What volume of 0.5 M HCl is required to completely react with 0.1 moles of Na2CO3?
Practice Questions
1 question
Q1
What volume of 0.5 M HCl is required to completely react with 0.1 moles of Na2CO3?
200 mL
400 mL
100 mL
300 mL
The reaction is Na2CO3 + 2 HCl → 2 NaCl + H2O + CO2. 0.1 moles of Na2CO3 requires 0.2 moles of HCl. Volume = moles / concentration = 0.2 moles / 0.5 M = 0.4 L or 400 mL.
Questions & Step-by-step Solutions
1 item
Q
Q: What volume of 0.5 M HCl is required to completely react with 0.1 moles of Na2CO3?
Solution: The reaction is Na2CO3 + 2 HCl → 2 NaCl + H2O + CO2. 0.1 moles of Na2CO3 requires 0.2 moles of HCl. Volume = moles / concentration = 0.2 moles / 0.5 M = 0.4 L or 400 mL.
Steps: 6
Step 1: Write down the balanced chemical equation for the reaction: Na2CO3 + 2 HCl → 2 NaCl + H2O + CO2.
Step 2: Identify how many moles of HCl are needed for the reaction. From the equation, 1 mole of Na2CO3 reacts with 2 moles of HCl.
Step 3: Calculate the moles of HCl needed for 0.1 moles of Na2CO3. Since 0.1 moles of Na2CO3 requires 2 times that amount in HCl, you need 0.1 moles * 2 = 0.2 moles of HCl.
Step 4: Use the formula for volume: Volume = moles / concentration. Here, you have 0.2 moles of HCl and the concentration is 0.5 M.
Step 5: Plug in the values: Volume = 0.2 moles / 0.5 M = 0.4 L.
Step 6: Convert the volume from liters to milliliters. Since 1 L = 1000 mL, 0.4 L = 0.4 * 1000 = 400 mL.
