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Vesnalui [34]
3 years ago
13

(GIVING BRAINLIEST!!!)What is the correct formula for the ionic compound that forms when oppositely- charged ions of magnesium a

nd ions of oxygen attract?
(ANSWERS ARE IN THE IMAGE!!)​

Chemistry
1 answer:
allochka39001 [22]3 years ago
6 0
Pretty confident that MgO is the answer
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Classify each of the following as a physical or chemical property
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Identify the mixture of powdered charcoal and powdered sugar and suggest a technique for separating their components
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The mixture of powdered charcoal and powdered sugar is considered as a homogeneous mixture. This means that you cannot identify the components with naked eye as they are uniformly distributed in the mixture.

B- Separate components:
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Which of the following is true regarding the law of conservation of mass?
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Acid formulas usually start with ______________ because they have hydrogen atoms combined with other atoms in their molecules
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8 0
3 years ago
A generic salt, AB 2 , has a molar mass of 345 g/mol and a solubility of 8.70 g/L at 25 °C. AB 2 (s) − ⇀ ↽ − A 2 + (aq) + 2B − (
Brrunno [24]

Answer : The value of K_{sp} of the generic salt is, 1.60\times 10^{-5}

Explanation :

As we are given that, a solubility of salt  is, 8.70 g/L that means 8.70 grams of salt present in 1 L of solution.

First we have to calculate the moles of salt (AB_2)

\text{Moles of }AB_2=\frac{\text{Mass of }AB_2}{\text{Molar mass of }AB_2}

Molar mass of AB_2 = 345 g/mol

\text{Moles of }AB_2=\frac{8.70g}{345g/mol}=0.0252mol

Now we have to calculate the concentration of A^{2+}\text{ and }B^-

The equilibrium chemical reaction will be:

AB_2(s)\rightleftharpoons A^{2+}(aq)+2B^-(aq)

Concentration of A^{2+} = \frac{0.0252mol}{1L}=0.0252M

Concentration of B^- = \frac{0.0252mol}{1L}=0.0252M

The solubility constant expression for this reaction is:

K_{sp}=[A^{2+}][B^-]^2

Now put all the given values in this expression, we get:

K_{sp}=(0.0252M)\times (0.0252M)^2

K_{sp}=1.60\times 10^{-5}

Thus, the value of K_{sp} of the generic salt is, 1.60\times 10^{-5}

8 0
3 years ago
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