In a titration 2.7 cm33 of 0.100 mol dm−3−3 sodium hydroxide, NaOH solution is added to 25.0 cm33 of 0.125 mol dm−3−3 benzoic acid, C66H55COOH, solution. Calculate the pH of the resulting solution given that the pKa of benzoic acid is 4.19.

In a titration 2.7 cm33 of 0.100 mol dm−3−3 sodium hydroxide, NaOH solution is added to 25.0 cm33 of 0.125 mol dm−3−3 benzoic acid, C66H55COOH, solution. Calculate the pH of the resulting solution given that the pKa of benzoic acid is 4.19.

Chemistry & Chemical Reactivity

9th Edition

ISBN:9781133949640

Author:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel

Publisher:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel

Chapter16: Principles Of Chemical Reactivity: The Chemistry Of Acids And Bases

Section: Chapter Questions

Problem 106GQ: The hydrogen phthalate ion, C8HsO4, is a weak acid with Ka = 3.91 106....

See similar textbooks

Related questions

Q: The weak base NH3 (concentration 0,10 mol∙dm–3) is titrated with strong acid HCl (concentration…

A: The quantitative chemical reaction of an acid and a base with each other is known as neutralization…

Q: A 0.3654 g portion of pure formic acid (CH2O2, FW=46.03 g/mol, Ka=1.77 x 10-4) is dissolved in 50.00…

A: Given that, Mass of formic acid = 0.3654 g Molecular mass of formic acid = 46.03 g/mol Volume of…

Q: Calculate the pH and [H3O+] of a buffer solution prepared by dissolving 0.218 mol of NaC2H3O2 in…

A: In this case, the buffer solution is maintained between a weak acid (CH3COOH) and its conjugate ion.…

Q: At temperature 25°C, 0.02 M hydrazine, N2H4 solution is 0.69% ionised. Calculate the i.…

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

Q: Calculate the pH in the titration of 50.00ml of 0.060 M of benzoic acid with a 0.120 M sodium…

A: Given:Titration of 50.00 mL of 0.060 M benzoic acid with 0.120 M sodium hydroxide.Consider benzoic…

Q: The pk, for the acid dissociation reaction of bicarbonate is 10.33. HCO3 (aq) + H2O(1) 2 CO32-(aq) +…

Q: What is the pH of a buffer solution containing 1.25 M NH₃ and 0.75 M NH₄NO₃? Note that the base…

Q: A buffer solution contains 0.753 M KClO2 (Ka = 1.1 x 10-2) and 0.659 M HClO2. If 0.244 moles of NaOH…

Q: 8. What is the pH in the preceding problem if the mixture consists of 0.1 M acetic acid and 0.25 M…

A: The acidity of a solution is expressed in pH scale and is furnished in terms of hydrogen ion…

Q: You are studying an unusual enzyme that produces hydronium ions (H3O+) during the course of the…

A: This question is from ionic equilibrium. We will figure out it answer with proper explanation.

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: What is the pH of a buffer that results when 5.46 mole of H3PO4 is mixed with 2.97 mole of NaOH and…

A: · Moles of H3PO4 = 5.46 mol· Moles NaOH = 2.97 mol· Volume of solution = 1.00 L· Ka1 = 7.5 × 10–3

Q: Which

A: Those solution when resist to change the pH when small amount of acid or base added on it's then…

Q: A student has a sea water sample which contains Ca 2+ ions . Describe briefly how he will determine…

A: The seawater is hard water and contains calcium and magnesium ions. These calcium ions can be…

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: value

A: According to the question, oxalic acid is treated with sodium hydroxide. The reaction equation is…

Q: (0.025 +0.0258) = 7-14×10" = x², 01.0492 3. If 50.00 mL of 1.00 M HC₂H₂O₂ (K = 1.8 x 105) is…

A: a.) When 0.00 mL base is added , we only have acid , so using Ka and concentration we can calculate…

Q: (iii) 5.0, 25.0, 50.0 and 100.0 g aliquots of MgCl2 were dissolved in 4 separate 250 ml samples of…

A: Reaction of MgCl2 with water: MgCl2 + H2O → MgO + 2 HCl

Q: Find the pH of a solution produced by the reaction of 250 mL 0.1 M NaOH and 150 mL 0.03 M acetic…

A: Gvien, 250 mL 0.1 M NaOH and 150 mL 0.03 M acetic CH3COOH

Q: A mixture of ascorbic acid (CH706H, K2 = 6.8 X 105) and sodium ascorbate is prepared such that…

Q: Question attached

A: Given, [C5H5N] = 0.170 M Volume = 25.0 mL = 0.025 L [HBr] = 0.170 M pH = ?

Q: Calculate the pH in the titration of 20 mL of o.5M Acetic acid solution (CH3COOH) by 0.5M NaOH…

A: Since the volume of NaOH added is 0 mL hence the solution has only acetic acid Assuming that y…

Q: Which of the following 1:1 mixtures would be best suited to form a buffer closest to a pH of 3.70?

A: In order to prepare a buffer closest to a pH value of 3.70, the buffering range of the resulting…

Q: mixture of solid chloride salts known to contain only some of the cations of Experiment 12 is…

A: Precipitation is process transforming a dissolved substance into an insoluble solid. The…

Q: A buffer solution contains 0.10M benzoic acid (C6H5COOH, Ka= 6.3 x 105) and 0.10M potassium benzoate…

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

Q: Find the pH of a solution produced by the reaction of 250mL 0.1 M NaOH and 150mL 0.03 M acetic…

A: PH of the solution can be calculated as follows

Q: Calculate the ratio of pyridine (C3H,N) to it's conjugate acid, the Pyridinium ion (C3H,NH"), CHN in…

Q: The pKa of lactic acid is 3.86. You have a mixture of lactic acid and sodium lactate, where the…

Q: One drop, 0.200 cm3, of 1.00 mol dm-3 of aqueous sodium hydroxide, NaOH, solution is added to 25.0…

Q: Calculate the molar solubility of Ca(OH), in a solution buffered at pH = 11.0, if the solubility…

A: Given, Ca(OH)2 solution. pH of the solution is: 11.0 Ksp of Ca(OH)2 is --- 8.0×10-6. What is the…

Q: Find the pH of a solution produced by the reaction of 250 mL 0.1 M NaOH and 150 mL 0.03 M acetic…

Q: Consider the list of acids and their pKa values to the right. What two compounds would be best to…

A: Buffers are effective when the pKa values are closest to pH.

Q: Tris(hydroxymethyl)aminomethane [(HOCH,)3CNH, Tris or THAM] is a weak base frequently used to…

A: It is an example of a basic buffer solution. Molar mass of THAM is 121 g/mol

Q: In order to determine the concentration of benzylamine (pKa = 9.33) in a urine sample, acid-base…

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

Q: Consider the titration of 40.0 ml of 0.200 M HClO4 by 0.100 M KOH. What is the pH after 80.0 ml of…

A: During the neutralization reaction base is added to the acid and depending in the concentration of…

Q: Is it possible to use phenolphthalein as indicator in the titration of a strong base with a strong…

A: Phenolphthalein is an acid-base indicator and shows a color change in the pH range: 8.3 to 10. In…

Q: What volume of 4.00 M HCL (aq) must be added to 10.0 mL of 2.00 M NH3 (aq) to obtain the solution…

Q: Calculate the pH of a 1.00L solution containing 0.52M sodium acetate and 0.48M acetic acid after the…

A: Given that, concentration of CH3COONa in 1 L solution = 0.52 M = 0.52 mole L-1 and concentration of…

Q: Determine the pH at the equivalence point for the titration of a 40.0 mL sample of 0.100 MHNO2 by…

A: Given: Concentration of HNO2 = 0.100 M Concentration of KOH = 0.200 M Volume of HNO2 = 40.0 mL pKa…

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: Please complete the calculation of the pH of the equivalence point below. Concentration of NaOH…

A: Aspirin is an organic compound containing carboxylic acid group. The chemical name of aspirin is…

Q: Calculate the pH during the titration of 20.00 mL of 0.1000 M ethylamine, C2H5NH2(aq), with 0.2000 M…

A: Volume of ethylamine = 20.00 mL Molarity of ethylamine = 0.100 M Molarity of nitric acid = 0.200 M…

Q: The half-equivalence point of a titration occurs half way to the equivalence point, where half of…

A: Given : 1. Moles of monoprotic acid = 0.540 mole 2. Ka = 1.7 × 10-5

Q: if the change in pH after addition of 1.0mL of 0.10N HCI is 0.09, what is the total buffer capacity…

A: Given-> Volume of HCl = 1.0 ml Normality = 0.10 N Change in pH = 0.09 Volume of solution = 20 ml…

Q: The weak base NH3 (concentration 0,10 mol∙dm–3) is titrated with strong acid HCl (concentration…

A: Given - Concentration of HCl = 0.050 mol/dm3 = M Concentration of NH3 = 0.10 mol / dm3 Volume of…

Q: Calculate the pH of a 0.26 M solution of a weak acid, AH, for instance CH3COOH, and 1.01 M of a…

Q: Determine the pH of a buffer solution containing 0.451 M benzoic acid (C6H5COOH) and 0.317 M sodium…

A: GivenC6H5COOH = 0.451 MC6H5COONa = 0.317 MKa = 6.3 * 10-5pKa = -log KapKa = -log (6.3 * 10-5)pKa =…

Q: Calculate the pH of a buffer solution prepared by mixing 25 mL 0.400 M butyric acid, HC4H7O2 and 35…

A: Buffer solution has prepared by mixing 25 ml acid and 35 ml its salt. Ka for acid is given . We…

Q: Consider the following buffer systems: H,CO3 HCO, + H+ pka = 6.4 %3D H2PO, + НРО + нt pКа 3D 7.2 HPO…

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

Question

Expert Solution

This question has been solved!

Explore an expertly crafted, step-by-step solution for a thorough understanding of key concepts.

This is a popular solution!

SEE SOLUTION Check out a sample Q&A here

Step 1

VIEW

Step 2

VIEW

Step 3

VIEW

Trending now

This is a popular solution!

Step by step

Solved in 3 steps

SEE SOLUTION Check out a sample Q&A here

Similar questions

The simplest amino acid is glycine, H2NCH2CO2H. The common feature of amino acids is that they contain the functional groups: an amine group, -NH2, and a carboxylic acid group, -CO2H. An amino acid can function as either an acid or a base. For glycine, the acid strength of the carboxyl group is about the same as that of acetic acid. CH3CO2H, and the base strength of the amino group is slightly greater than that of ammonia, NH3. (a) Write the Lewis structures of the ions that form when glycine is dissolved in 1 M HCl and in 1 M KOH. (b) Write the Lewis structure of glycine when this amino acid is dissolved in water. (Hint: Consider the relative base strengths of the -NH2 and -CO2- groups.)
Consider the titration of a 50.00 mL sample of 0.100 M ethylamine, C2H5NH2, with 0.100 M HCl (aq., 25 oC). The Kb C2H5NH2 = 6.41 x 10–4. What is the pH after 25.00 mL of HCl has been added?
Calculate the change in pH when 10.0 mL of 0.100 M NaOH(aq) is added to 100.0 mL of a buffer that is 0.100 M in CH3COOH(aq) and 0.100 M in CH3COO−(aq). Take pKa = 4.74 for CH3COOH(aq). My textbook gives a complicated solution and I'm looking for a simpler way to do this
Which statement describes the action of a buffer composed of acetic acid (CH3COOH) and sodium acetate (NaCH3COO)? How does a buffer resist change in pH upon addition of a strong acid? By titration, it is found that 73.3 mL of 0.189 M NaOH(aq) is needed to neutralize 25.0 mL of HCl(aq). Calculate the concentration of the HCl solution.
Which of the following pairs of solution would you use to prepare a buffer with pH = 7.45? (A) Acetic acid + sodium acetate; (CH3CO2H has Ka = 1.8 x 10–5) (B) Sodium dihydrogen phosphate + sodium hydrogen phosphate; (H2PO4– has Ka = 6.2 x 10–8) (C) Ammonium chloride + ammonia; (NH3 has Kb = 1.8 x 10–5) (D) Sodium hydrogen carbonate + sodium carbonate; (HCO3– has Ka = 5.6 x 10–11)
Calculate the change in pH when 8.00 mL of 0.100 M HCl(aq) is added to 100.0 mL of a buffer solution that is 0.100 M in NH3(aq) and 0.100 M in NH4Cl(aq). Consult the table of ionization constants as needed. Then, Calculate the change in pH when 8.00 mL of 0.100 M NaOH is added to the original buffer solution.
A solution is formed by adding 6.00 grams of solid potassium acetate, KC₂H₃O₂, to 200.0 ml of 0.0240M calcium acetate, Ca(C₂H₃O₂)₂. Calculate the pH of the resulting solution. You may assume that the potassium acetate dissolve completely and that the change in volume is negligible with the addition of the solid.
2.60 g of sodium acetate, CH3COONa was dissolved in 150.0 mL ofwater, H2O. A solution of 0.025 M ethanoic acid, CH3COOH was addedinto the above salt solution. Calculate the pH of the mixed solution.
One drop, 0.200 cm3, of 1.00 mol dm-3 of aqueous sodium hydroxide, NaOH, solution is added to 25.0 cm3 of a phosphate buffer that is 0.040 mol dm-3 in KH2PO4(aq) and 0.020 mol dm-3 in K2HPO4(aq). Calculate the resulting pH of the solution given that the second acid dissociation constant, pKa2, for phosphoric acid is 7.21.
Calculate the pH during the titration of 20.00 mL of 0.1000 M ethylamine, C2H5NH2(aq), with 0.2000 M HNO3(aq) after 7.24 mL of the acid have been added. Kb of ethylamine = 6.5 x 10-4.
Calculate the change in pH when 7.00 mL of 0.100 M HCI(aq) is added to 100.0 mL of a buffer solution that is 0.100 M in NH, (aq) and 0.100 M in NH CI(aq). Consult the table of ionization constants as needed. 壬 ApH = Calculate the change in pH when 7.00 mL of 0.100 M NaOH is added to the original buffer solution. ApH Question Source: McQuarrie, Rock, And Gallogly e Gan WhatsApp Image..jpeg
1 mL of 0.01 M NaOH and 1 mL of 0.01 M CH3COOH are mixed. What is the pH of the solution. Explain your observations