Calculate the value of the equilibrium constant for the balanced net ionic equation for the weak acid-strong base titration. OH-(aq) + CH3COOH (aq) -->CH3COO-(aq) + H2O(l) NaOH = 0.3060M and volume 19.85mL CH3COOH= 0.2429 and volume 25mL

Calculate the value of the equilibrium constant for the balanced net ionic equation for the weak acid-strong base titration. OH-(aq) + CH3COOH (aq) -->CH3COO-(aq) + H2O(l) NaOH = 0.3060M and volume 19.85mL CH3COOH= 0.2429 and volume 25mL

Chemistry: Principles and Practice

3rd Edition

ISBN:9780534420123

Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Publisher:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Chapter16: Reactions Between Acids And Bases

Section: Chapter Questions

Problem 16.54QE

See similar textbooks

Related questions

Q: Calculate the pH at the equivalence point for titrating0.200 M solutions of each of the following…

A: (a) Given, The concentration of NaOH solution is 0.200 M The concentration of HBr solution is 0.200…

Q: Determine the pH at the point in the titration of 40.0 mL of 0.200 M H2NNH2 with 0.100 M HNO3 after…

A: given values : Kb =3×10-6pKb=-log (3×10-6) =5.52 for weak base hydrazine : molarity = 0.2 M…

Q: Calculate the pH of the solution in the titration of 0.05M HBr with 40mL of 0.02M CsOH when the…

Q: Using a relevant ICE Table, calculate the expected pH of the solution when 5.99 mL of 0.200 M HCl…

A: Calculate the expected pH of the solution when 5.99 mL of 0.200 M HCl solution is added to the 50.0…

Q: One function of our blood is to carry CO2CO2 from our tissues to our lungs. It is critical that the…

Q: 2.1 The correct indicator was added to 25.00 mL of a 0.1340 M solution of pentanoic acid…

A: Pentanoic acid is a weak organic acid. Its Ka is 1.4 x 10-5. Its concentration is 0.1340 M and…

Q: A 245.0 mL sample of 0.15 M Ba(OH)2 is added to 438. mL of 0.20 M HNO3. What is the pH of the…

Q: Sodium benzoate, NaC6H5COO (molar mass 144.1 g mol-1) is a common food preservative. The Ka of…

A: Given data, Ka of Benzoic acid = 1.6 x 10-5 Molarity of HCl = 1.20 M Molar mass of sodium benzoate =…

Q: In the equation PbI2(s)------> Pb ^2+(aq)+2I^-(aq), calculate the molar solubility of PBI2, will be…

A: The solubility product constant, Ksp is the equilibrium constant for a solid substance dissolving in…

Q: 0.750 M KOH(aq) is added to a 100.0 mL 0.500 M CH3COOH/NaCH3COO buffer. What is the expected pH of…

A: Given pKa = 4.74 Molarity of Acid = 0.50 M Molarity of salt = 0.50 M Volume of buffer = 100 mL Mmol…

Q: Please complete the calculation of the pH of the equivalence point all numbers required are here…

A: given molarity of NaOH is 0.00180 the volume of NaOH is 17.95ml asprin molarity is 0.00180

Q: In order to standardize a solution of NaOH, 1.05 mL of NaOH is titrated with 0.100 M oxalic acid…

A: Given,Volume of NaOH = 1.05 mL = 1.05 × 10-3 L (1 mL = 10-3 L)Volume of H2C2O4 = 295 µL = 295 ×…

Q: Calculate the change in pH when 9.00 of 0.100 M HCl * (aq) is added to 100.0 of a buffer solution…

Q: You have75.0 mL of a 0.25M solution of a weak base, ethanol amine, HOC2H4NH2, with a kb= 2.8x10^-5.…

A: Given data:

Q: Please answer 1A, 1B, 1C, and 1D

A: Hello. Since your question has multiple sub-parts, we will solve first three sub-parts for you. If…

Q: HCl and Na2CO3 undergo a neutralization reaction. To neutralize the acid and base, 0.0144L of…

A: The reaction for neutralization between Na2CO3 and HCl is: Na2CO3 + 2 HCl → 2 NaCl + H2O + CO2…

Q: A solution of nitric acid, HNO2, at a concentration of 0.495M was found to be 1.83 = pH.

Q: Of the following solutions, which has the greatest buffering capacity? 0.821 M HC,H30,and 0.713 M…

A: Buffer capacity = 2.303 ( a × b )( a + b ) Buffer capacity is maximum for solution having maximum…

Q: in water as shown in the equation below. A 40.0 mL sample of an aqueous solution of benzoic acid…

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

Q: Twenty-five milliliters of 0.10 M HCl(aq) is titrated with 0.10 M NaOH(aq). What is the pH at…

A: The pH at the equivalence point has to be identified.

Q: ACID-BASE EQUILIBRIA Doc Jill wants to determine the Ao of a weak acid she isolated called…

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: Buffer capacity is a measure of a buffer solution's resistance to changes in pH as strong acid or…

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

Q: Benzoic acid, C6H5COOH, dissociates in water as shown in the equation below. A 40.0 mL sample of an…

A: Weak acid and strong base titration: The direct transfer of protons from the weak acid to the…

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: A buffered solution contains 0.50 M acetic acid (HC₂ H₂O₂. Ka 1.8 x 105) and 0.50 M sodium acetate…

A: We have to predict the new pH value after adding the base to buffer solution.

Q: 100.0 mL of a 0.200 M H3PO4(aq) solution is titrated with 325.0 mL of a 0.100 M NaOH(aq) solution.…

Q: You are titrating 10.00 mL 0.100 M H3PO4 with 0.100 M NaOH. At the point where you have added…

A: H3PO4 (aq) + Na+(aq) + OH- (aq) → Na+(aq) + H2PO4-(aq) + H2O…

Q: 16.75 mL of 0.100M H2SO4(aq) is placed in a beaker. After 17.65 mL of NaOH is added to the beaker,…

Q: ACID-BASE EQUILIBRIA Doc Jill wants to determine the Ao of a weak acid she isolated called…

A: Answer: When a weak acid is added into the water, its partial ionization takes place which causes…

Q: Calculate the pH for the complete titration of 100.0 mL of 0.122 M hydrazine, H2NNH2, with 0.200 M…

Q: B represents an acid-base indicator and behaves like a base. Its dissociation equilibrium in an…

Q: What is an acid–base indicator?

A: As per our guidelines, you have posted multiple questions we can only answer first one.

Q: Calculate the pH of a solution formed by adding 6.00 grams of solid sodium formate, NaCHO₂, to 200.0…

A: pH is the negative logarithm of hydrogen ions. pH values can be ranges from 0 to14. 0 is very acidic…

Q: CH,Cоон (аq) + NaOH (aq) ---сн,соONa (aq)+ H,0 () CH3CO0 (aq)+ H* (aq) + Na*(aq) + OH (aq)----CH3CO0…

A: The complete ionic reaction taking place is given as, => CH3COO- (aq) + H+ (aq) + Na+ (aq) + OH-…

Q: The pH of a 1.00 M NaCH3COO (aq) solution is 9.38. a) HCl (aq) is added to 1.00 L solution of 1.00…

A: The buffer solution is the solution that resists changes in the pH of the solution when a small…

Q: We dissolve 2.66 g of an unknown acid, HA, in enough water to produce 25.0 mL of solution. The pH of…

Q: ACID-BASE EQUILIBRIA Doc Jill wants to determine the Ao of a weak acid she isolated called…

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

Q: Calculate the ka value and the equilibrium constant for the balanced net ionic equation for the weak…

A: The net ionic equation for the given reaction is:

Q: The correct indicator was added to 25.00 ml of a 0.1345 M solution of propanoic acid (CH,CH;COOH)…

A: Propanoic acid is titrated with sodium hydroxide.

Q: In a titration, the equivalence point is the moment at which the number of moles of H+ from the acid…

A: Molarity gives the concentration of a solution. It gives the number of moles of the solute dissolved…

Q: HCN(aq)+H2O(l) ⇄ H3O+(aq)+CN−(aq) Ka=[H3O+][CN−] / [HCN]=6.2×10−10 The equilibrium…

Q: 2.1 The correct indicator was added to 25.00 mL of a 0.1345 M solution of propanoic acid…

A: Propanoic acid is titrated with sodium hydroxide.

Q: Which statement about acid-base indicators is not correct? * A- A weak acid can be used as an…

A: Acid-base indicators made of weak acids and weak bases. Due to common ion effect.

Q: You are asked to prepare a buffer solution with a pH of 3.50. The following solutions, all 0.100 M,…

A: A buffer works well in the pH range of (+/-)1 of the pKa of the weak acid used in the buffer. Closer…

Q: Write the balanced NET IONIC equation for the reaction that occurs when nitric acid and calcium…

A: Formula for Nitric acid is HNO3 Calcium hypochlorite is Ca(ClO)2

Q: For each buffer system, calcutate the amounts (volume of stock solution or mass of solid) necessary…

A: Given, 100 mL of 0.100 M of acetate buffer having pH 4.0 pKa of acetic acid = 4.74 Concentration of…

Q: A 50.0-mL solution of 0.100 M propanoic acid (HC3H5O2; Ka= 1.34 x 10–5) is titrated with 0.200 M…

A: Hii there, since there are multiple subparts posted. we are answering first three subparts. if you…

Concept explainers

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.

Question

Calculate the value of the equilibrium constant for the balanced net ionic equation for the weak acid-strong base titration.

OH^-_(aq) + CH₃COOH_(aq) -->CH₃COO^-_(aq)+ H₂O_(l)

NaOH = 0.3060M and volume 19.85mL

CH3COOH= 0.2429 and volume 25mL

Definition Definition Method of quantitative analysis for determining the concentration of an acid or base by exactly neutralizing it with a standard solution of base or acid having known concentration.

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

Trending now

This is a popular solution!

Step by step

Solved in 2 steps with 3 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

Calculate the ka value and the equilibrium constant for the balanced net ionic equation for the weak acid-strong base titration. OH-(aq) + CH3COOH (aq) -->CH3COO-(aq) + H2O(l) NaOH = 0.3060M and volume 19.85mL CH3COOH= 0.2429 and volume 25mL
A 50.0-mL solution of 0.100 M propanoic acid (HC3H5O2; Ka= 1.34 x 10–5) is titrated with 0.200 M NaOH solution. The net ionic equation for the reaction is as follows: HC3H5O2(aq) + OH–(aq) --> C3H5O2–(aq)+ H2O (a) What is the initial pH of the acid solution? (b) Calculate the pH of the resulting solution after each of the following amount of 0.200 M NaOH has been added, and the limiting reactant is completely reacted. (i) 10.0 mL of 0.200 M NaOH; (ii) 15.0 mL of 0.100 M NaOH; (iii) 20.0 mL of 0.100 M NaOH; (iv) 25.0 mL of 0.100 M NaOH; (v) 30.0 mL of 0.200 M NaOH
A 20.00 mL aliquot of lactic acid solution (HCH3H5O3) was titrated with 0.0980 M KOH(aq) using both an indicator and a pH meter. Ka (HCH3H5O3), is 1.38 x10-4. A total of 28.64 mL of 0.0980 M KOH(aq) was required to reach the equivalence point 1. Calculate the molarity of the lactic acid solution. 2. Calculate the pH of the lactic acid solution 3. Calculate the pH and [CH3H5O3-] at the half-equivalence point. 4. Calculate the pH at the equivalence point of the titration. 5. Suggest an appropriate indicator for titration. 6. Calculate the pH of the solution after 10.00 mL of 0.0980 M NaOH(aq) was added
You have75.0 mL of a 0.25M solution of a weak base, ethanol amine, HOC2H4NH2, with a kb= 2.8x10^-5. It is to be titrated with 0.50 M HCl. What is the pH of the resulting solutions after the following additions? (d) at the equivalence point (E) after 40 mL of HCl has been added (f) what indicator would you choose to signal the endpoint, and WHY?
A 23mL sample of HCl is titration to phenolphthalein end point with 26.43 mL of a 0.09181 M NaOH standard solution. Calculate the molar concentration of the HCl solution.
What will be the pH of the buffer solution consisting of 94 mL butanoic acid (CH3CH2CH2COOH) 0.189 mol/L and 109 mL sodium butanoate (CH3CH2CH2COONa) 0.207 mol/L, if 10.9 mL KOH 0.5 mol/L is added?Give an answer to at least 3 decimal places.
A solution of nitric acid, HNO2, at a concentration of 0.495M was found to be 1.83 = pH. Schematically plot the titration curve of 20.0 mL HNO2 0.0125MWhich is purged with NaOH 0.0125M while specifying the names of the axes. Marked on topThe curve the buffer area and the equivalent point. Detail the calculationsWhich led to the drawing of the curve.
13,8mL of 0,176M H3P04(aq) is titrated with 0,110M NaOH(aq). How much volume of the base is needed to reach the titration eqivalence point? H3PO4(aq) + 3 NaOH(aq) ---> Na3PO4 + 3 H2O(l)
CH3COOH + NaCH3COO 35mL total solution 0.29M acetic acid concentration after mixing 0.71M sodium acetate concentration after mixing Calculate the expected pH of this buffer solution
Consider the titration of 50.00 mL of 0.100 M benzoic acid (HC7H5O2, Ka = 6.3 × 10−5) (aq) with 0.130 M LiOH(aq). What is the pH of the titration solution... a) before any LiOH is added? b) after 20.00 mL of LiOH is added? c) at the equivalence point? Also, what volume of LiOH is required to reach this? d) For this titration, which is the best indicator to use: phenolphthalein, bromothymol blue, or methyl orange? Justify your answer.
a. Determine the volumes of 0.350 M Na2CO3 (aq) and 0.225M NaHCO3 (aq) that would be needed to prepare 500.00 mL of a buffer with a pH of 10.0? b. Calculate the new pH of the buffer described in part a, if 5.00mL of 1.50 M HCl (aq) were added to 120mL of the buffer? c. Would the resulting solution (from part b) still be considered a buffer? Yes or no, explain.
A 0.025 M solution of an unknown organic acid has a pH of 3.23. 2.1 By means of a full calculation, determine the value of the ionisation constant of the conjugatebase of this acid..- You may use “HA” to denote the formula of the acid.- You may make certain assumptions to simplify your calculations2.2 A certain amount of the sodium salt of the conjugate base of the acid was added to the system.Will the pH of the resulting solution increase or decrease, compared to the original given value? Explain your answer in a short sentence or two.