Multiple Choice
What is the concentration of a solution of HCl in which a 10.0 mL sample of acid required 50.0 mL of 0.150 M NaOH solution for neutralization?
300
views
6. Chemical Quantities & Aqueous Reactions
Solution Stoichiometry
Multiple Choice
You have a beaker holding 25.0 mL of 1.5 M HCl. You then add 10.0 mL of 2.0 M NaOH to the beaker. What is the pH of the solution after the addition of the NaOH?
A
7.00
B
12.00
C
2.00
D
1.00
Verified step by step guidance1
Calculate the moles of HCl initially present using the formula: \( \text{moles of HCl} = Molarity \times Volume \). Convert the volume from mL to L by dividing by 1000.
Calculate the moles of NaOH added using the formula: \( \text{moles of NaOH} = Molarity \times Volume \). Again, convert the volume from mL to L.
Determine the limiting reactant by comparing the moles of HCl and NaOH. Since HCl and NaOH react in a 1:1 ratio, the reactant with fewer moles is the limiting reactant.
Calculate the moles of HCl or NaOH remaining after the reaction. Subtract the moles of the limiting reactant from the moles of the other reactant.
Determine the pH of the solution. If HCl is in excess, calculate the concentration of \( \text{H}^+ \) ions and use \( \text{pH} = -\log[\text{H}^+] \). If NaOH is in excess, calculate the concentration of \( \text{OH}^- \) ions, find the pOH using \( \text{pOH} = -\log[\text{OH}^-] \), and then find the pH using \( \text{pH} = 14 - \text{pOH} \).
Related Videos
Related Practice
