Chemistry problems on Bronsted base?

Question

Hi, I study at home and I am having a hard time with Chemistry. I need urgent help!! I added three problems that I would be very thankful if anyone helped solving them. THANK YOU VERY MUCH!!


Consider HSO-4 , NH+4 , H2O , SO2-2. Which one or which ones can be classified as Bronsted base?


a) HSO-4 , NH+4 , H2O ,

b) H2O and SO2-2

c) HSO-4 Only

d) NH+4 Only

e) SO2-2 Only



Fix the coefficient of the following reactions, using the oxi-reduction method.


a) P + HNO3 + H2O ---- H3PO4 + NO

b) Hg + HNO3 ----- Hg (NO3)2 + H2O + NO

c)MnO2 + HBr ---- MnBr2 + Br2 + H2O


In the reaction HNO3 + H2S --- H2O + NO + S , the sum of all coefficients after the adjustment will be:

( ) 16
( ) 20
( ) 14
( ) 12
( ) 18

Answer 1

Bronsted bases are proton acceptors. HSO4- is one, because it can become H2SO4. H2O is one, because it can become H3O+, the hydronium ion. NH4+ cannot be, because it has already accepted a proton and is thus called a conjugate acid in the Bronsted system. I do not know what you mean by SO2-2. Maybe add details.

Also, keep watching this space. I will return with more of your answers.

P + HNO3 + H2O ===> H3PO4 + NO
P---------------- -5e- ---------------H3PO4
HNO3---------- +3e---------------------NO

Electrons lost must equal electrons gained. So multiply the P by 3 and the HNO3 by 5, and you get:

3P +5HNO3 + 2H2O ===> 3H3PO4 = 5NO

Hint: After you multiply the two reactants, look at the H's on the right. There are 9. Once you have that, you get the coefficient for H2O = 4.