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Which of the following should be done in order to prepare 0.40 M NaCl starting with 100 ml. of 0.30 M NaCl (mol.wt.of NaCl=58.5)
- a)Add 5.85 g NaCl
- b)Add 20 ml water
- c)Add 0.010 mole NaCl
- d)Evaporate 10 ml water
Correct answer is option 'C'. Can you explain this answer?
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Steps to prepare 0.40 M NaCl starting with 100 ml of 0.30 M NaCl:
Step 1: Calculate the moles of NaCl in 100 ml of 0.30 M NaCl solution
- Molarity (M) = moles of solute / volume of solution (L)
- 0.30 M = moles of NaCl / 0.1 L (100 ml = 0.1 L)
- Moles of NaCl = 0.30 M x 0.1 L = 0.03 moles
Step 2: Determine the additional moles of NaCl needed to make 0.40 M NaCl
- Final moles of NaCl = 0.40 M x 0.1 L = 0.04 moles
- Additional moles needed = 0.04 moles - 0.03 moles = 0.01 moles
Step 3: Calculate the mass of NaCl needed to provide 0.01 moles
- Moles = mass / molar mass
- 0.01 moles = mass / 58.5 g/mol
- Mass = 0.01 moles x 58.5 g/mol = 0.585 g
Therefore, to prepare 0.40 M NaCl starting with 100 ml of 0.30 M NaCl, you should add 0.585 g of NaCl to the solution.
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Which of the following should be done in order to prepare 0.40 M NaCl starting with 100 ml. of 0.30 M NaCl (mol.wt.of NaCl=58.5)a)Add 5.85 g NaClb)Add 20 ml waterc)Add 0.010 mole NaCld)Evaporate 10 ml waterCorrect answer is option 'C'. Can you explain this answer?
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