,...

1.) A 1.00 L solution contains 18.52 g of nitrous acid, HNO2.What mass of sodium nitrite, NaNO2, should be added to it to make a buffer with a pH of 2.76? Ka (HNO2) = 4.0 × 10–4. 2.) Calculate the change in pH when 0.310 mol H+ is added to 1.00 L of each of the following buffers. a) a 0.580 M solution of pyridine (py) containing 0.480 M pyH+ (CHANGE IN PH?) b)a 0.600 M solution of aniline (an) containing...

What would be the pH of a buffer that contains 0.987 grams of Nitrous acid (HNO2)...

What would be the pH of a buffer that contains 0.987 grams of Nitrous acid (HNO2) and 1.242 grams of sodium Nitrite (NaNO2), in 250ml of solution?(Ka of Nitrous acid = 4.5X10-4)
Calculate the pH of 1.00 L of a buffer that is 1.00 M in acetic acid...

Calculate the pH of 1.00 L of a buffer that is 1.00 M in acetic acid and 1.00 M in sodium acetate after the addition of 0.150 mole of NaOH.
İl See Periodic Table O See Hint A 100 L solution contains 2132 of nitrous acid,...

İl See Periodic Table O See Hint A 100 L solution contains 2132 of nitrous acid, HNO, What mass of sodium nitrite NaNo, should be added to it to make a buffer with a pH of 3.267 K, THNO.) - 40*10

a) Calculate the pH of 0.500 L of a buffer solution that contains 0.200 M of...

a) Calculate the pH of 0.500 L of a buffer solution that contains 0.200 M of benzoic acid C6H5CO2H and 0.100 M sodium benzoate NaC6H5CO2. Ka = 6.3 x 10-5. b) Calculate the pH after .10 mL of 1.00 M H+ has been added. c) Calculate the pH after 10 mL of 1.00 M OH- has been added.