chem 102L final quizzes
Two trials in a kinetics experiment give relative initial rate values of 0.997, and 0.487. The general rate law for the reaction is R=k[A]x[B]y, where [A] = 0.250 M for both trials and [B] = 0.0100 in the first trial and 0.0050 M in the second trial. Assuming the value of x = 1, round the value of y determined in the experiment above to calculate the value of the rate coefficient, k, in the first trial. A. k = 2.51 x 10-5 M-2s-1 B. k = 399 M-1s-1 C. k =2.51 x 10-3 M-1s-1 D. The answer cannot be determined from the information given. E. k =3.99 x 104 M-2s-1 F. 466 M-1s-1 G. 1.60 x 103 M-2 s-1 H. 390 M-1s-1
ANSWER B. k = 399 M-1s-1
An unknown diprotic acid reached its second equivalence point at a volume of 12.93 mL of 0.1301 M NaOH, with a general chemical equation in the form: H2A + 2 NaOH → 2 H2O + Na2A. If the mass of the unknown acid sample was 0.118 g, the molecular weight of the unknown acid would be: Select one: A. 140 g/mol B. 14.3 g/mol C. 35.1 g/mol D. 70.1 g/mol
ANSWER: A. 140 g/mol ** pay attention to coefficients (multiply by 2 here because 2 NaOH)
If lnP is known to 4 significant figures, and 1/T is known to 3 significant figures, what are the correct significant figures for the intercept of the regression line? Select one: A. 3 B. Cannot be determined from the information given. C. 4 D. 2
ANSWER: A. 3
A solution of 0.613 g erucic acid in 8.115 g stearic acid is measured to have a freezing point of 68.60 ºC. What is the molar mass of erucic acid? HINT: MW stearic acid is 284.48 g/mol. Tf (stearic acid) = 69.60 ºC. Kf (stearic acid) = 4.50 ºC/m. Density (stearic acid) = 847 kg/m3. Select one: A. 338.57 g/mol B. 315 g/mol C. 0.340 g/mol D. 96.8 g/mol E. None of these answers is correct.
ANSWER: A. 338.57 g/mol
The end point in the titration of potassium hydrogen phthalate (KHP) with sodium hydroxide (NaOH) is determined to be the point when: I. A plot of pH vs titrant volume has a slope of zero. II. A plot of pH vs titrant volume has a slope approaching infinity. III. The plot pH vs volume of titrant shows the top of a peak. IV. The plot of the change in pH vs volume of titrant shows the top of a peak. V. The color of a phenolphthalein indicator added to the solution turns bright pinkpurple. VI. The color of a phenolphthalein indicator added to the solution turns very pale pink, but fades to colorless a few minutes later. VII. The color of a phenolphthalein indicator is still colorless, but will turn pink with the next addition of titrant. Select one: A. II, IV, and VI. B. I, IV, and VI. C. I, III, and V. D. I, IV, and V. E. II, III, and V. F. I, IV, and VII. G. II, IV, and VII.
ANSWER: A. II, IV, and VI.
Consider the uncertainties in your kinetics experiment. Which of the following statements is true? Select one: A. If the colorimeter has an error that causes the absorbance reading to be consistently 0.05 units higher than the true absorbance for both the calibration curve and the kinetic samples, the error will not cause any inaccuracy in either the order of reaction or the value of the rate coefficient. B. If the colorimeter has an error that causes the absorbance reading to be consistently 0.05 higher than the true absorbance for both the calibration curve and the kinetic samples, the error will cause the order of reaction to be calculated incorrectly, but the rate coefficient should be okay. C. None of these statements is correct. D. If the colorimeter has an error that causes the absorbance reading to be consistently 0.05 units higher than the true absorbance for both the calibration curve and the kinetic samples, the error will cause both the order and value of the rate coefficient to be calculated incorrectly. E. If the colorimeter has an error that causes the absorbance reading to be consistently 0.05 higher than the true absorbance for both the calibration curve and the kinetic samples, the error will cause the value of the rate coefficient to be calculated incorrectly, but the determination of reaction order should be okay.
ANSWER: A. If the colorimeter has an error that causes the absorbance reading to be consistently 0.05 units higher than the true absorbance for both the calibration curve and the kinetic samples, the error will not cause any inaccuracy in either the order of reaction or the value of the rate coefficient.
In the Clausius-Clapeyron plot shown, methanol, CH3OH, is represented by the red points. If the other two molecules shown are n-nonane and 3,3-diethylpentane, both with the formula C9H20, the molecules represented by Sample A and Sample B can best be identified by which statement: (See the structures of these molecules. Check all correct answers.) from top to bottom--> sample B, then methanol, then sample A Select one or more: A. Sample B is most likely 3,3-diethyl pentane, because it is branched and has the weakest dispersion forces. Sample A is most likely n-nonane, which has stronger dispersion forces due to its straight chain and high molecular weight, giving it slightly stronger IMF than methanol. Correct B. Sample B is most likely n-nonane, because it is a straight chain and has the weakest dispersion forces. Sample A is most likely 3,3-diethyl pentane, which has stronger dispersion forces due to its branched structure and high molecular weight, giving it slightly stronger IMF than methanol. C. Sample A cannot be either n-nonane or 3,3-diethylpentane, because neither has H-bonding and therefore must have weaker intermolecular forces than methanol. D. Sample A could be either n-nonane or 3,3-diethylpentane, because both have a much larger molecular weight than methanol and therefore must have stronger intermolecular forces. E. Sample B cannot be either n-nonane or 3,3-diethylpentane, because both have a much larger molecular weight than methanol and therefore must have stronger intermolecular forces. Feedback
ANSWER: A. Sample B is most likely 3,3-diethyl pentane, because it is branched and has the weakest dispersion forces. Sample A is most likely n-nonane, which has stronger dispersion forces due to its straight chain and high molecular weight, giving it slightly stronger IMF than methanol.
The results of an experiment with a solution of an unknown fatty acid in stearic acid are shown in the table. Unfortunately, the value of the molar mass of the unknown is significantly different in each calculation. What is a reasonable explanation for this result? Select one: A. The calculation of molar mass was done using the mass of each portion of the unknown acid added, but it should have been calculated for the total mass of unknown acid. When this calculation error is corrected, the calculated molar mass should be consistent for each trial. B. The experiment should have been carried out for the same mass of unknown in each trial. The differences in the mass of unknown leads to the different molar masses calculated. C. There is not enough information provided to determine the nature of the problem. D. The experiment wasn't carried out correctly. The dramatic increase in the temperature change indicates that the steps needed to prevent supercooling were not followed. Feedback
ANSWER: A. The calculation of molar mass was done using the mass of each portion of the unknown acid added, but it should have been calculated for the total mass of unknown acid. When this calculation error is corrected, the calculated molar mass should be consistent for each trial.
In an experiment, a container with a volume of 283 mL was filled with air and sealed. Pressure was allowed to vary with temperature in the container. Based on the best fit line, the number of moles of air in the container would be: Select one: A. 0.28 moles B. 0.020 moles C. 0.00027 moles D. 20 moles E. 3.3 moles
ANSWER: B. 0.020 moles
During a titration between KHP (204.221 g/mol) and sodium hydroxide (40.01 g/mol), the end point was determined to be at a volume of 21.37 mL of NaOH titrant for a 0.1111-g sample of solid KHP dissolved in 50.00 mL of water. What is the concentration of the NaOH titrant? HINT: The equation for the titration reaction is: KHP (aq) + NaOH (aq) Na+(aq) + K+(aq) + P2-(aq) + H2O(l) Select one: A. The concentration cannot be determined from the information provided. B. 0.02546 M C. 0.09854 M D. 0.04274 M E. 0.1299 M
ANSWER: B. 0.02546 M
A solution was prepared using 3000 microliters of distilled water, 325 microliters of 2.00 x 10-3 M NaSCN, and 175 microliters of 0.201 M Fe(NO3)3•9 H2O. What is the initial concentration of SCN- in solution before the reaction begins? (NOTE: NaSCN molar mass is 81.07 g/mol. Fe(NO3)3•9 H2O is 403.9 g/mol. Molarity is measured in moles of solute per liter of solution.) Select one: A. 2.17 x 10-4 M B. 1.86 x 10-4 M C. 0.0117 M D. 0.0101 M E. The concentration cannot be determined if the equilibrium constant is not known.
ANSWER: B. 1.86 x 10-4 M
After performing this experiment, a pair of students discover that their thermometer was miscalibrated and was reading consistently 1.82°C higher than the actual temperature. How will this impact their results? Select one: A. If the temperature reading is artificially high, the vapor pressure will appear to be higher than the true vapor pressure at that temperature. This will cause all of the intermolecular forces to appear to be weaker than they actually are, but the relative strengths of intermolecular forces will be correct. B. If the temperature reading is artificially high, the vapor pressure will appear to be lower than the true vapor pressure at that temperature. This will cause all of the intermolecular forces to appear stronger than they actually are, but the relative strengths of intermolecular forces will be correct. C. They should redo the entire experiment with a correctly calibrated thermometer, because the relative strength of intermolecular forces in the various liquids will be impossible to determine for certain. D. The relative strengths of the intermolecular forces will be the opposite of their true order if the measurements had been made correctly. Feedback
ANSWER: B. If the temperature reading is artificially high, the vapor pressure will appear to be lower than the true vapor pressure at that temperature. This will cause all of the intermolecular forces to appear stronger than they actually are, but the relative strengths of intermolecular forces will be correct.
A titration curve of an unknown diprotic acid has a first end point corresponding to 15.23 mL of 0.1094 M NaOH. The molar mass calculated from this end point is 154.32 g/mol. The curve shows two additional endpoints, giving pKa values of 3.80, 8.04, and 11.33. When compared with a chart of unknowns, the experimenter finds a triprotic acid with a mass of 155.16 g/mol but the pKas are very different. There is a second triprotic acid with pKa values of 3.96, 7.54, and 11.14. Which statement expresses the most likely identity of the unknown? Select one: A. There is no way to tell which unknown is a better fit because a poor calibration of the pH meter would throw off both the molar mass and the pKa values determined in the experiment. B. The unknown that matches closest in molar mass is most likely the correct one, because the rapid change in pH identifies the end point, and the volume of standardized base is the most accurate measurement in the experiment. C. There is no way to tell which unknown is a better fit because the standardized base and the pH sensor calibration are equally accurate and precise. D. The unknown that matches closest in pKa is most likely the correct one, because it is possible that the pH meters were poorly calibrated, but they are still probably the most accurate and precise measurement in the experiment.
ANSWER: B. The unknown that matches closest in molar mass is most likely the correct one, because the rapid change in pH identifies the end point, and the volume of standardized base is the most accurate measurement in the experiment.
An experiment is run that demonstrates that the rate law of a reaction has the form R =k [A]1[B]2, where k=0.25. If the reaction was run with initial concentrations of [A] = 0.25 M and [B] = 0.005 M, which graph would you expect to best fit a straight line that would confirm reaction order? Select one: A. R vs time B. 1/R vs time C. 1/[B] vs time D. ln [B] vs time E. [B] vs time F. [A] vs time Feedback
ANSWER: C. 1/[B] vs time
The equilibrium concentrations of Fe3+, SCN-, and [FeSCN]2+ are determined experimentally to be 1.43 x 10-3 M, 2.86 x 10-4 M, and 5.96 x 10-5 M, respectively, for the reaction Fe3+ + SCN- —► [FeSCN]2+. Assuming there was no [FeSCN]2+ at the beginning of the reaction, what was the initial concentration of SCN-? Select one: A. Initial concentrations of Fe3+ and SCN- can't be calculated until the equilibrium constant is known. B. 146 M C. 3.46 x 10-4 M D. 1.49 x 10-3 M E. Initial concentrations cannot be determined from the information given.
ANSWER: C. 3.46 x 10-4 M --> add up the products conc and the eq conc of the ion asked for (5.96E-5)+(2.86E-4)
Before the unknown concentration of the iron thiocyanate can be determined for the equilibrium experiment, a calibration curve was constructed using solutions with known concentration. If done correctly, a line fit of calibration curve data should provide: Select one: A. A polynomial curve in which the terms represent the molar absorptivity, the path length of the cuvette, and the wavelength of the absorbance. B. A straight line with a negative slope, in which the slope represents the rate at which the purple product is decreasing in solution and the intercept represents the initial concentration. C. A straight line with a positive slope, in which the slope represents the product of the molar absorptivity and the path length of the cuvette and the intercept represents absorbance or interferences that are not due to the red product species . D. A straight line whose slope represents the change in energy of the electron as it emits red light.
ANSWER: C. A straight line with a positive slope, in which the slope represents the product of the molar absorptivity and the path length of the cuvette and the intercept represents absorbance or interferences that are not due to the red product species .
For which of the following graphs will a linear fit provide the value of R, the ideal gas constant, in standard units? Select one: A. None of these. B. Graph I (pressure kPa vs. volume mL) C. Graph IV (pressure atm vs. 1/volume L-1) D. All of these. E. Graphs III and IV. F. Graph III (pressure kPa vs. 1/volume mL-1) G. Graphs I and II. H. Graph II (pressure atm vs. volume L)
ANSWER: C. Graph IV (pressure atm vs. 1/volume L-1)
Beer's law is useful for the [Fe(SCN)]2+ equilibrium experiment because: Select one: A. The colored iron thiocyanate will change the reflectivity of the solution. B. The absorbance of the iron thiocyanate in the red region of the spectrum is proportional to its concentration. C. The absorbance of the iron thiocyanate in the blue region of the spectrum is proportional to its concentration. D. The red color of the iron thiocyanate can be used to determine the energy of the electron transitions in the product.
ANSWER: C. The absorbance of the iron thiocyanate in the blue region of the spectrum is proportional to its concentration.
To determine the order of a reaction with respect to one reactant, A, experimentally, a useful experiment would be: A. Run a reaction until both [A] and [B] are much less than their initial values. B. None of these would work. C. Two of these would work. D. Run a reaction for three trials in which [B] has a concentration of 0.800 M and [A] has a concentration of 0.05 M, 0.04M, and 0.025 M, respectively. E. All of these would work. F. Run a reaction with a concentration of [A] = 0.800 M and a concentration of [B] = 0.001 M. Continue the run until [A] is <0.001 M and [B] ~ 0.001 M. G. Hold [B] at 0.25 M and vary [A] between 0.30, 0.25, and 0.20 M.
ANSWER: C. Two of these would work
A cooling curve to determine freezing point is shown in the figure. The behavior in the graph can be explained in the following way: Select one: A. When the heat source is removed, the molten substance cools. However, when the substance begins to freeze, the change to solid phase absorbs energy that allows it to maintain a stable temperature until the freezing is complete. B. The process of freezing is an endothermic process; therefore, the substance cools until the freezing process is complete. Once all of the material is in the solid phase, the temperature stops decreasing. C. When the heat source is removed, the molten substance cools. However, when the substance begins to freeze, the change to solid phase releases energy that allows it to maintain a stable temperature until the freezing is complete. D. None of these explanations is correct.
ANSWER: C. When the heat source is removed, the molten substance cools. However, when the substance begins to freeze, the change to solid phase releases energy that allows it to maintain a stable temperature until the freezing is complete.
During a titration of KHP with 0.1 M NaOH, when the equivalence point is reached, what is the pH of the solution? Molecular equation: KHP(aq) + NaOH (aq) →NaKP (aq) + H2O (aq) Select one: A. The answer cannot be determined without knowing the Ka value for KHP. B. pH < 7 C. pH >7 D. pH = 7
ANSWER: C. pH >7
In the attached titration curve, two unknown acids are titrated by the same standardized base. Based on the information in the plot, which of the following statements is true? --> 1 was a monoprotic acid --> 2 was a dioprotic acid I. Both unknowns have an end point at a volume of ~14.5 mL, which means it is likely that Unknown 1 and 2 are the same acid, but Unknown 1 wasn't titrated far enough to see the second end point. II. Both unknowns have an end point at a volume of ~14.5 mL, which means they must have very similar pKas. III. Both unknowns have an end point at a volume of ~14.5 mL, which means they must have similar molar mass. IV. Unknown 1 appears to be a monoprotic acid, while Unknown 2 is a diprotic acid. V. Unknown 1 has a lower pH when no base was added, so it must be the stronger of the two acids. VI. Unknown 1 has a pKa ~ 4, while unknown 2 has a pKa ~3.5, so unknown 2 would be the stronger acid. Select one: A. Both unknowns have an end point at a volume of ~14.5 mL, which means it is likely that Unknown 1 and 2 are the same acid, but Unknown 1 I. B. II. C. III. D. IV. E. V. F. VI. G. III, IV, and V are correct. H. II and IV are both correct.
ANSWER: D. IV.
The equation of the best fit line for a Beer's law plot for [FeSCN]2+ is determined to be A=(4328)C + 0.115, where A is the absorbance of the solution and C is its concentration. If the transmittance of a solution is measured at 34.4%, what is the concentration of the unknown solution? Select one: A. 5.29 x 10-5 M [FeSCN]2+ B. The answer cannot be calculated from the information given. C. 2.00 x 103 M [FeSCN]2+ D. 3.56 x 10-4 M [FeSCN]2+ E. 8.05 x 10-5 M [FeSCN]2+
ANSWER: E. 8.05 x 10-5 M [FeSCN]2+ use 2-log(%T) to find absorbance and then solve for C
In a gas law experiment, an experimenter uses the volume of a syringe, 5.00 mL and the density of dry air, 0.001185 g/mL, to calculate the mass of air in the syringe. A value of 28.96 g/mol is then used as the molar mass of air to calculated the number of moles of air in the syringe. This value, in turn, is used to calculate the value of the ideal gas constant, R. One valid criticism of this approach would be: I. The calculation was done incorrectly. The value of the density is not needed to correctly calculate R. II. The calculation was done correctly, however the value 28.96 g/mol is not a true molar mass because air is a mixture of gases. III. The experiment would be more accurate if pure nitrogen was used, because its molar mass and density are more accurately known. IV. The experiment would be more accurate if the humidity of the air was included in the calculation, because this would tend to reduce the effective molar mass when it was included in the weighted average. Select one: A. I. B. II. C. III. D. IV. E. All but I. are valid assessments. F. All but III. are valid assessments.
ANSWER: E. All but I. are valid assessments.
In the plot of pressure vs. temperature shown, the data appear somewhat scattered around the regression line. Which of the following statements offers a well-reasoned assessment of the data? I. The regression line likely offers the best value for the relationship between pressure and temperature, because individual points are more likely to have a higher error or uncertainty. II. Some of the data shown in the plot should be eliminated if they don't fall on the regression line to improve the accuracy and precision of the results. III. If the container was imperfectly sealed, "burping" of the stopper could cause some results to be inconsistent because the number of moles of air were allowed to change during the experiment. IV. If the stopper was inserted too far into the flask, some results could have been affected by the changing volume. Select one: A. I. B. II. C. III. D. IV. E. Both I and III are sound assessments. F. Both I and IV are sound assessments. G. All of these statements are sound assessments. H. None of these statements is a sound assessment of the data. Feedback
ANSWER: E. Both I and III are sound assessments.
In a Clausius-Clapeyron plot of lnP vs 1/T, the regression line for one sample has an equation of y = -4450x + 20.98. If the value of R is 8.3145 J mol-1 K-1, the value of the enthalpy of vaporization for the molecule would be: Select one: A. -535 J/mol B. -20.98 kJ.mol C. 20.98 kJ/mol D. -37.0 kJ/mol E. 535 J/mol F. 37.0 kJ/mol
ANSWER: F. 37.0 kJ/mol ln(Pvap) = (-DHvap/R) (1/T) + C
In an experiment studying colligative properties, a solid reagent was heated until it was fully molten, then allowed to cool to determine the freezing point. For this experiment to work, which of the following precautions must be taken to prevent supercooling? Select one: A. I. Temperature must be monitored to the nearest hundredth decimal place. B. II. The thermometer must be kept as still as possible near the middle of the material to avoid temperature fluctuations. C. III. The test tube holding the reagent must be insulated to minimize temperature gradients within the material. D. IV. The material must be stirred to encourage crystallization, so that freezing occurs uniformly throughout the material. E. I and II are correct. F. III and IV are correct.
ANSWER: F. III and IV are correct.
In the titration curve shown, the value of the pKa(s) are best indicated by: (select all that apply.) Select one or more: A. Region 3 B. Region 1 and Region 3. C. Region 4 D. Region 1 E. None of these. F. Region 2 Correct G. Region 2 and Region 4.
ANSWER: F. Region 2 (at the half equivalence points)
Based on the calibration curve of a crystal violet Beer's Law experiment shown, which of the following statements is true? Select one or more: A. The R2 value of 0.9921 indicates that the solutions used to make the calibration curve were prepared accurately. B. The y-intercept indicates that the absorber has a very small molar absorptivity. C. The concentration of a solution with an absorbance of 0.731 would be 2164 M. D. None of these answers is correct. E. The R2 value of 0.9921 indicates that the colorimeter is accurate. F. The spacing of points indicates that the colorimeter is very precise, but at least one solution could have been prepared more accurately. G. The concentration of a solution with an absorbance of 0.731 would be 2.35 x 10-4 M H. The value of the slope of the line indicates that the crystal violet has a very high concentration. Feedback
ANSWER: F. and C. The spacing of points indicates that the colorimeter is very precise, but at least one solution could have been prepared more accurately., The concentration of a solution with an absorbance of 0.731 would be 2.35 x 10-4 M
A primary standard material should be insoluble, of high purity, and unreactive in air. Select one: True False
ANSWER: FALSE --> should be soluble
During lab, a beaker containing a solid reagent cracks. To be safe you should ____________ Select one: a. immediately dispose of the solid reagent into a solid waste container in the hood, then dispose of the beaker in the glass waste container, and begin the experiment again. b. immediately place the beaker and contents into the glass waste container, then begin the experiment again. c. immediately place the beaker and contents into the solid waste container in the hood, then begin the experiment again. d. notify your TA and, as long as the beaker doesn't need to be heated, continue the experiment normally.
ANSWER: a. immediately dispose of the solid reagent into a solid waste container in the hood, then dispose of the beaker in the glass waste container, and begin the experiment again.
In an experiment to determine the Keq associated with a particular reaction, two different solutions are measured 3 times each on a colorimeter with the following results: Cuvet E1, %T Cuvet E2, %T 48.0 15.3 46.1 14.7 46.0 14.7 sigma 1.12 0.357 mean 46.7 14.9 Which of the following statements correctly assesses the data? Select one: a. Cuvet E2 was more accurate because the value of sigma was smaller. b. The two cuvets gave data of the same precision, because the value of the CV is the same for each. c. Cuvet E1 gave better data because the %T was higher. d. Cuvet E2 was more precise because the value of sigma was smaller. e. No assessment of accuracy or precision can be made until the value of Keq is determined from the data.
ANSWER: b. The two cuvets gave data of the same precision, because the value of the CV is the same for each.
While carrying a vial of an organic liquid from the hood, it drops on the bench and shatters, soaking the front of your lab coat and shirt. You should immediately ____________ Select one: a. proceed to the rest room on the same floor as your lab room where you can remove the lab coat and rinse the chemical from your shirt. b. try to rinse the chemical off in the lab sink. c. proceed to the safety shower located just inside the door to the hallway, remove both the lab coat and shirt, and rinse your skin for 15 minutes. d. remove the lab coat and ask your TA if the chemical is hazardous.
ANSWER: c. proceed to the safety shower located just inside the door to the hallway, remove both the lab coat and shirt, and rinse your skin for 15 minutes.
In Experiment 15, two sets of cuvets were prepared in which the same equilibrium reaction occurred. One set was used to define the Beer's Law relationship between Absorbance and the Concentration of the product ion. In the other set, the concentration of the product ion at equlibrium was treated as an unknown, and was used to solve for the value of Keq. What is the principal difference between these two sets of solutions that allow them to be used in different ways? Select one: a. In one set of cuvets there was a limiting reagent that allowed the concentration of the product ion to be known. b. Because the value of Keq is so small, the value of the change in concentration could be neglected when calculating the equilibrium concentrations of the reactants. c. Only one reagent was used in the cuvets used for the Beer's Law curve, while both reagents were used to determined Keq. d. None of these is true. e. In one set of cuvets, LeChatelier's principle was used to drive the equilibrium so nearly to completion that the equilibrium concentration could be assumed.
ANSWER: e. In one set of cuvets, LeChatelier's principle was used to drive the equilibrium so nearly to completion that the equilibrium concentration could be assumed.
Match the following safety equipment with its location in the lab room. Telephone Safety shower Fire Extinguisher Eye wash First Aid Kit and Incident Reports.
Telephone - Found on the wall just inside the door to the lab room. Safety shower- Just inside the lab room door overhead. Fire Extinguisher- Mounted near the TA bench., Eye wash- Mounted alongside the sink at the front of the room First Aid Kit and Incident Reports.- Mounted on the outside of the fume hood
Match the following types of waste with the appropriate disposal location. a) A paper towel that was used to wipe up a spilled solution. b) A Kim wipe that was used to polish the sides of a cuvet. c) A small amount of sodium bicarbonate solution that was not used in the experiment. d) Green or silver lab gloves.
a) into the solid waste container b) into the regular trash c) into the liquid waste container d) in a small bin just above the TA bench
