Quick Question

[BAJackson16]

---

Members don't see this ad.

How many ml of 10 M NaOH will take to completely titrate 3ml of 1M H3PO4?

Do I just use N1V1=N2V2
How does titration differ from dilution and neutralization?

 

[ems5184]

I think that for this problem, titration is equivalent to neutralization. I would choose to do it using N1V1=N2V2 as you said.

 

[sinned]

I think you are dealing with a strong base with a polyprotic acid with 3 acidic hydrogens.

so if you do a M1V1 = M2V2 you get, (10M)(V1) = (1M)(1mL)
therefore, V1=0.3mL

that is to neutralize one of the acidic hydrogens, so (3)(0.3mL)=0.9mL

is that the correct answer?

 

[BAJackson16]

yes that is what I was thinking...just making sure. Thanks for the help. I didnt have an answer for that one...just found that question in chem book

 

[ems5184]

yea thats the same as using N1V1=N2V2

with this equation you set it up as follows:
(10 N NaOH)(X mL) = (3 N H3PO4)(3 mL)

and then when rearranging, you get 9/10 = 0.9 mL, so same answer as you got sinned.

 

[sinned]

yea thats the same as using N1V1=N2V2

with this equation you set it up as follows:
(10 N NaOH)(X mL) = (3 N H3PO4)(3 mL)

and then when rearranging, you get 9/10 = 0.9 mL, so same answer as you got sinned.

😉