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mariarad [96]
2 years ago
14

Calculate the solubility of Ca(OH)2 in a 0.469M CaCl2 solution at 31°C, given that the Ksp of Ca(OH)2 is 4.96 x 10-6 at that tem

perature. Give your answer in milliMolar units 2.927 mM 1.626 mM 2.764 mM 1.382 mM 1.463 mM 3.252 mM​
Chemistry
1 answer:
Ghella [55]2 years ago
3 0

The solubility of Ca(OH)2 in a 0.469M CaCl2 solution at 31°C, at given Ksp of Ca(OH)2 is determined as 1.626 mM.

<h3>Dissociation reaction of Ca(OH)2</h3>

The dissociation reaction of Ca(OH)2 is given as follows;

Ca(OH)₂  ⇄ Ca²⁺  + 2OH⁻¹

                     x           2x

Concentration of Ca²⁺ = 0.469 M

Ksp = [x][2x]²

ksp = (0.469)(2x²)

ksp = 4(0.469)x²

ksp = 1.876x²

4.96 x 10⁻⁶ = 1.876x²

x² = (4.96 x 10⁻⁶)/(1.876)

x² = 2.643 x 10⁻⁶

x = √(2.643 x 10⁻⁶)

x = 1.626 x 10⁻³ M

x = 1.626 mM

Thus, the solubility of Ca(OH)2 in a 0.469M CaCl2 solution at 31°C, at given Ksp of Ca(OH)2 is determined as 1.626 mM.

Learn more about solubility here: brainly.com/question/23946616

#SPJ1

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The density of a metal is 9.80 g/mL. What is the mass of a sample of metal when dropped in 28.9 mL of water, the volume increase
yan [13]

The correct answer is 2.70 × 10² g or 270 g.  

It is given, that the density of a metal is 9.80 g/ml.  

Let the mass of a sample of metal be x.  

The sample of metal is dropped in 28.9 ml of water, due to which the volume of the water increases to 56.4 ml.  

In order to calculate the mass of a metal, there is a need to use the formula, mass = density * volume

Mass = (9.80 g/ml) (56.4 ml - 28.9 ml)

= (9.80 g/ml) (27.5 ml)

= 2.70 × 10² g or 270 g


6 0
3 years ago
For the aqueous solution containing 75 mg of compound C in 1.0 mL of water, what will be the total amount of the solute C that w
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Answer:

75 mg

Explanation:

We can write the extraction formula as

x = m/[1 + (1/K)(Vaq/Vo)], where

x = mass extracted

m = total mass of solute

K = distribution coefficient

Vo = volume of organic layer

Vaq = volume of aqueous layer

Data:

m = 75 mg

K = 1.8

Vo = 0.90 mL

Vaq = 1.00 mL

Calculations:

For each extraction,

1 + (1/K)(Vaq/Vo) = 1  + (1/1.8)(1.00/0.90) = 1 + 0.62 = 1.62  

x = m/1.62 = 0.618m

So, 61.8 % of the solute is extracted in each step.

In other words, 38.2 % of the solute remains.

Let r = the amount remaining after n extractions. Then  

r = m(0.382)^n.

If n = 7,

r = 75(0.382)^7 = 75 × 0.001 18 = 0.088 mg

m = 75 - 0.088 = 75 mg

After seven extractions, 75 mg (99.999 %) of the solute will be extracted.

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True or false: environmental science concentrates on the study of earth's natural hazards.
algol [13]

The correct answer for this question is 'False'

Environmental science is not the study of the earth's natural hazards

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8 0
2 years ago
What volume of H2O(g) is produced when 8.00 mol of C2H4(g) reacts at STP?
sweet-ann [11.9K]
* Mole ratio:

C2H4 + 3 O2= 2 CO2 + 2 H2O

1 mole C2H4 --------------- 2 moles H2O
8.00 moles C2H4 ---------- ?

8.00 x 2 / 1 => 16 moles of H2O

Therefore:

1 mole --------- 22.4 L at ( STP)
16 moles ------- ?

16 x 22.4 / 1 => 358.4 L

hope this helps!
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3 years ago
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