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.

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