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fgiga [73]
3 years ago
8

Classify each of these soluble solutes as a strong electrolyte, a weak electrolyte, or a nonelectrolyte. solutes formula nitric

acid hno3 lithium hydroxide lioh hydrofluoric acid hf ammonia nh3 potassium chloride kcl ethanol c2h5oh glucose c6h12o6
Chemistry
1 answer:
seropon [69]3 years ago
5 0
<span>For a solute to be a strong electrolyte, the compound must almost completely dissolve into ions. Weak electrolytes only dissolve partially into ions. While nonelectrolytes do dissolve, none of the products are ions. Strong Electrolytes: Nitric Acid (HNo3), Potassium Chloride (KCl), Lithium Hydroxide (LiOH) Weak Electrolytes: Ammonia (NH3), Hydrofluoric Acid (HF) Nonelectrolytes: Ethanol (C2H5OH), Glucose (C6H12O6)</span>
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List the first 20 elements chemistry
timama [110]

Answer:

h- Hydrogen

He - Helium

Li - Lithium

Be - Beryllium

B - Boron

C - Carbon

N - Nitrogen

O - Oxygen

Explanation:

Happy to help:)

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Why do rats like cheese? &lt;&gt;-&lt;&gt; Im freaking out here dudes
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Calculate the hydronium ion concentration in an aqueous solution with a ph of 9.85 at 25°c.
UkoKoshka [18]

Answer:

1.41 × 10⁻¹⁰ M

Explanation:

We have a solution with a pH of 9.85 at 25 °C. We can calculate the concentration of H⁺ using the following expression.

pH = -log [H⁺]

[H⁺] = antilog -pH

[H⁺] = antilog -9.85

[H⁺] = 1.41 × 10⁻¹⁰ M

H⁺ is usually associated with water molecules forming hydronium ions.

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Then, the concentration of H₃O⁺ ions is 1.41 × 10⁻¹⁰ M.

8 0
3 years ago
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A 29.7 g sample of iron ore is treated as follows. The iron in the sample is all converted by a series of chemical reactions to
Softa [21]

<u>Answer:</u> The mass of iron in the ore is 10.9 g

<u>Explanation:</u>

We are given:

Mass of iron (III) oxide = 15.6 g

We know that:

Molar mass of Iron (III) oxide = 159.69 g/mol

Molar mass of iron atom = 55.85 g/mol

As, all the iron in the ore is converted to iron (III) oxide. So, the mass of iron in iron (III) oxide will be equal to the mass of iron present in the ore.

To calculate the mass of iron in given mass of iron (III) oxide, we apply unitary method:

In 159.69 g of iron (III) oxide, mass of iron present is (2\times 55.85)=111.7g

So, in 15.6 g of iron (III) oxide, mass of iron present will be = \frac{111.7g}{159.69g}\times 15.6g=10.9g

Hence, the mass of iron in the ore is 10.9 g

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3 years ago
A molecule consisting of more than one element that are chemically combined.
BaLLatris [955]

Answer:

compound, but I could be wrong

4 0
3 years ago
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