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- What is the pH of the solution of 20mL IM H,PO, (pKa values = 2.16, 7.21, and 12.32) at the given points in the titration with a 1 M NaOH solution. (a) Initially (b) After 10 mL of NaOH. (c) After 20 mL of NaOH (d) After 35 mL of NaOH (e) After 50 mL of NaOH (f) After 70 mL of NaOHIn conductometric titration of strong acid with the strong base and weak acid with strong base the similarity is: A: decrees in conductance before end the point B: decrees in conductance after the end point C: increase in conductance before the end point D: increase in conductance after the end pointIf you were to overshoot tje endpoint in the titration of your unknown acid, would youncalculated molar mass be higher, lower or equal to the actual molar mass
- why we use methyl orange as indicator in titration of strong base with weak base and not the phenolphthaleinDo you think it is possible to use conductometric titration to determine the concentration of a mixture of a strong acid and a weak acid against potassium hydroxide?If yes, how many break/s the curve will show?You need to determine the pKa of a weak acid. You can obtain the necessary data for this by titrating a sample of the weak acid with a standardized solution of ... HCI using a pH meter HCI using methyl orange indicator O NaOH using methyl orange indicator NaOH using a pH meter NaOH using phenolphthalein indicator O HCI using phenolphthalein indicator
- In general, why should titrants be strong acids or bases? A For a broader end point For a sharper equivalence point For a broader equivalence point D For a sharper end pointWhat conditions must be followed to perform complexometric titration?ANSWER BI AND ANY OTHER THREE QUESTIONS SECTION D Question B1 One way to delermine the pKa value is by use ofa pli curve. One student used thie pH curve to determine thc pka value of the weak monoprotic acid. She transferred 25.0 cm' of 0.100 M solution of the acid into a conical flask and measured the pll of the acid solution using a pH mcter accurate to one decimal place. A solution of sodium hydroxide of concentration 0.100 mol dni was added from the burette in small portions until the alkali was present in excess. The pH of the mixture was recorded after each addition of the sodium hydroxide solution. Then she plotted the pH of the solution versus volume of alkali added from the burette and used this graph to determine the acid dissociation constant. 14 12 10- 10 20 30 40 50 VNaOH (ml) a) Calculate mass of the acid required to prepare 100 cm' of 0.1 solution of this acid.(Molar mass of the acid 150 g mol) b) What is the volume of sodium hydroxide added at cquivalence point? c) What…
- Give the name of another weak acid that will have a similar titration curve. Briefly explain the reason for the similarity.Which of the titration curves A or B corresponds to the stronger acid?Learning Goal: To calculate the pH at the equivalence point for various types of titrations. The equivalence point in an acid-base titration is the point at which stoichiometrically equivalent quantities of acid and base have been mixed together. At this point the reaction is complete because all analyte has been consumed by titrant. On a titration curve, the equivalence point is represented by the point of inflection (where the curve changes concavity). The figure (Figure 1) shows the titration of 40.0 mL of 0.100 M HCl with 0.100 M NaOH. When 40.0 mL of the NaOH solution is added, the acid-base neutralization reaction is complete. When analyzing titrations involving weak acids or bases, consider how the neutralization reaction will impact the pH of the system. For example, when titrating a weak acid with a strong base, at the equivalence point all the base has been used to neutralize the acid forming its conjugate weak base Figure E 14 12 10 8 6 4 2 0 0 Equivalence point 20.0 40.0 mL…
