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3 years ago

List 2 underlying causes of water pollution

Chemistry

2 answers:

olga_2 [115]3 years ago

6 0

Answer:

industrialization and rapid human population growth.

Explanation:

Hope this helps

lawyer [7]3 years ago

4 0

Answer:

Water Pollution

Explanation:

Dumping industrial waste in ocean

Accidental oil leakages

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To measure the amount of nickel in some industrial waste fluid, an analytical chemist adds sodium hydroxide solution to a sample

Cloud [144]

Answer:

The final balanced equation is

Ni2+ + 2NaOH --> Ni (OH)2 + 2Na+

Explanation:

It is given that sodium hydroxide is added to collect the solid nickel(II) hydroxide product

The empirical equation for this statement is

Ni2+ + NaOH --> Ni (OH)2 + Na+

We will first balance the hydroxide molecule. On the right side there are two OH molecules.

Thus, on the left side we will take 2 sodium hydroxide

Ni2+ + 2NaOH --> Ni (OH)2 + Na+

Now we will balance the sodium ion which are 2 in numbers on the left side and 1 on the right side

Ni2+ + 2NaOH --> Ni (OH)2 + 2Na+

So, the final balanced equation is

Ni2+ + 2NaOH --> Ni (OH)2 + 2Na+

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3 years ago

A reaction that is NOT thermodynamically favored at low temperatures can become thermodynamically favored at high temperatures

Rom4ik [11]

Explanation:

Its gonna be D

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3 years ago

each element is designated by its __________ which is usually from the first letters of the elements name

klemol [59]

Answer:

each element is designated by its Chemical Symbol which is usually from the first letters of the elements name

Explanation:

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3 years ago

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dezoksy [38]

Answer:

double replacement

Explanation:

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3 years ago

Read 2 more answers

g If 50.0 mL of a 0.75 M acetic acid solution is titrated with 1.0 M sodium hydroxide, what is the pH after 10.0 mL of NaOH have

V125BC [204]

Answer:

pH = 2.66

Explanation:

Acetic Acid + NaOH → Sodium Acetate + H₂O

First we calculate the number of moles of each reactant, using the given volumes and concentrations:

0.75 M Acetic acid * 50.0 mL = 37.5 mmol acetic acid

1.0 M NaOH * 10.0 mL = 10 mmol NaOH

We calculate how many acetic acid moles remain after the reaction:

37.5 mmol - 10 mmol = 27.5 mmol acetic acid

We now calculate the molar concentration of acetic acid after the reaction:

27.5 mmol / (50.0 mL + 10.0 mL) = 0.458 M

Then we calculate [H⁺], using the following formula for weak acid solutions:

[H⁺] = $\sqrt{C*Ka}=\sqrt{0.458M*1.76x10^{-5}}$

[H⁺] = 0.0028

Finally we calculate the pH:

pH = -log[H⁺]

pH = 2.66

8 0

3 years ago