After preparing the buffer, Joey decided to determine the buffer capacity of the solution by titration using 0.500 M NaOH as titrant. Given the data he obtained below, calculate the prepared buffer system's buffer capacity (B). Parameter Value/Measurement Volume of buffer, mL 75.0 Initial pH reading 7.10 Final pH reading 8.10 Final buret reading, mL 45.50 Initial buret reading, mL 33.80 A. ApH = B. AV NaOH (ML): = C. Moles of titrant = D. Buffer Capacity (B) =

After preparing the buffer, Joey decided to determine the buffer capacity of the solution by titration using 0.500 M NaOH as titrant. Given the data he obtained below, calculate the prepared buffer system's buffer capacity (B). Parameter Value/Measurement Volume of buffer, mL 75.0 Initial pH reading 7.10 Final pH reading 8.10 Final buret reading, mL 45.50 Initial buret reading, mL 33.80 A. ApH = B. AV NaOH (ML): = C. Moles of titrant = D. Buffer Capacity (B) =

Fundamentals Of Analytical Chemistry

9th Edition

ISBN:9781285640686

Author:Skoog

Publisher:Skoog

Chapter15: Complex Acid/base Systems

Section: Chapter Questions

Problem 15.26QAP

See similar textbooks

Similar questions

A buffer is prepared by dissolving 0.062 mol of sodium fluoride in 127 mL of 0.0399 M hydrofluoric acid. Assume no volume change after NaF is added. Calculate the pH of this buffer.
fter preparing the citrate buffer, Vegas and Pete determined the buffer capacity of the solution by titration using 0.25 M NaOH as titrant. Parameter Value Volume of citrate buffer, mL 50.0 Initial pH of citrate buffer 4.25 Final pH of citrate buffer 5.25 Final buret reading, mL 49.00 Initial buret reading, mL 35.50 Calculate the following. Show your complete solution. Moles of NaOH used Buffer capacity (β)
After preparing the citrate buffer, Vegas and Pete determined the buffer capacity of the solution by titration using 0.25 M NaOH as titrant. Parameter Value Volume of citrate buffer, mL 50.0 Initial pH of citrate buffer 4.25 Final pH of citrate buffer 5.25 Final buret reading, mL 49.00 Initial buret reading, mL 35.50 Calculate the following. Show your complete solution. ΔpH ΔVNaOH in mL
b) In the development of a method for the determination of formic acid by neutralization volumetry, the pH was calculated as a function of the addition of NaOH for the titration of 25.00 mL of 0.1280 mol/L formic acid with NaOH standardized with concentration of 0.0670 mol/L. With reference to this titration curve, determine the pH of the solution after the addition of 5.00 mL of titrant and at the equivalence point. Data: Ka=1.70x10-4. Present the results with two places after the comma and show your calculations. c) Based on the table below, indicate which indicators could be used to determine the end point of this titration.
If you would like to practice the Henderson-Hasselbalch calculations for the buffers in-lab exercise (attached) please use the following information for the buffer preparation: You are provided a 0.1M citric acid solution, a 0.1M sodium citrate solution and distilled water. You are to prepare a 50mL buffer at 25mM at a pH of 4.5. Citrate has three pKas at pH 3.128, 4.671, & 6.396.
A 250.0mg sample of an organic monoprotic weak acid was dissolved in an appropriate solvent and titrated with 0.091M NAOH , requiring 29.5ml to reach end point. Determine equivalent weight
Using the derived endpoints for both phosphoric acid titrations, calculate theconcentration of the phosphoric acid solution and report the mean value. Vol Mid Point 1st Derivative 3.96 0.089821268 5.91 0.229138878 7.105 0.257152358 8.345 0.562805368 9.025 1.958394009 9.175 4.406074475 9.215 10.52631579 9.27 5.043426253 9.355 4.129394633 9.415 7.738714375 9.465 2.260096883 9.505 13.04347826 9.605 1.258033788 9.8 0.85812357 10 0.845641773 10.25 0.636571666 10.65 0.415019763 11.2 0.31048471 11.95 0.277373275 12.925 0.270438943 13.875 0.273865319 14.55 0.391304348 15.025 0.421607378 15.425 0.567030224 15.7 0.934574579 15.9 0.898689411 16.05 1.831703765 16.125 4.911587269 16.175 4.137715831 16.25 3.061160807 16.325 7.932182234 16.375 6.403162055 16.45 3.070522155 16.55 1.981485334 16.675 1.751612232 16.875 0.8562513 17.075 1.352194716 17.375 0.427848277 17.85 0.434990639 18.475 0.249635948 19.275…
Which of the following statements is advantageous? A). The main differences between potentiometric and conductometric titrations are that potentiometric titrations exemplify the analyte sample-by-sample while conductometric titrations show the potential of the analyte B). A conductivity is analyl from the people of the charge. C.) Conductivity increases rapidly as close as equivalence, as a strong acid and a strong base will decrease D). The conductor remains constant according to the viscosity of the pixel, the decomposer and its size, which consists of design modelling.
10. 50 cm3 of 0.05 M weak acid solution is titrated with 0.1 M NaOH solution. The measured pH valuesare 7.345 and 7.497 at the consumptions of 6.0 and 6.1 cm3, respectively. What value of the buffer capacity can be calculated in the solution at pH = 7.421?11. Based on the data given in question 10, what is the total concentration of the anion of the weak acid atthe given point?
Sources of Error Determine the relationship between the observed/apparent value (EX) VERSUS that of the true value (ET) for the quantity being sought by writing either <, >, or = on the space provided TOPIC: Standardization of Titrant Question 7 Distilled water was not equilibrated to room temperature before the preparation of NaOH titrant. EX __ ET TOPIC: Determination of Molar Concentration of each component (Double Indicator Titration) Question 8 No blank correction Ex ___ ET Question 9 Bubbles trapped in the tip of burette: EX ___ ET Question 10 Measuring the sample volume using a volumetric pipet while looking downwards at the meniscus: EX ___ ET
A 0.4071-g sample of CaCO3 (MM: 100.09 g/mole) is transferred to a 500-mL volumetric flask, dissolved using a minimum of 6 M HCl, and diluted to volume. A 50.00-mL aliqout of this solution was mixed with 5 mL of a pH 10 NH3-NH4Cl buffer that contains a small amount of Mg2+--EDTA to adjust the pH to 10. After adding calmagite as an indicator, the solution is titrated with the EDTA, requiring 42.63 mL to reach the end point. Report the molar concentration of EDTA in the titrant. 9.543 x 10-3 M 5.748 x 10-3 M 3.266 x 10-4 M 1.018 x 10-4 M
Calculate the Molar Solubility and Ksp of Borax. I have included the data and some calculation that can help with solving, but I am unsure if the calculation I have provided are accurate Data: 1. Concentration of standardized HCl Solution (mol/L) = 0.1563M 2. volume of saturated borax (mL) = 5 mL 3. Buret reading, initial (mL) = 24.60 mL 4. Buret reading, final (mL) = 29.53 mL 5. Volume of HCl added (mL) = 4.93mL Calculations: 6. Amount of HCl added (mol) = 0.00077mol 7. Amount of OH- in saturated solution (mol) = 8. [OH-] equillirium (mol/L) = Molar solubility of borax=? Ksp of borax=?