1.5mL of a 0.05M solution of calcium chloride (CaCl2) was diluted with water to a volume of 10L. What was the concentration of Cl- ions in the diluted solution in ppm.
mols CaCl2 = M x L = (1.5/1000) x 0.05 = approx 7E-5 but you need a better number than that.
Convert to grams CaCl2 = mols x molar mass = approx 0.008. Again, you must get a better number. Convert to grams Cl.
Thats 0.008 g CaCl2 x (2*35.5/111) = approx 0.05 g Cl^-.
1 ppm = 1 mg/L. You have approx 50mg/10 L = ? ppm
Check my work.
To find the concentration of Cl- ions in the diluted solution in parts per million (ppm), we can follow these steps:
Step 1: Calculate the moles of CaCl2 in the original solution.
Given:
Volume of solution = 1.5 mL = 0.0015 L
Molarity of CaCl2 solution = 0.05 M
To calculate moles:
moles of CaCl2 = Molarity x Volume
moles of CaCl2 = 0.05 mol/L x 0.0015 L
moles of CaCl2 = 0.000075 mol
Step 2: Calculate the moles of Cl- ions in the original solution.
Since CaCl2 contains two chloride ions (Cl-) per molecule, the moles of Cl- ions can be calculated as:
moles of Cl- ions = 2 x moles of CaCl2
moles of Cl- ions = 2 x 0.000075 mol
moles of Cl- ions = 0.00015 mol
Step 3: Calculate the concentration of Cl- ions in the diluted solution.
The diluted solution has a total volume of 10 L.
To calculate the concentration:
Concentration of Cl- ions = Moles of Cl- ions / Total Volume
Concentration of Cl- ions = 0.00015 mol / 10 L
Concentration of Cl- ions = 0.000015 mol/L
Step 4: Convert the concentration to parts per million (ppm).
1 ppm = 1 mg/L
To convert:
Concentration in ppm = Concentration in mol/L x Molecular weight of Cl-
Molecular weight of Cl- = 35.45 g/mol
Concentration in ppm = 0.000015 mol/L x 35.45 g/mol x 1000 mg/g
Concentration in ppm = 0.53175 ppm
Therefore, the concentration of Cl- ions in the diluted solution is approximately 0.53175 ppm.
To determine the concentration of Cl- ions in the diluted solution in parts per million (ppm), we need to follow these steps:
Step 1: Calculate the number of moles of CaCl2 initially present.
Given:
- Volume of the CaCl2 solution = 1.5 mL = 1.5 x 10^-3 L
- Concentration of the CaCl2 solution = 0.05 M
Using the formula: moles = concentration x volume
moles of CaCl2 = 0.05 M x 1.5 x 10^-3 L
Step 2: Calculate the number of moles of Cl- ions initially present.
Since there are two Cl- ions in every mole of CaCl2, we can multiply the moles of CaCl2 by 2 to get the moles of Cl- ions.
moles of Cl- = 2 x moles of CaCl2
Step 3: Calculate the moles of Cl- ions in the diluted solution.
Since we diluted the initial solution to a volume of 10 L, the moles of Cl- ions remain the same.
Step 4: Calculate the concentration of Cl- ions in the diluted solution.
Concentration = moles of Cl- ions / volume of diluted solution
Since the diluted solution has a volume of 10 L, the concentration of Cl- ions in the diluted solution is:
Concentration = moles of Cl- ions / 10 L
Step 5: Convert the concentration to parts per million (ppm).
To convert concentration to ppm, since ppm is equivalent to mg/L or mg/kg.
Since our concentration is in moles per liter (mol/L), we need to convert it to mg/L by multiplying by the molar mass of Cl-.
molar mass of Cl- = 35.45 g/mol
Concentration in ppm = (moles of Cl- ions / 10 L) x (molar mass of Cl- / 1 L) x 1000
By plugging in the values from the previous steps, we can calculate the concentration of Cl- ions in the diluted solution in ppm.