For a litre volume, what is the mass of calcium chloride present in a $2 \cdot m M$ $2*mM$ solution of $C a C l_{2}$ $CaCl_2$ ?

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For a litre volume, what is the mass of calcium chloride present in a $2 \cdot m M$ $2*mM$ solution of $C a C l_{2}$ $CaCl_2$ ?

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Answer 1 · 2016-09-17T18:46:37

A stoichiometric quantity, approx. $222$ $222$ $m g$ $mg$ .

Explanation:

$Molarity$ $"Molarity"$ $=$ $=$ $\frac{Moles of solute}{Volume of solution}$ $"Moles of solute"/"Volume of solution"$ , and thus $molarity$ $"molarity"$ has units of $m o l \cdot L^{- 1}$ $mol*L^-1$ . And thus,

$Moles of solute = Volume of solution \times molarity$ $"Moles of solute"="Volume of solution"xx"molarity"$

We have a $2 mM$ $2"mM"$ solution, i.e. a $2.0 \times 10^{- 3} m o l \cdot L^{- 1}$ $2.0xx10^-3mol*L^-1$ of $C a C l_{2}$ $CaCl_2$ , and, clearly, there are $2.0 \times 10^{- 3} m o l$ $2.0xx10^-3mol$ of $C a C l_{2}$ $CaCl_2$ present in solution.

Thus, with respect to $C a C l_{2}$ $CaCl_2$ there are ............

$1*cancelLxx2.0xx10^-3cancel(mol*L^-1)xx110.98*g*cancel(mol^-1)$ $=$ $0.222*g$ calcium chloride. What is the concentration of this solution with respect to $Cl^-$ ion?

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For a litre volume, what is the mass of calcium chloride present in a $2 \cdot m M$ $2*mM$ solution of $C a C l_{2}$ $CaCl_2$ ?

1 Answer

Explanation:

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For a litre volume, what is the mass of calcium chloride present in a 2*mM2⋅mM2*mM solution of CaCl_2CaCl2CaCl_2?

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For a litre volume, what is the mass of calcium chloride present in a $2 \cdot m M$ $2*mM$ solution of $C a C l_{2}$ $CaCl_2$ ?