How to Calculate the Total Grams of Potassium Fluoride Needed for a Solution
What is the total number of grams of potassium fluoride needed to make 9.4 liter of a 6.17 M solution?
Given data:
Molar mass of potassium fluoride (KF) = 58 g/mol
Volume of solution = 9.4 liters
Molarity of solution = 6.17 M
What is the formula to calculate the grams of potassium fluoride needed?
A) molarity = no. of moles of solute/solution in litres
B) no. of moles = given mass / molar mass
Answer:
The total number of grams of potassium fluoride needed can be calculated as follows:
First, we need to determine the number of moles of potassium fluoride in the solution using the formula for molarity:
molarity = no. of moles of solute / solution in litres
6.17 M = no. of moles of solute / 9.4 L
6.17 x 9.4 = no. of moles of solute
57.9 = no. of moles of potassium fluoride (KF)
Next, we calculate the mass of potassium fluoride needed using the formula:
no. of moles = given mass / molar mass
57.9 = given mass / 58
Given mass = 57.9 x 58
Given mass = 3358.2 grams
Therefore, the total number of grams of potassium fluoride needed to make a 6.17 M solution in 9.4 liters is 3358.2 grams.