Problem: A water sample containing calcium ions (Ca²⁺) is titrated with a 0.01 M EDTA solution. If 25.0 mL of the water sample required 15.0 mL of the EDTA solution to reach the end point, calculate the concentration of calcium ions in the water sample.
Question
Problem: A water sample containing calcium ions (Ca²⁺) is titrated with a 0.01 M EDTA solution. If 25.0 mL of the water sample required 15.0 mL of the EDTA solution to reach the end point, calculate the concentration of calcium ions in the water sample.
Solution
To solve this problem, we need to use the concept of stoichiometry in a titration reaction. The reaction between calcium ions and EDTA is a 1:1 reaction. This means that one mole of calcium ions reacts with one mole of EDTA.
Step 1: Calculate the number of moles of EDTA used in the titration. The number of moles of a substance can be calculated using the formula:
Moles = Molarity x Volume
In this case, the molarity of the EDTA solution is 0.01 M and the volume used is 15.0 mL. However, the volume needs to be in liters for the calculation, so we convert it:
15.0 mL = 15.0/1000 = 0.015 L
Now we can calculate the moles of EDTA:
Moles of EDTA = 0.01 M x 0.015 L = 0.00015 moles
Step 2: Calculate the concentration of calcium ions in the water sample. Since the reaction between calcium ions and EDTA is a 1:1 reaction, the number of moles of calcium ions in the water sample is the same as the number of moles of EDTA used in the titration. Therefore, there are 0.00015 moles of calcium ions in the water sample.
The concentration of a substance can be calculated using the formula:
Concentration = Moles / Volume
The volume of the water sample is 25.0 mL, which is 25.0/1000 = 0.025 L. So, the concentration of calcium ions in the water sample is:
Concentration of Ca²⁺ = 0.00015 moles / 0.025 L = 0.006 M
So, the concentration of calcium ions in the water sample is 0.006 M.
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