What is the pH of a solution with [OH-] = 2.0 x 10-10 M?

4.30

Explanation:

[

H

+

]

[

O

H

−

]

=

1

×

10

−

14

Substitute the known values.

[

H

+

]

[

2.0

×

10

−

10

M

]

=

1

×

10

−

14

[

H

+

]

=

1

×

10

−

14

2.0

×

10

−

10

[

H

+

]

=

5

×

10

−

5

The formula to determine the pH of the solution is as follows:

p

H

=

−

log

[

H

+

]

Substitute the known values.

p

H

=

−

log

[

5

×

10

−

5

]

=

4.30

Therefore, the pH of the solution is 4.30.

it has two answers first :-

We find

p

H

≅

4

Explanation:

We interrogate the equilibrium:

2

H

2

O

⇌

H

3

O

+

+

H

O

−

We know that in aqueous solution under standard conditions that:

[

H

3

O

+

]

[

H

O

−

]

=

K

w

=

10

−

14

We take

log

10

OF BOTH SIDES:

log

10

[

H

3

O

+

]

+

log

10

[

H

O

−

]

=

log

10

(

10

−

14

)

But by definition, the logarithmic function is that power to which you raise the base to get the specific answeri.e. if

log

a

B

=

c

, then

a

c

=

B

.

And thus

log

10

(

10

−

14

)

=

−

14

And so

log

10

[

H

3

O

+

]

+

log

10

[

H

O

−

]

=

−

14

OR

−

log

10

[

H

3

O

+

]

−

log

10

[

H

O

−

]

=

14

But we define

p

H

=

−

log

10

[

H

3

O

+

]

, and

p

O

H

=

−

log

10

[

H

O

−

]

, and so

14

=

p

H

+

p

O

H

.

And now finally,

p

H

=

14

−

p

O

H

14

−

(

−

log

10

(

2.0

×

10

−

10

)

=

4.30

Explanation:

2 method :-

Right off the bat, if you don't understand the

general concepts of pH and pOH, I suggest you watch this 5-minute video before proceeding to read this answer.

Recall that pH is an index for describing the concentration of hydronium ion. Mathematically, pH is described as:

p

H

=

−

log

[

H

3

O

+

]

A common mistake to make in this sort of problem is to move too quickly, and take

−

log

(

2.0

⋅

10

−

10

)

, and get your pH as 9.70. This is wrong, because you're not given a hydronium ion concentration, but a hydroxide ion concentration. Therefore, what you've calculated is really something called the pOH, not the pH.

So how do you work this out? Basically, you'll need to know that the product of the concentration of hydroxide and hydronium ions in a solution will always equal

10

−

14

at

24

o

C

Mathematically speaking:

[

H

3

O

+

]

[

O

H

−

]

=

10

−

14

Taking the negative log of both sides of the equation yields:

p

H

+

p

O

H

=

14

Given this, there's 2 ways to do this problem. Method one is to use the 1st equation, and solve for

[

H

3

O

+

]

. Then, you just take the negative log of that.

Method 2 (easier, in my opinion) is to solve for the pOH, and then subtract it from 14.

Either way, you should get an answer of 4.30.

Do a reality check: your concentration of hydroxide is very small. Therefore, your pOH value would be fairly large, meaning that your pH would be small. This aligns with what we got.

Hope that helps :)

14 days is the half-life of phosphorus-32