Given below are two statements: one is labelled as Assertion (A) and the other is labelled as Reason (R).
Assertion (A): Cu$$^{2+}$$ in water is more stable than Cu$$^{+}$$.
Reason (R): Enthalpy of hydration for Cu$$^{2+}$$ is much less than that of Cu$$^{+}$$.
In the light of the above statements, choose the correct answer from the options given below:

We need to analyze the Assertion-Reason statement about Cu$$^{2+}$$ and Cu$$^{+}$$ stability in water.

Assertion (A): Cu$$^{2+}$$ in water is more stable than Cu$$^{+}$$.

Reason (R): Enthalpy of hydration for Cu$$^{2+}$$ is much less than that of Cu$$^{+}$$.

Analysis of Assertion:

Cu$$^{2+}$$ is indeed more stable than Cu$$^{+}$$ in aqueous solution. This is because Cu$$^{+}$$ undergoes disproportionation in water:

$$2\text{Cu}^+(aq) \rightarrow \text{Cu}^{2+}(aq) + \text{Cu}(s)$$

So Assertion A is correct.

Analysis of Reason:

The enthalpy of hydration of Cu$$^{2+}$$ is much more negative (more exothermic) than that of Cu$$^{+}$$, due to the higher charge density of Cu$$^{2+}$$. The reason states that the enthalpy of hydration of Cu$$^{2+}$$ is "much less" than that of Cu$$^{+}$$, which is incorrect - it should be "much more negative" or "much greater in magnitude".

However, the large hydration enthalpy of Cu$$^{2+}$$ compensates for the high second ionization energy, making Cu$$^{2+}$$ more stable in water. But the Reason as stated says hydration enthalpy of Cu$$^{2+}$$ is less than Cu$$^{+}$$, which is incorrect.

Therefore, A is correct but R is not correct.

The correct answer is Option B: (A) is correct but (R) is not correct.