Question

Calculate the pH of an aqueous 0.03M nitrous acid solution (HNO.) at 25°C if the K of HNO, IS 4.0x 10 at this temperature Question 30 Not yet answered Marked out of 2.50 P Flag question Select one O a. 3.46 x 10 O b .2.46 C 1.37 d. 13.44 e. 10.8

Answer 1

let xa degree of can change i concentration Answers of this question ; HNO, get dissociated as- - Ka= 4,0810-4 HNO - H+ + Nož c= Initial Initially -e [ 1 0 0 concentration final = 0.03 M (C-ca) , cal ca CHA) (NO) Then, ka= dissociation then, (HNO2) (ca) (ex) (C-ca) is as we know a is a very small quantity which is ka= cat se kajka ne e then (1-2) 1 (H+)= ca sexta Teo (H+). 70.03 x 4.0X10-4 0.12 x10-4 = 0.3464x10-2 polt) = -log (H1) - pH o log (0.3464 x10^2) = 2.4604 2.46 $ So, the correct answer is 2.46: са clla) negligeble to 0

Select o a. 3.46810-3 sob. 2.46 oc, 1:37 O d. 13:44 o e. 10.8