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

the answer is either b or c

when [oh-] is 10-5  m, and [h3o+] is 10-9  m, the poh is 5 and ph is 9. again in both cases the sum of ph and poh is 14. however, the hydrogen ion concentration is not always going to be equal to exactly 1 x 10 raised to a negative number. for example, we skipped over the value of 2.0 x 10-7.