24. What is the pH of a buffer solution containing 0.50 M acetic acid and 0.50 M sodium acetate? Theacid dissociation constant for acetic acid is equal to 1.8 x 105Hint: no dilution occurredc. 4.74d. 9.62a.5.11b. 4.3825. What is the pH of a buffer solution containing 1.25 M NH: and 0.78 M NH-NO:? The base dissociationconstant for ammonia is equal to 1.8 x 10-5a. 4.54b. 9.46C. 4.95d. 9.05

The PH of the buffer solution can be calculate by using below formula PH = Pka + log…

Answered: 4. What is the pH of a buffer solution…

4. What is the pH of a buffer solution containing 0.50M acetic acid and 0.50 M sodium acetate? The acid dissociation constant for acetic acid is equal to 1.8 x 105. Hint: no dilution occurred

Chemistry: The Molecular Science

5th Edition

ISBN:9781285199047

Author:John W. Moore, Conrad L. Stanitski

Publisher:John W. Moore, Conrad L. Stanitski

Chapter15: Additional Aqueous Equilibria

Section: Chapter Questions

Problem 93QRT: When 40.00 mL of a weak monoprotic acid solution is titrated with 0.100-M NaOH, the equivalence...

See similar textbooks

Related questions

Q: Determine the pH at the point in the titration of 40.0 ml. of 0.200 M HC.H.O. with 0.100 M Sr(OH),…

A: Answer:- Given 40ml of 0.200M HC4H7O2 With 10ml of 0.100M of Sr(OH)2 Ka of HC4H7O2 is 1.5 ×…

Q: Determine the pH during the titration of 26.8 mL of 0.447 M hypochlorous acid (K,= 3.5x10-8) by…

Q: Calculate the pH of the solution for every 0.1 ml of the titrant (from 0 mL to 30 mL) and generate a…

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

Q: How much 5.70 M NaOH must be added to 430.0 mL of a buffer that is 0.0180 M acetic acid and 0.0240 M…

A: Concentration of NaOH = 5.70 M Concentration of acetic acid = 0.0180 M Concentration of sodium…

Q: HCN] ka=4.0x10^-10 pka=10.32 An aqueous solution contains 0.447 M hydrocyanic acid. How many mL…

Q: A 60.00 mL sample of 0.075 M benzoic acid was titrated using 0.050 M KOH. What will the pH be at the…

A: The information about the H+ ions (hydrogen ions) is derived by the calculation of any certain…

Q: Calculate the pH during the titration of 40.00 mL of 0.1000 M HCl with 0.1000 M NaOH solution after…

A: Given : strong acid HCl with concentration = 0.1000 M and volume = 40.00 mL = 0.040 L…

Q: The next 9 questions are related to the titration of 20.00 mL of a 0.0750 M acetic acid solution…

A: The balanced equation for the given titration reaction is,

Q: A 20.0 mL sample of 0.150 M ethylamine is titrated with 0.0981 M HCI. You may want to reference…

Q: Calculate the pH during the titration of 20.0 mL of 0.10 M NaOH (Ka = 1.8 × 10-5) after the addition…

A: NaOH is actually a strong monoacidic base and doesn't need a Ka value. HCl is also a strong…

Q: Calculate the pH of 1.00 L of a buffer that is 1.00 M in acetic acid and 1.00 M in sodium acetate…

A: pKa value for acetic acid = 4.75

Q: 25 mL of 0.10 M acetic acid is titrated with 0.10 M NaOH. What is the pH after 30 ml of NaOH have…

Q: At a hydrogen ion concentration of 1.75 x 10-5 (pH = 4.76), what is the capacity of a buffer…

A: Given data Acid dissociation constant: Ka=1.75×10-5 hydrogen ion concentration: H+=1.75×10-5 M mole…

Q: What is the pH at the equivalence point when 0.100 M hydroxyacetic acid is titrated with 0.050 0 M…

A: pH is the measure of acidity or basicity of a solution. Mathematically, it is defined as negative…

Q: Consider the following reaction: CH3 COOH + OH- -----> CH3COO- + H2O How much 5.90M NaOH must be…

Q: A 100.0 mL sample of 0.20 M HF is titrated with 0.10 M KOH. Determine the pH of the solution after…

Q: A 1.48 L buffer solution consists of 0.100 M butanoic acid and 0.294 M sodium butanoate. Calculate…

A: Given that : The volume of buffer solution = 1.48 L The molarity of butanoic acid = 0.100 M The…

Q: Consider the titration of 115.0 mL of 0.100 M HI by 0.250 MNAOH. Part 1 Calculate the pH after 35.0…

Q: 10 ml of a 1 M acetic acid (pK, = 4.75) are titrated with 0.5 M NaOH. a. Calculate the pH value of…

A: a. When 0 mL of the base NaOH is added, pH depends only on the concentration of the acid.

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

A: The reaction between an acid molecule and a base molecule to form an ionic compound along with water…

Q: 5) Calculate the volume of concentrated ammonia (molecular weight = 17) needed to prepare 100 ml of…

A: Given : Kb = 1.8 x 10-5 Density of solution = 0.9 g/ml Concentration of ammonia solution = 28%…

Q: Suppose we titrate 20.0 mL of 0.100 M HCHO2 (Ka = 1.8 × 10–4) with 0.100 M NaOH. Calculate the pH.…

Q: Calculate the pH of 100.0 mL of a buffer that is 0.0700 M NH4CI and 0.110 M NH3 before and after the…

A: Henderson Hasselbalch equation pH of a buffer is calculated using Henderson Hasselbalch equation.…

Q: 26) A 100.0 ml sample of 0.20 M HF is titrated with 0.10M KOH. Determine the pH of the solution…

A: Given data,Molarity of HF=0.20MVolume of HF=100mL=0.100LMolarity of KOH=0.10MVolume of…

Q: Calculate the pH of 1.00 L of a buffer that is 1.00 M in acetic acid and 1.00 M in sodium acetate…

A: Given: The volume of buffer is 1.00 L. The concentration of acetic acid is 1.00 M. The…

Q: A titration of 51.0 mL of a phosphoric acid (H_ concentration with a standardized 1.05 M Ca 40.2 mL…

A: Dear student I have given answer to your question in the image format.

Q: Calculate the pH of 100.0 mL of a buffer that is 0.0700 M NH4Cl and 0.105 M NH3 before and after…

Q: What is the pH of a 500 mL buffer containing 0.200 moles NH3 and 0.350 moles NH4CI? Kb = 1.8 x 10-5…

A: Buffer solution: The solution that resists the change in pH is known as a buffer solution. The…

Q: 7) The next 9 questions are related to the titration of 20.00 mL of a 0.0750 M acetic acid solution…

A: Reaction taking place at the equivalence point is given. CH3COO- from CH3COOK reacts with water to…

Q: How much 5.50M NaOH must be added to 550.0 mL of a buffer that is 0.0190 M acetic acid and 0.0245…

A: The question is based on the concept of buffer solution. A buffer is a solution which resist any…

Q: The arterial blood plasma is buffered by the carbonic acid and bicarbonate ion, with a ratio of…

Q: What is the pH of a buffer solution containing 0.25 M acetic acid and 0.030 M sodium acetate? The…

A: Given that, [Acetic acid] = [Acid] = 0.25 M [Sodium acetate] = [Salt] = 0.030 M Ka= 1.8×10-5 pH =…

Q: (a) Calculate the pH of a 0.500 L buffer solution composed of 0.700 M formic acid (HCOOH, Ka = 1.77…

A: Given data: Molarity of HCOOH = 0.7 M Molarity of HCOONa = 0.5 M Volume of buffer = 0.5 L Ka of…

Q: A buffer containing 0.30 M HA and 0.65 M NaA has a pH of 4.74. Find the pH after 0.0015 mol of HCl…

Q: 5) Part 1 Calculate the pH at the stoichiometric point when 25 mL of 0.10 M pyridine is titrated…

A: Pyridine ( a weak base) reacts with HCl ( a strong acid ) to undergo neutralisation reaction to form…

Q: 2. A. Calculate the pH of a 0.500 L buffer solution composed of 0.700 M formic acid (HCOOH, Ka =…

A: Use the Henderson-Hasselbalch equation to calculate pH of buffer solution for part A and then solve…

Q: Calculate the pH during the titration of 40.0 mL of 0.25 M HI with 0.25 M RBOH after 32.67 mL of the…

A: Since your question has multiple parts, we will answer the first question for you. If you want the…

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

A: Concentration of KOH = 0.1 M Volume of KOH = 30 mL Moles of KOH = Concentration x Volume (l) Moles…

Q: How much 5.50 M NaOH must be added to 580.0 mL of a buffer that is 0.0200 M acetic acid and 0.0275 M…

Q: #6 Calculate the pH during the titration of 40.00 mL of 0.1000 M HCl with 0.1000 M NaOH solution…

A: Given, Volume of HCl = 40.00 mL = 0.040 L (1mL = 0.001 L) Molarity of HCl = 0.1000 M = 0.1000…

Q: Calculate the pH during the titration of 40.00 mL of 0.1000 M HCl with 0.1000 M NaOH solution after…

Q: Calculate the mass of Ba(ClO)2 needed to prepare 315.0 mL of the pH 7.60 buffer that is 0.100 M in…

A: The solution is given a buffer solution of a weak acid HClO and its conjugate base ClO- The Ka of…

Q: A 30.0 mL sample of 0.165 M propanoic acid (Ka = 1.3x10^-5) is titrated with 0.300 M KOH. Calculate…

A: Molarity of propanoic acid = MP = 0.165 M Volume of propanoic taken = VP = 30.0 mL No of moles of…

Q: A chemistry student is asked to maked a buffer of pH = 4.0. Which of the following acids would be…

Q: In a titration of 25.0 mL of 0.10 M phosphoric acid (a triprotic weak acid) with 0.20 M NaOH, what…

A: TITRATION Titration is a technique used to determine the concentration of a given analyte in a…

Q: Calculate the pH after the addition of 0.00, 25.00, 50.00 mL of 0.1000 M NaOH in the titration of…

Q: For the titration of 75.00 mL of 0.1000 M0.1000 M acetic acid with 0.1000 M0.1000 M NaOH, calculate…

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

Q: 5.00 mL of 0.100 M ammonia (NH3, K, = 1.8x10 5) is titrated with 0.100 M HNO3. Calculate the pH…

A: Given data: Volume of NH3 = 5 mL Molarity of NH3 = 0.1 M Molarity of HNO3 = 0.1 M Kb of NH3 = 1.8 x…

Q: Titrate 50 ml of a 0.150 M solution of HBr with 0.00 ml of 0.150 M KOH.What is the pH initially?

Q: Determine the pH during the titration of 25.8 mL of 0.487 M benzoic acid (K, 6.3x105) by 0.456 M…

A: a.) Before addition of NaOH there would be only benzoic acid , so we would use its Ka value to…

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

24. What is the pH of a buffer solution containing 0.50 M acetic acid and 0.50 M sodium acetate? The
acid dissociation constant for acetic acid is equal to 1.8 x 105
Hint: no dilution occurred
c. 4.74
d. 9.62
a.
5.11
b. 4.38
25. What is the pH of a buffer solution containing 1.25 M NH: and 0.78 M NH-NO:? The base dissociation
constant for ammonia is equal to 1.8 x 10-5
a. 4.54
b. 9.46
C. 4.95
d. 9.05

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 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

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.
When 40.00 mL of a weak monoprotic acid solution is titrated with 0.100-M NaOH, the equivalence point is reached when 35.00 mL base has been added. After 20.00 mL NaOH solution has been added, the titration mixture has a pH of 5.75. Calculate the ionization constant of the acid.
. How is the strength of an acid related to the fact that a competition for protons exists in aqueous solution between water molecules and the anion of the acid?
A good buffer generally contains relatively equal concentrations of weak acid and conjugate base. If you wanted to buffer a solution at pH = 4.00 or pH = 10.00, how would you decide which weak acidconjugate base or weak baseconjugate acid pair to use? The second characteristic of a good buffer is good buffering capacity. What is the capacity of a buffer? How do the following buffers differ in capacity? How do they differ in pH? 0.01 M acetic acid/0.01 M sodium acetate 0.1 M acetic acid/0.1 M sodium acetate 1.0 M acetic acid/1.0 M sodium acetate
A buffer is prepared by dissolving 0.062 mol of sodium fluoride in 127 mL of 0.0399 M hydrofluoric acid. Assume no volume change after NaF is added. Calculate the pH of this buffer.
A buffer is prepared using the butyric acid/butyrate (HC4H7O2/C4H7O2)acid-base pair. The ratio of acid to base is 2.2 and Ka for butyric acid is1.54105. (a) What is the pH of this buffer? (b) Enough strong base is added to convert 15% of butyric acid to the butyrate ion. What is the pH of the resulting solution? (c) Strong acid is added to the buffer to increase its pH. What must the acid/base ratio be so that the pH increases by exactly one unit (e.g., from 2 to 3) from the answer in (a)?