How do I calculate the concentration of HCl in a beaker using NaOH titration?

[Jaramide]

Normally i wouldn't post this in here and I am very sorry if I am breaking any rules but i need quick help or I am toast. already posted in the chem forum but I am afraid it will take to long to get an answer.

I need to return an asignment today and i just can't figure it out (should probably be a piece of cake for the people that hangs around here)

There is 10ml HCl with an unknown concentration i a beaker. You let NaOH with the concentration 0,100 mol/dm3 drip into the acid until it is neutralized.
It takes 10,5ml NaOH to neutralize the acid.

With this you should be able to calculate the concentration of the acid or so my teacher say. And all i can do is sit here and look dumb while my brain refuses to cooperate

Could anyone help me i would owe you a life debt. If i don't get this in today i won't get a grade in chemistry

 

[himanshu121]

Apply the normality equation

$$N_{HCl}V_{HCl}=N_{NaOH}V_{NaOH}$$

Here normality is equal to Molarity

Hence Concentration is either given by normality/molarity

Stength is given by Molarity*Molecular Weight

 

[Jaramide]

Ok, just to check.

So i take
10,5ml * 0,1 = 1,05
10 * x = 1,05
1,05 / 10 = 0,105
10 * 0,105 = 1,05

So the concentration of HCl is 0,105mol/dm3 or have i gotten it completley wrong?

*edit* After checking that over i don't think it can be that simple.
I know that knowing what type of acid it is is instrumental to the calculations and this don't involve that at all so I am dead wrong.
Back to square one :(

 

[himanshu121]

Yes it is correct and it is that simple.

I believe u know the equation that i quoted
It definitely gives correct results

 

[Jaramide]

...Wow. I managed to get it right
I thank you for helping me out. Without that little kick in the right direction i wouldn't have manged to solve it.
Thank you again, i owe you.

 

[himanshu121]

u owe me