Answered: What volumes (in mL) of 1.0 M HC2H3O2…

What volumes (in mL) of 1.0 M HC2H3O2 and 0.70 M NAOH must be used to prepare 50.0 mL of a buffer with a pH of 4.50? Ka for HC2H302 = 1.8 x 10-5 %3D

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: 2). What is the pH of 0.250L of a buffer that is 0.0200M boric acid H3BO3 and 0.250M sodium borate?…

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

A: pH of a buffer solution is calculated from Henderson Equation. If HCl is added to a buffer system pH…

Q: A buffer solution is 0.40 M in acetic acid and 0.38 M sodium acetate (Ka=1.75X10°). Calculate the…

A: Given, Molarity of CH3COOH = 0.40 M Volume of buffer = 200.0 mL = 0.200 L Molarity of CH3COONa =…

Q: Assuming 0.10 M Na2HAsO4, 0.40 M NaOH and 0.50 M HCl solutions are available in your laboratory.…

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

Q: How many grams of solid sodium cyanide should be added to 1.00 L of 0.116 M hydrocyanic acid…

A: Given-> Volume of HCN = 1.00 L Molarity of HCN = 0.116 M pH = 9.990 Ka(HCN) = 4.00 × 10-10

Q: What is the pH of a buffer that is 0.307 M HF and 0.417 M LiF? The Ka for HF is 3.5 x 10-4.

Q: how many mols NaC2H2ClO2 must be added to 1.00 L of 0.25 M HC2H2ClO2 to prepare a buffer with pH =…

A: Buffer solution are those solution whose pH remains constant even on addition of strong acid or base…

Q: What quantity in moles of CH3NH3CI need to be added to 200.0 mL of a 0.500 M solution of CH3NH₂ (Kb…

A: To calculate the number of moles of salt needed to prepare a buffer of given pH

Q: Calculate the volume (mL) of 1.6 M HCl that should be added to 200 mL of 0.2 M NaA solution to…

A: The pH of a buffer solution is calculated by the Henderson-Hasselbalch equation. It can be given as:…

Q: What is the pH of a buffer that is 0.307 M HF and 0.417 M LiF? The Ka for HF is 3.5 x 10-4.

Q: How many moles of HCl need to be added to 200.0 mL of a 0.200 M solution of NaF to make a buffer…

A: Mole is the amount of the substance that contains the same number of particles or atoms or…

Q: A 175 mL buffer solution is 0.177 M in HONH2 and 0.149 M in HONH3 CL What is the pH of the solution…

Q: what would the pH of 0.250L of a buffer that is 0.0200M boric acid H3BO3 and 0.250M sodium borate?…

Q: Determine the volumes of 0.12 M CH3COOH and 0.15 M CH3COONa required to prepare 10 mL of the…

A: This can be solved from Henderson-Hasselbalch equation, pH = pKa + log10[salt][acid] Here,…

Q: You are given 100.0 mL of the following buffer: 0.010 M HC2H3O2 and 0.010 M NaC2H3O2. What is the…

A: Given, HC2H3O2=0.010 M ; NaC2H3O2 =0.010 MKa=1.7×10-5we are asked to calculate the effective pH…

Q: What olume of 17.1 M glacial acetic acid (HC2H3O2) must be added to 100.0 mL of 1.25 M KOH to form a…

A: Given, Molarity of glacial acetic acid=1.71M Volume of KOH=100mL Molarity of KOH=1.25M pH of…

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

A: The pOH of a basic buffer solution can be expressed as: pOH = pKb + logC2H5NH3NO3C2H5NH2pOH = pKb…

Q: Calculate the [H3O+] of 114.48 mL of a buffer initially consisting of 0.1320 M NH2OH and 0.1429 M…

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

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

Q: Which of the following combinations would make a buffer closest to pH 5.0?

Q: What is the pH of 0.250L of a buffer that is 0.0200M boric acid H3BO3 and 0.250M sodium borate? The…

A: Ans.

Q: How much (in grams) Na2HPO4 must be added to 100 mL 1.0 M NaH2PO4 solution to prepare a buffer…

Q: Which of the following would be the best choice to prepare a buffer with pH = 3.00 ? A. C5H5N:…

A: Acidic buffer solution - a buffer solution that made of weak acid and its conjugate base ( strong…

Q: What is the component concentration ratio, [CH₃COO⁻]/[CH₃COOH], of a buffer that has a pH of 4.39…

A: The dissociation of weak acid takes place as follows: HA+H2Ol⇌H3O++A- The expression for the…

Q: What concentration of sodium chloroacetate is need to prepare a buffer with 0.15 M chloroacetic acid…

Q: Calculate how you would prepare 1.000 l of a pH 4.00 buffer made from HC2H3O2 and NaC2H3O2 You are…

A: Henderson-Hasselbalch equation is used for the pH of buffer solution.

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 is the pH of a buffer that is 0.200M HC2H3O2 and 0.100M NaC2H3O2 (Ka =1.8 x 10-5).

A: The buffer system in this case is made up of acetic acid (HC2H3O2) and its conjugate base, the…

Q: How many grams of NaC3H6O3 should be dissolved in 500.0 ml of 0.100 M HC3H6O3 (lactic acid) to make…

A: An acid buffer is a mixture of a weak acid and its salt with a strong base. It is given that pH of…

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

A: moles of HCl added to prepare the buffer solution

Q: What mass of NH4Cl (Mw = 53.492 g mol-1) has to be dissolved in 750 mL of 0.25 M NH3 (pKa = 9.26) to…

A: 750 mL of 0.25 M NH3 pKa = 9.26 solution is mixed with a certain amount of NH4Cl to prepare a…

Q: What will be the pH of a buffer

A: Given :- Concentration of weak acid i.e. HCN = 0.65 M Concentration of conjugate base i.e. CN- =…

Q: Which of the following combinations would make a buffer with pH closest to 9.0? HClO2 Ka = 1.1 ×…

A: Concept: Buffer A buffer solution is an aqueous solution that consists of a mixture of a weak acid…

Q: what is the ph of a buffer that consists of 0.86 m HBrO (ka= 2.29 x 10-9) and 0.41 M KBr

A: The pH of a buffer solution can be determined using Handerson Hasselbach equation that suggests the…

Q: 1.00L of a buffer is created to be 0.100M in HOAc and 0.100M in NaOAc. What is the pH of the…

Q: What is the pH of a buffer that is 0.76 M in HF and 0.98 M in NaF? Ka = 7.1 x 10-4

A: pH = pKa + log [salt]/[acid] pKa = -logKa

Q: A buffer solution is 0.40 M in acetic acid and 0.38 M sodium acetate (Ka= 1.75X10-5). Calculate the…

A: Mn

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

A: Given data isvolume of NaF solution = 200.0 mLMolarity of NaF solution = 0.200 MpH of the buffer =…

Q: How many grams of solid sodium nitrite should be added to 1.50 L of a 0.0963 M nitrous acid solution…

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

Q: How many grams of solid ammonium chloride should be added to 0.500 L of a 0.190 M ammonia solution…

A: Note: As per our guidelines, we are supposed to answer only first question if multiple questions are…

Q: A buffer is prepared by mixing 16 mL 1M CH3COONa and 4 mL 1M CH3COOH pKa = 4.74. What is the…

A: Given : Concentration of CH3COONa = 1 M Concentration of CH3COOH = 1 M Volume of CH3COONa = 16 ml…

Question

What volumes (in mL) of 1.0 M HC2H3O2 and 0.70 M NAOH must be used to
prepare 50.0 mL of a buffer with a pH of 4.50? Ka for HC2H302 = 1.8 x 10-5
%3D

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

Step 7

Trending now

This is a popular solution!

Step by step

Solved in 7 steps with 7 images

SEE SOLUTION Check out a sample Q&A here

Similar questions

Find the pH of a buffer that consists of 0.50 Mmethylamine(CH₃NH₂) and 0.60 M CH₃NH₃Cl (pK(b) of CH₃NH₂=3.35)
How many grams of solid calcium acetate, Ca(C₂H₃O₂)₂ must be added to 500.0 ml of 0.340M acetic acid in order to form a buffer with a pH = 4.85? pKa of acetic acid = 4.75
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
What is the pH of a buffer made by mixing 0.155M HC2H3O2 with 0.225M NaC2H3O2 to a total volume of 1.00L? The Ka of HC2H3O2 is 1.82x10-5.
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 buffer with a pH of 3.60? (Ka for HF is 6.8 × 10-4)
What mass (in g) of ammonium chloride (NH4Cl) should be added to 2.60 L of a 0.155 M NH3 to obtain a buffer with a pH of 9.45? (Kb for NH3 is 1.8 x 10-5)
Which of the following aqueous mixtures will result in a buffer with a pH higher than 7.0? (For HCNO, Ka = 2.2×10-4, for NH3, Kb = 1.8×10-5 ) 10 mL of 0.1 M NH3 + 10 mL of 0.1 M HCl 10 mL of 0.1 M HCNO + 5.0 mL of 0.1 M NaOH 10 mL of 0.1 M HCNO + 10 mL of 0.1 M NaOH 10 mL of 0.1 M NH3 + 5.0 mL of 0.1 M HCl 10 mL of 0.1 M NH3 + 10 mL of 0.1 M HCNO
Calculate the volume of tris*HCl (in mL) required to prepare 115.0 mL of a buffer with a final concentration of 35.0 mM and pH = 7.6 using 0.400 M tris*HCl and 0.400 M tris (pKa = 8.3).
How many moles of HCl need to be added to 200.0 mL of a 0.200 M solution of NaF to make a buffer with a pH of 2.50? (Ka for HF is 6.8 × 10-4)
A 1.000L buffer is made of 0.7 M CH3COOH and 0.6 M CH3COONa . What is the resulting pH of this buffer solution when 5mL of 4.0M NaOH is added? [Ka CH3COOH = 1.8 × 10-5]
How much solid NaCH3CO2•3H2O must be added to 0.300 L of a 0.50-M acetic acid solution to give a buffer with a pH of 5.00?
Be sure to answer all parts. A buffer consists of 0.30 M KHCO3 and 0.69 M K₂CO3. Carbonic acid is a diprotic acid with Kal-4.5 x 107 and K₁2 = 4.7 x 10-¹1. (a) Which K, value is more important to this buffer? Kat is more important. OK₁2 is more important. (b) What is the buffer pH?