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vlada-n [284]
3 years ago
8

Naming the hydrates?

Chemistry
2 answers:
slamgirl [31]3 years ago
8 0
HEY mate here your answer

CoBr2 . 6 h2o = Cobalt(II) Bromide Hexahydrate
-BARSIC- [3]3 years ago
7 0

Cobalt(II) bromide hexahydrate.

<h3>Explanation</h3>

Name of the hydrate of an ionic compound:

Name of the ionic compound + Number of water molecules + "hydrate".

What's the name of the ionic compound CoBr₂ without all the H₂O?

There are two ions in this compound:

  • Co²⁺, and
  • Br⁻.

As a transition metal, cobalt Co can form ions of more than one possible charges. Hence, it's necessary to indicate the oxidation state of cobalt in the name. The oxidation state of Co in Co²⁺ is +2. The Co²⁺ ion will be called cobalt(II).

Bromine Br is a nonmetal. The Br⁻ ion is named as bromide.

Thus the name of the salt without H₂O: CoBr₂ Cobalt(II) bromide.

There are six water molecules for every one formula unit of the salt. Hence the prefix hexa-.

Name of the hydrate:

Cobalt(II) bromide hexahydrate.

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PH + pOH = 14. What is the hydroxide concentration of a solution with pH of 8?
sladkih [1.3K]
PH + pOH = 14
pOH=14-8=4
(OH-)=10^-4
4 0
3 years ago
What mass of HBO2 is produced from the<br> combustion of 139.5 g of B2H6?<br> Answer in units of g.
aliina [53]

Answer:

m_{HBO_2}=441.8gHBO_2

Explanation:

Hello there!

In this case, since the combustion of B2H6 is:

B_2H_6+3O_2\rightarrow 2HBO_2+2H_2O

Thus, since there is 1:2 mole ratio between the reactant and product, the produced grams of the latter is:

m_{HBO_2}=139.5gB_2H_6*\frac{1molB_2H_6}{27.67gB_2H_6} *\frac{2molHBO_2}{1molB_2H_6} *\frac{43.82gHBO_2}{1molHBO_2}

m_{HBO_2}=441.8gHBO_2

Best regards!

5 0
2 years ago
What is 2.75 mol of O2
ANTONII [103]

Answer:

2,75 mol of O2 it's 88 g of O2.

Explanation:

The weight of the diatomic molecule O2 is 32 g/mol. So considering that, you should multiply 2,75 mol · 32 = 88g :)

3 0
2 years ago
If I have 8 moles of Iron atoms in the products, how many moles of Iron atoms did I start with?
Vika [28.1K]

Answer: You started with 8

Explanation: the amount of products is equal to the amount of reactants

6 0
3 years ago
Read 2 more answers
How many grams of aluminum chloride are produced when 5.96 grams of aluminum are reacted with excess chlorine gas? Start with a
Vadim26 [7]

Answer:

29.47 g of AlCl₃.

Explanation:

We'll begin by writing the balanced equation for the reaction. This is illustrated below:

2Al + 3Cl₂ —> 2AlCl₃

Next, we shall determine the mass of Al that reacted and the mass of AlCl₃ produced from the balanced equation. This can be obtained as follow:

Molar mass of Al = 27 g/mol

Mass of Al from the balanced equation = 2 × 27 = 54 g

Molar mass of AlCl₃ = 27 + (35.5× 3)

= 27 + 106.5

= 133.5 g/mol

Mass of AlCl₃ from the balanced equation = 2 × 133.5 = 267 g

SUMMARY:

From the balanced equation above,

54 g of Al reacted to produce 267 g of AlCl₃.

Finally, we shall determine the mass of AlCl₃ produced by the reaction of 5.96 g of Al. This can be obtained as follow:

From the balanced equation above,

54 g of Al reacted to produce 267 g of AlCl₃.

Therefore, 5.96 g of Al will react to produce = (5.96 × 267)/54 = 29.47 g of AlCl₃.

Thus, 29.47 g of AlCl₃ were obtained from the reaction.

3 0
2 years ago
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