You have found that 14.37mL of 0.162M sulfuric acid reacts with exactly 20.00mL of barium hydroxide solution of unknown concentration. What is the molarity of the barium hydroxide solution? Round your answer to 3 decimal places and include units.
I know that this has something to do with Molarity and that the molarity equation is (M) = moles of solute / volume of solution (in liters) What I'm unsure of is how do set it up wit the unknown?
That's right. M = mols/L or mols = M x L = ?
Four steps.
1. Write and balance the equation.
Ba(OH)2 + H2SO4 ==> BaSO4 + 2H2O
2. Convert what you have to mols.
mols Ba(OH)2 = M x L = ?
3. Using the coefficients in the balanced equation, convert mols Ba(OH)2 to mols H2SO4. The coefficients are 1:1 therefore, mols Ba(OH)2 = mols H2SO4.
4. Then M H2SO4 = mols H2SO4/L H2SO4 = ?
To determine the molarity of the barium hydroxide solution, you can follow these steps:
Step 1: Convert the given volumes to liters.
- Given: 14.37 mL of sulfuric acid and 20.00 mL of barium hydroxide solution
- Conversion to liters: 14.37 mL = 0.01437 L (divide by 1000) and 20.00 mL = 0.02000 L
Step 2: Calculate the moles of sulfuric acid using its molarity and volume.
- Molarity of sulfuric acid = 0.162 M (given)
- Moles of sulfuric acid = Molarity × volume
=> Moles of sulfuric acid = 0.162 M × 0.01437 L
Step 3: Determine the mole ratio between sulfuric acid and barium hydroxide.
- The balanced chemical equation for the reaction is:
H2SO4(aq) + Ba(OH)2(aq) → BaSO4(s) + 2H2O(l)
- From the equation, you can see that the mole ratio between sulfuric acid (H2SO4) and barium hydroxide (Ba(OH)2) is 1:1.
Step 4: Use the mole ratio to determine the moles of barium hydroxide.
- Since the mole ratio is 1:1, the moles of barium hydroxide is also equal to the moles of sulfuric acid.
Step 5: Calculate the molarity of the barium hydroxide solution.
- Molarity of barium hydroxide = Moles of barium hydroxide / Volume of barium hydroxide solution
- Molarity of barium hydroxide = Moles of sulfuric acid / Volume of barium hydroxide solution
=> Molarity of barium hydroxide = (0.162 M × 0.01437 L) / 0.02000 L
Finally, simply perform the calculation to find the molarity of the barium hydroxide solution:
Molarity of barium hydroxide = (0.162 M × 0.01437 L) / 0.02000 L
Round the final answer to three decimal places and don't forget to include the units.