# What is the pH of a solutiont that is .1 M HCl (strong acid)?

( And a few more questions if you can answer these too:] )

What is the pH of a solution that has a pOH of 11?

What is the molarity, or concentration, of [H3O+] of a solution at pH 5?

(step by step answers would be ideal, thanks!)

### 5 Answers

- 1 decade agoBest Answer
Question 1:

Note the formula of dissociation for HCl:

HCl --> H+ + Cl-.

Because HCl is a strong acid, it totally dissociates in water.

In order to figure out the pH of this solution, we must know the molarity of [H+] in solution to plug it into an equation.

Because HCl is a strong acid, we can use stoichiometry to find out the molarity of [H+]:

0.1 M HCl (1 mol HCl/1 mol H+) = 0.1 M H+

Now plug the answer into this equation:

pH = -log[H+] = -log (0.1 M) = 1.0

The pH of the solution is 1.0

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Question 2:

To find the pH of a solution when we are given pOH, remember that in 25 degrees Celsius, pH + pOH = 14.00. Algebraically manipulate this equation and substitute pOH:

pH + pOH = 14.00 --> pH = 14.00 - pOH = 14.00 - 11 = 3

The pH of this solution is 3

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Question 3:

[H3O+] is another way of saying [H+].

In order to figure the concentration of [H+] from pH, we must manipulate the equation used in question 1 to find [H+]:

pH = -log[H+] --> [H+] = 10^-pH = 10^-5 = 1*10^-5 M

The concentration of H3O+ ions in solution is 1*10^-5 M

- Anonymous4 years ago
This Site Might Help You.

RE:

What is the pH of a solutiont that is .1 M HCl (strong acid)?

( And a few more questions if you can answer these too:] )

What is the pH of a solution that has a pOH of 11?

What is the molarity, or concentration, of [H3O+] of a solution at pH 5?

(step by step answers would be ideal, thanks!)

Source(s): ph solutiont 1 hcl strong acid: https://biturl.im/HGZ9P - How do you think about the answers? You can sign in to vote the answer.
- AlineLv 44 years ago
For the best answers, search on this site https://shorturl.im/7nM8M

pH you are given to be 1.0 in your question not 1.1 this means the concentration of H+ is 10^-1 100 times weaker is 10^-1/10^-2 = 10^-3 and thus acetic acid has a pH of 3.0