### Buffer Preparation Problem**Question:**What volumes of 0.200 M HCOOH and 2.00 M NaOH would make 0.600 L of a buffer with the same pH as a buffer made from 475 mL of 0.200 M benzoic acid and 25 mL of 2.00 M NaOH?**Answer:**- Volume of HCOOH = ____ L HCOOH- Volume of NaOH = ____ L NaOH**Explanation:**The problem involves preparing a buffer solution with a specific pH. It requires calculating the necessary volumes of formic acid (HCOOH) and sodium hydroxide (NaOH) to achieve the desired pH, matching a reference buffer made from benzoic acid and NaOH.**Steps to Consider:**1. **Calculate the pH of the Reference Buffer:** - Use the concentrations and volumes of benzoic acid and NaOH to find the pH. - Apply the Henderson-Hasselbalch equation to determine the reference pH.2. **Determine Required Volumes:** - Use the reference pH to calculate the necessary volumes of 0.200 M HCOOH and 2.00 M NaOH to achieve the same pH in the new buffer solution. - Ensure that the total volume of the buffer solution is 0.600 L.This task involves using molarity concepts, buffer calculations, and the Henderson-Hasselbalch equation.

Given: The concentration of formic acid (HCOOH) is 0.200 M The concentration of NaOH (sodium…

What volumes of 0.200 M HCOOH and 2.00 M NaOH would make 0.600 L of a buffer with the same pH as a buffer made from 475 mL of 0.200M benzoic acid and 25 mL of 2.00 M NaOH? Volume of HCOOH = L HCOOH Volume of NAOH= L NAOH

What volumes of 0.200 M HCOOH and 2.00 M NaOH would make 0.600 L of a buffer with the same pH as a buffer made from 475 mL of 0.200M benzoic acid and 25 mL of 2.00 M NaOH? Volume of HCOOH = L HCOOH Volume of NAOH= L NAOH

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Related questions

Q: 1.00 mL of 12.0 M HCl is added to 1.00 L of a buffer that contains 0.100 M HNO2 and 0.200 M…

Q: How many mL of 0.200 M NaOH or 0.200 M HCl must be added to a 100.0 mL buffer solution containing…

A: Molarity of NaOH = 0.200 MMolarity of HCl = 0.200 MTotal volume of buffer solution = 100.0…

Q: What is the pH of the buffer solution that contains 2.0 g of NH4Cl in 250 mL of 0.050 M NH3? Is the…

A: Buffer solutions are designated as alkaline buffer solutions and acidic buffer solutions. Given…

Q: How many grams of glyonylic acid and sodium plyanylate ae needed to prepare 1.25 Lof a1.80 M buffer…

A: Given data,Molarity of buffer=1.80MVolume of buffer=1.25LpH=3.60pKa=3.34

Q: What is the pH of a benzoic acid/ benzoate buffer that is made by combining 0.3275 g of a benzoic…

A: The question is based on the concept of buffer solution. we have been given a buffer made up of…

Q: A 500 mL buffer solution consists of 0.200 M HNO2 and 0.300 M LiNO2. What volume of 0.400 M HClO4…

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

Q: ou need to prepare 100.0 mL of a pH 4.00 buffer solution using 0.100 M benzoic acid (pKa = 4.20) and…

Q: What is the hydronium ion concentration in a buffer solution prepared by mixing 50.00 mL of 0.10 M…

Q: A buffer solution contains 0.950 mol of HF and 0.150 mol of NaF in 1.00 L of solution. What is the…

Q: What is the pH of a buffer made by combining 0.89 moles HNO2 with 0.96 moles NaNO2 in a 100.00mL…

Q: How many grams of solid potassium fluoride should be added to 1.00 L of a 0.140 M hydrofluoric acid…

A: Given -Volume= 1.00L Concentration of hydrofluoric acid= 0.140 M pH= 4.097 Ka(HF)=7.20×10-4Mass of…

Q: What ratio of NaCN to HCN is needed to prepare a pH 10.00 buffer? (Ka of HCN is 4.9 × 10⁻¹⁰) b.…

A: According to the Bartleby guidelines we have to answer only first three subparts. So please submit…

Q: Which of the following is a means of creating a buffer of H₂CO₃/NaHCO₃? A) Mixing 10 mL of 1 M HNO₃…

Q: 1) Which one of the following combinations of solutions will NOT form a buffer solution? a. NaCl and…

A: As per bartleby Q&A lines.we can solve first question only .please re upload remaining another…

Q: What is the pH of a solution of 0.400 M CH₃NH₂ containing 0.110 M CH₃NH₃I? (Kb of CH₃NH₂ is 4.4 ×…

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

Q: Suppose you wanted to make a buffer of exactly pHpH 7.00 using KH2PO4KH2PO4 and Na2HPO4Na2HPO4. If…

A: Henderson – Hasselbalch equation can be used here, i.e pH=pKₐ+log₁₀([A⁻]/[HA])

Q: What volumes of 0.200 M HCOOH and 2.00 M NaOH would make 0.450 L of a buffer with the same pH as a…

A: The volume of the benzoic acid solution is 475 mL which is equal to 0.475 L and the volume of the…

Q: What quantity in moles of NaOH need to be added to 200.0 mL of a 0.200 M solution of HF to make a…

Q: Which combination will not act as a buffer? A. 0.25 M KHSO3 and 0.20 M H₂SO3 B. 0.20 M NH4Br and…

A: A question based on equilibrium concept. Four choices about different combinations are prescribed,…

Q: Which of the following chemicals would be the best buffer for a pH 9.00 solution: NH3 (Kb =…

Q: What volumes of 1.0 M 1.0 M C6H5COONa are 250. mL of a buffer soluti Кас нҫсоон = 6 A. 116 mL…

Q: None

A: The pH of a buffer solution is associated with the Henderson-Hasselbalch Equation (HHE). pKa is the…

Q: What mass in grams of potassium fluoride is needed to make 150.0 mL of a 0.450 M hydrofluoric…

A: Buffer solutions:- Buffer solutions are a mixture of acid and its conjugate base or base and its…

Q: How many grams of solid sodium fluoride should be added to 2.00 L of a 0.175 M hydrofluoric acid…

A: Given - Volume= 2.00L Concentration of hydrofluoric= 0.175M pH=2.271 Ka(HF)=7.20×10-4 Mass=?

Q: A buffer solution contains 0.350 mol of HF and 0.450mol of NaF in 1.00 L of solution. What is the pH…

A: The buffer solution contains HF which is a weak acid and NaF salt of its conjugate base,F- ion. When…

Q: NaOH and 2.00 M HCl solutions are available in your laboratory. Using only the two of these…

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

Q: How many of the following solutions would result in an adequate buffer? i. equal volumes of 0.25…

Q: What mass in grams of potassium fluoride is needed to make 150.0 mL of a 0.450 M hydrofluoric…

A: Buffer solutions: When a tiny amount of acid or base is added to a solution, buffer solutions resist…

Q: A student needs to prepare a buffer solution with a pH of 4.07. Assuming a pKa of 4.59, how many mL…

A: Given : pH of buffer solution = 4.07 pKa of acid = 4.59 Concentration of NaOH = 0.1 M Concentration…

Q: Assuming 1.00 M Na2HAsO4, 2.00 M NaOH and 2.00 M HCl solutions are available in your laboratory.…

Q: What mass in grams of potassium fluoride is needed to make 150.0 mL of a 0.450 M hydrofluoric…

A: Given the pH of the buffer = 4.25 Given the total molarity of HF/KF buffer, C = 0.450 M Total…

Q: Use each of the two methods of buffer preparation to make a 1.0 M buffer with a 1:2 conjugate ratio…

A: The objective of the question is to calculate the amount of conjugate acid needed to prepare a…

Q: Calculate the pH of a solution that is 0.20 M HOC1 and 0.92 M KOCI. Ka = 3.5x10-8 pH = 8.16 b In…

Q: buffer is made up of 0.3 L each of a 0.5 M KH2PO4 and 0.317 M K2HPO4. assuming that volumes are…

A: #(a): The dissociation equation for the weak acid conjugate base pair is: H2PO4-(aq) ⇌HPO42-(aq),…

Q: A buffer contains 0.175 moles C2H5NH3NO3 and 0.225 moles C2H5NH2 in 800.0 mL water. Kb (C2H5NH2) =…

A: Calculation of pKb: pKb=-log Kb=-log 4.3×10-4=3.37 Calculation of initial pOH:…

Q: What quantity in moles of HCl need to be added to 200.0 mL of a 0.200 M solution of NaF to make a…

A: A buffer is a solution which resist any change in pH on adding a small amount of acid or base . it…

Q: What is the buffer capacity of a solution made from 500 mL NaOH (0.5 M) and 500 mL HCl (0.5 M)? O…

A: NaOH and HCl mixture cannot form buffer solution and it has zero buffer capacity.

Q: When 30 .00 mL of 0.1011 M HCl in 50 mL of deionized water is titrated against 0.09889 M NaOH, the…

A: ANsweR: We’ll answer the first question since the exact one wasn’t specified. Please submit a new…

Q: Assuming 1.00 M Na2HAsO4, 2.00 M NaOH and 2.00 M HCl solutions are available in your laboratory.…

A: A buffer solution contains both acid and base species in the same solution simultaneously. These…

Q: What would be the molar ratio of cyanic acid (HCNO)/sodium cyanate (NaCNO) buffer having a pH of…

Q: phosphate buffer in the lab that resembles the bloods phosphate buffer. You start by mixing 1.0 M…

Q: part a: A 0.500-L buffer solution was made with 0.25 M NH3 (Kb = 1.8 × 10-5) and 0.40 M NH4Cl. What…

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

Q: Be sure to answer all parts. What volumes of 0.200 M HCOOH and 2.00 M NaOH would make 0.800 L of a…

A: The objective is to determine the volume of HCOOH and NaOH from a buffer solution.Given:The…

Q: Which of the following would make the best buffer with the highest "buffer capacity"? 100 mM NH4+…

A: Henderson equation for buffer solution is for best buffer solution, [salt] = [base]That is with…

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

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

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

1. A buffer is prepared using 0.522 mol of NH4CI and 0.812 mol of NH3 to make 1.00 L of solution. What is the pH of the solution after adding 0.153 mol of NaOH. Assume that the volume change is negligible. The pKa of NH4Cl is 9.26. 2. A buffer is prepared using 0.636 mol of HO2C2H3 and 0.848 mol of NaO2C2H3 to make 1.00 L of solution. What is the pH of the solution after adding 0.137 mol of HCI. Assume that the volume change is negligible. The pKa of HO2C2H3 is 4.74.
A buffer with pH = 8.96 must be created. 8.90 g of the acid component of the best buffer system will be used, and the volume of the solution will be 1 L. Choose which is the best buffer system, then compute the mass of the salt or base component of the chosen system. Choices: HClO (Ka = 2.9 x 10-8 , 52.46 g/mol)& KClO (90.55 g/mol) NH3 (Ka = 5.65 x 10-10 , 17.031g/mol) &NH4Cl (53.491 gmol) CH3COOH (Ka = 1.77 x 10-5 , 60.052 g/mol) & CH3COOK (98.15 g/mol) HClO2 (Ka = 1.1 x 10-2 , 68.46 g/mol)) & KClO2 (106.55 g/mol)
How many grams of solid ammonium chloride should be added to 0.500 L of a 0.190 M ammonia solution to prepare a buffer with a pH of 9.850? Mass= g
What is the [H3O+] and the pH of a benzoic acid-benzoate buffer that consists of 0.13 M C6H5COOH and 0.30 M C6H5COONa? (Ka of benzoic acid = 6.3 × 10−5) Be sure to report your answer to the correct number of significant figures. [H3O+] = ___× 10___MpH =____
You need to prepare 100.0 mL of a pH 4.00 buffer solution using 0.100 M benzoic acid (pKa 4.20) and 0.240 M sodium benzoate. How many milliliters of each solution should be mixed to prepare this buffer? benzoic acid: mL sodium benzoate: mL
Assuming 1.00 M Na2HAsO4, 2.00 M NaOH and 2.00 M HCl solutions are available in your laboratory. Using only the two of these solutions, how would you prepare a 1.0 L buffer with a pH of 8.0 For H3AsO4 Ka1=5.8x10-3, Ka2=1.1x10-7, Ka3=3.2x10-12
How many grams of sodium acetate must be added to 2.00L of 0.105M acetic acid to make a buffer that has a pH of 4.90? (Ignore volume changes due to the addition of the NaC2H3O2).
For humans to maintain the pH of their blood close to 7.4, the body uses three buffer systems: carbonate, phosphate and proteins. If the pH of the blood goes below 6.8 or above 7.8, death may result. Imagine you want to make a phosphate buffer in the lab that resembles the bloods phosphate buffer. You start by mixing 0.95 M NaH2PO4 and 0.68 M Na2HPO4. H2PO4- + H2O ⇌ HPO42- + H+ pKa= 7.21 (5 marks total) a. From the reaction above indicate the weak acid and the conjugate base involved in making this buffer. (2 marks) b. Calculate the pH of the phosphate buffer solution. Provide your answer with 2 decimal places (2 marks) c. If the pH calculated in b. was the blood pH of an actual patient, would you say this patient’s blood pH is in the normal range or are they suffering from alkalosis or acidosis? (1 mark)
What volumes of 0.200 M HCOOH and 2.00 M NaOH would make 0.800 L of a buffer with the same pH as a buffer made from 475 mL of 0.200 M benzoic acid and 25 mL of 2.00 M NaOH?
you are given 1.8 M acetic acid solution (CH3COOH) and solid sodium acetate trihydrate (NaOOCCH3 X 3 H2O) you want to make 100.0 mL of a 0.5 M acetic acid buffer at pH 5.00. what volume in mL of the 1.8M acetic acid solution, NaOH solution and deionized water should you combine?