If a $0.3 \cdot m o l$ $0.3mol$ quantity of calcium chloride is dissolved in a $1 \cdot L$ $1L$ water solvent what are the concentrations of $C a^{2 +}$ $Ca^(2+)$ and $C l^{-}$ $Cl^-$ ?

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If a $0.3 \cdot m o l$ $0.3mol$ quantity of calcium chloride is dissolved in a $1 \cdot L$ $1L$ water solvent what are the concentrations of $C a^{2 +}$ $Ca^(2+)$ and $C l^{-}$ $Cl^-$ ?

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Answer 1 · 2017-09-30T17:16:16

$Molar concentration = \frac{Moles of solute}{Volume of solution}$ $"Molar concentration"="Moles of solute"/"Volume of solution"$

Explanation:

Now calcium chloride speciates in aqueous solution according to the following chemical equation.....

$C a C l_{2} (s) H_{2} O - - \to C a^{2 +} + 2 C l^{-}$ $CaCl_2(s) stackrel(H_2O)rarrCa^(2+) + 2Cl^-$

And thus if $0.3 \cdot m o l$ $0.3*mol$ of calcium chloride are dissolved, we gets $0.6 \cdot m o l$ $0.6*mol$ of CHLORIDE ions in solution, and $0.3 \cdot m o l$ $0.3*mol$ of calcium ions....

Capisce?

Answer 2 · 2017-09-30T17:18:08

0.6

Explanation:

$Molar concentration = \frac{Number of moles}{Volume}$ $"Molar concentration"="Number of moles"/"Volume"$

In your example:
$Number of moles = 0.3 mol$ $"Number of moles"=0.3 " mol"$
$Volume = 1000 ml$ $"Volume"=1000 " ml"$

To change the volume into Liters, we have to divide the volume by thousand (1L contains 1000 ml):
$Volume = \frac{1000 ml}{1000 ml/L} = 1 L$ $"Volume"=(1000 " ml")/ (1000 " ml/L") =1" L"$

$\to Molar concentration = \frac{0.3}{1} = 0.3 mol/L$ $rarr "Molar concentration"=0.3/1=0.3 " mol/L"$

Since we are finding the molar concentration of chloride ions:
$C a C l_{2} \to C a^{2 +} + 2 C l^{-}$ $CaCl_2rarrCa^(2+)+2Cl^-$

Therefore the concentration of Chloride ions is double the concentration of Calcium chloride:
$Molar concentration of Chloride = 2 \cdot 0.3 = 0.6 mol/L$ $"Molar concentration of Chloride"= 2*0.3=0.6" mol/L"$

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If a $0.3 \cdot m o l$ $0.3mol$ quantity of calcium chloride is dissolved in a $1 \cdot L$ $1L$ water solvent what are the concentrations of $C a^{2 +}$ $Ca^(2+)$ and $C l^{-}$ $Cl^-$ ?

2 Answers

Explanation:

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If a 0.3⋅mol0.3*mol quantity of calcium chloride is dissolved in a 1⋅L1*L water solvent what are the concentrations of Ca2+Ca^(2+) and Cl−Cl^-?

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Explanation:

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If a $0.3 \cdot m o l$ $0.3mol$ quantity of calcium chloride is dissolved in a $1 \cdot L$ $1L$ water solvent what are the concentrations of $C a^{2 +}$ $Ca^(2+)$ and $C l^{-}$ $Cl^-$ ?