Determining the volume of base needed to titrate a given mass of acid. A chemistry student weighs out 0.420 g of citric acid (H,C,H,0,), a triprotic acid, into a 250. mL volumetric flask and dilutes to the mark withdistilled water. He plans to titrate the acid with 0.1500M NaOH solution.Calculate the volume of NaOH solution the student will need to add to reach the final equivalence point. Be sure your answer has the correctnumber of significant digits.|mLx10

The quantitative analysis for determining the concentration of an acid or base by neutralizing it…

Answered: A chemistry student weighs out 0.420 g…

Fundamentals Of Analytical Chemistry

9th Edition

ISBN:9781285640686

Author:Skoog

Publisher:Skoog

Chapter16: Applications Of Neutralization Titrations

Section: Chapter Questions

Problem 16.20QAP

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The pH of a saturated soloution of magnesium hydroxide, Mg(OH)2, (milk of magnesia) was found to be (1.080x10^1). From this, find the Ksp for magnesium hydroxide. Express your answer to three significant figures. Note: Your answer is assumed to be reduced to the highest power possible.
please calculate the neutralization equivalent for each run for part II. and for part III, calculate the neutralization equivalent for malonic acid and maleic acid
Following titration analysis, a sample of a fruit juice was found to contain 8.9 mg cm-3 ascorbic acid. Given that the Mr value for ascorbic acid is 176.1 Da, calculate the value of the ascorbic acid concentration expressed in units of mmols dm-3 then enter it
The pH of a saturated soloution of calcium hydroxide, Ca(OH)2, (lime water) was found to be (1.241x10^1). From this, find the Ksp for calcium hydroxide. Express your answer to three significant figures. Note: Your answer is assumed to be reduced to the highest power possible.
Students Mola and Rity were tasked to analyze the acidity of a 10.0-mL fermented milk sample diluted with water in a 250-mL volumetric flask. Mola obtained a 15.0-mL aliquot of this solution, diluted it to 50.0 mL, and then titrated this diluted sample. Titration data were given to Rity and she found out that the 50.0-mL diluted sample contains 0.21 mmol of lactic acid. MW: Lactic Acid (90.08) a. What is the lactic acid concentration (in M) of the titrated sample? b. Determine the lactic acid content (in M) of the 10.0-mL fermented milk sample. c. What is the lactic acid concentration (in %w/v) of the 10.0-mL fermented milk sample?
A commercial vinegar was analyzed by titration to determine the percent acetic acid. Briefly, 10.00 mL of vinegar sample was diluted to 100. mL solution in a volumetric flask. A 25.00 mL aliquot from the diluted vinegar required 25.55 mL of 0.1005 M sodium hydroxide to reach the phenolphthalein endpoint From this experiment which is the standard solution used in titration? CH3COOH NaOH NaCH3COO C20H14O4
A student delivers several drops of titrant from their buret, but the drops land on the side of the Erlenmeyer flask. The student ultimately finishes the titration and the drops are still on the side of the flask. How is the % acetic in their determination affected by this error? Briefly, 1 - 2 sentences,
In a Complexometric Titration Experiment, the preparation of the EDTA solution is as follows: In a 250 mL beaker, weigh 0.10 g MgCl2*6H2O and 1.0 g NaOH. Add approximately 200 mL distilled water and stir to dissolve. Add about 2.0 g of EDTA and transfer the solution quantitatively to a 1-L volumetric flask. Dilute to the mark with distilled water. What is the purpose of adding MgCl2*6H2O? Please show COMPLETE solution.
Determine the Concentration of Ethanoic Acid in Vinegar Equipment / Apparatus:  250-mL conical flasks  Clamp  Burette  Graduated cylinder  Pipette Reagents / Materials:  Vinegar  Phenolphthalein indicator  0.2 M NaOH (standardized) Calculation: Molarity (M) of ethanoic acid  The average measured volume of the NaOH from titration: Average volume of NaOH used = (21.5ml + 21.5ml + 21.6ml) / 3 =21.5ml No of mole of NaOH = Concentration of NaOH (0.2M) × Average volume of NaOH used When an acid is completely neutralized: No of moles of CH3COOH = No of moles of NaOH Using the moles of CH3COOH, the molarity of ethanoic acid in the 5.0-mL sample of vinegar is calculated: Molarity (M) CH3COOH = moles CH3COOH / volume of vinegar (0.005 dm3). Calculation: Mass / Volume Percent (m/v) of ethanoic acid To calculate the percent (m/v) of CH3COOH in vinegar, we convert the moles of ethanoic acid to grams using the molar mass of ethanoic acid, 60.1 g/mole. Mass of CH3COOH =…
1. What would you observe in procedural step 2 under flowcharts if 6M HNO3 were used in place of 6M HCL?
Bay Water Titration The concentration of Cl- in ocean water is about 500-600 mM. The baywater is diluted by a factor of 12.5 using a 20.00 mL volumetric pipet and a 250 mL volumetric flask. Using a 15.00 mL volumetric pipet, 15.00 mL is transferred into three clean Erlenmeyer flasks. 10 mL of 1% dextrin solution, 20 mL of de-ionized water, and 3-4 drops of indicator are added and titrated each with the AgNO3 solution. From the procedure, find: Dilution factor Volume of diluted bay water Then calculate: The [Cl-] of diluted bay water The [Cl-] of bay water Consider this information: [AgNO3] = 0.04043177 trial # Veq 1 13.91 2 13.73 3 13.9 4 13.86 5 13.87 6 13.84 average 13.85167 [Cl-]Bay = ([AgNO3](Veq(ave))/Vdil bay water pipeted) (Vflask/Vbay water)
If the test tube used in the determination of the ΔHrxn for nitric acid (neutralization with NaOH) was still wet with water, will the magnitude of ΔHrxn increase, decrease, or remain the same?Please explain.

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