How do I find the equivalence point given two different molarities of a acid/base without volume?

Question

I mean, how do you get the moles if you don't know the volume?
Let's say, for example:

0.008 M NaOH and 0.01 M HBr. How would you find the equivalence point?

Ok, I understand that, but how would one calculate the pH of the solution? Would it be 7.00 since it's strong acid/strong base?

Supposed the acid was a weak acid such as HF...how would you calculate the pH at equivalence point in terms of strong base/weak acid?

Thanks.

Answer 1

Your equation is
NaOH + HBr -> HOH + Na+ Br-
If you had a certain volume, say V(HBr), you would have available M(HBr) x V(HBr) moles, where M is the molarity of HBr. Then, you need to provide that number of moles of NaOH. From the analogous equation for NaOH from above, you can compute V(NaOH). While you don't know specific volumes, you do know the ratio of volumes needed. In this case you would have to provide 1.25 V(HBr) of NaOH.

Answer 2

if you have the K value (ration between the concentrations of the products and reactants at equilibrium), you can use the initial concentrations (what you have) and assign the change in concentration a variable and the equilibrium concentrations with that variable in it can be set equal to the K value you were given in order to find the change. If this is what you're looking for, e-mail me and I'll explain further.

Answer 3

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