Which are the two Bronsted-Lowry acids in the following equation? NH 3 + HOH ->

Question

1. Which are the two Bronsted-Lowry acids in the following equation?
   
   NH3 + HOH -> NH4+1 + OH-1
   a. NH3 and HOH b. NH3 and NH4+1 c. NH3 and OH-1 d. NH4+1 and HOH
   
   I think it is A or D but I am not sure .
   
   1. What is the concentration of a H2SO4 solution if 10.0 mL of the solution is neutralized by 7.8 mL of a 0.20 M NaOH solution?
      a. 0.0026 M b. 0.078 M c. 0.156 M d. 0.31 M

Which are the two Bronsted-Lowry acids in the following equation?

NH3 + HOH -> NH4+1 + OH-1
a. NH3 and HOH b. NH3 and NH4+1 c. NH3 and OH-1 d. NH4+1 and HOH

I think it is A or D but I am not sure .

1. What is the concentration of a H2SO4 solution if 10.0 mL of the solution is neutralized by 7.8 mL of a 0.20 M NaOH solution?
   a. 0.0026 M b. 0.078 M c. 0.156 M d. 0.31 M

Which are the two Bronsted-Lowry acids in the following equation?

NH3 + HOH -> NH4+1 + OH-1
What is the concentration of a H2SO4 solution if 10.0 mL of the solution is neutralized by 7.8 mL of a 0.20 M NaOH solution?
a. 0.0026 M b. 0.078 M c. 0.156 M d. 0.31 M What is the concentration of a H2SO4 solution if 10.0 mL of the solution is neutralized by 7.8 mL of a 0.20 M NaOH solution? a. 0.0026 M b. 0.078 M c. 0.156 M d. 0.31 M

Explanation / Answer

1) d

2) M(H2SO4) x V(H2SO4) x 2 = M(NaOH) x V(NaOH)

M(H2SO4) = 0.20 x 7.8 / (2 x 10.0) = 0.078 M

answer b is correct.

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