The definition of a 5% w/v solution is: 5g of solute dissolved
in 100mL of solution
Now you know that you have 5g of HF dissolved in water to make a
final solution volume of 100mL
That is equivalent to 50g HF in 1000mL of solution or 1.0L of
solution
Molar mass HF = 20.0g/mol
Mol of HF = 50/20 = 2.5 mol HF dissolved in 1.0L solution
Molarity of HF solution = 2.5M
The definition of a 5% w/v solution is: 5g of solute dissolved
in 100mL of solution
Now you know that you have 5g of HF dissolved in water to make a
final solution volume of 100mL
That is equivalent to 50g HF in 1000mL of solution or 1.0L of
solution
Molar mass HF = 20.0g/mol
Mol of HF = 50/20 = 2.5 mol HF dissolved in 1.0L solution
Molarity of HF solution = 2.5M
Now you know that you have 5g of HF dissolved in water to make a
final solution volume of 100mL
That is equivalent to 50g HF in 1000mL of solution or 1.0L of
solution
Molar mass HF = 20.0g/mol
Mol of HF = 50/20 = 2.5 mol HF dissolved in 1.0L solution
Molarity of HF solution = 2.5M (answer)
let volume of solution=100 mL
mass of solute=mass of HF=5 g
mole of HF=mass/molar mass=5/20=0.25 mole
molarity=mole/volume=0.25/100*10-3=2.5 M
Consider the HF solution with the concentration of 5%(w/v). Calculate its concentration in the molarity.
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