Multiple Choice
Calculate the pH of a solution that is 0.075 M in HNO₃ and 0.170 M in HC₇H₅O₂, given that HNO₃ is a strong acid and HC₇H₅O₂ is a weak acid.
382
views
17. Acid and Base Equilibrium
pH of Strong Acids and Bases
Multiple Choice
What is the pH of a solution at ? Assume is a strong base that dissociates completely.
A
B
C
D
Verified step by step guidance1
Identify that LiOH is a strong base and dissociates completely in water, so the concentration of OH⁻ ions is equal to the initial concentration of LiOH, which is 0.050 M.
Calculate the pOH of the solution using the formula: \(\text{pOH} = -\log[\text{OH}^-]\). Substitute the OH⁻ concentration into this formula.
Use the relationship between pH and pOH at 25°C, which is: \(\text{pH} + \text{pOH} = 14.00\).
Rearrange the equation to solve for pH: \(\text{pH} = 14.00 - \text{pOH}\).
Substitute the calculated pOH value into this equation to find the pH of the solution.
Related Videos
Related Practice
