Describe the difference between equivalence point and endpoint. For a monoprotic weak acid titrated with a strong base, are the two equivalent?
Equivalent point: The point at which the concentration of titrant is equal to the concentration of the analyte is called Equivalent point.
Endpoint: The indicator will not show any visible color change at the equivalent point. Almost every indicator's physical changes (color) is seen after the addition of a slight excess of titrant into analyte. The point at which indicator undergoes the color change is called Endpoint. The endpoint and equivalent point are not the same.
Titration error = Equivalent point - Endpoint
The titration error is very small. even it is in negligible amount.
Titration curve of acetic acid Vs sodium hydroxide (weak acid Vs strong base). In this graph, the equivalent point is the midpoint of the sigmoid curve. As we know that, Endpoint is depends on the indicator, by changing the indicator the endpoint also changes. From this, you can conclude that the equivalent point and endpoint are not same.
Describe the difference between equivalence point and endpoint. For a monoprotic weak acid titrated with a...
HF is a weak acid (a monoprotic one). When HF is titrated with a strong base (like NaOH), it will eventually reach an equivalence point where exactly all of the HF has been reacted with exactly the needed amount of NaOH. What will the pH be when HF reaches equivalence point? (Hint: think about what products will be present and whether they are weak acids, weak bases or neutral...) pH will be 7.0 pH will be greater than 7.0 pH...
in a titration -If given an endpoint PH and moles of a weak acid at an endpoint in mL, given Molarity of strong base of a buffer solution, could one find the equivalence point if they forgot to record data points at the equivalent point?
When a weak acid is titrated with a strong base, if the pH at the half-equivalence point is 6.04, what is the Ka of the acid?
Mark each of the following statements about the ½ equivalence point of an acid-base titration TRUE or FALSE. a. It is the point in the titration when the concentration of weak acid (HA) being titrated is equal to the concentration of the conjugate base (A− ). b. It is the point halfway between the beginning of the titration of a weak acid or weak base and the equivalence point. 2 c. When a strong acid is titrated with a strong...
If the pH at the equivalence point for titration of a monoprotic weak acid with NaOH is 9.00, and 10 mL of base is required to reach the equivalence point, how would you determine the pKa of the acid? the pKa is 9.00 determine the pH after 5 mL of base is added; this is the pKa determine the pH when 20 mL of base is added; this is the pKa the pKa is -log(9)
5. The Ka and Molar Mass of a Monoprotic Weak Acid a. Suppose that–unknown to you–the primary standard KHP (potassium hydrogen phthalate, KHC8H4O4) had a potassium iodide impurity of approximately one percent by mass. How would this have influenced the calculated molarity of your sodium hydroxide solution? Would your calculated value be too low, too high, or unchanged? Explain your answer. b. Sketch a typical titration curve for a monoprotic weak acid titrated with a strong base. Label the axes...
If 0.360 moles of a monoprotic weak acid (Ka = 8.6 × 10-5) is titrated with NaOH, what is the pH of the solution at the half-equivalence point?
Describe how you expect the pH of your weak acid solution to change when strong base is slowly added to it. When making this description, assume you have a monoprotic acid. Comment on how much the pH changes at the beginning of the titration, when about half the acid has been titrated, and when nearly all the acid has been titrated. Use the terms half-equivalence point and equivalence point in this discussion. How would the titration curve of a diprotic...
help plwase 2. For a weak acid (e.g., CH.COOH) that is titrated with a strong base, (e.g., NaOH), what species (ions and/or molecules) are present in the solution at the equivalence point? 3. For a weak acid (e.g. CH3COOH) that is titrated with a strong base (e.g., NaOH), what species (ions and/or molecules) are present in the solution at the half-equivalence point?
Which of the following conditions is/are met at the equivalence point of the titration of a monoprotic weak base with a strong acid? 1. The moles of acid added from the buret equals the initial moles of weak base. 2. The volume of acid added from the buret must equal the volume of base titrated. 3. The pH of the solution is less than 7.00.