How many grams of CaCl2 would be dissolved in 1.4 L of a 0.11 M solution of CaCl2?
To calculate the number of grams of CaCl2 dissolved in a solution, you need to use the formula:
grams = moles * molar mass
First, let's find the number of moles of CaCl2 in the solution. The given information is:
Volume of solution (V) = 1.4 L
Molarity of solution (M) = 0.11 M
The formula for molarity is:
Molarity (M) = moles / volume (in L)
Rearranging the equation, we can solve for moles:
moles = Molarity * volume (in L)
Substituting the given values:
moles = 0.11 M * 1.4 L
= 0.154 mol
Now we need to find the molar mass of CaCl2. The molar mass of Ca is 40.08 g/mol, and the molar mass of Cl is 35.45 g/mol. Since there are two Cl atoms in CaCl2, we multiply the molar mass of Cl by 2:
molar mass of CaCl2 = molar mass of Ca + 2 * molar mass of Cl
= 40.08 g/mol + 2 * 35.45 g/mol
= 110.98 g/mol
Finally, using the formula to calculate the grams:
grams = moles * molar mass
= 0.154 mol * 110.98 g/mol
= 17.09 g
Therefore, there would be 17.09 grams of CaCl2 dissolved in 1.4 L of a 0.11 M solution of CaCl2.