Formic acid, HFor, has a Ka value of 1.8x10-4. You need to prepare a buffer having a pH of 3.25 from 0.10M HFor solution and a ).10M NaFor solution. How many mL of the NaFor solution should you add to 20mL of the 0.10M HFor solution to make your buffer?

Formic acid, HFor, has a Ka value of 1.8x10-4. You need to prepare a buffer having a pH of 3.25 from 0.10M HFor solution and a ).10M NaFor solution. How many mL of the NaFor solution should you add to 20mL of the 0.10M HFor solution to make your buffer?

Fundamentals Of Analytical Chemistry

9th Edition

ISBN:9781285640686

Author:Skoog

Publisher:Skoog

Chapter14: Principles Of Neutralization Titrations

Section: Chapter Questions

Problem 14.38QAP

See similar textbooks

Related questions

Q: An analytical chemist is titrating 230.5 mL of a 0.1500M solution of isopropylamine ((CH3), CHNH₂)…

A: Isopropylamine, (CH3)2CHNH2(aq) is a monoacidic weak base with pKb = 3.33 HNO3(aq) is a monoprotic…

Q: 136.7mL of a 0.4800M solution of dimethylamine CH32NH with a 0.3900M solution of HNO3 . The pKb…

A: The question is based on the concept of titrations. we have to calculate pH of the solution at the…

Q: An analytical chemist is titrating 226.0mL of a 0.8900M solution of diethylamine ((C2H5)2 NH) with…

A: Given that,

Q: What is the pH of a buffer that is created by mixing 24.1 mL of 0.47 M NH3 and 23 mL of 0.35 M…

A: We have to find pH of given buffer

Q: A 75.0-mL volume of 0.200 M NH3 (Kb=1.8×10−5) is titrated with 0.500 M HNO3. Calculate the pH after…

A: Given: Volume of NH3 is 75 mL Molarity of NH3 is 0.200 M Molarity of HNO3 is 0.500 M Volume of HNO3…

Q: A chemist titrates 110.0 mL of a 0.3936M dimethylamine ((CH3), NH) solution with 0.7244M HNO,…

Q: An analytical chemist is titrating 222.2 mL of a 0.3600M solution of methylamine (CH3NH₂) with a…

Q: Answer the following three questions based on the information given below. Consider a buffer made…

A: Buffer are the solution which try to resist any change in pH by addition of acid or base

Q: Lactic acid, (abbreviated HLac) is a key acid in making sauerkraut and tasty sourdough bread. The Ka…

A: Answer: A buffer solution is a type of solution that resists the change in its pH on adding small…

Q: A 1.00 L buffer solution is 0.150M in HC-H5O2 and 0.250 M in LiİC,H5O2. Calculate the pH of the…

A: The reaction can be given as follows: C7H5O2-(aq)+HCl(aq)→HC7H5O2(aq)+Cl-(aq) Now, moles of each…

Q: A buffer solution is 0.405 M in HF and 0.200 M in KF. If Ka for HF is 7.2×10-4, what is the pH of…

Q: Answer the following three questions based on the information given below. Consider a buffer made…

Q: A solution contains 0.300 g HC2H3O2 in 50.0 mL of water. (Ka = 1.80*10-5) -What is the pH of the…

Q: Calculate the pH at the points indicated below if 50.0 mL of 0.100 M aniline hydrochloride (…

A: Aniline hydrochloride (fC6H5NH3+Cl¯) is a salt of the weak base aniline (C6H5NH2) and the strong…

Q: Question attached

A: Buffer solution: Buffer solution is the solution which can resist the change in its pH. It is made…

Q: A chemist titrates 140.0 mL of a 0.8882M methylamine (CH,NH,) solution with 0.4821M HNO, solution at…

Q: A chemist titrates 130.0 mL of a 0.8034M pyridine (C,HşN) solution with 0.2958M HCl solution at 25…

Q: capitalization. A buffer solution is prepared by combining (1.4300x10^1) mL of (2.40x10^-1) molar…

A: Acetic acid and sodium acetate form buffer

Q: An analytical chemist is titrating 169.0 mL of a 0.8600M solution of methylamine (CH3NH₂) with a…

A: The buffer is defined as the solution containing equal amount of a weak acid and its conjugate base…

Q: An analytical chemist is titrating 90.6 mL of a 0.2800 M solution of diethylamine ((C₂H₂)₂NH) with a…

Q: 4. Formic acid, HFor, has a K, value equal to about 1.8 × 10¬4. A student is asked to prepare a…

A: A buffer solution is formed by the mixture of acid and its conjugate base in such a way so that it…

Q: You have prepared a 0.11 M acetate buffer solution in a volume of 1 L at pH 5.76. You then added 80…

A: Topic-- Mechanism of buffer action when HCl is added to the buffer solution and determining the…

Q: An analytical chemist is titrating 160.3mL of a 0.8600M solution of benzoic acid HC6H5CO2 with a…

Q: 1. When 50.00ml of 1.000M HCl is titrated with 0.750M NaOH, the pH increases. What volume of NaOH is…

A: Titration is the process that helps to determine the concentration of a substance reacting in a…

Q: A buffer is prepared by adding 150mL of KOH 1.00M to 250mL of H2PO4 1.00M. Calculate the moles of…

A: In the given question we have to calculate the mole of HCl that will be addade to this system to…

Q: Calculate the pH of the following buffer solutions:

A: a)Moles of KH2PO4 =2.668g/136gmol-1 =0.019617 mol Moles of K2HPO4=2.095g/174.2gmol-1 =0.0120264 mol…

Q: An analytical chemist is titrating 83.7 mL of a 0.3300M solution of isopropylamine ((CH,) CHNH,)…

A: Given that : The volume of isopropylamine = 83.7 mL The molarity of isopropylamine = 0.3300 M The…

Q: A student needs to prepare a buffer solution with a pH of 4.67. Assuming a pkg of 4.69, how many ml…

A: According to Henderson Hasselbalch equation, the pH of a buffer is given by, pH = pKa + log Volume…

Q: A chemist titrates 210.0 mL of a 0.4409M hypochlorous acid (HC10) solution with 0.7835M NaOH…

Q: Formic acid, HFor, has a Ka value of 1.8 x 10^-4. You need to prepare a buffer having a pH of 3.25…

Q: What must be the minimum concentration of hydrocyanic acid in 1.00L buffer solution of a pH 9.8…

A: Answer: Buffer solution is a type of solution in which on adding small quantity of acid or base, it…

Q: An analytical chemist is titrating 92.3 mL of a 0.6600M solution of ethylamine (C₂H5NH₂) with a…

Q: 3) 5. 7 8 6. 10 11 12 13 14 A chemist titrates 210.0 mL of a 0.5893 M potassium hydroxide (KOH)…

Q: An analytical chemist is titrating 64.9 mL of a 0.5800M solution of isopropylamine ((CH, CHNH, with…

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

Q: An analytical chemist is titrating 77.9 mL of a 1.000M solution of hydrazoic acid (HN3) with a…

A: Given-> Volume of HN3 = 77.9 ml Molarity of HN3 = 1.000 M Volume of NaOH = 34.3 ml Molarity of…

Q: An analytical chemist is titrating 15.3 ml of a 0.4200M solution of hydrazoic acid (HN,) with a…

Q: Question 4 I'm not sure how to do this question.

Q: An analytical chemist is titrating 117.9 mL of a 0.4500M solution of dimethylamine ((CH3) NH) with a…

Q: For the titration exp., the pH of the vinegar used was found to be 2.45 which is equivalent to 0.700…

A: Number of moles of solute to the volume of solution in liters is known as molarity.

Q: An analytical chemist is titrating 220.1 mL of a 0.6700 M solution of benzoic acid (HC H₂CO₂) with a…

A: pH of the resulting solution can be calculated by considering the total moles of remaining benzoic…

Q: What must be the minimum concentration of hypobromous acid in 1.00L buffer solution of a pH 8.02…

Q: A chemist titrates 190.0mL of a 0.5533M ammonia NH3 solution with 0.8320M HCl solution at 25°C…

Q: ACDS AND BASES Calculating the pit at equivalence of a titration Megan V A chemist titrates 130.0…

A: we have to calculate the pH at equivalence point

Q: An analytical chemist is titrating 208.7 mL of a 0.5200M solution of isopropylamine ((CH,),CHNH,)…

A: Answer: 10.10

Q: 1. A chemist, , wishes to prepare 100.0 mL of a buffer of pH 10.0000 using the base methyl amine,…

Q: A chemist titrates 90.0mL of a 0.7014M ammonia NH3 solution with 0.8617M HBr solution at 25°C.…

A: When Ammonia (weak base) reacts with strong acid, HBr. A salt of weak base and strong acid will be…

Q: A chemist titrates 90.0 mL of a 0.7050M methylamine (CH3NH₂) solution with 0.5016M HBr solution at…

Q: A student needs to prepare a buffer solution with a pH of 4.60. Assuming a pK a of 4.12, how many mL…

A: A solution which resists change in pH when a small amount of acid or base is added to it is known as…

Q: Calculate the pH of the following buffer solutions: (a) a solution made by dissolving 2.733 g…

A: a) Given: Mass of KH2PO4 = 2.733 g. Mass of K2HPO4 = 4.508 g. And pKa of H2PO4- = 7.2

Q: Formic acid, HFor, has a K, value of 1.8 x 10-4. You need to prepare 125 mL of a buffer hav- ing a…

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

100%

Formic acid, HFor, has a Ka value of 1.8x10^-4. You need to prepare a buffer having a pH of 3.25 from 0.10M HFor solution and a ).10M NaFor solution. How many mL of the NaFor solution should you add to 20mL of the 0.10M HFor solution to make your buffer?

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

Step 2

Step 3

Step 4

Step 5

Step 6

Trending now

This is a popular solution!

Step by step

Solved in 6 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

Ammonia gas is bubbled into 275 mL of water to make an aqueous solution of ammonia. To prepare a buffer with a pH of 9.56, 15.0 g of NH4Cl are added. How many liters of NH3; at 25C and 0.981 atm should be used to prepare the buffer? Assume no volume changes and ignore the vapor pressure of water.
Water is accidentally added to 350.00 mL of a stock solution of 6.00 M HCI. A 75.00-mL sample of the diluted solution is titrated to pH 7.00 with 78.8 mL of 4.85 M NaOH. How much water was accidentally added? (Assume that volumes are additive.)
Calculate the pH of solutions that are 0.25 M formic acid and 0.40 M sodium formate. 0.50 M benzoic acid and 0.15 M sodium benzoate.
A sodium hydrogen carbonate-sodium carbonate buffer is to be prepared with a pH of 9.40. (a) What must the [ HCO3 ]/[ CO32 ]ratio be? (b) How many moles of sodium hydrogen carbonate must be added to a liter of 0.225 M Na2CO3 to give this pH? (c) How many grams of sodium carbonate must be added to 475 mL of 0.336 M NaHCO3 to give this pH? (Assume no volume change.) (d) What volume of 0.200 M NaHCO3 must be added to 735 mL of a 0.139 M solution of Na2CO3 to give this pH? (Assume that volumes are additive.)
For an aqueous solution of acetic acid to be called distilled white vinegar it must contain 5.0% acetic acid by mass. A solution with a density of 1.05 g/mL has a pH of 2.95. Can the solution be called distilled white vinegar?
What is the pH of a buffer that is 0.150 M in a weak acid and 0.150 M in the acids conjugate base? The acids ionization constant is 6.8 106.
Choose a weak-acid/weak-base conjugate pair from which you could prepare a buffer solution with pH = 7.5. Explain how you chose the conjugate pair. Calculate the ratio [weak base]/[weak acid) required to give pH = 7.5.
Enough water is added to the buffer in Question 29 to make the total volume 10.0 L. Calculate (a) the pH of the buffer. (b) the pH of the buffer after the addition of 0.0500 mol of HCl to 0.600 L of diluted buffer. (c) the pH of the buffer after the addition of 0.0500 mol of NaOH to 0.600 L of diluted buffer. (d) Compare your answers to Question 29(a)-(c) with your answers to (a)-(c) in this problem. (e) Comment on the effect of dilution on the pH of a buffer and on its buffer capacity.