What is the molality of an acetic acid solution that contains 0.500 mol of HC2H3O2 (molar mass: 60g/mol) in 0.800 kg of water?
1 answer:
Answer: The molality of given acetic acid solution is 0.625 m.
Explanation:
Given: Moles of solute = 0.5 mol
Mass of solvent = 0.8 kg
Molality is the number of moles of solute present in a kg of solvent.
Therefore, molality of the given solution is calculated as follows.
Substitute the values into above formula as follows.
Thus, we can conclude that the molality of given acetic acid solution is 0.625 m.
You might be interested in
Answer:
1. 0.35 moles NaOH
2. moles
3. 505.4 g Pb
4. 1.46 g HCl (if that is wrong it's 1.5 g HCl due to sig figs)
5. atoms of Ag
6. atoms of Cu
Explanation:
1. The mass of NaOH is 40g. 22.99(Na)+16(O)+1.01(H)=40 g
14 g NaOH * = 0.35 moles of NaOH
2. Mass of
0.05 g ×
3. mass of Pb = 106.4 g
4.75 moles Pb×
4. mass of HCl = 1.01 +35.45 = 36.36 g
0.04 mol HCl x
5. 5.00 mol Ag x
6. Cu x
atoms of Cu