ionic equation for this titration formula (1 Viewer)

[deadbeat]

I know for say HCl

its H+ + Cl-


however given this


H2So4 + 2NaOH -> Na2SO4 + 2H20


how do i write the ionic equation for it?

2H+ ... ??

or

H2+ ... ??

or H+ + H+



what do we do for the subscript 2 for the H2SO4 and the 2 mole of NaOH

 

[deadbeat]

thanks buddy

 

[deadbeat]

can u check my answer to this?

Calculate the molarity of a Sodium Hydroxide solution if it required 2.96mL of 0.225M H2S04 to completely react with 2.00ml of the Hydroxide.



My answer

in 2.96mL 0.225M H2s04 => 0.225mol/1000ml x 2.96mL = 0.00066 mol H2SO4

therefore 0.00066 mole in 2mL of OH

therefore [OH] = 0.00066/2ml x 1000 = 0.333 mol/L

[OH] = [NaOH] = 0.333M

not sure about the last line now, since you divided the whole net ionic equation by 2. is the mole ration between OH and NaOH still 2:2 or is it now 1:2 ???

 

[Mark576]

H₂SO_4(aq) + 2NaOH_(aq) -> Na₂SO_4(aq) + 2H₂0_(l)

As you can see, the mole ratio of H₂SO_4(aq) to NaOH_(aq) is 1:2.

 

[WantToDoBetter]

not sure about the last line now, since you divided the whole net ionic equation by 2. is the mole ration between OH and NaOH still 2:2 or is it now 1:2 ???

Don't worry about the ionic equation when it comes using the mole ratio. Just look at your neturalisation reaction and use the ratio that appears there.
Cheers.