**Titration Calculations**1. **Calculation of Moles of NaOH Consumed** If a titration used 23.75 mL of a 0.100 M NaOH solution to reach the endpoint, then how many moles of NaOH were consumed?2. **Calculation of Moles of Ascorbic Acid** How many moles of ascorbic acid reacted from Q#2?3. **Calculation of Moles of KIO₃ Consumed** If a titration used 8.50 mL of a 0.0300 M KIO₃ solution to reach the endpoint, then how many moles of KIO₃ were consumed?- **Explanation:** For each calculation, use the molarity formula: \( \text{Moles} = \text{Volume (L)} \times \text{Molarity (M)} \) This relationship helps determine the number of moles of the titrant used in the titration process. - For NaOH: Given Volume \( = 23.75 \text{ mL} \) (convert to Liters: \( 23.75 \text{ mL} = 0.02375 \text{ L} \)) Given Molarity \( = 0.100 \text{ M} \) \[ \text{Moles of NaOH} = 0.02375 \text{ L} \times 0.100 \text{ M} = 0.002375 \text{ moles} \] - For ascorbic acid: This value typically is derived from a previous calculation or information provided in a preceding problem (Q#2). Assuming a 1:1 molar ratio in the reaction: \[ \text{Moles of Ascorbic Acid} = \text{Moles of NaOH} = 0.002375 \text{ moles} \] - For KIO₃: Given Volume \( = 8.50 \text{ mL} \) (convert to Liters: \( 8.50 \text{ mL} = 0.00850 \text{ L} \)) Given Molarity \( = 0.0300 \text{ M} \) \[ \text{Moles of

Here we have to determine the moles of NaOH taken and moles of asorbic acid reacts in

Answered: 18 If a titration used 23.75mL of a…

18 If a titration used 23.75mL of a 0.100M NaOH solution to reach the endpoint, then how many moles of NaOH were consumed? How many moles of ascorbic acid reacted from Q#2?

Chemistry: The Molecular Science

5th Edition

ISBN:9781285199047

Author:John W. Moore, Conrad L. Stanitski

Publisher:John W. Moore, Conrad L. Stanitski

Chapter15: Additional Aqueous Equilibria

Section: Chapter Questions

Problem 100QRT

See similar textbooks

Similar questions

San Pellegrino mineral water is 208 mg of calcium per liter according to the FDA. A. What is the calculated molarity of calcium for this drinking water? B. From the titration data below how does the student data compare with this actual value? San Pellegrino 25 mL water sample took net volume of 75 mL to turn from pink to blue (student had to fill buret more than once and add 2 net volumes together).
Calculate the grams of Acetic Acid ( M. W. 60.05g/ mole) in a unknown sample. A sample of Acetic Acid was titrated to the end point using 23.76M NaOH solution. The initial buret reading was 0.6559mL and the final reading was 0.02435mL.
b. Calculate the molar concentration of the malonic acid if 38.17 mL of 0.315 M potassium hy- Calculate the mass percent concentration of malonic acid using the molar concentration cal- droxide was required to neutralize 25.0 mL of malonic acid to a phenolphthalein end point. с. culated in part b and assuming the density of the solution is 1.01 g/ml. lo ba Citric acid (abbreviated H,Cit) is a triprotic acid, so 3 moles of hydroxide ions are required per mole of citric acid for complete neutralization. Write the balanced chemical equation for the reaction of citric acid with sodium hydroxide. (Note that citrate ion is actually a polyatomic ion with carbon, hydrogen, and oxygen atoms and an overall charge of -3. For now, express citrate ion as Cit.) a. ele booald sh w h Jf 36.10 mL of 0.223 M NaOH is used to neutralize a 0.515 g sample of citric acid, what is the molar mass of the acid?
Thank you! Data included in picture! No hand drawn graphs!! Determine the equivalence point of sudsy ammonia/citric acid reaction by graphing the titration data (pH vs volume citric acid) from Table 1: No Indicator Data Table. Draw a green arrow (use ‘Insert Shape’ feature to do this once you have copied your graph from Excel) on your graph indicating the data point that represents your equivalence point. Use a graphing software to create the x-y scatter plot showing the pH of the experimental solution as a function of the volume of citric acid (the titrant) added for the titration in Part 4. On your graph, the x-axis should be the volume of citric acid added (mL), and the y-axis should be the pH of the experimental solution at that volume. Do NOT connect your points; no trend line needed and make sure to: · Label the axes including the units in parentheses. · Include a figure legend (text below the graph) explaining the data in your graph that includes the arrow…
ACID-BASE TITRATION PRELA BOUESTIONS NAME NaOH according to the following equation HC,H O2 NAOH NACH O2 НОН acid. WELBL0 2. Calculate the grams of acetic acid in one liter of the vinegar. 52.5g S. The 4.00 mL sample of vinegar had a mass of 4.056 g. Calculate the grams of vinegar in one liter. 3. 4. Calculate the % acetic acid in the vinegar. g acetic acid x 100 g vinegar % acetic acid || 95
The flask contains 10.0 mL of HCl and a few drops of phenolphthalein indicator. The buret contains 0.140 M NAOH. It requires 16.4 mL of the NAOH solution to reach the end point of the titration. What is the initial concentration of HCl? concentration: M HCI about us careers privacy policy terms of use contact us help docx DII F5 PrtScn 8 Home F9 End F10 PgUp F11 F4 F6 F7
To determine the m/m% of CaCO3 in limestone, 0.5 g sample of limestone was crushed and reacted with 23.5 ml of 0.6M HCI. The excess of acid was titrated with 22.5 ml of 0.45M NaOH. Calculate: a. Total number of moles of HCI added = b. Number of moles of CaCO3 in the sample = c. m/m% of CaCO3 in the sample= % mol mol
Cs Scanned with CamScanner 7.0 QUESTIONS 1. Calculate the molarity of a NaOH solution if 32.02 mL of the solution neutralizes 0.2262 g of oxalic acid dihydrate. 2. Predict whether the calculated molarity of the NaOH solution will be too high or too low if a student 'overshoots' the end point of titration. Give the reason to your answer.
Calculate the mass of acetic acid in 100ml of both samples in vinegar. given: NaOH vs CH3COOH Burette solution is NaOH and the pipette solution is 5.0 mL of Vinegar Titration Initial burette reading Final burette reading Volume of NaOH consumed Average volume of NaOH Approximate 0.0 mL 20.1 mL 20.1 mL 20.3 mL Titration 1 0.0 mL 20.9 mL 20.9 mL Titration 2 0.0 mL 20.0 mL 20.0 mL To find the average volume Average volume = 20.1 mL + 20.9 mL + 20.0 mL320.1 mL + 20.9 mL + 20.0 mL3 = 20.3 mL Concentration of Vinegar = Volume of NaOH * Concentration of NaOHVolume of vinegarVolume of NaOH * Concentration of NaOHVolume of vinegar = 20.3 mL * 0.0647 M5.0 mL20.3 mL * 0.0647 M5.0 mL = 0.2627 M Concentration of NaOH = Volume of H2SO4 * Concentration of H2SO4Volume of NaOHVolume of H2SO4 * Concentration of H2SO4Volume of NaOH = 10.0 mL…
Questions: 1. Write a balanced equation for the titration of NaOH with: a. Citric acid (acid in candy) b. Lactic acid (acid in milk) 2. Which sample did you expect to have more acid (candy or milk) and why? Does your experiment agree with your expectation? 3. How would having a large air bubble in the buret tip at the start of the experiment affect the calculated value of g acid/g of sample?
In the experiment, the amount of acetic acid in vinegar was determined by titrating with 0.1 M NaOH solution. In the analysis, three trials were performed to obtain more precise result. The table shows the initial and final burette readings for three titrations: Initial Burette Reading (mL) Final Burette Reading (mL) Trial 1 2.9 10.6 Trial 2 10.6 18.1 Trial 3 18.1 25.7 According to the given data, calculate molarity of acetic acid in the commercial vinegar. Please be sure that your answer includes followings; a) moles of NaOH for each trial b) average mole of NaOH c) average mole of acetic acid in 50 mL solution d) average mole of acetic acid in 250 mL solution e) molarity of acetic acid in vinegar.
Acid Base Titrations Given the information below, calculate the acid concentration: show work and use correct number of significant figures Unknown acid ID#: ____HCl_____(concentration unknown) Concentration of NaOH: 0.10 M Initial Buret reading (mL) : 4.0 Final Buret reading (mL): 14.2 Volume of NaOH added (mL): 10.2 Calculated acid concentration (M): ???