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AURORKA [14]
3 years ago
12

You have an aqueous solution of chromium(III) nitrate that you titrate with an aqueous solution of sodium hydroxide. After a cer

tain amount of titrant has been added, you observe a precipitate forming. You add more sodium hydroxide solution and the precipitate dissolves, leaving a solution again. What has happened?1) The precipitate was chromium hydroxide, which then reacted with more hydroxide to produce a soluble complex ion, Cr(OH)4?.2) The precipitate was chromium hydroxide, which dissolved once more solution was added, forming Cr3+(aq).3) The precipitate was sodium nitrate, which reacted with more nitrate to produce the soluble complex ion Na(NO3)2?.4) The precipitate was sodium hydroxide, which re-dissolved in the larger volume.
Chemistry
1 answer:
barxatty [35]3 years ago
7 0

Answer:

The precipitate was chromium hydroxide, which then reacted with more hydroxide to produce a soluble complex, Cr(OH)4

Explanation:

The following reaction takes place when chromium(III) nitrate reacts with NaOH:

Cr(NO)_{3} +3 NaOH → Cr(OH)_{3} (s)+ NaNO_{3}

The precipitate that is formed is chromium hydroxide, Cr(OH)_{3}

When more NaOH is added, the precipitate reacts with it which then results in the formation of a soluble complex ion:

Cr(OH)_{3}(s) + OH^{-}(aq) → Cr(OH)_{4} ^{-}(aq)

Cr(OH)_{4} ^{-} is soluble complex ion

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yawa3891 [41]

Answer:

a. 2 HgO(s) ⇒ 2 Hg(l) + O₂(g)

b. 0.957 g

Explanation:

Step 1: Write the balanced equation

2 HgO(s) ⇒ 2 Hg(l) + O₂(g)

Step 2: Convert 130.0 °C to Kelvin

We will use the following expression.

K = °C + 273.15

K = 130.0°C + 273.15

K = 403.2 K

Step 3: Calculate the moles of O₂

We will use the ideal gas equation.

P × V = n × R × T

n = P × V/R × T

n = 1 atm × 0.0730 L/0.0821 atm.L/mol.K × 403.2 K

n = 2.21 × 10⁻³ mol

Step 4: Calculate the moles of HgO that produced 2.21 × 10⁻³ moles of O₂

The molar ratio of HgO to O₂ is 2:1. The moles of HgO required are 2/1 × 2.21 × 10⁻³ mol = 4.42 × 10⁻³ mol.

Step 5: Calculate the mass corresponding to 4.42 × 10⁻³ moles of HgO

The molar mass of HgO is 216.59 g/mol.

4.42 × 10⁻³ mol × 216.59 g/mol = 0.957 g

5 0
3 years ago
How can you use chemistry to enhance ground transportation vehicles and reduce pollution?
Svetradugi [14.3K]

Answer:

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Take public transit. ...

Carpool. ...

Avoid idling. ...

Use alternative fuels.

3 0
2 years ago
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Knees and elbows are two of the most common ones.
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B is the correct answer

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Free_Kalibri [48]

Answer:

  • Option d. i<u><em>t is higher than the energy of both reactants and products</em></u>

Explanation:

<em>Activated complex</em>, also known as transition state, is the intermediate structure formed in the course of a chemical reaction.

The activated complex is very unstable and of short life: it is at the peak of the potential chemical diagram, and can transform either into the reactants (backward) or the products (forward).

The activation energy of the reaction is the energy needed to reach the activated complex, then both reactants and products are lower in potential chemical energy than the activated complex, which is what explains why the activated complex can transform into one or another, reactants or products.

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