a solution was prepared by dissolving 25.0 grams of ethanoic acid CH3COOH with 15 grams of sodium ethanoate CH3COONa in a volume of 750 ml. The dissociation constant of ethanoic acid is 1.8 × 10-⁵. Find the pH of the solution

a solution was prepared by dissolving 25.0 grams of ethanoic acid CH3COOH with 15 grams of sodium ethanoate CH3COONa in a volume of 750 ml. The dissociation constant of ethanoic acid is 1.8 × 10-⁵. Find the pH of the solution

Chemistry: The Molecular Science

5th Edition

ISBN:9781285199047

Author:John W. Moore, Conrad L. Stanitski

Publisher:John W. Moore, Conrad L. Stanitski

Chapter14: Acids And Bases

Section: Chapter Questions

Problem 66QRT: Complete each of these reactions by filling in the blanks. Predict whether each reaction is...

See similar textbooks

Related questions

Q: What is the pH of a solution that contains 0.12 M HC2H3O2 and 0.29 M C2H3O2? Use Kb = 5.6 x 10-10…

Q: What is the pH in the titration of 100 ml of a 0.030 M solution of NH3 with 21.00 ml of 0.150 M HCl?…

A: Given: Kb for NH3 = 1.8×10-5 [HCl] = 0.150 M [NH3] = 0.030 M

Q: Consider the titration of 20.0 mL of a sample of 0.105 M HC2H3O2 with 0.125M NaOH. (Ka = 1.8 x 10-5)…

Q: Find the pH during the titration of 20.00 mL of 0.1000 M butanoic acid, CH;CH,CH,COOH (K, = 1.54 x…

A: Moles of butanoic acid = Molarity × Volume = 0.1 M × 20 ml = 2…

Q: Calculate the pH of a solution made by dissolving 26.5 g potassium acetate in 150 mL solution.…

A: We have to calculate the pH of solution.

Q: Calculate the pH of a solution containing 0.75 M lactic acid (ka = 1.4 x 10-4) and 0.25 M sodium…

A: pKa = -log Ka pKa = - log (1.4 x 10-4 ) = 3.85 pH of an acidic buffer solution: pH = pKa + log…

Q: In titrating 10 ml of 0.1 M neutral amino acid (pKal= 2, pKa2 = 8),the pH after the addition of 5 ml…

Q: Consider a titration of formic acid (HCOOH, Ka = 1.8 x 10-4) with KOH in water. If 40.00 mL of the…

A: according to Henderson–Hasselbalch equation,…

Q: Calculate the pH during the titration of 30.00 mL of 0.1000 M KOH with 0.1000 M HBr solution after…

A: (a)

Q: A 0.100 M HNO3 solution is used to titrate 50.0 mL of 0.100 M trimethylamine ((CH3)3N, Kb = 7.4 x…

A: The reaction of weak base and nitric acid is: At equivalence point the entire base will be…

Q: Which of the following titration systems will have the largest ApH at the equivalence point region?…

A: In acid-base titration is an example of neutralization reaction, so the pH at equivalence point is…

Q: Calculate the ph of a solution made by adding 0.40g of NaOH to 100 cm^3 of 0.4 mol/dm^3 ethanoic…

A: given, the weight of NaOH = 0.40g volume of ethanoic acid = 100 cm3 = 0.1 dm3 concentration of…

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

Q: Find the pH during the titration of 20.00 mL of 0.1000 M triethylamine, (CH3CH)3N (K, = 5.2 x 104),…

A: Since there are multiple questions, we will answer only the first one. If you require the answers to…

Q: Calculate the pH during the titration of 30.00 mL of 0.1000 M KOH with 0.1000 M HBr solution after…

Q: What is the pH of a 3.1 M OCI", hypochlorite, solution with a dissociation constant of K =9.1 x…

Q: A Mohr titration of NaCl is done at pH 2. Is there a positive error, negative error, no effect, or…

A: A question based on general chemistry that is to be accomplished.

Q: Calculate the pH if 0.30M Acetic Acid, with Ka 1.8 x 10-5 is added to 0.20M Sodium Acetate.

Q: 9-3. Neglecting activity coefficients, calculate the pH of 5.0 x 10-8 M HCIO4. What fraction of H+…

Q: Calculate the pH during the titration of 30.00 mL of 0.1000 M ammonia with 0.1000 M HCl(aq) after…

A: Given: Molarity of ammonia = 0.100 M Volume of ammonia = 30.00 mL Volume of HCl= 12.46 mL Molarity…

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: What is the pH of the solution at the end of the titration? The pH is very near or equal to 7. The…

A: Since the curve is moving from basic zone to acidic zone as shown in the curve And the pH values…

Q: In the titration of 50.0 mL 0.20 M acetic acid with 0.40 M NaOH, what is the pH of the solution…

Q: 10. Calculate the pH at the equivalence point for the following titration: 0.20 M HC1 versus 0.20 M…

A: Weak base (WB) and its salt with strong acid will acts as like basic buffer Basic buffer pH can…

Q: A 0.100 M HNO3 solution is used to titrate 50.0 mL of 0.100 M trimethylamine ((CH3)3N, Kb = 7.4 x…

A: Given that, The molarity of HNO3 solution =0.100 M , Molarity of trimethylamine (CH3)3N =0.100 M,…

Q: Calculate the pH during the titration of 25.0 mL of 0.100 M NH3 after the addition of 25.0 mL of…

A: NH3 + HClà NH4Cl PKa = log 5.7 x 10-10 = log 5.7 x 10-10 =9.25 We know on adding NH3 with HCl, NH4+…

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: Determine the pH of an equimolar buffer of ammonia and its conjugate base ion. (NH3; Kb = 1.8 x…

A: Solutions which are resisits it pH by addition of strong acid or base are called buffer solutions…

Q: Number 2

A: Buffer solution:A solution which can resist its pH when small amount of acid and base is added to…

Q: In the titration of 50.0 mL 0.20 M acetic acid with 0.40 M NaOH, what is the pH of the solution…

A: Given information is as follows; Volume of acetic acid = 50.0 mL = 0.05 L Molarity of acetic acid =…

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 titration 35.0mL of 0.250M methylamine CH NH2 and 0.200 M HNO3. K. = 5.9 x 104 a.…

A: Whenver an acid and base reacts with each other than they form salt and water and the process is…

Q: 2. Calculate the pH after the addition of 0.00 mL, 15.0 mL, 50.0 mL, and 60.0 mL of 0.100 M HCl in…

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

Q: Calculate the pH of an acetic acid solution (initial concentration 0.01 M, Ka = 1.8 x 10-5) and the…

A: i) CH3COOH dissociates as follows: CH3COOH⇋CH3COO-+H+Initial 0.01…

Q: The hydronium ion concentration in pure water at some temperature other than 25 °C is 2.43 x 10-6.…

Q: ritration of 100.0mL 0.1ONH 3 with 1on- 0.10M HN0 3. what is the pH afteR 50.0mL oL O.10M HNO

A: titration is the process through which we can calculate the concentration of the unknown solution…

Q: If the concentration of the weak base ammonia is 0.10 M and it is titrated with 0.1 M HCl, and the…

A: Calculation of pH of ammonia solution

Q: Add 20 cm3 of 0.4 M sodium-formate solution to 20 cm3 of 0.6 M formic acid solution. What is the pH…

A: Value of pH is used to measure the acidity or basicity of a solution. At room temperature, value of…

Q: A 0.100 M HNO3 solution is used to titrate 50.0 mL of 0.100 M trimethylamine ((CH3)3N, Kb = 7.4 x…

Q: 7. Calculate the pH during the titration of 20.00 mL of 0.1000 M CH3COOH with 0.2000 M NaOH solution…

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

Q: What is a 3 point pH calibration in Titration? How is it useful?

Q: Q.3: Determine the pH of the dissociation of 0.1 M HCN (ag). For which the dissociation constant is…

A: Given information: Concentration of HCN = 0.1 M Dissociation constant = 4.9×10-5 Mass of conjugate…

Q: Q 1(h) Which buffer system will have the greatest buffer capacity at pH 5.5? Acetic acid/sodium…

A: h) Buffer capacity is more when it's pKa is nearer to its pH. pH = -log(H+) and pKa= - log (Ka)…

Q: Calculate the pH for each case in the titration of 50.0 mL of 0.110 M HClO(aq)0.110 M HClO(aq) with…

A: the given data: Ka=4×10-8 50ml of 0.110 M HClO 0.11 M KOH The volume of HClO is 50ml=0.050 litre…

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

Q: Calculate the pH if 0.30M Acetic Acid, with Ka = 1.8 x 10-5 is added to 0.20M Sodium Acetate.

Q: Calculate the pH and [H3O+] of a solutio n prepared by dissolving 0.25 mol of NaC2H3O2 in 500. mL of…

A: For a buffer solution: pH = pKa + log[salt]/[acid]

Q: What is the molar ratio of CH;COOH to CH3COONA that should be used in order to prepare an acetic…

A: Given-> pH = 4.00 Ka(CH3COOH) = 1.8 × 10-5

Q: 3.5 x 10-8) What is the pH at the equivalence point in the titration of 100.0 mL of 0.0500 M HOCI…

Question

100%

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

calculation

VIEW

result

VIEW

Trending now

This is a popular solution!

Step by step

Solved in 2 steps with 1 images

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

Complete each of these reactions by filling in the blanks. Predict whether each reaction is product-favored or reactant-favored, and explain your reasoning. (a) _________ (aq) + Br(aq) NH3(aq) + HBr(aq) (b) CH3COOH(aq) + CN(aq) ________ (aq) + HCN(aq) (c) ________ (aq)+H2O () NH3(aq) + OH(aq)
You are given four different aqueous solutions and told that they each contain NaOH, Na2CO3, NaHCO3, or a mixture of these solutes. You do some experiments and gather these data about the samples. Sample A: Phenolphthalein is colorless in the solution. Sample B: The sample was titrated with HCl until the pink color of phenolphthalein disappeared, then methyl orange was added. The solution became pink. Methyl orange changes color from pH 3.01 (red) to pH 4.4 (orange). Sample C: Equal volumes of the sample were titrated with standardized acid. Using phenolphthalein as an indicator required 15.26 mL of standardized acid to change the phenolphthalein color. The other sample required 17.90 mL for a color change using methyl orange as the indicator. Sample D: Two equal volumes of the sample were titrated with standardized HCl. Using phenolphthalein as the indicator, it took 15.00 mL of acid to reach the equivalence point; using methyl orange as the indicator required 30.00 mL HCl to achieve neutralization. Identify the solute in each of the solutions.
You prepared 500 mL buffer solution that contains 0.50 moles monoprotic weak acid (HA) and 0.30 moles conjugate base (NaA). The solution has a pH of 4.20. (a) What is the Kp of the conjugate base, NaA? (b) What is the pH of the buffer solution after adding 400 mL of 0.30 M H,SO4? pH = pKa – log(THA), [A*]
In the titration of 25.00 mL of a water sample, it took 20.590 mL of 3.150x 10−3 M EDTA solution to reach the endpoint. The total hardness is due to one or a combination of Ca2+, Mg2+, and Fe2+ in your sample. It is convenient to express this hardness as though it was entirely due to Ca2+. Making this assumption, determine the number of moles of Ca2+ present in the bottled water sample titrated. (enter your answer with 3 significant figures)
In a titration experiment, 15.0 mL of 0.15 M Ba(OH)2 is required to titrate a 20.0 mL of an unknown solution of HNO3. Calculate the concentration of the HNO3 solution using the data. 2HNO3 + Ba(OH)2 → Ba(NO3)2 + 2H2O
A student titrates 20.0 mL of 1.84 M HCl with a weak base (Kb = 2.33 x 10−6). The weak base and HCl react in a 1:1 ratio. A buffer is created using 100 mL of the weak base and 100 mL of 1.35 M salt containing the conjugate acid. Determine the pH of the buffer.
A solution (50.00 mL) of citric acid (a weak acid with concentration 0.0950 M and Ka = 1.8 × 10−5) was titrated with 0.0848 M NaOH. What was the pH after 27.00 mL of NaOH had been added?
Consider the titration of 25.0 mL of 0.125 M acetic acid (CH, COOH, pKa = 4.75) with 0.102 M NaOH. CH, COОН(aq)+NaOH(aq) — СH, СОО" (аq) + H,О1) + Na*(aq) Determine the initial pH of the 0.125 M acetic acid solution before NaOH is added. pH = Determine the pH of the solution after 10.0 mL of 0.102 M NaOH is added. pH = Determine the volume of 0.102 M NaOH required to reach halfway to the stoichiometric point of the titration.
You have a 18 mL sample of acetylcholine (a neurotransmitter) with an unknown concentration and a pH of 8.35. You incubate this sample with the enzyme acetylcholinesterase to convert all of the acetylcholine to choline and acetic acid. The acetic acid dissociates to yield acetate and hydrogen ions. At the end of the incubation period, you measure the pH again and find that it has decreased to 6.03. Assuming there was no buffer in the assay mixture, determine the number of nanomoles of acetylcholine in the original 18 mL sample.
You have a 18 mL sample of acetylcholine (a neurotransmitter) with an unknown concentration and a pH of 7.82. You incubate this sample with the enzyme acetylcholinesterase to convert all of the acetylcholine to choline and acetic acid. The acetic acid dissociates to yield acetate and hydrogen ions. At the end of the incubation period, you measure the pH again and find that it has decreased to 5.66. Assuming there was no buffer in the assay mixture, determine the number of nanomoles of acetylcholine in the original 18 mL sample. Tip: your answer should have two significant digits! Only the mantissa (the digits to the right of the decimal) are significant when you raise a decimal number to a power. CH,—C−O−CH,—CH,—*N—CH, Acetylcholine CH 3 acetycholine in original sample: CH3 H₂O CH3 HO–CH,—CH,—*N–CH, + CH, Choline CH3 CH, T Acetate O + H+ nmol
The concentration of acetylcholine (a neurotransmitter) in a sample can be determined from the pH changes that accompany its hydrolysis. When the sample is incubated with the enzyme acetylcholinesterase, acetylcholine is converted to choline and acetic acid, which dissociates to yield acetate and a hydrogen ion. CНз CHз Нао — сHz— CH "N— снз но-сн— сH,-"N-CH; + CH;— с-о+ н* CH3-C-0- сHз CHз Choline Acetylcholine Acetate In a typical analysis, 11 mL of an aqueous solution containing an unknown amount of acetylcholine had a pH of 7.70. When incubated with acetylcholinesterase, the pH of the solution decreased to 6.89. Assuming there was no buffer in the assay mixture, determine the number of moles of acetylcholine in the 11 mL sample.
The titration of 100.mL of 0.100 M NH3 (in the flask) with 0.200 M HCL (in the burette) was carried out. Calculate the pH solutions at the following volumes of HCL added