QuestionFind the pH of a solution with hydronium ion concentration of $1 \times 10^{-11} M$ , considering significant figures.

Studdy Solution

STEP 1

Assumptions1. The hydronium ion concentration is $1 \times10^{-11} M$ . . The pH of a solution is calculated using the formula $pH = -\log[H3^+]$ , where $[H3^+]$ is the hydronium ion concentration.
3. The logarithm is base10.

STEP 2

We need to calculate the pH of the solution using the given hydronium ion concentration. We can do this by plugging the given concentration into the formula for pH.
$pH = -\log[H^+]$

STEP 3

Now, plug in the given value for the hydronium ion concentration to calculate the pH.
$pH = -\log[1 \times10^{-11} M]$

STEP 4

The logarithm of a product can be written as the sum of the logarithms of the individual numbers. So, we can rewrite the logarithm in the formula as follows $pH = -(\log[1] + \log[10^{-11}])$

STEP 5

The logarithm of1 is0, and the logarithm of $10^{-11}$ is -11. So, we can simplify the formula as follows $pH = -(0 + -11)$

STEP 6

Calculate the pH of the solution.
$pH = -(-11) =11$ The pH of the solution is11.

Was this helpful?

QuestionFind the pH of a solution with hydronium ion concentration of $1 \times 10^{-11} M$ , considering significant figures.

Studdy Solution

STEP 1

Assumptions1. The hydronium ion concentration is $1 \times10^{-11} M$ . . The pH of a solution is calculated using the formula $pH = -\log[H3^+]$ , where $[H3^+]$ is the hydronium ion concentration.
3. The logarithm is base10.

STEP 2

We need to calculate the pH of the solution using the given hydronium ion concentration. We can do this by plugging the given concentration into the formula for pH.
$pH = -\log[H^+]$

STEP 3

Now, plug in the given value for the hydronium ion concentration to calculate the pH.
$pH = -\log[1 \times10^{-11} M]$

STEP 4

The logarithm of a product can be written as the sum of the logarithms of the individual numbers. So, we can rewrite the logarithm in the formula as follows $pH = -(\log[1] + \log[10^{-11}])$

STEP 5

The logarithm of1 is0, and the logarithm of $10^{-11}$ is -11. So, we can simplify the formula as follows $pH = -(0 + -11)$

STEP 6

Calculate the pH of the solution.
$pH = -(-11) =11$ The pH of the solution is11.

Get Studdy

Studdy solves anything!

Start learning now

Download Studdy AI Tutor now. Learn with ease and get all help you need to be successful at school.

QuestionFind the pH of a solution with hydronium ion concentration of 1×10−11M1 \times 10^{-11} M1×10−11M, considering significant figures.

Studdy Solution

STEP 1

Assumptions1. The hydronium ion concentration is 1×10−11M1 \times10^{-11} M1×10−11M. . The pH of a solution is calculated using the formula pH=−log⁡[H3+]pH = -\log[H3^+]pH=−log[H3+], where [H3+][H3^+][H3+] is the hydronium ion concentration.3. The logarithm is base10.

STEP 2

We need to calculate the pH of the solution using the given hydronium ion concentration. We can do this by plugging the given concentration into the formula for pH.pH=−log⁡[H+]pH = -\log[H^+]pH=−log[H+]

STEP 3

Now, plug in the given value for the hydronium ion concentration to calculate the pH.pH=−log⁡[1×10−11M]pH = -\log[1 \times10^{-11} M]pH=−log[1×10−11M]

STEP 4

The logarithm of a product can be written as the sum of the logarithms of the individual numbers. So, we can rewrite the logarithm in the formula as followspH=−(log⁡[1]+log⁡[10−11])pH = -(\log[1] + \log[10^{-11}])pH=−(log[1]+log[10−11])

STEP 5

The logarithm of1 is0, and the logarithm of 10−1110^{-11}10−11 is -11. So, we can simplify the formula as followspH=−(0+−11)pH = -(0 + -11)pH=−(0+−11)

STEP 6

Calculate the pH of the solution.pH=−(−11)=11pH = -(-11) =11pH=−(−11)=11The pH of the solution is11.

Get Studdy

Studdy solves anything!

Start learning now

Download Studdy AI Tutor now. Learn with ease and get all help you need to be successful at school.

QuestionFind the pH of a solution with hydronium ion concentration of $1 \times 10^{-11} M$ , considering significant figures.

Assumptions1. The hydronium ion concentration is $1 \times10^{-11} M$ . . The pH of a solution is calculated using the formula $pH = -\log[H3^+]$ , where $[H3^+]$ is the hydronium ion concentration.
3. The logarithm is base10.

We need to calculate the pH of the solution using the given hydronium ion concentration. We can do this by plugging the given concentration into the formula for pH.
$pH = -\log[H^+]$

Now, plug in the given value for the hydronium ion concentration to calculate the pH.
$pH = -\log[1 \times10^{-11} M]$

The logarithm of a product can be written as the sum of the logarithms of the individual numbers. So, we can rewrite the logarithm in the formula as follows $pH = -(\log[1] + \log[10^{-11}])$

The logarithm of1 is0, and the logarithm of $10^{-11}$ is -11. So, we can simplify the formula as follows $pH = -(0 + -11)$

Calculate the pH of the solution.
$pH = -(-11) =11$ The pH of the solution is11.