Physics and Chemistry cannot be separated

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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