Asked by Lena

Calculate the pH of 0.20 M NaCN solution.

NaCN ---> Na+ + CN-

CN- + H20+ ---> HCN+ + OH-

Initial conc. of CN- = 0.20 mol/L
change = -x
equillibrium = 0.20-x

HCN equill. = +x
OH equill. = 1x10^-7+x

Ka= 6.2 x 10^-10

Kb = KW/Ka = 1x10^-14/6n2 x 10^-10 = 1.6 x 10^-5

1.6 x 10^-5 = [x][1x10^-7+x]/0.2
QUADRATIC FORMULA:
x= 1.8 x 10^-3

pOH = -log(1.8x10^-3)
= 2.73

Ph = 14 - POH
=11.26

DID I DO THIS CORRECTLY?
How would I determine whether or not the CN- was an acid or a base. I was thinking this. The HCN is an acid so when you take the H off of it it becomes the conjugate base. Is this also correct?
Answered by DrBob222
Calculate the pH of 0.20 M NaCN solution.

NaCN ---> Na+ + CN-

CN- + H20+ ---> HCN+ + OH-

Initial conc. of CN- = 0.20 mol/L
change = -x
equillibrium = 0.20-x

HCN equill. = +x <b>OK to here.</b>
OH equill. = 1x10^-7+x <b> This is also +x.
I will let you redo the math to get pH but I solve for pH and obtained 11.25.</b>

Ka= 6.2 x 10^-10

Kb = KW/Ka = 1x10^-14/6n2 x 10^-10 = 1.6 x 10^-5

1.6 x 10^-5 = [x][1x10^-7+x]/0.2
QUADRATIC FORMULA:
x= 1.8 x 10^-3

pOH = -log(1.8x10^-3)
= 2.73

Ph = 14 - POH
=11.26

DID I DO THIS CORRECTLY?
How would I determine whether or not the CN- was an acid or a base. I was thinking this. The HCN is an acid so when you take the H off of it it becomes the conjugate base. Is this also correct? <b>Yes, HCN is an acid, you remove the H and the CN^- becomes the conjugate base (because it will accept a proton).</b>
Answered by Lena
I redid it and I got 11.25 :) Thanks :)
Answered by geeta
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