please help within five minutes

Chemistry
Tutor: None Selected Time limit: 1 Day

Calculate the pH of a 1.40×10-1 M aqueous solution of hydrazine hydrochloride (H2NNH3Cl).

(For hydrazine, H2NNH2Kb = 3.00×10-6.)

Feb 14th, 2015

H2NNH3+        =>    H2NNH2     +       H+      ;     Ka = Kw/Kb = (10^-14)/(3.00*10^-6)   = 3.34 * 10^-9

   0.140                           0                      0 

      -x                             +x                     +x

 (0.140-x)                      (x)                     (x)  

Ka = (3.34*10^-9) = (x^2) / (0.140-x)      

Rearrange and quadratic formula gives    =>   x = 2.16 * 10^-5 M 

pH = -log(2.16*10^-5) = 4.7 


Feb 14th, 2015

Studypool's Notebank makes it easy to buy and sell old notes, study guides, reviews, etc.
Click to visit
The Notebank
...
Feb 14th, 2015
...
Feb 14th, 2015
May 30th, 2017
check_circle
Mark as Final Answer
check_circle
Unmark as Final Answer
check_circle
Final Answer

Secure Information

Content will be erased after question is completed.

check_circle
Final Answer