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A student titrates 50mL apple juice and reports the following in the titration to the phenolphthalein end point with .1011M NaOH

final buret reading:17.86mL
initial buret reading:1.47

A)What is the concentration of the total available acid in moles/L of the apple juice?
B)A drop is .05mL, what will be the percent error if the final reading is 2 drops past the actual endpoint?
C)What is the percent error in the result if the volume of the juice titrated was actually 51mL?
D)If the pH of the pure apple juice is 4.0, what is the Ka of the acid?

Do you have some idea about how to do some of this?

A. moles NaOH used = M x L.
moles acid = same as moles NaOH.
Then moles/L = moles acid/0.05.

B. The easiest way to do this is to add 0.1 mL to the volume and recalculate the molarity of the apple juice.
%error = [(experimental value-actual value)/actual value]*100.
Use the value from A as the actual value and the revised answer from B as the experimental value.

C.same procedure

To solve these questions, we need to follow the given data and perform calculations based on the principles of titrations and acid-base reactions. Let's break down each question step by step:

A) What is the concentration of the total available acid in moles/L of the apple juice?

To find the concentration of the total available acid in moles/L of the apple juice, we need to use the titration data and the equation of the reaction between the acid in apple juice and NaOH.

The balanced equation for the reaction is:

Acid (in apple juice) + NaOH → Salt + Water

From the titration data, we can calculate the moles of NaOH used:

Moles of NaOH = concentration (M) × volume (L)

The volume can be found by subtracting the initial buret reading from the final buret reading:

Volume of NaOH = Final buret reading - Initial buret reading

Now we can calculate the concentration of the acid in the apple juice:

Concentration of the acid = Moles of NaOH / Volume of apple juice (in liters)

Given the volume of apple juice is 50 mL (0.050 L), the concentration of the total available acid can be calculated.

B) A drop is 0.05 mL, what will be the percent error if the final reading is 2 drops past the actual endpoint?

To calculate the percent error, we need to compare the difference between the actual final reading and the recorded final reading, divided by the actual final reading, and multiplied by 100.

Percent error = ((Actual final reading - Recorded final reading) / Actual final reading) × 100

Given that one drop is 0.05 mL and the final reading is 2 drops past the actual endpoint, we can calculate the percent error.

C) What is the percent error in the result if the volume of the juice titrated was actually 51 mL?

To calculate the percent error for the volume, we need to compare the difference between the actual volume and the recorded volume, divided by the actual volume, and multiplied by 100.

Percent error = ((Actual volume - Recorded volume) / Actual volume) × 100

Given that the actual volume is 51 mL, we can calculate the percent error.

D) If the pH of the pure apple juice is 4.0, what is the Ka of the acid?

The pH of a solution is related to the concentration of H+ ions, which in turn depends on the concentration of the acid and its dissociation constant (Ka).

To find the Ka of the acid, we need to use the pH value and the equation for the dissociation of the acid:

Acid (in apple juice) ↔ H+ + Conjugate base

The Ka expression for this equilibrium is:

Ka = [H+][Conjugate base] / [Acid]

Given that the pH of pure apple juice is 4.0, we can calculate the concentration of H+ ions using the pH equation:

[H+] = 10^(-pH)

Now we can substitute the known values into the Ka expression to calculate the Ka of the acid in apple juice.

Follow these steps, and you'll be able to find the answers to each question. If you need further assistance with the calculations, let me know!