A 0.391 g sample of KHP will be titrated with a NaOH solution with an assumed concentration of 0.100 M. Calculate the volume of NaOH that should neutralize the KHP sample.
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To calculate the volume of NaOH solution that will neutralize the KHP sample, we need to use stoichiometry and the equation of the reaction between KHP (potassium hydrogen phthalate) and NaOH (sodium hydroxide).
The balanced chemical equation for the reaction is:
KHP + NaOH → NaKP + H2O
From the equation, we can see that the molar ratio between KHP and NaOH is 1:1. This means that 1 mole of KHP reacts with 1 mole of NaOH.
First, let's calculate the number of moles of KHP in the 0.391 g sample. To do this, we need to know the molar mass of KHP. The molar mass of KHP is 204.23 g/mol.
Number of moles of KHP = Mass of KHP / Molar mass of KHP
= 0.391 g / 204.23 g/mol
Next, we need to calculate the volume of NaOH solution using the molar ratio from the balanced equation and the known concentration of the NaOH solution.
Number of moles of NaOH = Number of moles of KHP (since the molar ratio is 1:1)
= 0.391 g / 204.23 g/mol
Volume of NaOH solution = Number of moles of NaOH / Concentration of NaOH
= (0.391 g / 204.23 g/mol) / 0.100 mol/L
Finally, we can calculate the volume of NaOH solution that should neutralize the KHP sample by substituting the values into the equation:
Volume of NaOH solution = (0.391 g / 204.23 g/mol) / 0.100 mol/L
Calculating this expression will give you the volume of NaOH solution in liters (L).
To calculate the volume of NaOH that should neutralize the KHP sample, you need to determine the moles of KHP and NaOH involved in the reaction.
Step 1: Convert the mass of KHP to moles.
The molar mass of KHP (potassium hydrogen phthalate) is 204.22 g/mol.
You have a mass of 0.391 g, so divide this by the molar mass to get moles:
0.391 g / 204.22 g/mol = 0.001914 mol of KHP
Step 2: Use the balanced chemical equation to determine the stoichiometry between KHP and NaOH.
The balanced equation for the reaction between KHP and NaOH is:
KHC8H4O4 + NaOH → NaKC8H4O4 + H2O
From the balanced equation, you can see that 1 mole of KHP reacts with 1 mole of NaOH.
Step 3: Determine the moles of NaOH required.
Since 1 mole of KHP reacts with 1 mole of NaOH, the moles of NaOH required to neutralize the KHP sample is also 0.001914 mol.
Step 4: Use the molarity of NaOH to calculate the volume.
The molarity (M) is defined as moles per liter (mol/L). In this case, the concentration of NaOH is given as 0.100 M.
Molarity = moles of solute / volume of solution in liters
0.100 M = 0.001914 mol / volume of NaOH in liters
Rearrange the equation to solve for the volume of NaOH:
Volume of NaOH = moles of NaOH / Molarity of NaOH
Volume of NaOH = 0.001914 mol / 0.100 mol/L
Volume of NaOH = 0.01914 L or 19.14 mL
Therefore, the volume of NaOH that should neutralize the KHP sample is approximately 19.14 mL.