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Lubov Fominskaja [6]

2 years ago

6

Why we are advice to use fossil fuel only when absolutely necessary?

1 answer:

trasher [3.6K]2 years ago

4 0

Answer:

Hello there! For some reason Brainly detects my answers as containing swear words in them when they do not. Hence, the answer is going to be in the comments. Enjoy!

Explanation:

Hope this helped!

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Which of the following is an irreversible physical change?

Yuliya22 [10]

Answer:

b) sharpening a pencil

Explanation:

If you melt lead, boil water, or dissolve sugar in water, you can return all of them back to their original state. If you sharpen a pencil, you can't reattach the shavings as they were originally.

3 0

3 years ago

Write a net ionic equation for the overall reaction that occurs when aqueous solutions of sodium hydroxide and oxalic acid (H2C2

belka [17]

Answer:

Oxalic acid is a dicarboxylic acid and forms sodium salt with NaOH and water

Explanation:

4 0

2 years ago

Read 2 more answers

What does this equation, 2 C(s) + O 2(g) ® 2 CO(g), tell us?

Zanzabum

Answer:

D. All of these.

Explanation:

For an equation to be balanced the number of atoms of each kind in the reactants and the products should be the same.

Then from this equation, CO is a product.

Last, two carbon atoms undergo reaction with the oxygen molecule for complete reaction to occur. Each atom combines with one oxygen atom.

7 0

2 years ago

Read 2 more answers

Ghella [55]

potassium reacts the most vigorously.

7 0

2 years ago

A phosphate buffer is involved in the formation of urine. The developing urine contains H2PO4 and HPO42- in the same concentrati

Katen [24]

Answer:

The ionization equation is

$H_{2}PO_{4}^{-} +H_{2}O$ ⇄ $HPO_{4}^{-2} +H_{3}O^{+}$ (1)

Explanation:

The ionization equation is

$H_{2}PO_{4}^{-} +H_{2}O$ ⇄ $HPO_{4}^{-2} +H_{3}O^{+}$ (1)

As the Bronsted definition sais, an acid is a substance with the ability to give protons thus, H2PO4 is the acid and HPO42- is the conjugate base.

The Ka expression is the ratio between the concentration of products and reactants of the equilibrium reaction so,

$Ka = \frac{[HPO_{4}^{-2}] [H_{3}O^{+}]}{[H_{2}PO_{4}^{-}] [H_{2}O]} = 6.2x10^{-8}$

The pKa is

$-Log (Ka) = -Log (6.2x10^{-8}) = 7.2$

The pKa of H2CO3 is 6,35, thus this a stronger acid than H2PO4. The higher the pKa of an acid greater the capacity to donate protons.

In the body H2CO3 is a more optimal buffer for regulating pH due to the combination of the two acid-base equilibriums and the two pKa.

If the urine is acidified, according to Le Chatlier's Principle the equilibrium (1) moves to the left neutralizing the excess proton concentration.

3 0

3 years ago