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# How many grams of $CaC{1_2}$ can dissolve in $200{\text{ }}g$ of water at ${10^o}C$ ?

Last updated date: 20th Jun 2024
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Hint: $Calcium{\text{ }}chloride$ is an inorganic compound, a salt with the artificial formula $CaC{l_2}$ . It is a white hued translucent strong at room temperature, and it is profoundly dissolvable in water. It very well may be made by killing hydrochloric acid with calcium hydroxide.

You should allude to a solvency bend chart, which shows the amount of every solute will disintegrate in $100g$ water at demonstrated temperatures.
We need to take a gander at the amount $CaC{l_2}$ will break up in $100g{H_2}O$ at ${10^o}C$ .
The purpose of convergence between the $CaC{l_2}$ bend (the orange line) and the ${10^o}C$ line seems to happen at the purpose of generally $64g$ per $100g{H_2}O$
This implies that at ${10^o}C$ , $64g$ $CaC{l_2}$ will break down in $100g{H_2}O$ , however the inquiry pose to how much will disintegrate in $200g{H_2}O$ . This can be discovered just enough by multiplying the solvency at ${10^o}C$ :
$64{\text{gCaC}}{{\text{l}}_2} \times 2 = 128{\text{gCaC}}{{\text{l}}_2}$.
In this way, $128{\text{gCaC}}{{\text{l}}_2}$ will disintegrate in $200{\text{g}}{{\text{H}}_2}{\text{O}}$ at ${10^o}C$ .
Calcium chloride breaks up in water, creating chloride and the aquo complex ${\left[ {Ca{{\left( {{H_2}O} \right)}_6}} \right]^{2 + }}$ . Thus, these arrangements are wellsprings of "free" calcium and free chloride particles. This portrayal is outlined by the way that these arrangements respond with phosphate sources to give a strong accelerate of calcium phosphate:
Note: Calcium chloride is usually experienced as a hydrated strong with conventional equation $CaC{l_2}{\left( {{H_2}O} \right)_x}$ , where $x{\text{ }} = {\text{ }}0$ , $1$ , $2$ , $4$ , and $6$ . These mixes are mostly utilized for de-icing and residue control. Since the anhydrous salt is hygroscopic, it is utilized as a desiccant