buffer solution is prepared from an unknown weak acid (HA) and its conjugate salt (NaA). If 500.00 ml of this buffer solution contains 0.025 moles of HA and 0.066 moles NaA, and has a measured pH of 4.61, what is the pKa of the unknown weak acid?

buffer solution is prepared from an unknown weak acid (HA) and its conjugate salt (NaA). If 500.00 ml of this buffer solution contains 0.025 moles of HA and 0.066 moles NaA, and has a measured pH of 4.61, what is the pKa of the unknown weak acid?

General Chemistry - Standalone book (MindTap Course List)

11th Edition

ISBN:9781305580343

Author:Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; Darrell

Publisher:Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; Darrell

Chapter17: Solubility And Complex-ion Equilibria

Section: Chapter Questions

Problem 17.125QP

See similar textbooks

Related questions

Q: A buffer solution is prepared by dissolving 1.00 g of sodium acetate (CH3COONa) into 100.00 mL of a…

Q: What mass (in grams) of sodium acetate (CH3COONa) must be added to 100.00 mL of a 0.115 M solution…

A: Mass (in grams) of sodium acetate (CH3COONa) must be added to 100.00 mL of a 0.115 M solution of…

Q: A buffer is prepared using lactic acid (HLac) and sodium lactate (NaLac). 0.300 dm3 of the 0.500…

A: Henderson – Hasselbalch equation: It gives a relationship between the pka, pH, and concentration of…

Q: The pk, for the acid dissociation reaction of bicarbonate is 10.33. HCO3 (aq) + H2O(1) 2 CO32-(aq) +…

Q: A solution is prepared by dissolving 0.23 mol of nitrous acid and 0.27 mol of sodium nitrite in…

Q: How the pH at the equivalence point is determined by the species present; why the pH at the midpoint…

A: pH is the measure of the acidic or basic nature of the substance. It is measured by the use of…

Q: Which

A: Those solution when resist to change the pH when small amount of acid or base added on it's then…

Q: Which of these factors influence buffer capacity? How?(a) Conjugate acid-base pair(b) pH of the…

A: Concept introduction: Buffer solution: The pH of the solution is not changed when small amount of…

Q: An analytical chemist is titrating 190.8 mL of a 0.4600M solution of nitrous acid (HNO,) with a…

A: The titration reaction between Nitrous acid and KOH can be represented as- HNO2 + KOH ----> KNO2…

Q: The half‑equivalence point of a titration occurs half way to the equivalence point, where half of…

A: Given data: Moles of acid=0.220 Acid is monoprotic which gives only one H+. HA→H+ + A- Ka = 5.1×10-5…

Q: Choose the acid below that would make the most effective buffer for a solution to maintain a pH of…

Q: At 25oC, a 1-L buffer solution is prepared by mixing acetic acid and sodium acetate. A) If the…

A: Use Henderson Hesselbalch's equation to get the pH of buffer solution having weak acid and its salt…

Q: What will be the pH change when 20.0 mL of 0.100 M NaOH is added to 80.0 mL of a buffer solution…

A: Here we have a buffer solution which has:Concentration of NH4Cl/NH4+ = 0.181 MConcentration of NH3 =…

Q: An analytical chemist is titrating 134.4mL of a 0.6500M solution of nitrous acid HNO2 with a 0.7300M…

A: The molarity of an unknown solution can be determined by titrating it with a known solution by using…

Q: An analytical chemist is titrating 152.5 mL of a 0.9200 M solution of nitrous acid (HNO,) with a…

A: pH is used to determine the concentration of hydronium ion.

Q: A biochemist prepares two stocks of sodium phosphate buffer by titrating phosphoric acid with sodium…

A: Given: pKa of phosphoric acid are 2.15, 7.20 and 12.35 Volume of 7.20 buffer is 50.0 mL Volume of…

Q: We dissolve 3.54 g of an unknown acid, HA, in enough water to produce 25.0 mL of solution. We…

A: Any acid's strength always gets estimated by its dissociation constant which is symbolized as "Ka".…

Q: A solution is formed by adding 5.20 grams of solid potassium acetate, KC₂H₃O₂, to 500.0 ml of…

A: pH is negative logarithm of Hydrogen ion concentration

Q: 2.00 L of a buffer is prepared by combining 1000.0 mL of 0.500 M nitrous acid (HNO2 Ka = 7.1 x 10-4)…

Q: The half‑equivalence point of a titration occurs half way to the equivalence point, where half of…

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

Q: A buffer solution contains 0.202 M of a weak acid and 0.224 M of its conjugate base. The K, of the…

A: Buffer solution is a solution whose pH does not changes on standing as well as on addition of small…

Q: Derive an equation similar to the Henderson–Hasselbalch equation for a buffer composed of a weak…

Q: Phosphoric acid is a triprotic acid (Ka1=6.9×10−3Ka1=6.9×10−3, Ka2=6.2×10−8Ka2=6.2×10−8, and…

Q: If 0.02 M of NaOH will be added to the buffer solution prepared by mixing 0.215M sodium acetate and…

A: the Henderson equation is used to find pH of buffer solution

Q: What is the pH of a buffer prepared by adding 0.607 molof the weak acid HA to 0.609 molmol of NaA in…

Q: You are working in a lab and someone has just handed you a beaker filled with 110 ml of a mysterious…

A: pH of a buffer is calculated using Hasselbach Henderson equation: pH =pKa+log([Conjugate…

Q: An analytical chemist is titrating 219.6 mL of a 0.9100M solution of nitrous acid (HNO,) with a…

Q: A chemistry graduate student is given 450. mL of a 1.40 M nitrous acid (HNO, solution. Nitrous acid…

Q: Consider an acetate buffer system (Ka = 1.82 x 105). The buffer solution contains 0.200 M acetic…

A: Given, Ka = 1.82× 10-5 concentration of acetic acid, [CH3COOH] = 0.200M concentration of sodium…

Q: An analytical chemist is titrating 159.5 mL of a 1.200 M solution of nitrous acid (HNO,) with a…

A: The is a neutralization reaction which takes place as,…

Q: At 25oC, a 1-L buffer solution is prepared by mixing acetic acid and sodium acetate. A) If the…

A: Given: pH = 5 Ka of acetic acid = 1.8×10-5 Calculation for pKa of the acetic acid: Calculation…

Q: An acid–base buffer is able to resist changes in pH due to the addition of small amounts of strong…

A: Given:-molarity of NaOH=0.209 Mmolarity of CH3COOH=0.231 MTo find:-PH of Buffer solutionsolution:-As…

Q: The pH of a buffer prepared by adding 0.708 mol of the weak acid HA to 0.305 mol of Na in 2.00 L of…

A: Given, The pH of a buffer prepared by adding 0.708 mol of the weak acid HA to 0.305 mol of NaA in…

Q: The primary buffer in the blood is carbonate-bicarbonate buffer. If the pKa is 6.1 and the pH is set…

A: GIVEN DATA:-Buffer is Carbonate (CO32-) and Bicarbonate (HCO3-). pH=7.4…

Q: formic acid/sodium formate buffer solution can be prepared with 0.012 M each of formic acid (HCOOH)…

A: Molar mass of HCl = 35.5 + 1 = 36.5g/mol

Q: What is the pH of a buffer prepared by adding 0.708 mol of the weak acid HA to 0.305 mol of Na in…

A: Solution -

Q: The desired pH is 6.4 in creating a buffer system/buffer solution of about 50-60mL. Therefore, a…

A: A buffer solution is made of a weak acid and the salt of that weak acid. The pH of the buffer does…

Q: Given the values of Ka and Kh below, which of the systems given would be most suitable to use to…

A: The pH of a buffer solution remain close to the pKa value of its acid in weak acid / base and its…

Q: a.) A student titrated 50.0mL of a 0.10M solution of a certain weak acid with NaOH(aq). The results…

A: A student titrated 50.0mL of a 0.10M solution of a certain weak acid with NaOH. I) The approximate…

Q: What will be the pH change when 20.0 mL of 0.100 M NaOH is added to 80.0 mL of a buffer solution…

A: Here we have a buffer solution which has: Concentration of NH4Cl/NH4+ = 0.182 M Concentration of NH3…

Q: A 250-mL buffer solution contains 0.0510 mole of KH2PO4 and 0.0875 mole of K2HPO4. (a) Calculate…

Q: the pH of an acetate buffer prepared by dissolving sodium acetate (5.21 g) and acetic acid (2.19 g)

Q: The half‑equivalence point of a titration occurs half way to the equivalence point, where half of…

A: There are two types of bases/acids. One is strong base/acid which is completely dissociable in into…

Q: A)What is the pH of a buffer prepared by adding 0.506 molmol of the weak acid HAHA to 0.507 molmol…

Q: A buffer solution is prepared by dissolving 1.000 g of sodium acetate (CH3COONa) into 100.00 mL of a…

A: Given : Mass of CH3COONa = 1.000 g Volume of acetic acid solution = 100.00 mL = 0.100 L…

Q: ou want to prepare 1.00 L of a buffer solution with a pH of 3.5. You are given an 0.45 M solution…

A: pH =Pka + log[salt][acid][salt]=0.68yx+y=0.68y[acid]=0.45x-0.68yx+y[acid]=0.45-1.13ysubstititing the…

Q: A 25 mL sample of 0.150 M monoprotic organic acid is titrated with aqueous sodium hydroxide. After…

Q: pH indicator. A dye that is an acid and that appears as different colors in its protonated and…

Q: A buffer solution is prepared by mixing 75.0 ml of 0.275 M fluorobenzoic acid with 55.0 ml of 0.472…

A: The given buffer solution is a mixture of weak acid fluorobenzoic acid and conjugate base…

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

A buffer solution is prepared from an unknown weak acid (HA) and its conjugate salt (NaA). If 500.00 ml of this buffer solution contains 0.025 moles of HA and 0.066 moles NaA, and has a measured pH of 4.61, what is the pKa of the unknown weak acid?

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

Using the concentrations 0.100M and 0.1766M, and the pKa of 3.752, what is the theoretical pH of a buffer solution?
You are working in a lab and someone has just handed you a beaker filled with 110 ml of a mysterious buffer that has a PkA of 10.4 and a total concentration of 1M. You determine that the pH of the solution you have been handed is 10.4. After adding 45ml of 1M HCL to that solution, what is the final pH of the solution?
ACID-BASE EQUILIBRIA AND SALT EQUILIBRIA (COMMON-ION EFFECT, BUFFER AND SOLUBILITY EQUILIBRIA) A mixture of 0.15 M acetic acid and 0.34 sodium acetate is given. Calculate the pH of the medium if the pKa of the acetic acid is 4. 87.
What is the effective pH range of a buffer (relative to the pKa of the weak acid component)?
What will be the pH of a buffer solution containing an acid with a pKa of 5.4 with an acid concentration equivalent to that of its conjugate base?
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
Consider a buffer solution containing an acid with a pKa of 2.3 and an acid concentration that is one fourth the concentration of the conjugate base. What is the pH of the solution?
A buffer is made by mixing 40.00 mL of a 0.100 M solution of the fictitious acid HA (pKa = 6.44) with 20.00 mL of 0.100 M NaOH. This buffer is then divided into 4 equal 15.00 mL parts. If 0.15 mL of a 1.0 M solution of sodium hydroxide is added to one of these 15.00 mL portions of the buffer, what is the pH of the resulting solution?
At 25oC, a 1-L buffer solution is prepared by mixing acetic acid and sodium acetate.A) If the solution is to be buffered at pH = 5, what should be the molar ratio of sodium acetate to acetic acid?B) If the buffer is found to be 1.55M in acetic acid and 1.70M in sodium acetate, what will be the pH of the solution?C) If 0.15 mol of NaOH was added to the solution in B, what will be the pH of the solution?D) If the pH of the solution in B is 4.50, how many moles of HCl was added to the solution?
Describe the changes in pH that take place during the titration of: (a) a weak acid with a strong base, (b) a weak base with a strong acid .
if 0.0050 mole of NaOH is added to 0.50L of the buffer solution 0.24 M NH3 and 0.20 M NH4Cl) what is the delta pH (change in pH)? pKa = 9.25
You are asked to make a buffer to a pH of 4.00 and you have the following acids to do it with (pKa in parentheses): chloroacetic (2.85), nitrous (3.16), lactic (3.86), acetic (4.75), and propionic (4.87). Which acid (and its conjugate base) would be the best choice and why?

SEE MORE QUESTIONS

Recommended textbooks for you

General Chemistry - Standalone book (MindTap Cour…

Chemistry

ISBN:

9781305580343

Author:

Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; Darrell

Publisher:

Cengage Learning

General Chemistry - Standalone book (MindTap Cour…

Chemistry

ISBN:

9781305580343

Author:

Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; Darrell

Publisher:

Cengage Learning

SEE MORE TEXTBOOKS