how much of a 0.225 M KCl solution contains 55.8g of KCl
To determine how much of a 0.225 M (molar) KCl solution contains 55.8g of KCl, we can use the formula:
Molarity = moles of solute / liters of solution
First, we need to find the number of moles of KCl present in the solution. To do this, we'll use the formula:
moles of solute = mass of solute / molar mass of solute
The molar mass of KCl is calculated by adding the atomic masses of potassium (K) and chlorine (Cl), which are 39.10 g/mol and 35.45 g/mol, respectively:
molar mass of KCl = 39.10 g/mol + 35.45 g/mol = 74.55 g/mol
Now we can calculate the moles of KCl:
moles of KCl = 55.8 g / 74.55 g/mol = 0.7486 mol
Next, let's determine the volume (liters) of the solution. Recall that the molarity is defined as moles of solute per liter of solution. Rearranging the formula, we have:
liters of solution = moles of solute / molarity
Plugging in the values:
liters of solution = 0.7486 mol / 0.225 mol/L = 3.3267 L
Therefore, 55.8g of KCl is dissolved in approximately 3.33 liters of a 0.225 M KCl solution.