Calculate the pH of a buffer solution containing 10.0 cm³ of 0.100 mol dm-³ NaOH and 20.0 cm³ of 0.500 mol dm-³ ethanoic (acetic) acid made up to a total of 50.0 cm³ in a volumetric flask at 298 K. The pKa of ethanoic acid at 298 K is 4.77

Calculate the pH of a buffer solution containing 10.0 cm³ of 0.100 mol dm-³ NaOH and 20.0 cm³ of 0.500 mol dm-³ ethanoic (acetic) acid made up to a total of 50.0 cm³ in a volumetric flask at 298 K. The pKa of ethanoic acid at 298 K is 4.77

Principles of Modern Chemistry

8th Edition

ISBN:9781305079113

Author:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Publisher:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Chapter20: Molecular Spectroscopy And Photochemistry

Section: Chapter Questions

Problem 67CP

See similar textbooks

Related questions

Q: Calculate the pH of a buffer solution containing 10.0 cm3 of 0.100 mol dm–3 NaOH and 20.0 cm3 of…

Q: The pH of a 0.5L HNO2-NO2 buffer solution was determined to be 4.23. The solution was mixed with 5g…

A: Given, pH of buffer solution = 4.23 pKa = 4.35 Volume of buffer solution = 0.5 L weight of HNO2 = 5…

Q: Buffers that are based on 3-morpholinopropanesulfonicacid (MOPS) are often used in RNA analysis. The…

A: The pH range of the buffer solution is 6.5 to 7.9 The pKa value gives us the idea of the acidic…

Q: In solution, fentanyl is most stable in the pH range 3.5-7.5. What mass of acetic acid and sodium…

A: Solution- Data given- volume is 1 L, concentration is 30 mM, molecular mass (RMM) of acetic acid…

Q: what volume of 2.00 M NaOH should be added to 250.0 ml of 1.00 M glycolic acid(Ka = 1.48 x 104) to…

A: Given data: Molarity of NaOH = 2 M Molarity of glycolic acid = 1 M Volume of glycolic acid = 250 mL…

Q: The Henderson-Hasselbalch equation: a. relates the pH of a solution to the pKa and the…

Q: Determine the pH of (a) a 0.40 M CH3COOH solution and (b) a solution that is 0.40 M CH3COOH and 0.20…

A: a) CH3COOH dissociates in the solution as: CH3COOH⇌CH3COO-+H+Initial…

Q: You need to prepare 1L of 100 mM phosphate buffer at pH 7.1. What masses of monosodium phosphate…

A: Given: Total concentration of solute in buffer = 100 mM = 0.100 M Volume of buffer = 1 L And pH of…

Q: ACID-BASE EQUILIBRIA AND SALT EQUILIBRIA (COMMON-ION EFFECT, BUFFER AND SOLUBILITY EQUILIBRIA) A…

A: The mixture of Acetic acid and sodium acetate will form acidic buffer solution Give that…

Q: In this exercise, using the Henderson-Hasselbach equation, you will be asked to make the necessary…

A: Given: Volume of buffer solution = 100 mL pH of buffer solution = 9.02 Concentration of acid and…

Q: You are asked to prepare a buffer for an experiment. You have access to the following dolutions of…

Q: The dissociation constant, ka, of a weak acid is 5.9 x 10-6. What is the pKa of the acid?

Q: What is the pH and fraction of dissociation of a 0.100 M solution of the weak acid HA with Ka =1.00…

A: pH and fraction of dissociation of a 0.100 M solution of the weak acid HA with Ka =1.00 X10(-5) are…

Q: A 250 cm3 volumetric flask contains exactly 200,0 cm3 of a 0,025 mol.dm3 sulphuric acid solution.…

A: GIVEN Volume of sulphuric acid (H2SO4) =200.0 cm3 ( 1 Litre = 1000 cm3) = 0.200 L Concentration of…

Q: If K-2.35 & K,- 1.32 x 1010 Suppose 50ml of 0.010M aqueous amine is extracted with 100ml of benzene.…

A: Given: K = 2.35 Ka=1.32×10-10 Volume of aqueous amine = 50 mL Volume of benzene = 100 mL…

Q: Consider the titration of 50.00 ml of a solution of 0.2574 M of the fully protonated form of the…

A: Determine the number of moles. Number of moles of glycine = Molarity (M) × Volume (L)…

Q: A newly discovered extremely basic polar amino acid has pka values of 2.37, 13.01, and 11.89 for…

A: Here we are required to find the overall charge over amino acid at the given pH=13.01

Q: Calculation at the post-equivalence point region of a complexation titration: What is the pSr…

Q: A 31.6 mL aliquot of hypochlorous acid that has a concentration of 0.204 M will be titrated with…

A: To calculate pH, we would first Calculate moles of both acid and base . Then we would draw an ICE…

Q: You prepare a buffer solution from 10.0 mL of 0.100 M MOPS (3-morpholinopropane-1-sulfonic acid) and…

A: A buffer is a solution that can resist pH change upon the addition of an acid or base. It is able to…

Q: Malin just discovered a new protein, Malinase and for it not to unfold and lose its function, he…

A: Given the required pH of the buffer solution = 11.90 Volume of the buffer required = 50.0 mL Total…

Q: A standard solution contains 100 ppm of Fe, which was found to have an absorbance of 0.151 au at 508…

Q: "ooc-CH, H,C-coo EDTA is a hexaprotic system with the pK, values: pKa1 = 0.00, pK2 = 1.50, pK3 =…

Q: escribe the curve and why pH = pka at half equivalence point

A: pH is negative logarithm of Hydrogen ion concentration

Q: Propanoic acid, C₂H5COOH, is a weak acid, with Ka = 1.35 x 10-5 mol dm-³. i) Write an expression for…

Q: Calculate the pH of an acetate buffer that contains 0.0300 M CH3COOH and 0.0400 M CH3COO-. pKa =…

A: Henderson equation: pH = pKa + log[CH3COO-]/[CH3COOH]

Q: *D. Ksp = [Ag*]² · [SO4 1 %3D Ksp- pwidut/deacte.cauh una bulilor liguel. 2. If the gram solubility…

Q: The equilibrium constant for the dissolution of Mg (OH) 2: Kps = 5.6 x 10-12 What is the molar…

A: Given data,Ksp of Mg(OH)2=5.6×10-12

Q: You want to study the oxygen binding ability of hemoglobin at pH 7.4. You decide to use a phosphate…

A: Preparation of phosphate buffer

Q: Condition of permanganatometric titration of sodium oxalate includes: pH = 1 and heating of analyte…

A: Permanganatometric titration is a technique used in chemical quantitative analysis. It is a type of…

Q: Phenolphthalein (transition pH range 8.0-9.6) is very appropriate for the titration of KHP with…

A: Phenol saline which has an essential progress scope of a pH =8 guide gracious toward 9.6 would be…

Q: What is a 3 point calibration in titration?

A: Detail about 3 point calibration in titration is given below.

Q: Would the indicator bromocresol green, with a transition range of pH 3.8–5.4, ever be useful in the…

A: weak acid react with strong base, it give basic solution. So, the pH of the solution after…

Q: Why is the equilibrium between the acid NaH2PO4, and its conjugate base Na2HPO4, a suitable buffer…

A: When a solution is referred to as a weak acid or weak base, it means that the solution can undergo…

Q: A solution containing Mg2+ was buffered to pH 9.75 and titrated with EDTA. Eriochrome black T, with…

A: EBT is used as metal ion indicator.

Q: A standard solution contains 100 ppm of Fe, which was found to have an absorbance of 0.151 au at 508…

Q: Find the pH during the titration of 20.00 mL of 0.1000 Mtri-ethylamine, (CH₃CH₂)₃N…

A: Since we only answer up to 3 sub-parts, we’ll answer the first 3. Please resubmit the question and…

Q: Sketch a titration curve for the amino acid cysteine, and indicate the pKa values for all titratable…

A: Cysteine is a polar uncharged amino acid containing a thiol group (SH), which on reaction with thiol…

Q: Use the method of successive approximations to determine the pH and concentrations of H₂A, HA, and…

Q: Use the titration curve for the weak acid to calculate the pH of a 0.150 Msolution of that weak…

A: Solution: Equivalence point volume = Veq Half equivalence point volume = 1/2 Veq pH at half…

Q: Calculate the molar solubility of BaCO3in a 0.10 M solution of Na2CO3(aq). (Ksp(BaCO3) = 8.1 x 10-9)

A: The given reaction of BaCO3 - Now calculate the molar solubility of BaCO3 -

Q: The un-ionized form of the weak acid HA does not absorb in the visible region. When it ionizes, its…

A: A question based on equilibrium concept, which is to be accomplished.

Q: Inorganic Chemistry: Qualitative Analysis of Anions What is the importance or purpose of adding…

Q: A weak acid (HA) with a pKa of 4.0 has a distribution constant of 5.2 between an organic and aqueous…

A: The fraction of HA acid in the organic phase at pH 2 and 6 is calculated:

Q: The pH of a 4.0 × 10-3 mol dm-3 solution of weak base is 10.4. Calculate the Kb of the weak base.

A: A base is a chemical compound which takes a proton. Base which is not dissociated completely in a…

Q: Which of these compounds would be the best buffer at pH 5.0: formic acid (pKa = 3.8), acetic acid…

A: Given: The pH of the buffer solution = 5.0 The pKa of formic acid = 3.8 The pKa of acetic acid =…

Q: In this exercise, using the Henderson-Hasselbach equation, you will be asked to make the necessary…

A: Answer-a Henderson-hasslebalch equation is: pH=pKa+log[Base][Acid] if [Base]=[Acid}, then…

Q: DETERMINATION OF WATER HARDNESS BY EDTA TITRATION 1. Why is it needed to add a pH 10 buffer to the…

A: Interpretation : We have to tell it is need to add a pH 10 buffer to sample during EDTA titration…

Concept explainers

Precipitation Titration

Precipitation analysis is used to analyze drugs, and to measure the salt content in food and beverages. It is an important concept from the examination point of view many practical questions are asked on the topic. This topic is significant in the professional exams for both undergraduate and graduate courses, especially for

Question

Calculate the pH of a buffer solution containing 10.0 cm³ of 0.100 mol dm-3 NaOH and 20.0 cm³ of
0.500 mol dm³ ethanoic (acetic) acid made up to a total of 50.0 cm³ in a volumetric flask at 298 K.
The pKa of ethanoic acid at 298 K is 4.77
-3

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

Knowledge Booster

Learn more about

Need a deep-dive on the concept behind this application? Look no further. Learn more about this topic, chemistry and related others by exploring similar questions and additional content below.

Similar questions

What is the pH of a solution containing 1.316 mol L-1 of a weak acid with pKA = 7.47 and 0.521 mol L-1 of another weak acid with pKA = 4.23 ?
The value of Ksp for Mg3(AsO4)2 is 2.1 x 10-20. TheAsO43 - ion is derived from the weak acid H3AsO4 (pKa1 =2.22; pKa2 = 6.98; pKa3 = 11.50). (a) Calculate the molarsolubility of Mg3(AsO4)2 in water. (b) Calculate the pH of asaturated solution of Mg3(AsO4)2 in water.
How the pH at the equivalence point is determined by the species present; why the pH at the midpoint of the buffer region equals the pKa of the acid
During the course of the titration of a 20.0 ml of solution containing 0.1 M of NaOH and 0.08 M of hydrazine (NH2-NH2) (Ka = 1.05 x 10) by a 0.2 M standard perchloric acid (HC104) titrant, calculate the pH of the titration mixture after (a) 5.0 ml; (b) 10.0 ml; and (c) 15.0 ml of HC1O4 titrant is added.
A particular buffer has been made up at 25 °C to give a pH of 8.00 and is then warmed to 35 °C. The pH of the solution changes because the pKa of the acid used to make the buffer has changed. What is the pH of the buffer solution at this new temperature if it is known that the pKa of the acid at 25 °C is 8.14 and ΔpKa/ ΔT = -0.018 °C-1?
A hypothetical weak acid, HA, was combined with NaOH in the followingproportions: 0,20 mol HA, 0,08 mol NaOH. The mixture was diluted to a totalvolume of 1,0 L and the pH was found to be 4,80. a). What is the pKa of the acid?
Calculate the molar solubility of calcium oxalate in a solution that has been buffered so that its pH is constant and equal to 4.00. Data: Kps of CaC2O4 = 1.7x10 -9 ; Ka1 of H2C2O4 = 5.60x10-2 and Ka2 = 5.42x10-5 . Use systematic treatment.
At 15 °C, the solubility product of PbCrO4 is 1.69 × 10-14 mol2dm-6. (a) Write an expression for the solubility product of PbCrO4.(b) Calculate the solubility of PbCrO4.(c) On adding concentrated aqueous lead(II) nitrate dropwise to 0.010 moldm-3 potassium chromate (VI), what is the concentration of lead(II) ions when the first trace of precipitate appears?
Calculate the pH of a 0.05 mol dm-3 CH3COOH solution; the dissociation constant Ka for CH3COOH is 1.72 x 10-5 mol dm^-3 .
The following is list of weak acids and their pką values weak acid pKa benzoic acid 4.20 hydrogen citrate 6.40 hydrocyanic acid 9.31 hydrogen phosphate 12.38 Which would be the best buffer to use at pH 7 ? For benzoic acid, a 50:50 mixture of benzoic acid and its conjugate base, the benzoate ion, would have pH = The buffering capacity of a benzoic acid:benzoate buffer would be at pH = 7 A. 4.20 B. 6.40 C. 9.31 D. 12.38 E. benzoic acid F. hydrogen citrate G. hydrocyanic acid H. hydrogen phosphate I. good J. bad
pKa values are different in different solvents. For example, the pKa of hydrofluoric acid (HF) in water is 3.45, but the pKa of hydrofluoric acid in DMSO (dimethyl sulfoxide) is 15.0. Choose the best explanation for the difference
A buffer solution with a pH of 4,9, consists of 0,25 mol∙dm–3 acetic acid (HC2H3O2; Ka= 1,8 x 10–5) and 0,35 mol∙dm–3 potassium acetate (KC2H3O2). A small quantity (0,050 mol) of solid KOH is added to 1 dm3 of the buffer. This quantity is so small that it does not affect the volume of the buffer. Calculate the new pH of the buffer solution after the KOH has been added.