select the correct responses only
1) The Henderson-Hasselbalch Equation relates pH and pKa to [A-] and [HA].
2) Ka is known as the acid formation constant.
3)When titrating, the analyte is the standardized (known concentration) solution, and the titrant is the solution being analyzed.
4)Volumetric titrations can only ever be performed using a monoprotic weak acid and a strong base.
5) For monoprotic weak acids, the titration curve (pH on y-axis, volume of base added on x-axis) takes on an S-shape.
6)Volumetric titrations involve a
7)In titrations, an indicator (dye) solution is often used to signal the endpoint with a color change.
8) NaOH is the chemical formula for sodium hydroxide.
9) For the chemical reaction between an acid (H+) and base (OH-), there is a 1:1 molar ratio between H+ and OH-.
10) In the reaction of a weak acid HA with base NaOH, the product NaA is the conjugate acid salt.
11) In the reaction of a weak acid HA with base NaOH, sodium ion Na+ is a spectator ion.
12) Water is a product formed in the reaction of a weak acid HA with base NaOH.
13) As more titrant is added to the analyte solution and the solution becomes more basic, the pH increases.
14 The half-equivalence point of the titration occurs on the titration curve at the exact center/inflection point of the S-shape.
15) The equivalence point has been reached when the moles of weak acid present in the analyte solution is equal to the moles of base that have been added to the solution.
Step by stepSolved in 2 steps
- 30.0 mL of the 1.0 M LIOH is added to 50.0 mL of 0.20 M H2SO4. What is the pH at this point in the titration? H₂SO4 + 2LIOH → Li₂SO4 + 2H₂O pH = [?] Hint: How many moles of H+ and OH- are present? pH at 30 mL base Enterarrow_forwardWhich statement is TRUE for the following plot? Group of answer choices Compounds X and Y are both strong monoprotic acids. The pH at the equivalence point for compound X is approximately 8.5. The pKa of compound Y is approximately 1.5. Compound X is more concentrated than compound Y. Compounds X and Y have the same pH at the equivalence point of their titrations with the same base solution.arrow_forwardplease explain answer...arrow_forward
- What volume of stock 0.350 M KOH and what mass of N-2-Hydroxyethylpiperazine-N′-2-ethanesulfonic acid (HEPES, MW 238.30, pKa 7.56) is needed to prepare 100.0 mL 0.100 M buffer at pH 7.20?arrow_forwardPlease answer all part asap.arrow_forwardFor each scenario below, select the color of the solution using the indicator thymol blue during the titration. When you first add indicator to your Na2CO3 solution, the solution is basic (pH ~10), and the color is [Select] At the equivalence point for the titration, the moles of added HCI are equal to the moles of Na2CO3. One drop (or less!) past this is called the endpoint. The added HCI begins to titrate the thymol blue indicator itself. At the endpoint, the indicator color is [Select] When you weren't paying attention and added too much HCI (~12 mL extra), the color is [Select] When you really weren't paying attention and reached the second equivalence point of Na2CO3, the color is ✓ [Select] blue yellow red orange green Question 9arrow_forward
- Which of the following is a qualitative analysis technique? a) Gravimetric analysis b) Volumetric analysis c) Spectroscopy d) Titrationarrow_forwardFind the pH during the titration of 20.00 mL of 0.1000 M butanoic acid, CH3CH₂CH₂COOH additions of titrant. (a) 10.00 mL: pH = (b) 20.10 mL: pH (c) 25.00 mL: pH = (Ka 1.54 × 10¯), with 0.1000 M NaOH solution after the following =arrow_forward
- ChemistryChemistryISBN:9781305957404Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCostePublisher:Cengage LearningChemistryChemistryISBN:9781259911156Author:Raymond Chang Dr., Jason Overby ProfessorPublisher:McGraw-Hill EducationPrinciples of Instrumental AnalysisChemistryISBN:9781305577213Author:Douglas A. Skoog, F. James Holler, Stanley R. CrouchPublisher:Cengage Learning
- Organic ChemistryChemistryISBN:9780078021558Author:Janice Gorzynski Smith Dr.Publisher:McGraw-Hill EducationChemistry: Principles and ReactionsChemistryISBN:9781305079373Author:William L. Masterton, Cecile N. HurleyPublisher:Cengage LearningElementary Principles of Chemical Processes, Bind...ChemistryISBN:9781118431221Author:Richard M. Felder, Ronald W. Rousseau, Lisa G. BullardPublisher:WILEY