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2 years ago

4. Do you think there is a change in energy as the fireworks travel from the ground

Chemistry

1 answer:

Andru [333]2 years ago

4 0

Yes when a firework goes into the sky it releases chemical potential energy which is then changed into kinetic energy

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Write the chemical formula of the following:

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Answer:

1.Ca(OH)2

2.Mg(OH)2

3.Al2SO4

4.Na2CO3

5.Zn3(PO4)2

6.LiNO3

7.CuCO3

8. K2CO3

9.MgSO4

10.Ca3(PO4)2

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3 years ago

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3 years ago

Polyatomic ions

Vitek1552 [10]

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3 years ago

Which buffer would be better able to hold a steady pH on the addition of strong acid, buffer 1 or buffer 2? Explain. Buffer 1: a

Talja [164]

Answer:

Buffer 1.

Explanation:

Ammonia is a weak base. It acts like a Bronsted-Lowry Base when it reacts with hydrogen ions.

$\rm NH_3\; (aq) + H^{+}\; (aq) \to {NH_4}^{+}\; (aq)$ .

$\rm NH_3$ gains one hydrogen ion to produce the ammonium ion $\rm {NH_4}^{+}$ . In other words, $\rm {NH_4}^{+}$ is the conjugate acid of the weak base $\rm NH_3$ .

Both buffer 1 and 2 include

the weak base ammonia $\rm NH_3$ , and
the conjugate acid of the weak base $\rm {NH_4}^{+}$ .

The ammonia $\rm NH_3$ in the solution will react with hydrogen ions as they are added to the solution:

$\rm NH_3\; (aq) + H^{+}\; (aq) \to {NH_4}^{+}\; (aq)$ .

There are more $\rm NH_3$ in the buffer 1 than in buffer 2. It will take more strong acid to react with the majority of $\rm NH_3$ in the solution. Conversely, the pH of buffer 1 will be more steady than that in buffer 2 when the same amount of acid has been added.

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3 years ago