CameraIcon
CameraIcon
SearchIcon
MyQuestionIcon
MyQuestionIcon
Question

An acidified solution of 0.05M Zn2+ is saturated with0.1M H2S. What is the minimum molar concentration (M) of H+ required to prevent the precipitation of ZnS?

UseKsp(ZnS)=1.25x10-22 and overall dissociation constant of H2S, Knet=K1K2=1×10-21.


Open in App
Solution

Step 1: It is given that Zn2+=0.05M, H2S=0.1M, solubility product KspZnS=1.25×10-22, overall dissociation constant of H2S, KNET=K1K2=1×10-21.

Step 2: We know that, Zn2+S2-=Ksp

Step 3: So, S2-=1.25×10-220.05=2.5×10-21M

Now, dissociation of H2S is H2S2H++S2-

So, Knet=H+2S2-H2S

Putting the values in the equation,

we get, 10-21=H+2×2.5×10-210.1H+2=0.1×10-212.5×10-21=125=0.2M

Therefore, the minimum molar concentration (M) of H+ required to prevent the precipitation of ZnS is 0.2M.


flag
Suggest Corrections
thumbs-up
1
BNAT
mid-banner-image