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Chapter 13: Problem 29

Holman, Christian, and Ruzicka described an FIA method to determine the concentration of \(\mathrm{H}_{2} \mathrm{SO}_{4}\) in nonaqueous solvents. \({ }^{28}\) Agarose beads \((22-45 \mu \mathrm{m}\) diameter \()\) with a bonded acid- base indicator are soaked in \(\mathrm{NaOH}\) and immobilized in the detector's flow cell. Samples of \(\mathrm{H}_{2} \mathrm{SO}_{4}\) in \(n\) -butanol are injected into the carrier stream. As a sample passes through the flow cell, an acid-base reaction takes place between \(\mathrm{H}_{2} \mathrm{SO}_{4}\) and \(\mathrm{NaOH}\). The endpoint of the neutralization reaction is signaled by a change in the bound indicator's color and is detected spectrophotometrically. The elution volume needed to reach the titration's endpoint is inversely proportional to the concentration of \(\mathrm{H}_{2} \mathrm{SO}_{4} ;\) thus, a plot of endpoint volume versus \(\left[\mathrm{H}_{2} \mathrm{SO}_{4}\right]^{-1}\) is linear. The following data is typical of that obtained using a set of external standards. $$ \begin{array}{cc} {\left[\mathrm{H}_{2} \mathrm{SO}_{4}\right](\mathrm{mM})} & \text { end point volume }(\mathrm{mL}) \\ \hline 0.358 & 0.266 \\ 0.436 & 0.227 \\ 0.560 & 0.176 \\ 0.752 & 0.136 \\ 1.38 & 0.075 \\ 2.98 & 0.037 \\ 5.62 & 0.017 \end{array} $$ What is the concentration of \(\mathrm{H}_{2} \mathrm{SO}_{4}\) in a sample if its endpoint volume is \(0.157 \mathrm{~mL}\) ?

Short Answer

Expert verified
Use linear regression to determine the concentration of \(\mathrm{H}_2\mathrm{SO}_4\) from the given endpoint volume by solving the linear equation for \(\frac{1}{[ ext{H}_2 ext{SO}_4]}\).

Step by step solution

01

Understanding the Relationship

The problem states that the endpoint volume is inversely proportional to the concentration of \( \mathrm{H}_2 \mathrm{SO}_4 \). Mathematically, this means we are looking for a linear relationship between the endpoint volume \( V \) and \( [\mathrm{H}_{2} \mathrm{SO}_{4}]^{-1} \). This relationship can be represented as \( V = a \cdot \frac{1}{[\mathrm{H}_{2} \mathrm{SO}_{4}]} + b \) for some constants \( a \) and \( b \).
02

Calculating \( \frac{1}{[\mathrm{H}_{2} \mathrm{SO}_{4}]} \) for Standards

For each standard concentration, calculate \( \frac{1}{[\mathrm{H}_{2} \mathrm{SO}_{4}]} \) to determine the independent variable for our linear plot. - For \( [\mathrm{H}_{2} \mathrm{SO}_{4}] = 0.358 \, \mathrm{mM} \), \( \frac{1}{[\mathrm{H}_{2} \mathrm{SO}_{4}]} = \frac{1}{0.358} = 2.793 \)- For \( [\mathrm{H}_{2} \mathrm{SO}_{4}] = 0.436 \, \mathrm{mM} \), \( \frac{1}{[\mathrm{H}_{2} \mathrm{SO}_{4}]} = \frac{1}{0.436} = 2.294 \)- For \( [\mathrm{H}_{2} \mathrm{SO}_{4}] = 0.560 \, \mathrm{mM} \), \( \frac{1}{[\mathrm{H}_{2} \mathrm{SO}_{4}]} = \frac{1}{0.560} = 1.786 \)- For \( [\mathrm{H}_{2} \mathrm{SO}_{4}] = 0.752 \, \mathrm{mM} \), \( \frac{1}{[\mathrm{H}_{2} \mathrm{SO}_{4}]} = \frac{1}{0.752} = 1.330 \)- For \( [\mathrm{H}_{2} \mathrm{SO}_{4}] = 1.38 \, \mathrm{mM} \), \( \frac{1}{[\mathrm{H}_{2} \mathrm{SO}_{4}]} = \frac{1}{1.38} = 0.725 \)- For \( [\mathrm{H}_{2} \mathrm{SO}_{4}] = 2.98 \, \mathrm{mM} \), \( \frac{1}{[\mathrm{H}_{2} \mathrm{SO}_{4}]} = \frac{1}{2.98} = 0.336 \)- For \( [\mathrm{H}_{2} \mathrm{SO}_{4}] = 5.62 \, \mathrm{mM} \), \( \frac{1}{[\mathrm{H}_{2} \mathrm{SO}_{4}]} = \frac{1}{5.62} = 0.178 \)
03

Constructing the Linear Regression Model

Using the calculated \( \frac{1}{[\mathrm{H}_{2} \mathrm{SO}_{4}]} \) values as the independent variable and the endpoint volumes as the dependent variable, we construct a linear model. Plot these points and find the best-fit line using linear regression.The data points for the plot are:\[(2.793, 0.266), \ (2.294, 0.227), \ (1.786, 0.176), \ (1.330, 0.136), \ (0.725, 0.075), \ (0.336, 0.037), \ (0.178, 0.017)\]By performing linear regression, we calculate the slope \( a \) and the y-intercept \( b \) for the line \( V = a \cdot \frac{1}{[\mathrm{H}_{2} \mathrm{SO}_{4}]} + b \).
04

Solving for Unknown Concentration

Using the linear model \( V = a \cdot \frac{1}{[\mathrm{H}_{2} \mathrm{SO}_{4}]} + b \), substitute the given endpoint volume \( V = 0.157 \, \mathrm{mL} \) to find the unknown concentration. Solve\[0.157 = a \cdot \frac{1}{[ ext{H}_2 ext{SO}_4]} + b\]for \( [\mathrm{H}_2 \mathrm{SO}_4] \). Rearrange the equation to solve for \( \frac{1}{[\mathrm{H}_{2} \mathrm{SO}_{4}]} \) and then calculate \([\mathrm{H}_{2} \mathrm{SO}_{4}]\).
05

Calculating Concentration

Calculate \(\frac{1}{[ ext{H}_2 ext{SO}_4]}\) using the previously solved linear regression: \[\frac{1}{[ ext{H}_2 ext{SO}_4]} = \frac{0.157 - b}{a}\]Once you have \(\frac{1}{[ ext{H}_2 ext{SO}_4]}\), invert it to get the concentration \([ ext{H}_2 ext{SO}_4]\) in mM.

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Key Concepts

These are the key concepts you need to understand to accurately answer the question.

Acid-Base Titration
An acid-base titration is a method used to determine the concentration of an acid or base in a solution. This process involves gradually adding a solution of known concentration, called the titrant, to the solution being tested until the reaction reaches its endpoint. At this point, the acid and base have neutralized each other, often accompanied by a noticeable change in color due to an indicator.

In the described exercise, the titration takes place in a flow injection analysis (FIA) setup, where the sample containing \( \text{H}_2 \text{SO}_4 \) is injected into a stream containing NaOH. This leads to an acid-base reaction. The agarose beads with a bonded indicator change color when the endpoint is reached, signaling the completion of the reaction. This color change is detected spectrophotometrically.

This approach combines the principles of titration with FIA, where solutions mix in a controlled manner, making it a quick and efficient way to analyze substances in solvents like \( n \)-butanol. The endpoint volume, in this case, helps determine the concentration of \( \text{H}_2 \text{SO}_4 \) in the sample based on the known concentration of the titrant and the volume used to reach the endpoint.
Spectrophotometric Detection
Spectrophotometric detection is a technique used to measure how much a chemical substance absorbs light, by measuring the intensity of light as a beam of light passes through a sample solution. This method is widely used in chemical analysis for quantification of different analytes.

In this particular exercise, spectrophotometric detection is used to identify the endpoint of the acid-base reaction between \( \text{H}_2 \text{SO}_4 \) and NaOH. When the reaction reaches the endpoint, the indicator changes color, which alters the absorption of light. The spectrophotometer detects this change by measuring the light intensity before and after the reaction point.

The main advantage of using spectrophotometry in this setup is that it provides a precise and non-invasive way to determine the endpoint, improving the accuracy and reliability of titration, especially in non-aqueous solutions. This method is quick and can handle multiple samples in a sequence, as seen in the flow injection analysis.
Linear Regression
Linear regression is a statistical method used to model the relationship between a dependent variable and one or more independent variables. The aim is to find the best-fit line that predicts the dependent variable given the independent variables.

In this exercise, linear regression is applied to analyze the relationship between the inverse of the concentration of \( \text{H}_2 \text{SO}_4 \), \( \left[ \text{H}_2 \text{SO}_4 \right]^{-1} \), and the endpoint volume of the titration. By plotting these variables, you can draw a line that shows how the endpoint volume changes with different concentrations, which in this case is inversely proportional.

Through linear regression, each data point of endpoint volume and \( \left[ \text{H}_2 \text{SO}_4 \right]^{-1} \) is used to calculate a regression line. The resulting equation, \( V = a \cdot \frac{1}{\left[ \text{H}_2 \text{SO}_4 \right]} + b \), where \( V \) is the endpoint volume, \( a \) represents the slope, and \( b \) the y-intercept, allows for the estimation of unknown concentrations based on their endpoint volumes. This method is crucial for determining unknown concentrations in titration studies, offering a clear mathematical approach.

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Most popular questions from this chapter

The following data were collected for a reaction known to be pseudofirst order in analyte, \(A\), during the time in which the reaction is monitored. $$ \begin{array}{cc} \text { time }(s) & {[A]_{t}(\mathrm{mM})} \\ \hline 2 & 1.36 \\ 4 & 1.24 \\ 6 & 1.12 \\ 8 & 1.02 \\ 10 & 0.924 \\ 12 & 0.838 \\ 14 & 0.760 \\ 16 & 0.690 \\ 18 & 0.626 \\ 20 & 0.568 \end{array} $$ What is the rate constant and the initial concentration of analyte in the sample?

Deming and Pardue studied the kinetics for the hydrolysis of \(p\) -nitrophenyl phosphate by the enzyme alkaline phosphatase. \({ }^{23}\) The reaction's progress was monitored by measuring the absorbance of \(p\) -nitrophenol, which is one of the reaction's products. A plot of the reaction's rate (with units of \(\mu \mathrm{mol} \mathrm{mL}^{-1} \mathrm{sec}^{-1}\) ) versus the volume, \(V\), in milliliters of a serum calibration standard that contained the enzyme, yielded a straight line with the following equation. $$ \text { rate }=2.7 \times 10^{-7} \mu \mathrm{mol} \mathrm{mL}^{-1} \mathrm{~s}^{-1}+\left(3.485 \times 10^{-5} \mu \mathrm{mol} \mathrm{mL}^{-2} \mathrm{~s}^{-1}\right) V $$ A 10.00 -mL sample of serum is analyzed, yielding a rate of \(6.84 \times 10^{-5}\) \(\mu \mathrm{mol} \mathrm{mL}^{-1} \mathrm{sec}^{-1}\). How much more dilute is the enzyme in the serum sample than in the serum calibration standard?

In the presence of acid, iodide is oxidized by hydrogen peroxide $$ 2 \mathrm{I}^{-}(a q)+\mathrm{H}_{2} \mathrm{O}_{2}(a q)+2 \mathrm{H}_{3} \mathrm{O}^{+}(a q) \longrightarrow 4 \mathrm{H}_{2} \mathrm{O}(l)+\mathrm{I}_{2}(a q) $$ When \(\mathrm{I}^{-}\) and \(\mathrm{H}_{3} \mathrm{O}^{+}\) are present in excess, we can use the reaction's kinetics of the reaction, which is pseudo- first order in \(\mathrm{H}_{2} \mathrm{O}_{2},\) to determine the concentration of \(\mathrm{H}_{2} \mathrm{O}_{2}\) by following the production of \(\mathrm{I}_{2}\) with time. In one analysis the solution's absorbance at \(348 \mathrm{nm}\) was measured after \(240 \mathrm{~s}\). Analysis of a set of standard gives the results shown below. $$ \begin{array}{cc} {\left[\mathrm{H}_{2} \mathrm{O}_{2}\right](\mu \mathrm{M})} & \text { absorbance } \\ \hline 100.0 & 0.236 \\ 200.0 & 0.471 \\ 400.0 & 0.933 \\ 800.0 & 1.872 \end{array} $$ What is the concentration of \(\mathrm{H}_{2} \mathrm{O}_{2}\) in a sample if its absorbance is 0.669 after \(240 \mathrm{~s} ?\)

To study the effect of an enzyme inhibitor \(V_{\max }\) and \(K_{m}\) are measured for several concentrations of inhibitor. As the concentration of the inhibitor increases \(V_{\max }\) remains essentially constant, but the value of \(K_{m}\) increases. Which mechanism for enzyme inhibition is in effect?

To improve the sensitivity of a FIA analysis you might do any of the following: inject a larger volume of sample, increase the flow rate, decrease the length and the diameter of the manifold's tubing, or merge separate channels before injecting the sample. For each action, explain why it leads to an improvement in sensitivity.
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