What is the molarity of an HNO3 solution if 24.1mL of a 0.250M Ba(OH)2 solution is needed to titrate a 15.0mL sample of the acid? Can you tell me the process to finding this answer?

Print this out. This 4-step procedure will work all of this type.

1. Write and balance the equation.
2. mols HNO3 = M x L = ?
3. Use the coefficients in the balanced equation to convert mols HNO3 to mols Ba(OH)2.
4. Then M Ba(OH)2 = mols Ba(OH)2/L Ba(OH)2

0.803 M HNO3

To find the molarity of the HNO3 solution, we can use the stoichiometry of the balanced chemical equation between HNO3 and Ba(OH)2. The balanced equation is:

2HNO3 + Ba(OH)2 -> Ba(NO3)2 + 2H2O

In this reaction, 2 moles of HNO3 react with 1 mole of Ba(OH)2.

Given the volume and molarity of Ba(OH)2 solution used, we can first calculate the number of moles of Ba(OH)2 used.

Step 1: Calculate moles of Ba(OH)2 used
moles of Ba(OH)2 = volume (L) × molarity (mol/L)
moles of Ba(OH)2 = 0.0241 L × 0.250 mol/L

Step 1: Calculate moles of Ba(OH)2 used
moles of Ba(OH)2 = 0.006025 mol

Step 2: Determine the mole ratio between Ba(OH)2 and HNO3
From the balanced chemical equation, we know that 2 moles of HNO3 react with 1 mole of Ba(OH)2.

Step 3: Calculate moles of HNO3
moles of HNO3 = (moles of Ba(OH)2) × (2 moles of HNO3 / 1 mole of Ba(OH)2)
moles of HNO3 = 0.006025 mol × (2/1)

Step 3: Calculate moles of HNO3
moles of HNO3 = 0.01205 mol

Step 4: Calculate molarity of HNO3
molarity of HNO3 = moles / volume (L)
molarity of HNO3 = 0.01205 mol / 0.0150 L

Step 4: Calculate molarity of HNO3
molarity of HNO3 = 0.803 M

Therefore, the molarity of the HNO3 solution is 0.803 M.

To find the molarity of an HNO3 solution using titration, you need to use the balanced chemical equation and stoichiometry. Here's the step-by-step process to find the answer:

1. Write the balanced chemical equation for the reaction between HNO3 and Ba(OH)2:
2 HNO3 + Ba(OH)2 -> 2 H2O + Ba(NO3)2

2. Calculate the number of moles of Ba(OH)2 used by multiplying the volume of the solution (24.1 mL) by its molarity (0.250 M):
Moles of Ba(OH)2 = Volume of Ba(OH)2 solution (L) x Molarity of Ba(OH)2 solution (mol/L)

Convert the volume from mL to L by dividing by 1000:
Volume of Ba(OH)2 solution (L) = 24.1 mL / 1000 = 0.0241 L

Moles of Ba(OH)2 = 0.0241 L x 0.250 mol/L

3. Determine the stoichiometric ratio between HNO3 and Ba(OH)2 from the balanced equation. In this case, it is 2 moles of HNO3 for every 1 mole of Ba(OH)2.

4. Calculate the moles of HNO3:
Moles of HNO3 = Moles of Ba(OH)2 x (2 moles of HNO3 / 1 mole of Ba(OH)2)

5. Calculate the molarity of HNO3 by dividing the moles of HNO3 by the volume of the HNO3 solution in liters (15.0 mL = 0.015 L in this case):
Molarity of HNO3 = Moles of HNO3 / Volume of HNO3 solution (L)

By following these steps, you can find the molarity of the HNO3 solution.