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Dafna1 [17]
3 years ago
8

What is the hybridization state on the central N atom in the azide ion, N3−?

Chemistry
1 answer:
Sloan [31]3 years ago
4 0
The sp hybridization of the central nitrogen is consistent with the linear structure of the azide ion. In A, the terminal nitrogens may both be sp2 hybridized; after all the drawing looks similar to the double bond in ethylene.
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When naming a binary compound, what ending do you use to represent anions?
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What are the traditional states of matter, and what type of property is a matter's state?
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7 0
3 years ago
Calculate the ph of a 0.20 m solution of iodic acid (hio3, ka = 0.17).
saveliy_v [14]
Iodic acid partially dissociates into H+ and IO3- 
Assuming that x is the concentration of H+ at equilibrium, and sine the equation says the same amount of IO3- will  be released as that of H+, its concentration is also X.  The formation of H+ and IO3- results from the loss of HIO3 so its concentration at equilibrium is 0.20 M - x
Ka = [H+] [IO3-] / [HIO3]; 
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<span>At equilibrium [H+] ≈ [IO3-] = x and [HIO3] = 0.20 - x; </span>
<span>so 0.17 = x² / (0.20 - x); </span>
<span>Solving for x using the quadratic formula: </span>
<span>x = [H+] = 0.063 M or pH = - log [H+] = 1.2.</span>
7 0
4 years ago
Cho m gam FeO tác dụng hết với dung dịch H2SO4, thu được 200 ml dung dịch FeSO4 1M. Giá trị của m là
BaLLatris [955]

<u>Answer:</u> The mass of FeO required is 14.37 g

<u>Explanation:</u>

Molarity is calculated by using the equation:

\text{Molarity}=\frac{\text{Moles}}{\text{Volume}} ......(1)

We are given:  

Molarity of iron (II) sulfate = 1 M

Volume of solution = 200 mL = 0.200 L (Conversion factor: 1 L = 1000 mL)

Putting values in equation 1, we get:

\text{Moles of }FeSO_4=(1mol/L\times 0.200L)=0.200mol

The chemical equation for the reaction of FeO with sulfuric acid follows:

FeO+H_2SO_4\rightarrow FeSO_4+H_2O

By stoichiometry of the reaction:

If 1 mole of iron (II) sulfate is produced by 1 mole of FeO

So, 0.200 moles of iron (II) sulfate will produce = \frac{1}{1}\times 0.200=0.200mol of FeO

The number of moles is defined as the ratio of the mass of a substance to its molar mass. The equation used is:

\text{Number of moles}=\frac{\text{Given mass}}{\text{Molar mass}}

We know, molar mass of FeO = 71.84 g/mol

Putting values in above equation, we get:

\text{Mass of }FeO=(0.200mol\times 71.84g/mol)=14.37g

Hence, the mass of FeO required is 14.37 g

4 0
3 years ago
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