If 2.500 g of copper (II) chloride was added to 150.0 mL of a 0.500 M copper (II) chloride solution, what is the concentration of the new solution

0.624 M

Explanation:

Step 1: Calculate the moles of copper (II) chloride in the initial solution

We had 150.0 mL of a 0.500 M copper (II) chloride solution. The moles of copper (II) chloride present were:

0.1500 L × 0.500 mol/L = 0.0750 mol

Step 2: Calculate the moles of copper (II) chloride added (2.500 g)

The molar mass of copper (II) chloride is 134.45 g/mol.

2.500 g × (1 mol/134.45 g) = 0.01859 mol

Step 3: Calculate the total number of moles of solute in the final solution

0.0750 mol + 0.01859 mol = 0.0936 mol

Step 4: Calculate the molarity of the final solution

M = 0.0936 mol / 0.1500 L = 0.624 M

answer; i believe that the correct answer is (a) potassium(k)

metals are good conductor of electricity. it has free electrons on their surface. according to electron pool theory, each atom present in a metal crystal losses all of its valence electron and as a result a pool of free is form. these pool of electrons are free to move and   conduct electricity easily   while making metal as good conductor.

the correct answer is a. the ability of electrons to flow throughout the metal.

if it's not useful, feel free to report for mistake in answer.