What is the molarity of an NaOH solution if 4.37 mL is titrated by 11.1 mL of 0.0904 M HNO3?

What is the molarity of an NaOH solution if 4.37 mL is titrated by 11.1 mL of 0.0904 M HNO3?

• A. 0.230 M
• B. 0.460 M
• C. 0.355 M
• D. 0.620 M

Answer: (A)

To find the molarity of the NaOH solution, we can apply the principles of titration, in which the moles of titrant (in this case, HNO3) will equal the moles of the analyte (NaOH) at the equivalence point. The balanced chemical equation for the reaction between NaOH and HNO3 is: \[ NaOH + HNO_3 \rightarrow NaNO_3 + H_2O \] This indicates a 1:1 molar ratio between NaOH and HNO3. First, we calculate the moles of HNO3 used in the titration: 1. **Determine the moles of HNO3:** - Molarity (M) = moles of solute / volume of solution in liters - Convert 11.1 mL to liters: \( 11.1 \, \text{mL} = 0.0111 \, \text{L} \) - Calculate moles of HNO3: \[ \text{Moles of HNO3} = 0.0904 \, \text{M} \times 0.0111 \, \text{

To find the molarity of the NaOH solution, we can apply the principles of titration, in which the moles of titrant (in this case, HNO3) will equal the moles of the analyte (NaOH) at the equivalence point. The balanced chemical equation for the reaction between NaOH and HNO3 is:

[ NaOH + HNO_3 \rightarrow NaNO_3 + H_2O ]

This indicates a 1:1 molar ratio between NaOH and HNO3.

First, we calculate the moles of HNO3 used in the titration:

1. Determine the moles of HNO3:

• Molarity (M) = moles of solute / volume of solution in liters

• Convert 11.1 mL to liters: ( 11.1 , \text{mL} = 0.0111 , \text{L} )

• Calculate moles of HNO3:

[ \text{Moles of HNO3} = 0.0904 , \text{M} \times 0.0111 , \text{