2. (1 pt) A solution has an [OH] 3.6 x 10 M. Determine the [H\'] and pH of this

Question

2. (1 pt) A solution has an [OH] 3.6 x 10 M. Determine the [H'] and pH of this solution. Is this solution acidic or basic? Show all your work. (Refer to equations 1 and 2.) 3. (1 pt) Define buffer 4. (2 pts) Consider the following three solutions A, B, and C, all at the same pH 5.0.The pH of the solutions after the addition of a small amount of a strong acid, HCl and a small amount of a strong base, NaOH are given below. Calculate the change in pH after the acid and base addition. Of the three solutions, which solution is acting as a buffer? Explain your answer using the definition of a buffer and using the data provided. Solution | pH after acid addition | | pH l acid! pH after base addition! I pH 1 base 3.5 4.5 2.0 7.5 5.5 5.5

Explanation / Answer

2)

use:
[H+] = Kw/[OH-]
Kw is dissociation constant of water whose value is 1.0*10^-14 at 25 oC
[H+] = (1.0*10^-14)/[OH-]
[H+] = (1.0*10^-14)/3.6E-6
[H+] = 2.78*10^-9 M

use:
pH = -log [H+]
= -log (2.78*10^-9)
= 8.56

use:
pOH = -log [OH-]
= -log (3.6*10^-6)
= 5.4437

Since pH > pOH, this is basic in nature

Answers:
[H+] = 2.78*10^-9
[OH-] = 3.6*10^-6
pH = 8.56
It is basic

I am allowed to answer only 1 question at a time

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