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fenix001 [56]
3 years ago
6

How does the chemical formula for the nitrite ion differ from the chemical formula for the nitrate ion?

Chemistry
2 answers:
Darina [25.2K]3 years ago
8 0
The nitrite ion has one less oxygen than the nitrate ion. Nitrate is NO3-1 while the nitrite ion is NO2-.
stepladder [879]3 years ago
8 0

Answer:

nitrite ion is NO2- and nitrate ion is NO3-

Explanation:

The nitrite ion has two oxygen atoms and one nitrogen atom while nitrate ion has three oxygen atoms and one nitrogen atom. They are both univalent negative anions that form compounds with metallic cations as shown below;

Na+ + NO3- ⇒ NaNO3 (sodium nitrate)

Na+ + NO2- ⇒ NaNO2 (sodium nitrite)

Ca2+ + NO3- ⇒ Ca(NO3)2 (calcium nitrate)

Ca2+ + NO2- ⇒ Ca(NO2)2 (calcium nitrite)

You can deduce from the above ionic equations that nitrate ion is NO3- while nitrite ion is NO2-.

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Among the following options, a valid Lewis structure of __________ cannot be drawn without violating the octet rule.
Murrr4er [49]

Answer:

d. IF3

Explanation:

The Octet rule posits that atoms gain, atom lose, or share electrons in order to have a full valence shell of 8 electrons. This statement occurs when atoms also combine to form molecules until they attain or share eight valence electrons either by losing or gaining eletrons.

From the given options, a valid Lewis structure that cannot be drawn without violating the octet rule is IF3

8 0
2 years ago
In a titration, 10.0 ml of 0.0750 M HCl(aq) is exactly neutralized by 30.0 ml of KOH(aq) of unknown concentration. What is the c
Sphinxa [80]

Answer: 0.0250

Explanation: 10 X 0.0750 = .75

.75 / 30 = 0.0250 M

4 0
3 years ago
What are the chemical properties of oxygen?
wlad13 [49]
Hmm.... Oxygen support combustion. Other than that, rusting occur when oxygen is combined with metal. When iron rusts, it combines with oxygen. Hope it helps.
7 0
3 years ago
Chlorine can be prepared in the laboratory by the reaction of manganese dioxide with hydrochloric acid. HCl(aq), as described by
melisa1 [442]

Answer:

0.88 g

Explanation:

Using ideal gas equation to calculate the moles of chlorine gas produced as:-

PV=nRT

where,

P = pressure of the gas = 805 Torr

V = Volume of the gas = 235 mL = 0.235 L

T = Temperature of the gas = 25^oC=[25+273]K=298K

R = Gas constant = 62.3637\text{torr}mol^{-1}K^{-1}

n = number of moles of chlorine gas = ?

Putting values in above equation, we get:

805torr\times 0.235L=n\times 62.3637\text{ torrHg }mol^{-1}K^{-1}\times 298K\\\\n=\frac{805\times 0.235}{62.3637\times 298}=0.01017\ mol

According to the reaction:-

MnO_2+4HCl\rightarrow MnCl_2+2H_2O+Cl_2

1 mole of chlorine gas is produced when 1 mole of manganese dioxide undergoes reaction.

So,

0.01017 mole of chlorine gas is produced when 0.01017 mole of manganese dioxide undergoes reaction.

Moles of MnO_2 = 0.01017 moles

Molar mass of MnO_2 = 86.93685 g/mol

So,

Mass=Moles\times Molar\ mass

Applying values, we get that:-

Mass=0.01017moles \times 86.93685\ g/mol=0.88\ g

<u>0.88 g of MnO_2(s) should be added to excess HCl (aq) to obtain 235 mL of Cl_2(g) at 25 degrees C and 805 Torr.</u>

6 0
3 years ago
If exactly 59.6 g of nitrogen gas is needed to inflate your air bag to the
Inga [223]

Answer:

We need 92.3 grams of sodium azide

Explanation:

Step 1: Data given

Mass of nitrogen gas = 59.6 grams

Molar mass of nitrogen gas = 28.0 g/mol

Molar mass of sodium azide = 65.0 g/mol

Step 2: The balanced equation

2NaN3 → 2Na + 3N2

Step 3: Calculate moles nitrogen gas

Moles N2 = mass N2 / molar mass N2

Moles N2 = 59.6 grams/ 28.0 g/mol

Moles N2 = 2.13 moles

Step 4: Calculate moles NaN3

for 2 moles NaN3 we'll have 2 moles Na and 3  moles N2

For 2.13 moles N2 we need 2/3* 2.13 = 1.42 moles NaN3

Step 5: Calculate mass NaN3

Mass NaN3 = Moles NaN3 * molar mass NaN3

Mass NaN3 = 1.42 moles * 65.0 g/mol

Mass NaN3 = 92.3 grams

We need 92.3 grams of sodium azide

7 0
3 years ago
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