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2 years ago

Which could be the pH of an aqueous solution with a H3O+ ion concentration that is less than its OH- ion concentration?

Chemistry

1 answer:

anzhelika [568]2 years ago

4 0

Answer:

Explanation:

You can think of pH as "parts Hydrogen ion," but remember that the pH scale is "backwards." The pH scale ranges from 0 to 14, with zero being the most acidic (highest concentration of H+) and 14 being the most basic.

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Diagram of Krebs cycle.

Dmitry [639]

Answer:

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2 years ago

A.<br><br> A una atmósfera de presión (1atm), ¿cuál es el punto de solidificación del agua?

Ghella [55]

Answer:

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7 0

3 years ago

The chemical reaction in which ammonium sulfate and

Ganezh [65]

Answer:

Answer and Explanation: In this reaction ammonium sulfate reacts with potassium hydroxide to give aqueous potassium sulfate, gaseous ammonia, and liquid water as the products. This is essentially an acid-base reaction where the ammonium ion is donating a hydrogen ion to the hydroxide ion from the potassium hydroxide.

Explanation:

5 0

2 years ago

A sample of nitrogen gas has a temperature of 22.7oC when the volume of the container is 12.2L and it is under 150.4kPa of press

Marrrta [24]

Answer:

The final temperature of the gas would need to be approximately 158.4 K

Explanation:

The details of the sample of nitrogen gas are;

The initial temperature of the nitrogen gas, T₁ = 22.7°C = 295.85 K

The initial volume occupied by the gas, V₁ = 12.2 L

The initial pressure of the gas, P₁ = 150.4 kPa

The final volume of the gas, V₂ = 9.7 L

The final pressure of the gas, P₂ = 101.3 kPa

Let 'T₂', represent the final temperature of the gas, by the ideal gas equation, we have;

$\dfrac{P_1 \times V_1}{T_1} = \dfrac{P_2 \times V_2}{T_2}$

$\therefore \ T_2 = \dfrac{P_2 \times V_2 \times T_1 }{P_1 \times V_1}$

Plugging in the values gives;

$\therefore \ T_2 = \dfrac{101.3 \, kPa \times 9.7 \ L \times 295.85 K}{150.4 \ kPa \times 12.2 \ L} \approx 158.4327959 \ K$

The final temperature of the gas, T₂ ≈ 158.4 K

3 0

3 years ago

Calculate the molar mass of (NH4)2SO4. molar mass of (NH4)2SO4=__N*__+__*__+__*__+__ O*__=__ g/mol (total)

Alinara [238K]

Answer:

132 g/mol

Explanation:

(NH₄)₂SO₄ has 2 nitrogen atoms, 8 hydrogen atoms, 1 sulfur atom, and 4 oxygen atoms.

From the periodic table, the molar mass of each element is:

N: 14.0 g/mol

H: 1.01 g/mol

S: 32.1 g/mol

O: 16.0 g/mol

So the molar mass of the compound is:

2N × (14.0 g/mol N) + 8H × (1.01 g/mol H) + 1S × (32.1 g/mol S) + 4O × (16.0 g/mol O)

= 28.0 + 8.08 + 32.1 + 64.0 g/mol

= 132 g/mol

If you need more precision, use more significant figures for the element molar masses.

4 0

3 years ago