Titration Lab Practice Test

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• What requirement does a substance have to meet to be a primary standard?
• What indicates the endpoint in a titration curve?
• In a titration of a weak base (monobasic) with a strong acid, what indicates completion of the neutralization in the pH curve?
• What does a small standard deviation indicate about the reliability of experimental data in a titration?
• What is formed when solid sodium hydroxide is exposed to carbon dioxide in air?
• Describe the general shape of the titration curve for a strong acid titrated with a strong base and state the pH at the equivalence point.
• If the primary standard potassium hydrogen phthalate is not completely dry, how does that affect the reported NaOH molarity?
• What are common sources of systematic error in titration readings?
• What’s the minimum number of titration replicates you should do?
• Which metal ion can EDTA titrate effectively in a similar calcium determination?
• If you recorded a titrant volume of 25.00 mL but the buret read 27.50 mL due to an air bubble, what is the effect on the calculated acid molarity?
• How do you choose an appropriate indicator for an acid-base titration?
• Which factor is explicitly listed as contributing to the accuracy of a titration measurement?
• What is back-titration and when is it used?
• The end point in an acid-base titration is typically detected by which means?
• What pH is typically maintained with buffer in Ca2+ EDTA titration?
• What is used in an acid-base titration to indicate the right amount of titrant has been added to completely neutralize it?
• Which term describes a solution whose molarity has been calculated rather than measured directly?
• If 25.0 mL of 0.100 M HCl is titrated with 0.100 M NaOH, how many milliliters of NaOH are needed to reach the equivalence point?
• Why must the volume of the titrant be known with high precision?
• What is the purpose of using a primary standard such as KHP in titration standardization?
• What is the primary purpose of EDTA in this titration?
• For a titration of a monoprotic weak base with a strong acid, the equivalence point occurs at a pH:
• What is the name of the glassware used to measure an aliquot of a solution?
• Why is it essential to get rid of air bubbles in a buret's tip before you perform a titration?
• In titration, what is the name of the solution with known concentration used to reach the endpoint?
• If a titration curve shows two steep regions, what does this indicate about the analyte?
• How is the reactant solution of unknown concentration called in a titration?
• What is the buffer region in a titration curve, and why is it important when choosing an indicator?
• What is the goal of Part A of this experiment?
• What is the balanced molecular equation for the reaction of sodium hydroxide with potassium hydrogen phthalate?
• Why is a blank titration performed?
• How reliable was your data?
• If the pH at the equivalence point for a strong-strong titration is measured as 6.9 instead of 7.0, which issue could best explain this discrepancy?
• How many mL's of titrant apart maximum should titration replicates be from one another to be considered reliable data?
• What is the name of the glassware in which you prepare a solution by dissolving a solid sample and adding enough water to dilute it to the right volume?
• What is the primary difference between the end point and the stoichiometric point?
• Why is a buffer used in this titration?
• Which practice contributed to error by endpoint misreading in this experiment?
• What does hygroscopic mean?
• How many significant figures should buret readings be reported and why?
• Why is a blank important when standardizing a titration method?
• What is the primary standard used in this experiment?
• Which of the following describes factors that contribute to the accuracy of a titration measurement?
• What color does Eriochrome Black T indicator turn when it is free in basic solution?
• Should the buret's meniscus coincide with the zero milliliter mark at the start of titration?
• Which statement best explains why leaving the NaOH bottle uncapped would not affect molarity according to the material?
• Which device is commonly used to deliver the EDTA solution during the titration?
• What is ionic strength and how can it influence titration results?
• Why is it important to record buret readings to the nearest 0.01 mL during titration?
• What is a primary reason to perform titration replicates?
• During pH meter calibration, what step should be performed between solutions?
• How do you standardize a solution?
• What is the purpose of performing replicate titrations in a titration experiment?
• What data should you record immediately after reaching the end point of a titration?
• What is percent relative standard deviation (RSD) and how is it used in titration analysis?
• How is the reactant solution of known concentration called in a titration?
• What is a potential consequence of allowing the endpoint color to become too pink during titration?
• How many buret drops correspond to one milliliter?
• Which description best explains why polyprotic acids can exhibit multiple equivalence points in titration with a strong base?
• In a titration of a weak base with a strong acid, the equivalence point occurs at a pH less than 7. What does this indicate about the base?
• How is the equivalence point identified from the titration curve plotted as pH versus added volume?
• Which statement best describes the buret and its use in titration?
• Which container is typically used to hold the analyte while titrant is added from a buret?
• Which buffer is appropriate for maintaining pH around 10.5 during the titration?
• Which substance is commonly used as a primary standard in acid-base titration due to having a single ionizable hydrogen?
• What is a safe practice to minimize risk when handling acids and bases during titration?
• Which statement best describes a typical pH meter calibration procedure prior to titration?
• Explain how temperature can affect titration results.
• If a dirty buret causes a NaOH drop to cling to the wall and not be delivered, how is the reported molarity affected?
• If a buret reads consistently 0.03 mL low, how would you account for this in your data?
• What is the purpose of titration?
• A student titrates 25.00 mL of an unknown monoprotic acid with 0.1000 M NaOH and requires 32.50 mL NaOH to reach the equivalence point. What is the molarity of the unknown acid?
• When presented with a titration curve that shows two distinct steep regions, how should you report the results?
• Which indicator selection approach is appropriate for a titration?
• Distinguish between the stoichiometric point and the end point in an acid-base titration.
• Which of the following describes the effect of an air bubble initially trapped in the buret tip on the reported molarity?
• Which measurement best defines the end point of a titration?
• Which of the following best describes the effect on molarity when a trapped air bubble remains in the buret during titration?
• During analysis, rinsing the Erlenmeyer wall with water would affect the reported molar concentration of the acid solution?
• Which option best describes a source of error in an experimental titration measurement?
• Which explanation is given for why an uncapped NaOH bottle would not affect the measured molarity?
• A 25.0 mL sample of a 0.100 M monoprotic acid is titrated with 0.0800 M NaOH. What volume of NaOH is required to reach the equivalence point?
• How many equivalence points would you expect in the titration of phosphoric acid with NaOH, and why?
• In which piece of titration glassware is the titrant poured?
• In a polyprotic acid titration, how many equivalence points can occur?
• A student reports an accepted analyte concentration of 0.150 M, but their titration result is 0.145 M. What is the percent error?
• How can you determine the pKa of a weak acid from a titration curve?
• Differences in endpoint color between groups performing a titration are most likely due to what?
• How can temperature changes affect the color change of an indicator near the endpoint?
• In a titration of a weak diprotic acid with a strong base, how many equivalence points can occur and why?
• List the steps to standardize a NaOH solution using KHP as a primary standard.
• What is the main purpose of performing Part A and Part B in a titration lab practice?
• Describe a redox titration and give an example of a common redox titrant–analyte pair.
• In a titration, the solution being titrated is called the what?
• How can you ensure endpoint is close to the equivalence point if your indicator’s transition is not ideal?
• When combining measurements with 3 sig figs and 4 sig figs, the final reported result should have:
• Which statement best describes why drying a primary standard before weighing is important?
• If the primary standard is dissolved in 50 mL instead of 25 mL, how is the NaOH molarity affected?
• What is the stoichiometry of the complex formed between Ca2+ and EDTA?
• How many ionizable hydrogens does potassium hydrogen phthalate have?
• What qualifies as a primary standard for standardizing a NaOH solution?
• Define primary standard.
• In an EDTA titration of calcium ions, which indicator is typically used?
• Which term describes the solution whose concentration is unknown in a titration?
• What is the purpose of rinsing glassware between titrations?
• If an air bubble, initially trapped in the buret tip is passed from the buret during the titration, will the reported molar concentration of the acid be reported too high, too low, or unchanged as a result?
• How would you determine the number of significant figures to report in the calculated concentration?
• Which factor can affect the accuracy of endpoint detection in a titration?
• What is parallax?
• What is the proper way to minimize parallax error when reading the buret?
• Which buffers are used to calibrate a pH meter prior to titration?
• What is an appropriate final action after completing a titration data set?
• Which statement best describes the primary standard used in this experiment?
• In the described procedures, which factor would not affect the reported molarity given that the acid volume is known?
• Why is the zero mL mark at the top of the buret whereas the highest mark is at the bottom?
• How many reactants are used in an acid-base titration?
• Which two safety practices are essential in titration labs?
• Which statement best summarizes the overall effect of the three described scenarios on reported molarity?
• Which practice is correct for obtaining an accurate buret reading?
• Which metal ion is commonly quantified using an EDTA titration?
• In acid-base titration, how does the pH at the equivalence point depend on the strengths of the acid and base?
• What two unwanted things happen to solid sodium hydroxide when exposed to air?
• What is the goal of Part B of this experiment?
• Why might you use a pH meter instead of an indicator in a titration?
• In a titration of a weak acid with a strong base, why is the equivalence point pH greater than 7?
• A titration of a 50.00 mL sample requires 25.00 mL of titrant to reach equivalence; titrant concentration is 0.2000 M; what is the analyte concentration, assuming 1:1 stoichiometry?
• How is a half-drop of titrant dispensed from a buret?
• In analyzing repeated titration measurements, a small standard deviation indicates high precision.
• How do you calculate the concentration of your sodium hydroxide solution?
• Which statement best describes why rinsing with water does not alter the reported molar concentration when the volume used is known?
• What color is observed when the Ca2+-EDTA complex is present with Eriochrome Black T?
• What is the color of the indicator at the start of the titration before endpoint?
• What is a blank titration and why is it performed?
• What information does a titration curve provide about the reaction between base and acid?
• Why is it necessary to dry the primary standard in an oven at 100 C for at least one hour before massing samples?
• What is parallax error and how can you minimize it when reading a buret?
• What is the purpose of standardizing the titrant solution in a titration experiment?
• Define secondary standards.
• In a precipitation titration with AgNO3 and Cl−, how is the endpoint detected?
• What statistical value is computed from multiple titration trials to summarize precision?
• Which statement best describes a primary standard used in titration standardization?
• What improvement is recommended to enhance titration accuracy?
• What does it mean to standardize a solution?
• When reporting results for Part A and Part B, if one measurement has 3 sig figs and another has 4, how many sig figs should be reported overall?
• In a titration of a strong monoprotic acid with a strong base, what is the expected pH at the equivalence point and why?
• What is the effect on the NaOH molarity if the polyethylene bottle containing standardized NaOH solution is not tightly capped?
• Why must you standardize your titrant solution?
• What cleanup steps are essential after a titration lab?
• What is the most plausible explanation for observed differences in NaOH molarity between your group and others during a titration exercise?
• What would happen to the reported molarity if a trapped air bubble is expelled and the titration proceeds?
• Which term describes the solution with known concentration used to standardize the titration solution?
• In the described titration experiment, which substance is used as the secondary standard?
• Is the acid-base indicator generally added to the titrant or the analyte in a titration?
• Using 20 drops of phenolphthalein instead of 2 would make the analysis less accurate because:
• Which of the following statements about the equivalence point is true?
• How would you correct a titration data set if the buret readings consistently start at 0.50 mL instead of 0.00 mL?
• For a titration involving a weak base with a strong acid, which statement about the equivalence point is true?
• What is the purpose of titration curves in laboratory analysis?
• How would you identify multiple equivalence points in an acid-base titration of a polyprotic acid?
• Which statement correctly describes the EDTA-Ca2+ interaction?
• If the polyethylene bottle containing the standardized NaOH solution is not tightly capped for subsequent experiments, how does this affect the molar concentrations of the NaOH solution?
• In the titration of a weak base with a strong acid, the pH at the equivalence point is:
• In this titration experiment, the NaOH solution is standardized in Part A. What is NaOH most commonly called in this context?
• At the equivalence point for this titration, how many moles of titrant have been added?
• Which indicator is best suited for a strong acid–strong base titration?
• What is the stated consequence of not tightly capping the NaOH bottle on the molar concentration?
• Which statement best describes the endpoint in this titration?
• If the endpoint indicator changes color too early, what is the likely effect on the calculated concentration of the analyte?
• In titration terminology, what is the equivalence point?
• Which statement describes the titrant?
• What is the recommended approach to estimate the volume of titrant needed for the end point for a given analyte volume?
• Which ion is titrated in this procedure?
• What titration data must be collected for calculating the unknown concentration?
• Which statement describes the effect of rinsing with water on the acid molarity when the volume used is known?
• What color does the solution turn at the endpoint of the Ca2+ EDTA titration with Eriochrome Black T?
• Indicator color change reasoning near endpoint: why do some indicators change colorGradually while others transition sharply?
• What is the purpose of a volumetric flask in preparing solutions?
• Which factor can lead to false data when preparing titration solutions and is addressed by drying primary standards?
• Which statement best describes the endpoint in a titration?