If 50 mL of 0.1 M sulfuric acid is neutralized by sodium hydroxide, how many moles of NaOH are required?
Practice Questions
1 question
Q1
If 50 mL of 0.1 M sulfuric acid is neutralized by sodium hydroxide, how many moles of NaOH are required?
0.005
0.01
0.02
0.03
H2SO4 dissociates to give 2 H+ ions. Moles of H2SO4 = 0.1 M * 0.050 L = 0.005 moles. Therefore, moles of NaOH required = 0.005 moles * 2 = 0.01 moles.
Questions & Step-by-step Solutions
1 item
Q
Q: If 50 mL of 0.1 M sulfuric acid is neutralized by sodium hydroxide, how many moles of NaOH are required?
Solution: H2SO4 dissociates to give 2 H+ ions. Moles of H2SO4 = 0.1 M * 0.050 L = 0.005 moles. Therefore, moles of NaOH required = 0.005 moles * 2 = 0.01 moles.
Steps: 6
Step 1: Understand that sulfuric acid (H2SO4) dissociates into 2 hydrogen ions (H+) when it reacts with sodium hydroxide (NaOH).
Step 2: Calculate the volume of sulfuric acid in liters. Since we have 50 mL, we convert it to liters: 50 mL = 0.050 L.
Step 3: Use the molarity (M) of sulfuric acid to find the number of moles. Moles of H2SO4 = Molarity * Volume in liters = 0.1 M * 0.050 L.
Step 4: Calculate the moles of H2SO4: 0.1 * 0.050 = 0.005 moles.
Step 5: Since each mole of H2SO4 produces 2 moles of H+, we need to multiply the moles of H2SO4 by 2 to find the moles of NaOH required: 0.005 moles * 2 = 0.01 moles.
Step 6: Conclude that 0.01 moles of NaOH are required to neutralize the sulfuric acid.
