You titrated phosphoric acid H3PO4 (Ka1 = 7.5×10-3, Ka2 = 6.2×10-8, Ka3 = 4.2×10-13) with a strong base and you likely expected to observe 3 equivalence points on the titration curve.  However, the titration curve does not show a sharp pH increase at the third equivalence point.  Explain why this happens.

Q: What is the molar solubility of Agl Ksp= 8.3 x 10^-17 in the presence of 0.05 M KNO3? A. 1.29x10^-16…

A: Molarity of KNO3 = 0.05M KNO3 is a strong electrolyte and dissociates completely to furnish ions.…

Q: Using Excel, generate a titration curve for the titration of 25.00-mL 0.10-M NaoH with 0.10-M HCl.…

A: A titration graph is a graphical portrayal of the pH of a solution during a titration. On the left…

Q: A 50.0 mt of basic solute (K, 158 x 10 ) is titrated with a 25.0 ml of 0.100 M HCI solution. Which…

A: Given: Kb of base solute = 1.58 X 10-9  Volume of base solution = 50.0 mL = 0.050 L…

Q: acetic acid, CH3COOH is a commercially weak acid with a value of Ka = 1.8 x 10 ^ -5. In an…

A: Dissociation of weak acid: CH3COOH⇋CH3COO- + H+ Ka=CH3COO-H+CH3COOH

Q: 40.00 ml of 0.1200 benzoic acid is titrated with  0.1000 M NaOH.  Calculate the pH after the…

A: Step 1: Here, first of all the moles of benzoic acid should be calculated as follows: volume is…

Q: Calculate the pH during the titration of 40.00 mL of 0.1000 M propanoic acid (HPr; Ka = 1.3x10-5)…

A:

Q: A 50.0 mL of basic solute (Kb = 1.58 x 109) is titrated with a 25.0 mL of %3D 0.100 M HCI solution.…

A: Depending upon the PH of the solution,  one can determine which indicator is the best for this acid…

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: Calculate the pH after the addition of 60.0 mL of base in the titration of 50 mL of 0.100 M HA using…

A: Given: Vol of base(NaOH) = 60mL Concentration of NaOH = 0.100M vol of HA = 50mL Concentration of HA…

Q: Which of the following indicators is more suitable for the titration of a 25.00mL sample of 0.140 M…

A: Propanoic acid is a weak acid having pKa value 4.87. The pKb value of its conjugate base will be 14…

Q: Consider the titration of 25 mL of 0.15 M methylamine, CH3NH2, which has a Kb of 3.4 x 10-4 with…

A: The pH of a solution is the negative logarithmic of H+ ion concentration in the solution. The…

Q: In the titration of a weak acid HA with 0.100 M NaOH, the stoichiometric point is known to occur at…

A: pH range for an indicator is around the its pka value.  So we choose an indicator whoose pka value…

Q: 4.If the hydroxide concentration of a HNO3/NO3- buffer system is 0.00000025 M, what is the nitrate…

A: Given:   The concentration of hydroxide is 0.00000025 M. The concentration of nitric acid is 0.84 M.…

Q: A biochemist prepares two stocks of sodium phosphate buffer by titrating phosphoric acid with sodium…

A: Given: pKa of phosphoric acid are 2.15, 7.20 and 12.35 Volume of 7.20 buffer is 50.0 mL Volume of…

Q: Calculate pI for the titration of 100.0 mL of 0.1023 M I- with 0.1190 M AgNO3 for the addition of…

A: The titration between iodide ion and silver nitrate is a form of precipitation titration. It is a…

Q: A 50.0 ml of acidic solute (Ka = 1.20 x 10 2) is titrated with a 2.50 mL of %3D 1.00 x 10-5 M NaOH…

A: Given: Ka of acid solute = 1.20 X 10-2  Volume of acid solution = 50.0 mL = 0.050 L…

Q: Which indicator whose names and pH ranges are given would be suitable when 20 mL of 0.150 M HF is…

A:

Q: 2- Ahmed has done four types of titrations of 1M and 50 ml for both acid and base (Conductometric…

A: 1. Curve for Conductometric titration of strong acid Vs strong base :   2. Curve for Potentiometric…

Q: 5 x 10-14 of the following cases does have the lowest solubility f 1.6 x 1019 u(OH)2 in a buffer at…

A: For same types of salt. Lower the Ksp ,lower is the solubility  So, Cu(OH)2 has lower solubility.…

Q: Calculate the pH at the midpoint and at the equivalence point of the titration of 25.00 mL of 0.200…

A: The reaction of formic acid and sodium hydroxide can be shown as follows-

Q: An indicator (Ka = 1.7X10-6) is red but changes to blue when ionized. The indicator was used in the…

A: The pH range of the indicator is 4.77 - 6.77. So the correct option is option E.

Q: Consider the following titrations: i. 100.0 mL of 0.10 M HCl titrated by 0.10 M NaOH ii. 100.0 mL of…

A:

Q: 0-5 ) with 0.100 M NaOH. b. 0.0527 M solution of NH4Cl (Kb = 1.80 x 10-5) with 0.100 M NaOH. c.…

A: Here, the solution has titre which is analyses using the phenolphthalein. The range is pH 9.3 to…

Q: . Draw the titration curve you would expect to observe for the titration of 100 mL of 0.1 M C6H5COOH…

A: The question is based on the concept of titration. we are taking a weak acid benzoic acid with a…

Q: 1.2 (i) pH Volume (mL) of 0.1 M NaOH m Above is the titration curve of a weak acid (200 mM acetic…

A:

Q: Determine the pH during the titration of 39.6 mL of 0.226 M trimethylamine ((CH3)3N, Kp = 6.3x10-5)…

A: Since you have asked a question with multiples of parts we will answer only 1st 3 subparts for you.…

Q: What is the acid component and base component of the buffer solution? What are the moles of each…

A: Since you have asked a question with multiple subparts, we will answer only first 3 subparts for…

Q: Suppose you want to do a physiological experiment that calls for a pH 6.50 buffer. You find that the…

A:

Q: Shown below is the titration curve for the titration of 25 mL of 1.0 M aspirin (pK, = 3.5) with 1.0…

A: The titration curve given is,

Q: OOOO A 100.0-mL aliquot of 0.100 M diprotic acid H2A (pK1 =4.00, pK2 = 8.00) was titrated with 1.00…

A: The given acid is diprotic acid but at the first equivalent point, an equal mole of the acid reacts…

Q: Generate a titration curve for 25.0 mL of 0.7233 M H3PO4, with 1.256 M NaOH as the titrant, given…

A: The titration curve for the titration of 25.0 mL of 0.7233 M H3PO4 versus 1.256 M NaOH solution is…

Q: The following titration curve is expected from which acid-base pair? Equivalence Point pH > 7 pH…

A: To determine acid base pair , we would use pH at equivalence point and trend of curve.

Q: Generate a titration curve for 25.0 mL of 0.7233 M H;POs, with 1.256 M NAOH as the titrant, given…

A: The titration curve for the titration of 25.0 mL of 0.7233 M H3PO4 versus 1.256 M NaOH solution is…

Q: Let HA represent a weak acid. A 27.5 mL sample of 0.20 M HA was titrated with 0.25 M NaOH. The…

A:

Q: Find the pH of the solution obtained when 2.2 x 10-2 L of 6.3 x 10-2 M benzylamine, C7H7NH2, is…

A: At the equivalence point mole of acid = mole of the base. The reaction involved is as follows:

Q: Which of the following indicators would be the best to use when 0.050 M benzoic acid (Ka = 6.6 ×…

A: Benzoic acid reacts with NaOH to form sodium benzoate. C6H5COOH + NaOH ----> C6H5COONa +H2O…

Q: t the equivalence point of 25 mL hypobromous acid HBrO titrated with 54 ml of 0.132 M potassium…

A: We know that: At equivalence point, Moles of acid = Moles of base. Moles of base (KOH) added = (54…

Q: In order to determine the Ka of a weak, monoprotic acid, a student measured the pH of a solution of…

A:

Q: 2 Shown below is the pH curve for the titration of 0.30 M ethylamine (C,H&NH2(aq)) with 0.30 M…

A:

Q: Use an Excel spreadsheet to generate a titration curve for 50.00 ml. of 0.0200 M acetic acid (K, =…

A: The balanced chemical equation for the reaction between acetic acid and ammonia is:…

Q: A 50.0 ml of acidic solute (Ka = 2.6 x 10-2) is titrated with a 25.0 mL of %3D 0.001 M NAOH…

A: Given: Ka of acid solute = 2.6 X 10-2  Volume of acid solution = 50.0 mL = 0.050 L…

Q: A 50.0 mL of acidic solute (Ka = 2.6 x 10-2) is titrated with a 25.0 mL of 0.001 M NaOH solution.…

A: Since you have posted multiple questions, we are entitled to answer the first only.

Q: A chemist generates the titration curve shown by slowly 12 adding 1.0 M sodium hydroxide (NaOH) to…

A: Ka is the acid dissociation constant for weak acid like acetic acid. When Ka is taken -log value ,…

Q: A 65.20-mL sample of a 0.251 M solution of acetic acid (HC2H3O2) which is a weak acid with an acid…

A: At equivalence point acid is completely neutralized by base and salt formed is undergoing…

Q: 4. In the titration of15.00 mL of 0.200 M HC with 0.100 M NaOH, calculate the pH after the addition…

A:

Q: Suppose that you want to titrate a sample of vinegar with standard sodium hydroxide solution to…

A: For titration of weak acid ( Vinegar ) and Strong base ( Sodium hydroxide ) suitable indicator is…

Q: Which acid-base titration would yield a titration curve of the general form shown?       H2SO4…

A:

Q: 9. Phenolphthalein, a colorless weak acid (K₂= 6.31 x 10-10) which dissociates in water forming pink…

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

Q: 9.25 mL of 0.125 potassium hydroxide was titrated with 0.10 M carbonic acid. Calculate the pH after…

A: pH is defined as the negative logarithm of hydrogen ion concentration present in the solution. pH =…

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.