At a laboratory, there are two solutions inside beakers: \(200 \text{ cm}^{3}\) of an aqueous solution of sodium hydroxide \(0.3\) mole/L and \(200 \text{ cm}^{3}\) of an aqueous solution of hydrochloric acid \(0.25\) mole/L. These two solutions are mixed inside another beaker and the resulting solution is heated to \(400^\circ C\). What is the approximate concentration, in moles/L, of **sodium ions** on this resulting solution after the heating?

**Details and Assumptions:**

- Use the initial values to calculate things related to
*spilled*liquid (if there is), as concentrations and number of moles. - The laboratory's room temperature is 25°C and the system was,
*initially*, in complete thermal equilibrium. - Do not consider any heat release due to breakage of chemical bonds.
- The beakers' volumetric thermal expansion coefficient is \(5 \times 10^{-5} °C^{-1}\) and the resulting solution's volumetric thermal expansion coefficient is \( 5.43 \times 10^{-4} °C^{-1}\).
- Do not consider the middle stages of the heating process. Use in your calculations the values related to the moment after the heating.
- The resulting solution is unsaturated and its solutes are distributed homogeneously in the beaker's space.
- Do not consider any water production due to any chemical reaction.
- The beaker that contains the resulting solution is, at the end of all processes, completely full.
- Do not consider any volume contraction due to hydrogen bonds that might be formed.

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