You can predict the [O2] vs pressure and temperature using Henry's law and the van 'tHoff equation.

The Henry's law constant for O2 in water is 3.2 x 10-2, the van 'tHoff coefficient is 1700K.

The Henry's law coefficient given is dimensionless, so Caq = Hcc x Cg where both concentraltions are in mol / litre.

Translating mol / litre O2 in gas to pressure for O2 assuming 22.4 litres / mole at STP and mole / litre O2 in solution to the more familiar mg/l [O2] at 32 g / mol gives a Henry's Law coefficient of 0.42 mg / l. kPa, note that this is absolute pressure so you'll need to add 101 kPa to your gauge pressure.

The above applies at 25 oC (298 K), let's assume you are doing this at around 4 oC (277K), the van 'tHoff equation is then

H(T) = Ho . e [coefficient. (1/T-1/To)]

with the coefficient already given as 1700, so the quotient is e [ 1700 . (1/277 - 1/298)]

= e 0.43

= 1.54

so at 4 degrees the Henry's Law coefficient will be 0.65 mg/l/kPa, again note this is absolute pressure not gauge.

10 PSI is about 70 kPa gauge or about 170 kPa absolute, equilibrium [O2] is therefore about 110 mg/l .