How many moles of are in 179 ml of a 3.0 m of cacl2 solution?

0.537 moles

Explanation:

Hello, Let's first explain the term molarity

---> Molarity is the most commonly used term to describe the concentration of a solution. It is equal to the moles of solute divided by the liters of solution.

---> The solute is defined as the substance being dissolved, while the solvent is the substance where the solute is dissolved (usually water).

---> The solution is the combination of the solute and the solvent.

Molarity = moles of solution/Liters of

solution

Parameters given are

Volume(V) = 179ml of CaCl2 solution

Molarity = 3.0m

Therefore,

Molarity = number of moles of CaCl2 solution / Volume of CaCl2 in Liters (eqn 1)

First, convert 179ml to liters

1ml = 0.001L

179ml = ?

179ml = 179ml x 0.001L

= 0.179L

From (eqn 1)

Let the number of moles of CaCl2 solution be M

=> 3 = M/0.179

M = 0.179 x 3

= 0.537 moles

Hence the number of moles in 179ml of CaCl2 solution yields 0.537 moles

since the atomic number is the number of protons in the nucleus, as we move to the left on the periodic table, the electrostatic pull between the nucleus and the valence electron shell decreases. as we move down a group (vertical column), the valence shell energy level gets further and further from the nucleus.

"you start with 15.67 g mgco3-xh2o, when heated and all the water is removed, you are left with 7.58 g mgco3 only.

therefore, you had 15.67 - 7.58 = 8.09g h2o  

moles of each :

7.58g mgco3 = ? moles = 7.58g / 83.4g/mole = 0.09moles  

8 09g h2o = ? moles = 8.09g / 18g/mole = 0.44moles  

molar ratio between the two by dividing both numbers by the smallest number :

0.09 / 0.09 = 1  

0.44 / 0.09 = 4.8  

mgco3-5h2o"