A. no color change was observed indicating that changing temperature does not affect equilibrium. b. increasing the temperature changes the solution to blue indicating that the equilibrium shifts to the left and decreasing the temperature changes the solution to pink indicating that the equilibrium shifts to the right. c. increasing the temperature changes the solution to pink indicating that the equilibrium shifts to the right and decreasing the temperature changes the solution to blue indicating that the equilibrium shifts to the left.

As the reaction equation is:
COCl4(aq) + 6 H2O(l) ↔ CO (H2O)6(aq) +4 Cl + Heat (missing in your question)
(Blue)                                    (pink)

So the correct answer which reflects the temperature effects is (b) increasing the temperature changes the solution to blue indicating that the equilibrium shifts to the left and decreasing the temperature changes the solution to pink indicating that the equilibrium shifts to right.
- as when the heat increases (and it's a product) the reaction move towards the reactants to increase the reactants to make the equilibrium again so it shifts leftwards and  COCl4 which has the blue indicator will increase to make the equilibrium.
-But when the temperature decreases the reaction move towards the products to increase the products (which the heat one of them) to make equilibrium again so, it shifts rightwards and CO(H2O)6 (which has the pink indicator) will increase to make the equilibrium. 

Tolerance to high levels of salinity

The answer is the first option just took the test