What is the pH of a 0.250 M NaOCl solution? Kb = 3.4 x 10-7

Expert Solution

construct the ICE table

NaOCl (aq) + H2O (l) <====> HOCl (aq) + NaOH (aq)

I 0.25 0 0

C -x +x +x

E 0.25-x +x +x

Kb = [HOCl] [NaOH] / [NaOCl]

3.4 x 10^-7 = [x] [x] / [0.25-x]

x² + x 3.4 * 10^-7 - 8.5 x 10^-8 = 0

solve the quadratic equation

x = 2.91 x 10^-4 M = [NaOH]

pOH = -log(OH-) = -log(2.91 x 10^-4) = 3.53

pH + pOH = 14

pH = 14-pOH = 14-3.53 = 10.46M

queen_honey_blossom answered 1 year ago

What is the pH of a 1.3 x 10-7 M solution of HCl? Please note that...

What is the pH of a 1.3 x 10-7 M solution of HCl? Please note that you cannot simply add the contribution of H+ ions from the autoproteolysis of water and the contribution from the dissociation of HCl. You will need to use the quadratic equation to solve this problem and report the answer to 4 significant figures.

What is the pH of a 1 x 10-7 M solution of HCl? Please note that...

What is the pH of a 1 x 10-7 M solution of HCl? Please note that you cannot simply add the contribution of H+ ions from the autoproteolysis of water and the contribution from the dissociation of HCl. You will need to use the quadratic equation to solve this problem and report the answer to 4 significant figures. For a hint see the Acids and Bases handout on Canvas.

Calculate the [OH-] and pH of a 0.01 M solution of ammonia (Kb= 1.8 x 10^-5)

Calculate the pH of a liter of 0.125 M ammonium perchlorate solution. (kb= 1.7 x 10-5)...

Calculate the pH of a liter of 0.125 M ammonium perchlorate solution. (kb= 1.7 x 10-5) show ice chart!

What is the expected pH of a 0.250 M solution of oxalic acid with Ka =...

What is the expected pH of a 0.250 M solution of oxalic acid with Ka = 5.37 x 10^-5 ([H+] = 0.002197) and will the pH increase by one unit if the solution is diluted to 0.0250 M?

Calculate the pH of a 0.21 M solution of C5H5NHCl (Kb for C5H5N = 1.7 x...

Calculate the pH of a 0.21 M solution of C5H5NHCl (Kb for C5H5N = 1.7 x 10-9). Record your pH value to 2 decimal places. Calculate the pH of a 0.17 M solution of KNO2 (Ka for HNO2 = 4.0 x 10-4). Record your pH value to 2 decimal places.

Calculate the pH of 4.55 M aniline, C6H5NH2 ( Kb = 4.0 x 10^-10)

what is the Kb value for a .17 M solution whose pH is 9.45

What is the pH of a 0.608 M solution of ammonium bromide? The Kb value for...

What is the pH of a 0.608 M solution of ammonium bromide? The Kb value for ammonia is 1.8 x 10–5.

Calculate the pH of a .215 M aqueous solution of aniline C6H5NH2, Kb= 7.4x10^-10 and the...

Calculate the pH of a .215 M aqueous solution of aniline C6H5NH2, Kb= 7.4x10^-10 and the equilibrium concentrations of the weak base and it’s conjugate acid Calculate the pH of a 0.0454 M aqueous solution of triethelyene C2H5(3)N, Kb= 5.2x10^-4 and the equilibrium concentrations of the weak base and its conjugate acid

Question