How do I calculate the Molarity of NaOH(aq) for trail 1 ### Mass of KHP: | KHP Trial | Mass (g) | Final Buret (mL) | Initial Buret (mL) | Volume of NaOH Used (mL) ||-----------|-----------|-----------------|-------------------|--------------------------|| KHP 1 | 0.3130 g | 16.72 mL | 1.20 mL | (16.72 - 1.20) = 15.52 mL || KHP 2 | 0.3046 g | 31.80 mL | - | || KHP 3 | 0.3059 g | 15.3 mL | 0.00 mL | (15.3 - 0.00) = 15.3 mL |#### Additional Information:- **Molarity of NaOH Solution:** Not specified in the notes.- **Average NaOH Concentration Added:** 0.0988 M### Explanation:In this experiment, potassium hydrogen phthalate (KHP) is used to determine the concentration of a sodium hydroxide (NaOH) solution through titration. Three trials are conducted with varying masses and volumes to ensure accuracy. Each trial reflects the mass of KHP used, as well as initial and final readings from a buret used to measure the NaOH solution. The volume of NaOH used in each trial is the difference between the final and initial buret readings. The average concentration of NaOH calculated from these trials is given as 0.0988 M.This exercise demonstrates the titration process in a laboratory setting and provides insight into how to calculate solution concentrations accurately.

For trial 1 Mass of KHP = 0.3130 g Molar mass(MM) KHP = 204.2 g Moles of KHP = mass/MM =…

Answered: KHP I Trud 0.3130 9 16.72mL

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Chemistry

KHP I Trud 0.3130 9 16.72mL

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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Question

How do I calculate the Molarity of NaOH(aq) for trail 1

### Mass of KHP:

| KHP Trial | Mass (g) | Final Buret (mL) | Initial Buret (mL) | Volume of NaOH Used (mL) |
|-----------|-----------|-----------------|-------------------|--------------------------|
| KHP 1 | 0.3130 g | 16.72 mL | 1.20 mL | (16.72 - 1.20) = 15.52 mL |
| KHP 2 | 0.3046 g | 31.80 mL | - | |
| KHP 3 | 0.3059 g | 15.3 mL | 0.00 mL | (15.3 - 0.00) = 15.3 mL |

#### Additional Information:
- **Molarity of NaOH Solution:** Not specified in the notes.
- **Average NaOH Concentration Added:** 0.0988 M

### Explanation:
In this experiment, potassium hydrogen phthalate (KHP) is used to determine the concentration of a sodium hydroxide (NaOH) solution through titration. Three trials are conducted with varying masses and volumes to ensure accuracy. Each trial reflects the mass of KHP used, as well as initial and final readings from a buret used to measure the NaOH solution.

The volume of NaOH used in each trial is the difference between the final and initial buret readings. The average concentration of NaOH calculated from these trials is given as 0.0988 M.

This exercise demonstrates the titration process in a laboratory setting and provides insight into how to calculate solution concentrations accurately.

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