Is the water found in the watershed clean and safe for drinking?

1 answer:

8 0

I heard that most of the time water found in watersheds aren’t usually clean nor safe for drinking, but i know that there are very few that are somewhat safe for drinking. It’s just not usually common to find clean and healthy watersheds though.

You might be interested in

How do you know the ph level of 10^-8

sergiy2304 [10]

pH=6.98

Explanation:

This is a very interesting question because it tests your understanding of what it means to have a dynamic equilibrium going on in solution.

As you know, pure water undergoes self-ionization to form hydronium ions, H3O+, and hydroxide anions, OH−.

2H2O(l]⇌H3O+(aq]+OH−(aq]→ very important!

At room temperature, the value of water's ionization constant, KW, is equal to 10−14. This means that you have

KW=[H3O+]⋅[OH−]=10−14

Since the concentrations of hydronium and hydroxide ions are equal for pure water, you will have

[H3O+]=√10−14=10−7M

The pH of pure water will thus be

pH=−log([H3O+])

pH=−log(10−7)=7

Now, let's assume that you're working with a 1.0-L solution of pure water and you add some 10

5 0

3 years ago

Answer this question please

Luden [163]

A. 5 It can either 3 or 5 you search it up in google

3 0

3 years ago

Read 2 more answers

Particle motion in ice is __________than partlice motion in water.

seraphim [82]

Answer:

1. Faster

Explanation:

7 0

3 years ago

Read 2 more answers

The phenolic indicator (In-OH)has approximately the same pKa as a carboxylic acid. Which H is the most acidic proton in In-OH? C

Sidana [21]

The –OH+ group is most acidic proton in ln-OH as shown in figure (a). The proton is circled in the figure.

The stabilisation of the conjugate base produced is stabilises due to resonance factor. The possible resonance structures are shown in figure (b).

The acidity of a protonated molecule depends upon the stabilisation of the conjugate base produced upon deprotonation. The conjugate base of ln-OH is shown in figure (a).

The possible resonance structures are shown in figure (b). As the number of resonance structures of the conjugate base increases the stabilisation increases. Here the unstable quinoid (unstable) form get benzenoid (highly stable) form due to the resonance which make the conjugate base highly stabilise.

Thus the most acidic proton is assigned in ln-OH and the stability of the conjugate base is explained.