I hope this is the right place to ask. We have this exercise without solution
One litre of diluted sodium hydroxide solution (c = 0.15mol/litre) is to be prepared in the laboratory. The titer from the finished NaOH solution is then determined. For this purpose, 0.62 g potassium hydrogen phthalate (M = 204.2 g/mol, $pK_a = 5.4$) are dissolved in 0.05 litre of water and titrated with the prepared sodium hydroxide solution until turnover. The consumption is 0.022 litre. Calculate the titer of the prepared sodium hydroxide solution.
On Wikipedia, I found "In titration, the titer is the ratio of actual to nominal concentration of a titrant" https://en.wikipedia.org/wiki/Titer
So if I understand correctly, the titer is just a fraction of the form $ t = \frac {c_{real}} {c_{ideal}} $, so a fraction of the real concentration over the ideal concentration, is this correct ?
In our case, we would simply need to use the titration equation at equivalence point: $$V_1 \cdot M_1 = V_2 \cdot M_2$$ where $V$ is the volume and $M$ the molarity
So we would solve
$$M_2 = \frac{V_1 \cdot M_1}{V_2} $$
and then the titer is $$t = \frac{c_{real}}{c_{ideal}} = \frac{M_2}{0.15} $$ because 0.15 mol/litre is given as ideal concentration in the exercise
$V_1$ and $V_2$ are given as 0.05 litre and 0.022 litre, and $M_1$ could be found by dividing 0.62 g by the molar mass (M = 204.2 g/mol), and then divide again by the volume of 0.05 litre
I am really unsure because there aren't a lot of results when searching on the Internet, so it seems to me that this isn't a frequently searched topic. Is my understanding above correct ? Why are there relatively few search results for the titer in Chemistry ? Even on this site, I did not find a similar question. Is this topic considered "not important" or am I missing something ?