Dissolving NaOH(s) in water is exothermic. Two calorimetry experiments are set up.2 g of NaOH are dissolved in 100 mL of water. 4 g of NaOH are dissolved in 200 mL of water. Which of the following statements is true? a. the second temeprature change will be approximately twice the first.
b. the second temperature change will be approximately four times the first.
c. both temperature changes will be the same.
d. the second temperature change will be approximately one-half of the first.
e. the second temperature change will be approximately one-fourth the first.

c. both temperature changes will be the same

Explanation:

When NaOH is dissolved in water, heat is released. The reaction is:

NaOH(s) → Na⁺(aq) + OH⁻(aq) + Δ

That means a determined quantity of NaOH produces a determined quantity of heat.

Thus, 4g of NaOH produces twice the heat of 2g of NaOH. But, as the volume of the dissolution of 4g occurs in 200mL of water (Twice the volume of the other experiment) the net temperature change in both experiments will be the same, thus:

c. both temperature changes will be the same

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