Discharged volume of NaOH: ? Volume of HCI solution: 10mL pH of the solution over time at the equivalence point: 20.12 pH Molar concentration of the HCl solution (on the label): 0.1031M Molar concentration of the NaOH solution used (on the label): 0.1104M Molar concentration of the titrated HCl solution: ? Molar concentration of acid present in the solution after titration:? Molar concentration of NaOH base present in the solution after titration:?

Discharged volume of NaOH: ? Volume of HCI solution: 10mL pH of the solution over time at the equivalence point: 20.12 pH Molar concentration of the HCl solution (on the label): 0.1031M Molar concentration of the NaOH solution used (on the label): 0.1104M Molar concentration of the titrated HCl solution: ? Molar concentration of acid present in the solution after titration:? Molar concentration of NaOH base present in the solution after titration:?

Appl Of Ms Excel In Analytical Chemistry

2nd Edition

ISBN:9781285686691

Author:Crouch

Publisher:Crouch

Chapter7: Neutralization Titrations And Graphical Representations

Section: Chapter Questions

Problem 1P

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Similar questions

When titrating 50mL of 0.2MHCl, what quantity of 0.5M NaOH is needed to bring the solution to the equivalence point? a.80mL b.40mL c.20mL d.10mL
Prepared buffer solution GivenAmmonia Volume = 68 mL | Ammonia Concentration = 0.17 MAmmonium Chloride Volume = 42 mL | Ammonium Chloride Concentration = 0.13 MDissociation Constant of Ammonia: 1.8x10-5What is the total vol. of buffer
Reorder the following steps to the correct order of preparing a buffer. 1.Weigh out the calculated dry reagents into a beaker and dissolve them with deionized water only up to 70% capacity of the total volume. 2.Use an acid or a base to adjust the pH of the solution to the required pH level. 3.Calculate the mass required to prepare all the dry reagents, specific for concentration and volume. 4.Adjust the volume of the solution to the total volume required for the buffer with deionized water.
At what point will a buffer solution cease to moderate changes in pH? a. Only after all the acid or the base that needs to be buffered has been added. b. When waters equilibrium constant Kw has been reached. c. When the weak base acid and weak base salt concentration have been reached. d. When the acting buffering component is all neutralized.
A 50.000 mL aliquot of weak base that has a concentration of 0.285 M will be titrated with 0.684 M HCl. Calculate the pH of of the solution upon the addition of 20.851 mL of HCl. The Kb of the base is 7.5×10-6. Report your answer to the hundredths place. If the difference between moles of analyte and moles of titrant is less than 1x10-4, assume it is at the equivalence point.
When pH titrations occur, more data points become necessary at the vertical deflection near the equivalence point which is accomplished by adding smaller volumes of base from the pipers before taking the pH of the solution. Why are more points needed at this point in the titration curve? Why can larger volumes be used in the area outside of this region?
What among the following statements is false regarding the Henderson-Hasselbalch equation? a. A buffer cannot effectively buffer a system at pH = pKa b. It shows us the relationship of pH and a buffer system, which originally was derived by relating the pH and the carbonate buffer system of the blood c. That the pH of a compound can be calculated using two values, the negative log of the acid dissociation constant and ratio of the concentrations of the components in the buffer system d. Can be derived from the acid dissociation constant, Ka = [H+][A-]/[HA]
The graph below, which is related to a titration curve, shows the fraction (f) of the stoichiometric amount of acetic acid present as non-ionized CH3COOH and as acetate ion, CH3COO-, as a function of the pH of the solution containing these species. (Graph piture attached) Explain the significance of the point at which the two curves cross. What are the fractions and the pH at that point?
For a weak base/strong acid titration, the pH at equivalence point is <, >, or equal to 7?
A titration curve is constructed by plotting the pH of the analyte solution versus the volume ofthe reagent added as the titration progresses. As the equivalence point is approached, there is arapid change in the pH. Titration curves enable us to explain how end points are detected andtheir relationship to equivalence points. They can also serve as guides for choosing the properindicators for a particular acid-base titration. Explain how each plot can be used to interpret the acid-base titration.
A Total-ionic strength adjustment buffer with an acidic pH is needed to make a NaF stock solution to determine the concentration of F- of the standard solutions. Explain the importance of maintaining the pH and ionic strength of the buffer solution.
A buffer system works to keep pH within a narrow range. Buffer systemsare critical in all living cells/tissues. If pH were to measurably shift in a cell,what category of biological molecules would be most impacted, andwhat term refers to the resulting loss of their functional shapes? A buffer is a substance that, when it ionizes in water, creates a buffersystem. The substance and one of its ions represent a weak acid and aweak base. These form a pH-controlled equilibrium. Based on thedefinitions of acid and base, if [H+] increases, which would combine withthe H+, preventing a pH shift? If [H+] decreases, whichwould release H+ to counter a pH change? Check the one characteristic below that is important in a buffer system. maintains a neutral pH prevents pH from dropping prevents pH from rising minimizes change in p