The results of a titration experiment were as follows: Volume of aqueous NaOH pipetted into the conical flask = 10.00 mL Average volume of dilute HCI added from the burette to reach the endpoint = 12.54 mL Molarity of the dilute HCI = 1.196 M i)  Write the chemical reaction equation for the titration reaction  ii)  Calculate the number of moles of HCI added during the titration  iii)  What is the number of moles of NaOH that has reacted during the titration   iv)  What is the molarity of the aqueous NaOH

Questions: 1. Why does the tip of your buret need to be free of air bubbles? 2. Explain why the volume of water did not need to be exactly measured or recorded. 3. Define the endpoint of a titration. 4. What is a standard solution? Why is a standard solution necessary for titration? 5. A student starts a titration without phenolphthalein in the Erlenmeyer flask. The student realizes the mistake and adds the phenolphthalein during the titration. Once the phenolphthalein is added, the solution in the Erlenmeyer flask remains colorless. Can the results of this titration be used? Concisely explain. 6. Write a balanced equation for the neutralization of hydrobromic acid with potassium hydroxide. 7. What is the molarity of a 12.46 mL sulfuric acid solution if 18.22 mL of 0.100 M potassium hydroxide is required to reach the endpoint as indicated by a titration. 43

At the beginning of a titration, the acetic acid burette reads 0.30 mL. At the end of the titration. thé burette reads 27.70 mL. What volume had been added to the flask? Answer to two places past the decimal.

Please don't provide handwritten solution ......

Please type this, do not write it on a paper.

Would you be able to type out the precipitates? I can't see them clearly

The answer is not 4.8 x 10^-10 please find the correct answer. Thank you!

Match each term with its definition or description. 0000000 The point in a titration when the added amount of standard reagent is equal to the amount of analyte being titrated. A volumetric analysis technique used to determine the unknown concentration of a solution by using the known concentration of another. A solution of unknown concentration. The standard reagent of known concentration that is added from a buret to the analyte solution. A common concentration unit - moles per liter. The point in a titration when a change in the analyte solution is observed, indicating equivalency. It is added to the analyte solution and aids in the observation of the completion of the reaction. molarity equivalence point Answer Bank end point titration titrant analyte indicator

Calculate the molarity of an NaOH solution from the following titration data.  Be sure the answer has the correct amount of significant figures.  The chemical equation for this titration is as follows: NaOH  +  KHP  ⟶  NaKP  +  H2O NaOH buret reading, inital:  15.27 mL NaOH buret reading, final:     8.32 mL Mass of KHP (204.22 g/mol):  1.1592 g Calculate the molarity of an NaOH solution from the following titration data.  Be sure the answer has the correct amount of significant figures.  The chemical equation for this titration is as follows: NaOH  +  KHP  ⟶  NaKP  +  H2O NaOH buret reading, inital:  15.27 mL NaOH buret reading, final:     8.32 mL Mass of KHP (204.22 g/mol):  1.1592 g

While completing the titration required for the volumetric analysis, a student notices that a brown precipitate is forming. What does this mean?  In regards to the determination of chloride as silver chloride.