What is the molarity of a 5.00 x 102 ml solution containing 2490 g of KI?
How many moles of LiF would be required to produce a 2.5 M solution with a volume of 10.5 L?
How many grams of NaI would be used to produce a 2.0 M solution with a volume of 10.00 L?
Very confused on how to do this. I don't just want the answer, can someone please explain it?
To calculate the molarity of a solution, we need to know the number of moles of solute (the substance being dissolved) and the volume of the solution.
1. Molarity (M) is defined as moles of solute per liter of solution. The formula for molarity is:
Molarity (M) = moles of solute / volume of solution (in liters)
For example, let's solve the first question:
Question 1: What is the molarity of a 5.00 x 102 ml solution containing 2490 g of KI?
To find the molarity, we need to calculate the number of moles of KI and convert the volume from milliliters to liters.
Step 1: Calculate the moles of KI.
Moles = mass of KI / molar mass of KI
The molar mass of KI is the sum of the atomic masses of potassium (K) and iodine (I), which can be found on the periodic table. In this case, the molar mass of KI is:
1 mol of K = 39.10 g
1 mol of I = 126.90 g
Molar mass of KI = 39.10 g + 126.90 g = 166 g/mol
Now we can calculate the moles of KI using the mass provided:
Moles of KI = 2490 g / 166 g/mol
Step 2: Convert the volume to liters.
5.00 x 102 ml = 5.00 x 10-1 liter (since there are 1000 ml in a liter)
Step 3: Now we can calculate the molarity using the formula:
Molarity (M) = moles of KI / volume of solution (in liters)
Molarity = (2490 g / 166 g/mol) / (5.00 x 10-1 L)
Solving this equation will give you the molarity of the solution.
You can follow similar steps to solve the other questions. Just ensure you calculate the moles of the given substance and convert the volume to liters before using the molarity formula.