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3 years ago

9

I need helpppppppppppppppppppppppppppppppppppp

2 answers:

JulsSmile [24]3 years ago

8 0

Answer:

c

Explanation:

it is acidic due to carbon dioxide dissolving into it and forming a weak carbonic acid.

11Alexandr11 [23.1K]3 years ago

7 0

Answer:

A

Explanation:

Carbon dioxide in the air

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How many “p” orbital in principal energy level below?

marshall27 [118]

Answer:

Each principal energy level above the first contains one s orbital and three p orbitals. A set of three p orbitals, called the p sublevel, can hold a maximum of six electrons. Therefore, the second level can contain a maximum of eight electrons - that is, two in the s orbital and 6 in the three p orbitals.

Explanation:

5 0

3 years ago

ICE Princess25 [194]

Answer:

B. Experiments

Explanation:

conducting an experiment is an example of a research method while the other choices are not.

Hope I was able to help you!

4 0

2 years ago

All of the following increase from left to right across the second period of the periodic table (Na - Ar) EXCEPT

DerKrebs [107]

Answer: effective nuclear charge

Explanation: This is because electrons are added to tell same shell at about the same distance from the nucleus

4 0

3 years ago

A chemist added an excess of sodium sulfate to a solution of a soluble barium compound to precipitate all of the barium ion as b

AnnyKZ [126]

Answer : The mass percentage of barium in the compound is, 53.8 %

Explanation : Given,

Mass of barium compound = 441 mg

Mass of barium sulfate = 403 mg = 0.403 g (1 mg = 0.001 g)

The balanced chemical reaction will be:

$Ba^{2+}(aq)+Na_2SO_4(aq)\rightarrow BaSO_4(s)+2Na^+(aq)$

First we have to calculate the moles of $BaSO_4$

$\text{Moles of }BaSO_4=\frac{\text{Mass of }BaSO_4}{\text{Molar mass of }BaSO_4}$

Molar mass of $BaSO_4$ = 233.38 g/mole

$\text{Moles of }BaSO_4=\frac{0.403g}{233.38g/mole}=0.001727mole$

Now we have to calculate the moles of barium ion.

From the balanced chemical reaction, we conclude that

As, 1 mole of barium sulfate produced from 1 mole of barium ion

So, 0.001727 mole of barium sulfate produced from 0.001727 mole of barium ion

Now we have to calculate the mass of barium ion.

$\text{ Mass of }Ba^{2+}=\text{ Moles of }Ba^{2+}\times \text{ Molar mass of }Ba^{2+}$

Molar mass of barium = 137.3 g/mol

$\text{ Mass of }Ba^{2+}=(0.001727moles)\times (137.3g/mole)=0.2371g$

Now we convert the mass of barium ion from gram to mg.

Conversion used : (1 g = 1000 mg)

Mass of barium ion = 0.2371 g = 237.1 mg

Now we have to calculate the mass percentage of barium in the compound.

Mass percent of barium = $\frac{237.1mg}{441mg}\times 100=53.8\%$

Thus, the mass percentage of barium in the compound is, 53.8 %

8 0

4 years ago

NEED RIGHT NOW PLEASE HELP

Marysya12 [62]

NH4Cl + heat forms NH4 + + Cl-

8 0

3 years ago