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6. Error analysis. If the NaOH solution (titrant) was not standardized with KHP, how would this...
Titration of acetic acid. 4. What is the advantage of doing three trials, especially since you...
Titration of acetic acid.
4. What is the advantage of doing three trials, especially since you are doing exactly time? What does your standard deviation tell you about the precision of your results'? is, especially since you are doing exactly the same thing each 5. Error analysis. Suppose during the titration you added NaOH sufficient to change the indicator to a much darker pink color. How would this affect your experimental result? Would this increase of decrease your experimental acetic...
Titration of acetic acid . Error analysis. Suppose during the titration vou added NaOH sufficient to...
Titration of acetic acid
. Error analysis. Suppose during the titration vou added NaOH sufficient to change the indicator to a much darker pink color. How would this affect your experimental result? Would this increase or decrease your experimental acetic acid content? Explain.
1. A solution of sodium hydroxide (NaOH) was standardized against potassium hydrogen phthalate (KHP). A known...
1. A solution of sodium hydroxide (NaOH) was standardized against potassium hydrogen phthalate (KHP). A known mass of KHP was titrated with the NaOH solution until a light pink color appeared using phenolpthalein indicator. Using the volume of NaOH required to neutralize KHP and the number of moles of KHP titrated, the concentration of the NaOH solution was calculated. Molecular formula of Potassium hydrogen phthalate: HKC8H404 Mass of KHP used for standardization (g) 0.5100 Volume of NaOH required to neutralize...
A solution of NaOH is standardized with potassium acid phthalate (KHP), KHC8H8O4, molar mass = 204...
A solution of NaOH is standardized with potassium acid phthalate (KHP), KHC8H8O4, molar mass = 204 g/mol. If 2.550 g of KHP is titrated with 54.50 mL of the NaOH solution, what is the molarity of NaOH?
please show me how to answer this 9. A solution of NaOH is standardized with potassium...
please show me how to answer this
9. A solution of NaOH is standardized with potassium acid phthalate (KHP), KHC,H,O, molar mass = 204 g/mol. If 2.550 g of KHP is titrated with 54.50 mL of the NaOH solution, what is the molarity of NaOH?
Question 9 Status: Incomplete answer Points possible: 1.00 Before using a solution of NaOH as titrant...
Question 9 Status: Incomplete answer Points possible: 1.00 Before using a solution of NaOH as titrant in a titration experiment, you should standardize the solution. Standardization is the process of titrating a solution prepared from a carefully measured mass of solid accurately determine the concentration of the titrant. In particular, NaOH solutions need to be standardized because their concentrations depend on color due to the compound's Choose... Please put an answer in each box Suppose you are given solutions of...
1. How many grams of pure, solid NaOH are required to make 400 mL of 0.1M NaOH solution? 2. How many grams of a sol...
1. How many grams of pure, solid NaOH are required to make 400 mL of 0.1M NaOH solution? 2. How many grams of a solution that is 50% by weight NaOH is required to make 400 mL of 0.1M NaOH solution? 3. The density of a 50% solution of NaOH is 1.525 g/mL. What volume of a solution that is 50% by weight NaOH is required to make 300 mL of 0.1M NaOH solution? 4. Why does weighing by difference...
The titrant solution is on the last page. All the info needed is on the pages provided. paticularly on t...
The
titrant solution is on the last page.
All
the info needed is on the pages provided. paticularly on the last
page
Table 1: Standardization Data Trial 3 Trial 1 Trial 2 O.47644 0.4701 25. mL ou779 12.7mL 25. mL 12.4 mL Mass of KHP Initial burette reading 2.7mL 37,Sm 2.4m Final burette reading 12.7mL Volume of base used Data Analysis: 1. Write a balanced molecular equation (with phases, of course) for the reaction between the KHP and the titrant...
If the titrand in this exercise was sodium hydroxide and the titrant a standardized solution of...
If the titrand in this exercise was sodium hydroxide and the titrant a standardized solution of vinegar, how would the end point of the titration be determined when using phenolphthalein as the indicator? Be specific in your answer
Answer both questions please Suppose a sodium hydroxide solution is to be standardized against pure, solid, primary-...
Answer both questions please
Suppose a sodium hydroxide solution is to be standardized against pure, solid, primary-standard grade KHP. If 0.4538 g of KHP requires 44.12 mL of the sodium hydroxide solution to reach a phenolphthalein endpoint, what is the molarity of the NaOH solution? Show your calculations. 5. If 36.32 mL of the NaOH solution described in question 4 was required to titrate a 5.00 mL sample of vinegar, calculate the molarity of acetic acid in the vinegar. Show...
Titration of acetic acid.
4. What is the advantage of doing three trials, especially since you are doing exactly time? What does your standard deviation tell you about the precision of your results'? is, especially since you are doing exactly the same thing each 5. Error analysis. Suppose during the titration you added NaOH sufficient to change the indicator to a much darker pink color. How would this affect your experimental result? Would this increase of decrease your experimental acetic...
Titration of acetic acid
. Error analysis. Suppose during the titration vou added NaOH sufficient to change the indicator to a much darker pink color. How would this affect your experimental result? Would this increase or decrease your experimental acetic acid content? Explain.
1. A solution of sodium hydroxide (NaOH) was standardized against potassium hydrogen phthalate (KHP). A known mass of KHP was titrated with the NaOH solution until a light pink color appeared using phenolpthalein indicator. Using the volume of NaOH required to neutralize KHP and the number of moles of KHP titrated, the concentration of the NaOH solution was calculated. Molecular formula of Potassium hydrogen phthalate: HKC8H404 Mass of KHP used for standardization (g) 0.5100 Volume of NaOH required to neutralize...
please show me how to answer this
9. A solution of NaOH is standardized with potassium acid phthalate (KHP), KHC,H,O, molar mass = 204 g/mol. If 2.550 g of KHP is titrated with 54.50 mL of the NaOH solution, what is the molarity of NaOH?
Question 9 Status: Incomplete answer Points possible: 1.00 Before using a solution of NaOH as titrant in a titration experiment, you should standardize the solution. Standardization is the process of titrating a solution prepared from a carefully measured mass of solid accurately determine the concentration of the titrant. In particular, NaOH solutions need to be standardized because their concentrations depend on color due to the compound's Choose... Please put an answer in each box Suppose you are given solutions of...
1. How many grams of pure, solid NaOH are required to make 400 mL of 0.1M NaOH solution? 2. How many grams of a solution that is 50% by weight NaOH is required to make 400 mL of 0.1M NaOH solution? 3. The density of a 50% solution of NaOH is 1.525 g/mL. What volume of a solution that is 50% by weight NaOH is required to make 300 mL of 0.1M NaOH solution? 4. Why does weighing by difference...
The
titrant solution is on the last page.
All
the info needed is on the pages provided. paticularly on the last
page
Table 1: Standardization Data Trial 3 Trial 1 Trial 2 O.47644 0.4701 25. mL ou779 12.7mL 25. mL 12.4 mL Mass of KHP Initial burette reading 2.7mL 37,Sm 2.4m Final burette reading 12.7mL Volume of base used Data Analysis: 1. Write a balanced molecular equation (with phases, of course) for the reaction between the KHP and the titrant...
Answer both questions please
Suppose a sodium hydroxide solution is to be standardized against pure, solid, primary-standard grade KHP. If 0.4538 g of KHP requires 44.12 mL of the sodium hydroxide solution to reach a phenolphthalein endpoint, what is the molarity of the NaOH solution? Show your calculations. 5. If 36.32 mL of the NaOH solution described in question 4 was required to titrate a 5.00 mL sample of vinegar, calculate the molarity of acetic acid in the vinegar. Show...
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