1. Given data

• Mass of ice: $m = 600\text{ g} = 0.6\text{ kg}$
• Initial temperature of ice: $-12^\circ\text{C}$
• Heat supplied: $Q = 184\text{ kJ}$
• Specific heat of ice: $c_i = 2222.3\,\text{J kg}^{-1}\,^\circ\text{C}^{-1}$
• Latent heat of fusion of ice: $L = 336\text{ kJ/kg}$

We must determine the final state.

2. Heat required to raise ice from $-12^\circ\text{C}$ to $0^\circ\text{C}$

$Q_1 = mc_i\Delta T$

$Q_1 = (0.6)(2222.3)(12)\,\text{J}$

$Q_1 = 15999\approx 16000\,\text{J} = 16\text{ kJ}$

So, $16\text{ kJ}$ is needed to bring the ice to $0^\circ\text{C}$.

3. Remaining heat for melting

Total heat given is $184\text{ kJ}$, so remaining heat after bringing ice to $0^\circ\text{C}$ is

$Q_{\text{rem}} = 184 - 16 = 168\text{ kJ}$

4. Heat required to melt all the ice

$Q_{\text{melt, all}} = mL = (0.6)(336)\text{ kJ}$

$Q_{\text{melt, all}} = 201.6\text{ kJ}$

But only $168\text{ kJ}$ is available for melting, which is less than $201.6\text{ kJ}$.

Therefore, all the ice will not melt.

Hence the final temperature remains:

$0^\circ\text{C}$

So statement A is true and statement B is false.

5. Amount of ice melted

$m_{\text{melted}} = \frac{Q_{\text{rem}}}{L} = \frac{168}{336} = 0.5\text{ kg}$

So, water formed = $0.5\text{ kg}$.

Initial ice mass = $0.6\text{ kg}$, so ice left =

$0.6 - 0.5 = 0.1\text{ kg}$

Thus final mixture is:

• Ice = $0.1\text{ kg}$
• Water = $0.5\text{ kg}$

Ratio of ice : water =

$0.1:0.5 = 1:5$

So statement D is true and statement C is false.

Also, statement E is false because some ice remains.

6. Checking given options

• A: A and E only $\to$ false
• B: B and D only $\to$ false
• C: A and C only $\to$ false
• D: A and D only $\to$ true

7. Final answer

The correct option is:

$\boxed{\text{D: A and D only}}$