What is the pOH of a solution of HNO3?
Table of Contents
What is the pOH of a solution of HNO3?
pH = -log[H+] = -log(0.00340) = 2.47 2) Determine the pOH of a 0.00340 M HNO3 solution. To find pOH, take the –log of 2.26 x 10-4, which is 3.65. To find pH, subtract 3.65 from 14. The pH of this solution is 10.35.
What is the pH of a HNO3?
pH of Common Acids and Bases
| Acid | Name | 100 mM |
|---|---|---|
| HNO3 | nitric acid | 1.08 |
| H3PO4 | orthophosphoric acid | 1.63 |
| H3AsO4 | arsenic acid | 1.70 |
| H2SeO3 | selenous acid | 1.90 |
What is the pH of 0.0001 M hno3?
Explanation: log10{0.0001} = log10(10−4)=−4 , by definition of the log function. Thus pH = 4 , and, necessarily, pOH=10 .
What is the pH of 0.1 M hno3 nitric acid?
1.0
The concentration of H₃O⁺ in a strong acid solution is therefore equal to the initial concentration of the acid. For example, a solution of 0.1 M HNO₃ contains 0.1 M H₃O⁺ and has a pH of 1.0.
What is relationship of pH and pOH?
pH and pOH are related to one another; THEY ARE NOT INDEPENDENT OF EACH OTHER. As pH increases, pOH decreases. As pH decreases, pOH increases. By knowing what ion you are measuring on which scale, this will tell you whether or not the solution is acidic or basic.
Which is the correct relationship between pH and pOH?
The pOH scale is similar to the pH scale in that a pOH of 7 is indicative of a neutral solution. A basic solution has a pOH less than 7, while an acidic solution has a pOH of greater than 7. The pOH is convenient to use when finding the hydroxide ion concentration from a solution with a known pH.
How do you calculate pH and pOH?
To find the pOH, simply subtract the pH from 14. In order to calculate the pOH, take the negative log of the hydroxide ion concentration. To find the pH, simply subtract pOH from 14.