Multiple Choice
What is the pH of a solution after mixing 250 mL of 0.250 M HBr with 250 mL of 0.125 M NaOH?
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
What is the pH of a solution made by mixing 0.30 mol of NaOH, 0.25 mol of Na2HPO4, and 0.20 mol of H3PO4 with water and diluting to 1.00 L?
A
pH = 7.0
B
pH = 1.0
C
pH = 3.0
D
pH = 13.0
Verified step by step guidance1
Identify the species in the solution: NaOH is a strong base, Na2HPO4 is a salt that can act as a weak base, and H3PO4 is a weak acid.
Calculate the moles of OH⁻ ions contributed by NaOH. Since NaOH is a strong base, it dissociates completely in water, providing 0.30 mol of OH⁻ ions.
Consider the reaction between H3PO4 and OH⁻. H3PO4 can react with OH⁻ to form H2PO4⁻ and water. Calculate the moles of OH⁻ that will react with H3PO4.
Determine the remaining concentration of OH⁻ ions after the reaction with H3PO4. Subtract the moles of OH⁻ that reacted with H3PO4 from the initial moles of OH⁻.
Calculate the pOH of the solution using the concentration of remaining OH⁻ ions, and then convert pOH to pH using the relation: \( \text{pH} = 14 - \text{pOH} \).
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