Answered: How many grams sodium formate (HCOONa),…

How many grams sodium formate (HCOONa), 68.0069 g/mol) do you need to add to 250 mL of0.40 M formic acid (HCOONa) for a pH 3.5 buffer. Ka = 1.77 × 10 -4.

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 98QRT: Does the pH of the solution increase, decrease, or stay the same when you (a) Add solid sodium...

See similar textbooks

Related questions

Q: You need to produce a carbonic (H 2 CO3)/bicarbonate buffer solution that has a pH of 4.50. You…

A: Carbonic/bicarbonate buffer solution has a pH of 4.50 . 0.60 L solution contains 0.20 moles of…

Q: Consider the reaction of a 20.0 mL of 0.220 M C₅H₅NHCl (Ka = 5.9 x 10⁻⁶) with 12.0 mL of 0.223 M…

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

Q: You want to prepare 100.0 mL of a buffer solution with a pH of 4.95 by mixing appropriate volumes of…

A: Given : pH of buffer solution = 4.95 Concentration of CH3CO2H = 0.10 M Concentration of CH3CO2Na =…

Q: What is the pH (in two decimal places) of a weak base-strong acid titration when 25.0 mL of 0.56 M…

A: Volume of NaOCl = 25.0 mlMolarity of NaOCl = 0.56 MVolume of HCl = 23.0 mlMolarity of HCl = 0.34 MKa…

Q: Determine the mass of solid NaCH3COO that must be dissolved in an existing 500.0 mL solution of…

A: Given: Initial concentration of CH3COOH = 0.2 M Volume of solution = 500.0 mL = 0.5 L pH of solution…

Q: Assume you titrate 20.0 mL of 0.11 M NH3 with 0.10 M HCl. (a) What is the pH of the NH3…

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

Q: A chemist needs a buffer with pH 4.15. How many milliliters of pure acetic acid (density = 1.049…

A: The expression of Henderson-Hasselbalch displays that to calculate the pH of any buffer solution,…

Q: You are asked to prepare a pH = 3.00 buffer starting from 2.00 L of 0.025 M solution of benzoic acid…

A: buffer solution A buffer solution is an aqueous solution consisting of a mixture of a weak acid and…

Q: Calculate the pH of a buffer solution containing 0.659 mol HA weak acid and 0.602 mol A- in 288.3 mL…

A: We have to calculate the pH of solution

Q: A solution contains 0.363 M HA (Ka = %3D 6.74-10-46.74-10-4) and 0.677 M NaA. What is the pH of this…

A: A solution contains 0.363 M HA and 0.677 M NaA.Ka of HA is 6.74 × 10-4We have to calculate the pH…

Q: What volume, in milliliters, of 0.240 M NaOH should be added to a 0.135 L solution of 0.030 M…

A: Here we have to determine the volume of 0.240M NaOH solution required to be added to 0.135L of…

Q: a) What is the pH of a buffer prepared by adding 0.506 mol of the weak acid HA to 0.507 mol of NaA…

A: the solution is as follows:

Q: Consider a beaker containing 50 mL of 0.20 M of a weak acid (HA) with a pKa of 5.25. How many…

A: Henderson equation is pH = pKa + log [salt][acid] when NaOH is added to weak acid then they react to…

Q: Enter your answer in the provided box. Calculate the pH of a bicarbonate/carbonate buffer in which…

Q: Classify the following solutions as one of these types AND calculate the pH: strong acid, strong…

A: Given,a) 0.040 M NaF (Ka for HF = 7.2 x 10-4)b) 10 M HClO4c) A solution made by mixing 10.0 mL of…

Q: Calculate the pH of a bicarbonate/carbonate buffer in which the concentration of sodium bicarbonate…

A: Given : Concentration of NaHCO3 = 0.31 M Concentration of Na2CO3 = 0.83 M Ka of HCO3- = 5.6 x…

Q: (a) Calculate the pH of the 0.30 M NH3 / 0.35 M NH4Cl buffer. What is the pH of the buffer after…

A: A buffer solution is made up of weak acid or base with its conjugate base or acid respectively. pH…

Q: Suppose you want to make a buffer with a pH of 6.90. Which of the following acid/conjugate base…

A: The pKa value of the acid gives an idea of which conjugate acid-base pair should be chosen for the…

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: If you have a ka = 8.25x10^-8, what buffer system will you use? Acetic acid (HC2H302) - Acetate ion…

A: Given: Ka of acid = 8.25 × 10-8

Q: A research wishes to prepare a buffer with a pH of 4.74 from weak acid HA (Ka = 2.57 x 105) and the…

Q: What is the pH of a buffer solution that is 0.20 M methyl amine, CH3NH2 and 0.18 M methylammonium…

Q: What is the pH of a 75.0 mL of a 0.1 M NH3 solution (Kb= 1.8 x 10- 5) when 100.0 mL of a 0.0.75 M…

A: Hello. There are multiple subparts in the question. The first three subparts have been solved. To…

Q: You have 150 mL of 1 M ammonia solution (pKa=9.25). What volume of 1 M hydrochloric acid is needed…

A: pKa=9.25-log(Ka)=9.25Ka=5.62×10-10pH=-logH+=9.5H+=3.16×10-10

Q: Calculate the pH of a buffer solution containing 0.584 mol HA weak acid and 0.703 mol A- in 130.1 mL…

A: It is based on the concept of buffer Here we are required to find the pH of the buffer solution…

Q: A butanoic acid/sodium butanoate (C3H7COOH/NAOOCC3H7) buffer is prepared to 1.14x10-2 mol L-1…

A: pH = pKa + log(salt / acid) pKa = -log Ka

Q: What is the pH of a buffer solution that is 0.602 M in hydrofluoric acid and is 0.455 M is potassium…

Q: A student wants to make a pH 4.0 buffer solution. She decides to use a buffer made from formic acid…

A: Henderson Hasselbalch equation gives the equation to estimate the pH of buffer solution. pH=pKa +…

Q: The titration curve as shown is for the titration of 25.00 mL of 0.100 M CH3CO2H with 0.100 M NaOH.…

A: We are authorized to answer three subparts at a time, since you have not mentioned which part you…

Q: What is the pH of the buffer that results when 2.3 g of NH3 and 6.46 g of NH4Cl are dissolved in 250…

A: To solve the above problem by means of the Henderson-Hasselbalch equation, the explanation is given…

Q: A buffer is made by adding 0.18 mol/L of sodium propanoate (NaPr) to 0.12 mol/L solution of…

A: All solutions hold specific characteristics in pH value terms. This value describes how acidic or…

Q: How many moles of hydrofluoric acid, HF, must be added to 150 mL of 0.31 M sodium fluoride to give a…

A: Since the pH of a buffer solution is given by Henderson-Hasselbalch equation as pH = pKa + log(…

Q: A buffer prepared by dissolving oxalic acid dihydrate (H2C2O4·2H2O) and disodium oxalate (Na2C2O4)…

A: The objective of the question is to calculate the amount of oxalic acid dihydrate.It is given…

Q: A buffer system is prepared by combining 0.603 moles of ammonium chloride (NH4CI) and 0.713 moles of…

A: Moles of weak base ammonia = 0.713 mole Moles of conjugate acid (NH4+) = 0.603 mol Moles of HNO3…

Q: When a strong base is added to buffer it will react to become neutralized. Determine the pH after…

A: From the Henderson-Hasselbalch equation: Since, Ka = 5.8×10-10 Therefore,

Q: You start with 100.0 mL of 0.20 M CH3COOH in a flask. The Ka of CH3COOH is 1.8 x 10-5. You add…

A: After adding NaOH we get buffer solution as it form mixture of weak acid and salt of this weak acid…

Question

100%

How many grams sodium formate (HCOONa), 68.0069 g/mol) do you need to add to 250 mL of
0.40 M formic acid (HCOONa) for a pH 3.5 buffer. Ka = 1.77 × 10 ^-4.

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

Trending now

This is a popular solution!

Step by step

Solved in 1 steps

SEE SOLUTION Check out a sample Q&A here

Similar questions

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.
Does the pH of the solution increase, decrease, or stay the same when you (a) add solid sodium oxalate, Na2C2O4, to 50.0 mL of 0.015 M oxalic acid, H2C2O4? (b) add solid ammonium chloride to 75 mL of 0.016 M HCl? (c) add 20.0 g of NaCl to 1.0 L of 0.10 M sodium acetate, NaCH3CO2?
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.
A student wants to make a pH 4.0 buffer solution. She decides to use a buffer made from formic acid and sodium formate (HCOONa). She adds 50.0 grams of sodium formate to a 1 L volumetric flask. The Ka of formic acid is 1.77×10-4. How many mL of 3.0 M formic acid should she add to the 1 L volumetric flask so that when the flask is diluted to the mark the pH will be 4.00?
What is the pH of a buffer solution that is 0.20 M methyl amine, CH3NH2 and 0.18 M methylammonium chloride CH3NH2Cl? The Kb for CH3NH2 is 4.4x10-4. You do not need to solve the quadratic equation for this problem. Express your answer to two decimal places.
What is the pH of the buffer that results when 2.3 g of NH3 and 6.46 g of NH4Cl are dissolved in 250 mL water? (Ka for NH4+ = 5.60 × 10-10) Please give the answer to 2 decimal places.
If you have a ka = 8.25x10^-8, what buffer system will you use? Acetic acid (HC2H302) - Acetate ion (C2H302-) Carbonic acid (H2co3) - Hydrogen carbonate ion (HCO3-) Dihydrogen phosphate ion (H2P04-) - Hydrogen phosphate ion (HPO4 2-) Hypochlorous acid (HCIO) - Hypochlorite ion (CIO-)
When a strong base is added to buffer it will react to become neutralized. Determine the pH after 0.15 mol of OH- is added to a buffer consisting of 2.0 mol of HA and 1.0 mol of A-. (Ka = 5.8 x 10-10) HA + OH- → A- + H2O
You need to make a buffer whose pH is 7.0, and you can choose from the weak acids shown. Briefly explain your choice
Suppose you want to make a buffer with a pH of 6.90. Which of the following acid/conjugate base pairs should you choose? Group of answer choices HOCl and OCl- (Ka = 3.5 x 10-8) HSO4- and SO42- (Ka = 1.2 x 10-2) C6H5CO2H and C6H5CO2- (Ka = 6.5 x 10-5) HF and F- (Ka = 6.6 x 10-4)
A buffer is made by adding 0.18 mol/L of sodium propanoate (NaPr) to 0.12 mol/L solution of propanoic acid (HPr, K«= 1.3 x 10-5). Assume the volume of the solution to be 1.0 L. a) Write the chemical equation for the acid hydrolysis reaction. | b) What is the acid-base conjugate pair that governs the pH of the buffer? c) Calculate the pH of the buffer. Be sure to justify and validate any approximations used.
What is the pH (in two decimal places) of a weak base-strong acid titration when 25.0 mL of 0.56 M NaOCl (Ka = 3.0*10-8) is added to 23.0 mL of 0.34 M HCl?