How do I find the mass of KHP?

0.5050 grams of KHP was used and placed into a 250mL volumetric flask and diluted to the mark with distilled water. 50.00mL of this KHP solution was placed in a 250mL beaker. It took 14.75mL of 0.0067M of NaOH to reach the endpoint. What is the mass of the sample? What is the wt%?

You have the mass of the KHP sample. You weighed out 0.5050 g (of course you've diluted it; perhaps that is the question; i.e., what is the mass of the KHP in the titrated sample? :-).

How many moles NaOH did you use? M x L = moles = 0.0067M x 0.01475 = 9.88E-5 moles
NaOH. Since KHP has one H and NaOH has 1 OH, moles NaOH = moles KHP; therefore, moles KHP = 9.88E-5.
grams KHP = 9.88E-5 moles x molar mass KHP = ? grams KHP in the titrated sample. Convert that to grams in the original sample. That will be
?g titrated sample x (250/50) = x grams KHP in the original 0.5050 g sample.
%mass KHP = (x g in sample/0.5050)*100 = ??
Most don't work the problem as I did. Most do it this way.
mass KHP in the titrated sample = 0.5050 x (50/250) = 0.1010 g.
%KHP = (g titrated/0.1010)*100 =

To find the mass of KHP (potassium hydrogen phthalate), you need to follow the given information and do some calculations.

1. Calculate the number of moles of NaOH used:
Molarity (M) = moles/volume (L)
Given: Molarity (NaOH) = 0.0067 M
Volume (NaOH) = 14.75 mL = 0.01475 L

Moles (NaOH) = Molarity (NaOH) * Volume (NaOH)
= 0.0067 M * 0.01475 L

2. Use the balanced chemical equation to relate moles of NaOH to moles of KHP. From the equation:
NaOH + KHP → H2O + NaKP

The stoichiometric ratio of NaOH to KHP is 1:1.

Moles (KHP) = Moles (NaOH)

3. Calculate the mass of KHP:
Molar mass (KHP) = 204.22 g/mol (you can refer to the periodic table)

Mass (KHP) = Moles (KHP) * Molar mass (KHP)

The mass of the sample is the mass of KHP used to make the solution.

4. Calculate the weight percent (wt%):
Weight percent (wt%) = (Mass (KHP) / Mass of solution) * 100

The mass of the solution is the sum of the mass of KHP and the mass of water used to dilute it.

Mass of solution = Mass (KHP) + Mass of water

Now let's perform the calculations.

1. Moles (NaOH) = 0.0067 M * 0.01475 L
[Calculate moles of NaOH used]

2. Moles (KHP) = Moles (NaOH)
[Since the stoichiometric ratio of NaOH to KHP is 1:1]

3. Mass (KHP) = Moles (KHP) * Molar mass (KHP)
[Multiplying moles of KHP with its molar mass]

4. Mass of solution = Mass (KHP) + Mass of water
[Adding the mass of KHP and mass of water used]

5. Weight percent (wt%) = (Mass (KHP) / Mass of solution) * 100
[Calculating the weight percent]

By following these steps and performing the calculations, you will find the mass of the sample and the weight percent of KHP.