BQUESTION 1You need to make 1.0 L of a buffer solution having pH= 4.30 from CH3COOH and NACH3COO. What concentrations of CH3COOH and NACH3COO willno.you have to prepare? |Hint: Various concentrations are available. You need to explain your answers with reasonable rationale.]Ka for CH3COOH = 18 x 10-5Attach FileBrowse Local FilesBrowse Content CollectionBrowse DropboxClick Save and Saubmit to save and submit. Click Save All Answers to save all answers.Anyeska Mendoz. pdfMitosis Lab (1).docxMacBook AirFB.Ed%23247.6.5.8.1.4.E.R.AH.K.ockD.C.controloptioncommand

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

QUESTION 1 You need to make 1.0 L of a buffer solution having pH 4.30 from CH3COOH and NACH3COO. you have to prepare? [Hint: Various concentrations are available. You need to explain your answers with reasonable rationale.] What concentrations of CH3COOH and NaCH3COO will Ka for CH3COOH=18 x 10-5 %3D

QUESTION 1 You need to make 1.0 L of a buffer solution having pH 4.30 from CH3COOH and NACH3COO. you have to prepare? [Hint: Various concentrations are available. You need to explain your answers with reasonable rationale.] What concentrations of CH3COOH and NaCH3COO will Ka for CH3COOH=18 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: A buffer system is made of 0.725M HX (Ka = 5.2 x 10-5) and 0.250M NaX. a) Calculate the pH of this…

Q: An analytical chemist is titrating 163.0 ml of a 0.5900M solution of cyanic acid (HCNO) with a…

A: Given : We have to calculate pH .

Q: Question 5 - Calculate the pH of a buffer produced by mixing 50 mL of a 0.1M solution of sodium…

Q: Determine the pH at the point in the titration of 40.0 mL of .200 M HC4H7O2 with .100 M Sr(OH)2…

A: The reaction between acid and base is written below. 2C3H7COOH (aq) + Sr(OH)2 (aq) ⇌ 2H2O (l) +…

Q: Part A What is the pH of a buffer prepared by adding 0.708 mol of the weak acid HA to 0.608 mol of…

Q: Q1// A buffer solution prepared by adding adequate amount of Acetic acid and Sodium acetate to…

A: Firstly we will calculate pH of buffer solution CH3COOH - CH3COONa CH3COOH (aq) + H2O (l)⇌H3O+…

Q: How many grams of KHCOO (MM = 84.12 g/mol) must be added to 1.00 L of 0 838 M HCOOH to make a buffer…

A: A buffer solution is an aqueous solution. It consist of a mixture of a weak acid and its conjugate…

Q: Calculate the pH when 32.0 mL of 0.150 M KOH is mixed with 20.0 mL of 0.300 M HBRO (Ka = 2.5 x 10-9)…

A: 1- First calculate the mmoles of KOH and HBrO : a) mmoles of KOH = ( 32.0mL × 0.150M ) mmoles of…

Q: 2) The ionization constant for NH3 in water is 1.8 x 10 - 5. Determine the hydroxide ion…

A: Welcome to bartleby ! As per company norms we cannot answer more than one question per session .So,…

Q: What is the pH of a solution of 100 mL of 0.025 M HBr and 100 mL of 0.10 M NaF? (HF Ka= 7.2 x 10-4)

A: Given Volume of HBr solution = 100 mLConcentration of HBr solution = 0.025 MVolume of NaF solution =…

Q: I mix 50.0 mL of 0.150 M CH3COOH with 10.0 mL of 0.100 M NaOH. Calculate the pH of the mixture.…

A: Henderson equation: pH = pKa + log[CH3COONa]/[CH3COOH] pKa = -logKa

Q: You plan to make a buffer solution with sulfurous acid (H₂SO) and it undergoes dissociation reaction…

A: Henderson-Hasselbalch equation is used to prepare a buffer solution of desired pH: Desired pH is…

Q: If the ph of 24.0 ml of 1.0 M NaOAc is added to 1.0 M of HOAc is 4.97, what's the equilibrium [H+]…

A: The value of pH is given by the following equation pH= -log [H+] Or, [H+] = 10-pH pH of a buffer…

Q: You make 1.00 L of a buffered solution (pH solutions of each component of the buffered solution.…

A: A buffer solution can be made using a weak acid and the conjugate base of the weak acid. For…

Q: A buffer solution contains dissolved C6H5NH2 and C6H5NH3CI. The initial concentration of C6H5NH2 is…

A: A buffer solution is formed by the dissolution of weak acid and its pH and pKa values should be…

Q: A 16.8 mL solution of 0.100 mol L-1 CH3COOH is titrated using 0.150 mol L-1 NaOH. What is the pH of…

A: The balanced equation is CH3COOH (aq) + NaOH (aq) ------> CH3COONa (aq) + H2O (l) Ka for CH3COOH…

Q: An analytical chemist is titrating 215.7 mL of a 0.2900M solution of dimethylamine ((CH, NH) with a…

A: To Calculate the pH, we would first Calculate moles of both compounds and draw an ICE table. Based…

Q: A 19.5 mL solution of 0.100 mol L-1 CH3COOH is titrated using 0.150 mol L-1 NaOH. What is the pH of…

A: Given,Molarity of CH3COOH = 0.100 mol/Lvolume of CH3COOH = 19.5 mLMolarity of NaOH = 0.150…

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 is the pH of a buffer prepared by adding 0.809 mol of the weak acid HA to 0.507 mol of NaA in…

A: we have to calculate the pH of solution

Q: Calculate the pH after the addition of the following volumes of 0.2 M NaOH to 30 mL of 0.2 M H₂X…

A: The question is based on the concept of the pH of the solution.It is defined as a negative logarithm…

Q: Again consider the same buffer solution from the previous question, where [H2CO3] = [HCO3–] = 0.100…

Q: 30 mL of 0.1 M HCI is titrated with 0.1 M CH3NH₂ (Ka = 2.0 x 10-11) solution. Calculate the pH after…

Q: Complete an ICE box using the appropriate concentration values. e. f. Determine the pH at the…

Q: Calculate the pH when 20.0 mL of 0.150 M KOH is mixed with 33.0 mL of 0.300 M HBrO (Ka = 2.5 × 10°)

A: The reaction occurs as follows: KOH + HBrO --> KBrO + H2O The millimoles of KOH=Molarity x Volume…

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

Step 2

Step 3

Step 4

Trending now

This is a popular solution!

Step by step

Solved in 4 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

please answer both for a vote uofront. thanks (Please type answer no write by hend)
A solution contains 0.312 M HA (K₂ = 2.20-10-7) and 0.680 M NaA. What is the pH of this solution? What is the pH of this solution after 0.212 mol of HCI are added to 1.00 L of this solution? What is the pH of this solution after 0.424 mol of HCI are added to 1.00 L of this solution? Question Help: Video Submit Question [11
Consider a buffer solution prepared by adding 0.45 mol of CH3COOK to 1.00 L of 2.00 M CH3COOH. (K₁ = 1.8 x 10-5). If 0.05 mol of HCI is added to this buffer solution the pH of the solution will drop slightly. The pH does not drastically decrease because the HCI reacts with present in the buffer solution. Select one: O a. H₂O O b. CH3COOH O C. CH3COO O d. H+
10 11 12 13 14 15 16 17 18 19 20 A chemist titrates 170.0 mL of a 0.3333 M nitric acid (HNO, solution with 0.1703M NaOH solution at 25 °C. Calculate the pH at equivalence. Round your answer to 2 decimal places. Note for advanced students: you may assume the total volume of the soluțion equals the initial volume plus the volume of NaOH solution added. pH = %3D Submi Continue MacBook Air
Please answer correct and all step please
Let HA represent a weak acid. A 10.0 mL sample of 0.600M HA was titrated with 0.300 M NaOH. The table below is some of the data for this titration. Volume NaOH added (mL) 5.00 10.00 15.00 ? ? pH 6.98 7.46 7.93 ? ? Calculate the following: a) The volume of NaOH needed to reach the equivalence point is mL. (Report value to the correct number of significant figures.) b) The Ka for HA is Report value using no superscripts. For example, Kw = 1.0 x 10-14 or 1.0e-14 (Report value to the correct number of significant figures.) c) The Kp for A is Report value using no superscripts. For example, Kw = 1.0 x 10-14 or 1.0e-14 (Report value to the correct number of significant figures.) d) The pH of the solution at the equivalence point is e) On your sheet of paper, draw a reasonable diagram of the complete titration curve. Label both axis appropriately. Label the volumes and pH values at the MIDPOINT and the EQUIVALENCE POINT.
16) Calculate the Ka (aq., 25 oC) of a 0.525 M weak monoprotic acid that is 6.45% ionized. a) 2.65 x 10–4b) 1.25 x 10–5c) 8.65 x 10–6d) 5.42 x 10–3 e) 2.33 x 10–3f) 7.22 x 10–4
100 mL of 0.10 M NH3 (Kb = 1.8 x 10-5) are mixed with 100 mL of 0.10 M HCN (Ka = 4.9 × 10-10). Which statement is true? (3) The resulting solution is neutral O (2) The resulting solution is basic O (4) No answer is correct as not enough information is given. O (1) The resulting solution is acidic E D Moving to the next question prevents changes to this answer. 4 R F % S T G 6. & 7 H C 8 00 K M Question 2 of 37