Question

A solution is prepared by adding 0.0231moles of H3O+ ions to 3.33L of water. What is the pH of this solution

Answer 1

2.15

Step-by-step explanation:

For this question, we have to remember the pH formula:

`pH~=~-Log[H_3O^+]`

By definition, the pH value is calculated when we do the -Log of the concentration of the hydronium ions (
`H_3O^+`). So, the next step is the calculation of the concentration of the hydronium ions. For this, we have to use the molarity formula:

`M=(mol)/(L)`

We already know the number of moles (0.0231 moles) and the volume (3.33 L). So, we can plug the values into the molarity formula:

`M=(0.0231~moles)/(3.33~L)=0.00693~M`

With this value, now we can calculate the pH value:

`pH~=~-Log[0.00693~M]~=~2.15`

The pH would be 2.15

I hope it helps!