What mass of CsCl must be added to 0.55 liters of water to produce a 0.430 m solution?
Molar Mass(CsCl) = 168.35 g/mol and Density(H₂O) = 1.00 g/mL

Question

What mass of CsCl must be added to 0.55 liters of water to produce a 0.430 m solution? Molar Mass(CsCl) = 168.35 g/mol and Density(H₂O) = 1.00 g/mL

Quizplus · Accepted Answer

1. Calculate the moles of CsCl needed for the solution:

0.430 mol/L = moles/0.55 L

moles = 0.430 mol/L x 0.55 L = 0.2365 mol

2. Calculate the mass of CsCl needed using its molar mass:

mass = moles x molar mass = 0.2365 mol x 168.35 g/mol = 39.8 g

Therefore, the mass of CsCl needed to produce a 0.430 m solution is 39.8 g. Choice C is correct.

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