Multiple Choice
Calculate the pH of a 0.10 M HNO3 solution and a 5.0 × 10^-2 M NaOH solution.
441
views
17. Acid and Base Equilibrium
pH of Strong Acids and Bases
Multiple Choice
What is the pH of a solution of , assuming it is a strong acid that dissociates completely in water?
A
B
C
D
Verified step by step guidance1
Recognize that HNO\_3 (nitric acid) is a strong acid, which means it dissociates completely in water. Therefore, the concentration of H\_3O\^+ ions (or H\^+ ions) in solution is equal to the initial concentration of the acid.
Write the dissociation equation: HNO\_3 \(\rightarrow\) H\^+ + NO\_3\^- , indicating that for every 1 mole of HNO\_3, 1 mole of H\^+ is produced.
Since the concentration of HNO\_3 is 0.0040 M, the concentration of H\^+ ions is also 0.0040 M.
Use the formula for pH, which is defined as pH = -\(\log\)[H\^+], where [H\^+] is the molar concentration of hydrogen ions.
Substitute the concentration of H\^+ into the pH formula: pH = -\(\log\)(0.0040). Calculate this logarithm to find the pH value.
Related Videos
Related Practice
