If 5.3g of the strong base NaOH is dissolved in water to form 1500 ml of solution what are the pH [H3O+] and [OH-]

I got up to OH=0.0883 but idk what to do after

NaOH is a strong base therefore it completely ionises to give out hydroxide ions.

Number of moles of NaOH added - 5.3 g / 40 g/mol = 0.1325 mol

molarity of NaOH - 0.1325 mol/1.5 L = 0.088 mol/L

since NaOH - - > Na⁺ + OH⁻

molarity of OH⁻ is 0.088 M

we can calculate pOH value to find the pH value and then [H₃O⁺]

pOH = - log (0.088 M)

pOH = 1.05

pH + pOH = 14

Therefore pH = 14 - 1.05 = 12.95

[H₃O⁺] = antilog (-pH)

Therefore

[H₃O⁺] = 1.12 x 10⁻¹³ M