What is the molarity of a NaOH solution if 28.50 mL are needed to titrated a 0.7154 g sample of KHP?
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To find the molarity of the NaOH solution, we first need to determine the number of moles of KHP (potassium hydrogen phthalate) using its molar mass and the given mass of the sample.

Calculate the number of moles of KHP: [ \text{moles of KHP} = \frac{\text{mass of KHP}}{\text{molar mass of KHP}} ]

Use the balanced chemical equation between KHP and NaOH to relate the number of moles of KHP to the number of moles of NaOH.

Once we know the number of moles of NaOH, we can find the molarity of the NaOH solution using the volume of NaOH used in the titration.
Given:
 Mass of KHP = 0.7154 g
 Volume of NaOH used = 28.50 mL
First, we find the molar mass of KHP: [ \text{Molar mass of KHP} = 204.22 , \text{g/mol} ]
Now, we calculate the number of moles of KHP: [ \text{moles of KHP} = \frac{0.7154 , \text{g}}{204.22 , \text{g/mol}} ] [ \text{moles of KHP} ≈ 0.003502 , \text{mol} ]
From the balanced chemical equation between KHP and NaOH: [ \text{1 mol KHP} \rightarrow \text{1 mol NaOH} ]
Thus, the number of moles of NaOH is also approximately 0.003502 mol.
Now, we calculate the molarity of the NaOH solution: [ \text{Molarity (M) of NaOH} = \frac{\text{moles of NaOH}}{\text{volume of NaOH (in liters)}} ]
Converting the volume of NaOH from milliliters to liters: [ \text{Volume of NaOH} = \frac{28.50 , \text{mL}}{1000 , \text{mL/L}} = 0.02850 , \text{L} ]
[ \text{Molarity (M) of NaOH} = \frac{0.003502 , \text{mol}}{0.02850 , \text{L}} ] [ \text{Molarity (M) of NaOH} ≈ 0.1229 , \text{M} ]
Therefore, the molarity of the NaOH solution is approximately 0.1229 M.
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