Question

The pH of mixture of 0.01 M HCl and 0.1 M CH3COOH is approximately equal to?

Answer 1

Hope it helps!!!!


0.01M Hcl and 0.1M CH3COOH is Given 

So H+  in HCl will be 10-2 and also in CH​3COOH is 10-1 

Let volume of HCl and CH3COOH be V 

According to formula H+ =N1V1 + N2V2/ total
volume 

Here,

N1=1* 10-2 and N2=1*10-1 

So by putting in formula,

H+= 10-2* V +10-1* V/2V

H​+=11*10-2/2

H+= 5.5 * 10-2

So, PH= - log[H+] 

Therefore  PH= - log[5.5 * 10-2]

PH=2- log 5.5
PH=2-0.74 
PH=1.26

#Be Brainly✌️

Answer 2

Answer:the ans is 2

Explanation:CH3COOH is a weak acid . Inspite of having greater molarity its dissociation into ions would be very less. So the H+ ions formed by the dissociation of CH3COOH would be very lessas compared to the dissociation pf HCl. So we would consider only the H+ ion concentration of HCl

pH = -log (0.01)

pH = -log (1+10^-2)

pH = 2

HOPE THIS HELPS✌