This is an example of a Schott bottle:
Using the volume markings would not be very accurate, so you would weigh the water.
Citric acid solution is indeed less dense than you would calculate from the volumes and densities of water plus citric acid. 30% solution has a density of 1.13, but the arithmetically calculated density is 1.1995 from citric acid density = 1.665 and water = 1 (CRC Handbook, 62 ed). There were no data for more concentrated solutions.
As Poutnik points out, 59.2% w/w means 59.2% of the final solution is citric acid - yes, it's that soluble! But a better way to make the solution and fill the bottle to the 100 mL mark (if that is important) is to prepare the solution in another flask, by weight. Since you want 100 mL, which will weigh 113 grams, I suggest you go for 125 grams, to have a little extra. 125 x 0.592 = 74 grams citric acid; add 51 grams of warm water (to insure more rapid and complete solution) and swirl till clear. (Swirl the flask, not yourself.)
When the solution is clear, fill the Schott bottle. What to do with the excess solution? Do not fret. Citric acid solution is available commercially as a toilet bowl cleaner. 12 grams of saturated citric acid will not do much cleaning for a really dirty toilet bowl, but at least it won't damage the ecology any more than we normally do.