Multiple Choice
A 25.00 mL sample of 0.175 M HCl is being titrated with 0.250 M NaOH. What is the pH when 0 mL of NaOH has been added?
17. Acid and Base Equilibrium
pH of Strong Acids and Bases
Struggling with General Chemistry?
Join thousands of students who trust us to help them ace their exams!Watch the first videoMultiple Choice
Calculate the concentration of OH⁻ in a 0.01 M HCl solution at 25 °C, and classify the solution as acidic or basic.
A
1.0 x 10⁻¹² M, acidic
B
1.0 x 10⁻⁷ M, neutral
C
1.0 x 10⁻¹⁰ M, basic
D
1.0 x 10⁻² M, basic
Verified step by step guidance1
Start by understanding that HCl is a strong acid, which means it dissociates completely in water. Therefore, the concentration of H⁺ ions in the solution is equal to the initial concentration of HCl, which is 0.01 M.
Use the ion product of water (Kw) at 25 °C, which is 1.0 x 10⁻¹⁴. The relationship between the concentrations of H⁺ and OH⁻ ions in water is given by the equation: .
Substitute the known values into the equation: . Solve for the concentration of OH⁻ ions.
Calculate the concentration of OH⁻ ions by rearranging the equation: .
Determine the nature of the solution. Since the concentration of H⁺ ions is greater than that of OH⁻ ions, the solution is classified as acidic.
2:39mWatch next
Master pH of Strong Acids and Bases with a bite sized video explanation from Jules
Start learningRelated Videos
Related Practice
pH of Strong Acids and Bases practice set
Problem sets built by lead tutorsExpert video explanations