Question

How do you solve titration problems?

Answer 1

Try using dimensions when you do the calculations.

Explanation:

With a titration a measured quantity of titrant is added to a known mass of known molar quantity.

We use the relationship, `"moles "="Mass"/"molar mass"`,

and `"Molarity (concentration)"` `=` `"Moles of stuff"/"Volume of solution"`

Now when we use `"molarity"` we can preserve the dimensions: `mol*L^-1` are the units for concentration.

When we multiply a concentration by a VOLUME, we get the product, `mol*cancel(L^-1)xxcancelL=mol`.

Now a chemical reaction is VITAL when you do a titration. For acid/base titrations this is typically:

`H_3O^+ + HO^(-) rarr2H_2O(l)`

The stoichiometric equivalence must be borne in mind, when you do the calculation. So, as a general rule, you must have the appropriate, stoichiometrically balanced chemical equation. Most of the time, there is 1:1 molar equivalence, and,

`C_1V_1=C_2V_2`, where `C-="concentration"` as we defined.