- 144/ Natural Sciences / Chemistry And Polymer Science / Chemizzes / Buffers en Titrasies | Buffers and TitrationsA 0.386 g sample of propanoic acid(CH3CH,COOH, K, = 1.3. x 10-5) was dissolvedto a final volume of 50.0 cm, This solutionunderwent titration with 0.32 M NaOH.Calculate the pH of solution at the equivalencepoint.%3Dfih-BiekPlease give the answer to 2 decimal places.GeplAnswer:Check

Given that, Weight of propanoic acid = 0.386 g Molar mass of propanoic acid = 74.08 g/mol Moles of…

A 0.386 g sample of propanoic acid (CH3CH,COOH, K, = 1.3. x 10) was dissolved to a final volume of 50.0 cm³ This solution underwent titration with 0.32 M NaOH. Calculate the pH of solution at the equivalence point. Please give the answer to 2 decimal places.

A 0.386 g sample of propanoic acid (CH3CH,COOH, K, = 1.3. x 10) was dissolved to a final volume of 50.0 cm³ This solution underwent titration with 0.32 M NaOH. Calculate the pH of solution at the equivalence point. Please give the answer to 2 decimal places.

Chemistry & Chemical Reactivity

10th Edition

ISBN:9781337399074

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

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

Chapter17: Principles Of Chemical Reactivity: Other Aspects Of Aqueous Equilibria

Section: Chapter Questions

Problem 31PS: Without doing detailed calculations, sketch the curve for the titration of 30.0 mL of 0.10 M NaOH...

See similar textbooks

Related questions

Q: 75.0 ml of 0.0200M Ca(OH)2 solution is combined with 100.0 ml of 0.0150M NaOH solution. Calculate…

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: Consider the titration of 40.0 mL of 0.200 HClO4 by 0.100 M KOH. Calculate the pH of the resulting…

A: Given that - Volume of HClO4 = 40.0 mL Molarity of HClO4 = 0.200 M Molarity of KOH = 0.100 M…

Q: Calculate the pH of a buffer solution prepared by dissolving 0.25 mol benzoic acid (CH,COOH) and…

Q: Question attached

A: The midpoint of titration is the point at which excess of titrant has been added to neutralize half…

Q: Calculate the pH at the stoichiometric point when 25 mL of 0.099 M nitric acid is titrated with 0.32…

A: A salt formed from a strong acid and a strong base is a neutral salt.

Q: Consider the titration of 100.0 mL of 0.100 M H2NNH2 by 0.200 M HN03. Calculate the pH of the…

Q: Suppose that a student is determining the total base content of an antacid tablet by performing a…

A: Given: Mass of tablet = 1.5312 g Mass of tablet dissolved = 0.3012 g Concentration of…

Q: Determine the pH of the solution by mixing 0.24 M CSH5N (pyridine) of 18.0 mL with 0.20 M HCI of…

A: Given Molarity of pyridine = 0.24 M volume = 18 ml Molarity of HCl = 0.20 M Volume = 15 ml

Q: 415 mL of 0.028 M hydroiodic acid is added to 656 mL of 0.056 M perchloric acid. Calculate the pH of…

A: Given acid s: hydroiodic acid (HI) : Concentration,M1 : 0.028 M Volume, V1: 415 mL perchloric acid…

Q: Determine the pH of a buffer solution that is a mixture containing 0.10M acetic acid and 0.050 M…

Q: When 30.00 mL of 0.1011 M HCl in 50 mL of deionized water is titrated against 0.09889 M NaOH, the pH…

A: The volume of 1 L is equal to 1000 mL. The number of moles of NaOH in 0.02 mL of 0.09889 M NaOH is…

Q: Estimate the mass of KHP (KHC8H4O4) that will require 20mL of 0.10M to reach the equivalence point…

Q: Derive and equation analogous to the Henderson-Hasselbalch equation but relating poH and pKb of a…

A: Henderson-Hasselbalch equation, Is an equation which shows the relationship between the pH and pOH…

Q: 2. The student wants to conduct the same titration with chloric (1) acid, HOCI. The acid…

A: Given: The acid constant of the chloric acid is Ka=3.2×10-8 To find, Here when the sodium hydroxide…

Q: 3) A) Calculate the pH of a buffer solution which contains the weak monoprotic acid, propanoic acid…

Q: A buffer solution is prepared by dissolving 1.50g each of benzoic acid (MM=122.1, Ka=6.3 x 10^-5),…

A: Given, Mass of benzoic acid (HC7H5O2) = 1.50g Molar mass of benzoic acid =122.1g/mol Mass of sodium…

Q: A mixture of ascorbic acid (C6H,06H, Ka = 6.8 x 105) and sodium ascorbate is prepared such that…

Q: Given: A magnesium hydroxide solution is prepared by adding 12.00 g of magnesium hydroxide to a…

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

Q: Using a relevant ICE Table, calculate the expected pH of the solution when 4.81 mL of 0.200 M NaOH…

A: ICE stands for initial concentration, change in concentration and equilibrium concentration. The…

Q: 2.) 175.0 ml of 0.00200M HNO3 solution is added to 400.0 ml of 2.50×10-4M HClO4 solution. Calculate…

A: The pH of a solution can be determined by the negative logarithm of hydrogen ion concentration. It…

Q: How to calculate the pH of a buffer solution 1) Calculate the pH of a solution prepared by…

Q: You add 19.00 mL of 0.800 M NaOH to 50.00 mL of pure water, and to this mixture you then add 7.00 mL…

Q: 1. The pH of a buffer solution containing 0.5 mole/litre of CH:COOH and 0.5 mole/litre CH.COONA has…

Q: C,HSCOOH (s) E→ CH&COO (aq) + H (aq) K, = 6.46 x 10 1. Benzoic acid, CoH,COOH, dissociates in water…

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

Q: 6. A Diprotic Acid: а. Write the sequential dissociation reactions for the acid H,CO, (aq). b.…

A: Acid dissociates into its conjugate base.

Q: Calculate the pH at the stoichiometric point when 25 mL of 0.10 M pyridine is titrated with 0.32 M…

A: Moles can be calculated by using following formula,Moles = Molarity × Volume

Q: Consider the titration of 50.0 mL of 0.10 M H3A (Ka1 5 5.0 3 10–4, Ka2 5 1.0 3 10–8, Ka3 5 1.0 3…

A: The question is based on the concept of titrations. we are titrating a weak acid with a strong base.…

Q: Consider the titration of 90.0 mL of .141 M Ba(OH)2 by .564 M HCl. Calculate the pH of the resulting…

A: In the given question we have to calculate the pH of Solution after adding acid of 11.0 mL and 27.0…

Q: x 10° if 21.65mL of the sat. calcium hydroxide solution was titrated with 14.82mL of The…

A: Given: Concentration of HCl = 0.041 M Volume of HCl required to titrate the saturate calcium…

Q: Consider the titration of 100.0 mL of 0.100 M acetic acid (Ka = 1.8 x 105). When 50.00 mL of 0.100 M…

A: Given data,Molarity of acetic acid=0.1MVolume of acetic acid=100mLMolarity of NaOH=0.1MVolume of…

Q: Calculate the pH at the equivalence point in titrating 1.06 M solution containing a weak acid, AH,…

Q: Consider the titration of 40.0 mL of 0.200 M HCIO4 by 0.100 M KOH. Calculate the pH of the resulting…

Q: You are given 250.0 mL of 0.100 M CH3CH2COOH (propionic acid, K, 1.35 x 10). Youd wish to adjust the…

A: pH is the proportion of hydrogen particle fixation in the solution. It is utilized to decide the…

Q: If you have 500 mL of a 0.10 M solution of the acid, what mass of the corresponding sodium salt of…

Q: What mass of sodium acetate, NACH3 CO2 , must be added to 1.00 L of 0.080 M acetic acid to give…

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 solution containing 23 mL of 1.54 M of a weak weak base B OH, like NH4OH, or…

Q: A 0.270 M solution of sodium formate, used in several fabric dyeing and printing processes, is…

A: Given: Concentration of HCOONa = 0.270 M Volume of HCOONa solution used = 75.0 mL. Concentration of…

Q: At each stage of the titration: A. Determine the amount (mol) of weak acid, weak base, and strong…

A: To determine the pH d) At equivalence point e) After adding 56.0 mL HI

Q: Acid Ka HF 6.7 x 10^-4 HC2H3O2 1.8 x 10^-5 A student…

A: At equivalence point, the number of moles of acetic acid will be equal to that of NaOH and whole…

Q: The pH of amino acid is adjusted to 1.5 prior to titration to make sure that the amino acid has a…

A: There are 20 naturally occurring amino acid. They contain one carboxylic group one amino group, an…

Q: Phenolphthalein, a colorless weak acid (K3 = 6.31 x 1010) which dissociates in water forming pink…

A: We are given a weak acid indicator phenolphthalein with Ka or Kin = 6.31*10-10.

Q: Calculate the pH of a buffer solution which contains the weak monoprotic acid, propanoic acid…

A: Given, Concentration of propanoic acid = [CH3CH2COOH] = 0.1 mol/L Concentration of sodium propanoate…

Q: 2.50 g of sodium acetate, CH3COONa was dissolved in 150.0 mL of water, H2O. A solution of 0.025 M…

A: Given Data: Mass of sodium acetate = 2.50 g Volume of sodium acetate = 150.0 mL…

Q: Determine the pH of the solution that results from mixing 0.100 mol of HCl with 0.400 mol of NH3.…

A: #(a): Moles of HCl taken = 0.100 mol Moles of NH3 taken = 0.400 mol

Question

- 144
/ Natural Sciences / Chemistry And Polymer Science / Chemi
zzes / Buffers en Titrasies | Buffers and Titrations
A 0.386 g sample of propanoic acid
(CH3CH,COOH, K, = 1.3. x 10-5) was dissolved
to a final volume of 50.0 cm, This solution
underwent titration with 0.32 M NaOH.
Calculate the pH of solution at the equivalence
point.
%3D
fi
h-
Bi
ek
Please give the answer to 2 decimal places.
Ge
pl
Answer:
Check

Expert Solution

This question has been solved!

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

SEE SOLUTION Check out a sample Q&A here

Step 1

VIEW

Step 2

VIEW

Step by step

Solved in 2 steps

SEE SOLUTION Check out a sample Q&A here

Similar questions

Without doing detailed calculations, sketch the curve for the titration of 30.0 mL of 0.10 M NaOH with 0.10 M HCl. Indicate the approximate pH at the beginning of the titration and at the equivalence point. What is the total solution volume at the equivalence point?
A 10.00-g sample of the ionic compound NaA, where A is the anion of a weak acid, was dissolved in enough water to make 100.0 mL of solution and was then titrated with 0.100 M HCl. After 500.0 mL HCl was added, the pH was 5.00. The experimenter found that 1.00 L of 0.100 M HCl was required to reach the stoichiometric point of the titration. a. What is the molar mass of NaA? b. Calculate the pH of the solution at the stoichiometric point of the titration.
Fifty cm3 of 1.000 M nitrous acid is titrated with 0.850 M NaOH. What is the pH of the solution (a) before any NaOH is added? (b) at half-neutralization? (c) at the equivalence point? (d) when 0.10 mL less than the volume of NaOH to reach the equivalence point is added? (e) when 0.10 mL more than the volume of NaOH to reach the equivalence point is added? (f) Use your data to construct a plot similar to that shown in Figure 14.10 (pH versus volume NaOH added).
Without doing detailed calculations, sketch the curve for the titration of 50 mL of 0.050 M pyridine, C6H5N (a weak base), with 0.10 M HCl. Indicate the approximate pH at the beginning of the titration and at the equivalence point. What is the total solution volume at the equivalence point?
Repeat the procedure in Exercise 61, but for the titration of 25.0 mL of 0.100 M NH3 (Kb = 1.8 105) with 0.100 M HCl.
The Handbook of Chemistry and Physics (http://openstaxcollege.org/l/16Handbook) gives solubilities of the following compounds in grams per 100 mL of water. Because these compounds are only slightly soluble, assume that the volume does not change on dissolution and calculate the solubility product for each. (a) BaSeO4, 0.0118 g/100 mL. (b) Ba(BrO3)2H2O, 0.30 g/100 mL. (c) NH4MgAsO46H2O, 0.033 g/100 mL. (d) La2(MoO4)3, 0.00179 g/100 mL
Figure 15-3 outlines the classic scheme for separating a mixture of insoluble chloride salts from one another. Explain the chemistry involved in the various steps of the figure.
When a drop (taken to be 0.20 cm3) of 1.0 M HCI(aq) is added to 25 cm3 of pure water, the resulting hydroniumion concentration rises to 0.0080 mol dm- 3 and so the pH changes from 7.0 t o 2.1, a big change. Now suppose the drop is added to 25 cm3 of an ethanoate buffer solution that is 0.040 MNaCH3CO2(aq) and 0.080 M CH3COOH(aq). What will be the change in pH?
The experimental Ksp of calcium hydroxide is _________ x 10-6 if 23.09mL of the sat. calcium hydroxide solution was titrated with 12.53mL of 0.049M HCl(aq), considering 4 as an exact value for the calculation?
A 0.4071-g sample of CaCO3 (MM: 100.09 g/mole) is transferred to a 500-mL volumetric flask, dissolved using a minimum of 6 M HCl, and diluted to volume. A 50.00-mL aliqout of this solution was mixed with 5 mL of a pH 10 NH3-NH4Cl buffer that contains a small amount of Mg2+--EDTA to adjust the pH to 10. After adding calmagite as an indicator, the solution is titrated with the EDTA, requiring 42.63 mL to reach the end point. Report the molar concentration of EDTA in the titrant. 9.543 x 10-3 M 5.748 x 10-3 M 3.266 x 10-4 M 1.018 x 10-4 M