The titration of a polyprotic acid with sufficiently different pKa ’s displays two equivalence points. Why?

Q: The equivalence point in the titration of this weak acid is 50.80 mL. At 25.40 mL, the pH was…

A: In the given figure they clearly mentioned at half-way to the equivalence point pH = pKa (dotted…

Q: Name at least three differences between the titration curve of a strong acid with a strong base and…

A: Titration curve of a strong acid with a strong base: 1.  One Equivalence point 2. Initial slow rise…

Q: Use the titration curve to calculate the pKa of HA at the equivalence point.  What value did you…

A: pKa value is the negative logarithm of dissociation constant as follows: pKa = -log(Ka)

Q: A di-protic weak acid was titrated with NaOH. After ploting the titration profile and the first and…

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Q: In the titration of a weak acid with NaOH, which following statement(s) a. Normality-molarity x (n);…

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Q: How does the Henderson Hadeelbalch equation prove that the pka of a weak acid is equal to the pH of…

A: The equilibrium reaction between the weak acid (HA) and its conjugate base(A-) forms a buffer…

Q: 3. The equivalence point of the ethanoic acid titration occurs when pH-8.7. The ionic product of…

A: Given: The pH at the equivalence point = 8.7 Kw = 1.0 × 10-14 mol2 dm-6 We have to calculate the…

Q: How the pH at the equivalence point is determined by the species present; why the pH at the midpoint…

A: pH is the measure of the acidic or basic nature of the substance. It is measured by the use of…

Q: Determine the pka of the weak acid based on the titration curve below. 12 10 6. 4 4 8. 12 16 20 24…

A: The solution is as follows:

Q: 4. Describe the pH changes as large or small in the vicinity of the: Tiratien of l.of a a.…

A: Disclaimer : The image contains multiple questions , hence we are solving only the 1st question. If…

Q: In the titration of a polyprotic acid, the volume required to reach the first equivalence point is…

A: When a polyprotic acid,H2SO3 with sufficiently two different pKa values is titrated with a strong…

Q: 8

A: Given   The value of pH is 4.13.

Q: 5==== A strong acid and a monoprotic weak acid are separately potentiometrically itrated with a…

A: Potentiometric Titration is done via the usage of two electrodes – an indicator electrode and a…

Q: encountered during the analysis in double indicator titration (determining of carbonates in a…

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Q: If KaKa is 1.85×10-5 for acetic acid, calculate the pH at the equivalence point for a titration of…

A: At equivalence point complete conversion of acetic acid into sodium acetate salt and here you have…

Q: In acid-base titration one of the following is incorrect: A suitable indicator should have pH of…

A: acid base titration  identify  incorrect  statement

Q: A 50.0 mL solution of 0.186 M sulfurous acid (H,SO, ) is titrated with 0.186 M NaOH. The pK values…

A: Sulfurous acid, H2SO3 is a dibasic acid. It can furnish two protons in solution. The pKa1 (indicated…

Q: The pH at the half-equivalence point of a weak acid-strong base titration is 5.23. What is the pKa…

A: Consider, a titration of Weak monoprotic acid (HA) with the strong base (OH-). As, we know that, at…

Q: 1) What is the different between volumetric titration and condumetric titration?

A: “Since you have asked multiple question, we will solve the first question for you. If you want any…

Q: The titration of a polyprotic acid with sufficiently different pKas displays two equivalence points.…

A: Polyprotic acid produces two different H+ ions upon ionization like diprotic acid. When a…

Q: Why is the equivalence point pH necessarily below 7 when a weak base is titrated with strong acid?

A: Equivalence point of a acid-base titration is a point when equivalent amount of acid and equivalent…

Q: In the titration of the weak acid (HA) by NaOH, what important species' concentration increases…

A: The point in titation in which the amount of added titrant ( NaOH) neutralize the analyte solution (…

Q: 13. Which of the following is TRUE for the titration of a weak base with a strong acid? C. the…

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Q: a) In the titration of a weak acid with a strong base what is the pH at the 50% equivalence point?…

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Q: The pH at one-half the equivalence point in an acid-base titration was found to be 5.67. What is the…

A: Given  pH = 5.67 Ka = ?

Q: Why does the titration of a weak acid with a strong base always have a basic equivalence point?

A: A weak acid can be react with strong base to form a basic (pH > 7) solution.

Q: A 65.0 mL solution of 0.158 M potassium alaninate ( H, NC, H, CO, K) is titrated with 0.158 M HCI.…

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Q: 3. (а) When 40 mL of benzoic acid (C,H5COOH) and 35 mL of potassium hydroxide were titrated, the pH…

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Q: 8. State True or False. In the titration of a weak acid with a strong base, pKa of the weak acid…

A: The equivalence point is the point where the number of moles of acid and base is approximately…

Q: A good rule-of-thumb for a weak acid-strong base titration is to choose an indicator whose…

A: In a corrosive base titration, the titration bend mirrors the qualities of the comparing corrosive…

Q: Which is the buffer region in the titration curve below? A 7 D mL of titrant Hd

A: A buffer is the solution of a weak acid and its conjugate base that resists any change in the pH…

Q: A mixture of 5.0 mL 1.0 M HCl and 15.0 mL acetic acid is titrated with 1.0 M NaOH solution. At…

A: Moles can be calculated as follows: M=nV where n: The number of moles of the solution V: Volume of…

Q: choice of indicator for acid base titration ?

A: We know that the selection of indicator is  pH lies between PH=pKin-1 to pkin+1 hence its depends on…

Q: in the titration of 50.0 mL 0.0200 M weak acid HA using 0.0150 M NaOH, what is the solution pH at…

A: Number of moles = Molarity x volume (L) Molarity of HA = 0.0200 M Volume of HA = 50.0 mL = 0.050 L…

Q: What is the pKa of the weak acid from t

A: From the given graph it is clear that, The pH at half equivalence point is approx 9.5 i.e pH = 9.5

Q: What are the differences in the titration curve of a strong acid-strong base versus a weak…

A: Titrations are an analytical technique most commonly used to calculate the concentration of an…

Q: Consider the titration of 200.00 mL of a 0.4529 M solution the monoprotic base ammonia (pKa of…

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Q: titration curve in acid-base titration is: a. less steep curve for strong analyte versus strong…

A: Given statements about titration curve in acid-base titration:

Q: The pH at one-half the equivalence point in an acid-base titration was found to be 8.2.  What is the…

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Q: At which point of a titration curve, is the pH value of the solution equal to the pKa of the weak…

A: pH The negative logarithmic of hydrogen ion Concentration is known as pH. pKa  The negative…

Q: 8. The pH at one-half of the equivalence point in a weak acid – strong base titration was determined…

A: Given, pH = 4.13

Q: A weak monoprotic acid is titrated with 0.100 M NaOH. Itrequires 50.0 mL of the NaOH solution to…

A: At equivalence point : No. of moles of base can be calculated as : Thus no. of moles of acid will…

Q: 2. Suggest a reason that K, is influenced by ionic strength. 3. Explain the difference between…

A: “Since you have posted a question with multiple sub-parts, we will solve the first three subparts…

Q: What indicators is best suitable for this titration curve of a weak acid & a strong base?

A: Answer: Since, here weak acid is being titrated against strong base. Therefore, at the equivalence…

Q: You were given a set a results on an Excel spreadsheet to complete. Following completion of this…

A: Answer: From the above data we make the graph of pH vs volume of titrant added.

Q: Calculate the pH at the equivalence point for the titration of 0.180 M methylamine (CH3NH₂) with…

A: pH at equivalence point can be calculated by considering the species present.

Q: What is the pH in titration of 100 ml 0.01 M benzoic acid with 0.02 M NaOH at equivalence point?

A: Volume of benzoic acid is 100ml and molarity = 0.01 M NaoH molarity = 0.02M Calculate the PH of…

Acid Base Titration

An acid-base titration is the method of quantitative analysis for determining the concentration of an acid and base by exactly neutralizing it with a standard solution of base or acid having known concentration.