375 ml of0.168 M DABCO (a base) solutionare mixed with 85ml of a 0.0110M Sodium hydroxideSolution. Calculate the PH values of the initialsolutions as well as of the mixed solution.State at every step if you have made any neglect.cifwhich onesand argue why theyandBoyes,possible.areркал сдавсоPhan CDABCO24/BABCOH)3.0PRaz (DABCO.Ht | DABCO) = 8.8=

Answered: 375 ml of 0.168 M DABCO (a base)…

375 ml of 0.168 M DABCO (a base) solution are mixed with 85ml of a 0.0110M Sodium hu Solution Calculate the PH Values of the initi solutions as well as of the mixed solution.

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: At what point will a buffer solution cease to moderate changes in ph.

A: A buffer solution is the mixture of weak acid or conjugate base with their respective salts. Buffer…

Q: A buffer solution is made that is 0.385 M in HNO2 and 0.385 M in KNO2. If Ka for HNO2 is 4.50 x 10,…

A: We have to find the pH

Q: Calculate the pH of the solution after the addition of each of the given amounts of 0.0530 M HNO, to…

A: We have to calculate the pH of solution

Q: What is the pH of a buffer solution containing 0.21 M HNO2 and 0.10 M NO, ?

A: Since HNO2 is a weak monoprotic acid with pKa = 3.15 And the solution is given buffer solution with…

Q: A 24.84 mL aliquot of weak acid that has a concentration of 0.58 M will be titrated with 0.32 M…

A: pH of weak acid titrated with strong base can be determined using Henderson hasselbalch equation.

Q: A solution of is known to contain 0.100 M pyridine and 0.300 M pyridinum hydrochloride. The Kb for…

A: The determination of H+ ions which are available in any specific solution is carried out with the…

Q: What are the requirements for a solution to be classified as a buffer solution?

Q: A buffer solution is 0.449 M in HNO, and 0.365 M in KNO, . If K, for HNO, is 4.5×104 , what is the…

A: Introduction : We have to calculate pH of HNO2

Q: It is a common practice to prepare buffer of different pH values from a single acid. Select a single…

A: Firstly this is a very relative question, that will be needing data values. A buffer is effective in…

Q: A 27.69 mL aliquot of weak acid that has a concentration of 0.648 M will be titrated with 0.33 M…

A: Since, you have posted multiple questions, we will answer the first the first one. If you want any…

Q: Determine the pH of a solution that is prepared by mixing 5.0mL hcl solution and that has 20% hcl by…

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

Q: A solution is prepared by diluting 28.6mL of 15.98 molar nitric acid in a total volume of 500mL.…

Q: A solution containing 572.0mL of 0.6300MHCl is diluted to a volume of 1.000L. What is the pH of this…

Q: When 42.6 mL of 0.100 M Ba(OH)2 is mixed with 98.6 mL of 0.200 M HCI, the reaction goes to…

A: A numerical problem based on pH concept, which is to be accomplished.

Q: 375 ml of 0.168 M DABCO (a base) solution are mixed with 85ml of a 0.0110M Sodium hydroxido Solution…

A: The aim is to calculate the pH of the resulting solution. It show that the contribution of both…

Q: The antacid TUMS was titrated using 0.3 m HCl. The buret reading was initally 0.53ml. After reaching…

A: Volume of HCl = Final reading of buret - Initial reading of buret Given that: Initial reading of…

Q: A 27.4 mL sample of 0.224 M ethylamine, C₂H5NH₂, is titrated with 0.379 M hydrobromic acid. After…

A: The question is based on the concept of PH. we need to calculate pH of the given solution after…

Q: A 50.000 mL aliquot of weak acid that has a concentration of 0.305 M will be titrated with 0.550 M…

A: Given: The volume of 0.305 M weak acid is 50.00 mL. The volume of 0.550 M NaOH is 27.727 mL. The…

Q: Buffer systems operate in a roughly 2.0 pH unit range, centered around what value?

A: Effective buffer range of an acidic buffer is from pKa-1 to pKa + 1. Centered value is pKa , at…

Q: An analytical chemist is titrating 118.6 mL of a 0.6400M solution of aniline (C,H,NH,) with a…

Q: What is the term for the amount of acid a buffering solution can handle without a change of pH? O…

A: A buffer solution is defined as the solution which can resist the change in pH on the addition of…

Q: Calculate the molarity determined by titration of the HCl solution. HCl volume = 5ml NaOH…

A: Given that, equivalence titration has; Volume of HCl solution, V1= 5mL Molarity of HCl solution, M1…

Q: Consider the titration of 25.00 mL of 0.100 M nitric acid HNO3 with the 0.100 M KOH. Compute the…

Q: A 38.05 mL aliquot of weak base that has a concentration of 0.577 M will be titrated with 0.39 M…

A: Concentration of weak base = 0.577 M = 0.577 mol/L Volume of weak base solution = 38.05 ml = 38.05…

Q: Discharged volume of NaOH: ? Volume of HCI solution: 10mL pH of the solution over time at the…

Q: A 100.0 mL of 0.1 M HCI solution is mixed with a 50.0 mL of 0.1 M of KOH solution. The resultant…

Q: The pkb values for the dibasic base B are pkb1=2.10 and pkb2=7.58. Calculate the pH at each of the…

Q: hat is buffer capacity, and when it is largest

A: The pH of the solution determines the concentration of H+ in the solution. A higher value of pH…

Q: Calculate the expected pH based on how the solution was prepared, again allowing for any dilution…

A: pH of a buffer solution can be calculated by using Henderson Hasselbalch equation, according to…

Q: in acid-base titration 50.0 mL of a solution of sodium hydroxide is neutralized by exactly 12.50 mL…

A: We know that for acid base titration of H2SO4 and NaOH H2SO4 is dibasic. So, 2M1V1 = M2V2 M1 =…

Q: 1.00g of acetylsalicylic acid is mixed with 120 mL of water. Then, 25.00 mL of the solution is…

A: To calculate the initial concentration of acetylsalicylic acid, we first need to determine the…

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: A 250.0 mL of 0.35 M HCl is mixed with 150.0 mL of 0.50 M NaOH. What is the net ionic equation and…

A: Applying concept of pH PH= -log [H+]

Q: calc ph of solution prepared by mixing 27.14ml of 0.06 M NaOH with 190.05 ml of 0.040M HCI

A: pH =14-pOH pH= -log [H+] pOH=-log [OH-]

Q: A 39.6 mL sample of a 0.270 M solution of NaCN is titrated by 0.330 M HCl. Kb for is CN- is…

A: Balanced Reaction NaCN + HCl --> NaCl + H2O NaCN is a salt of weak acid it reacts with HCl to…

Q: A 29.83 mL aliquot of weak base that has a concentration of 0.542 M will be titrated with 0.712 M…

A: The balanced chemical reaction is as follows B + HCl = BH+ + Cl- BH can reacts with water as given…

Q: Without detailed calculation and RICE table, determine whether the following solutions are acidic or…

A: ( a) Acidic, not buffer b) Basic, Basic buffer c) Acidic, not buffer d) Acidic , not buffer

Q: Calculate the molar concentration of the acid if 19.28 of nitric acid was required to neutralize…

A: Molar concentration of nitric acid to be calculated.

Q: a buffer is prepared by adding 115 mL of .30M NH3 to 135 mL fof .15 M NH4NO3. what is the pH of the…

A: A buffer is prepared by adding 115 mL of 0.30 M NH3 to 135 mL of 0.15 M NH4NO3. The pH of the final…

Q: 100ml of solution contains 0.4 gm caustic soda. in dissolved state. If 50ml of this solution is…

A: Caustic soda is NaOH with molar mass = 40 g/mol Hence moles of NaOH taken X molar mass of NaOH =…

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%

375 ml of
0.168 M DABCO (a base) solution
are mixed with 85ml of a 0.0110M Sodium hydroxide
Solution. Calculate the PH values of the initial
solutions as well as of the mixed solution.
State at every step if you have made any neglect.c
if
which ones
and argue why they
and
Bo
yes,
possible.
are
ркал сдавсо
Phan CDABCO24/BABCOH)3.0
PRaz (DABCO.Ht | DABCO) = 8.8
=

Expert Solution

This question has been solved!

Explore an expertly crafted, step-by-step solution for a thorough understanding of key concepts.

SEE SOLUTION Check out a sample Q&A here

Step 1: Introduction

VIEW

Step 2: Number of moles

VIEW

Step 3: Calculation of pH value

VIEW

Solution

VIEW

Step by step

Solved in 4 steps with 1 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

15.0 L of 1.4M HCI is mixed with 2.0 L of 0.02M NaOH, what pH does this solution have?
Calculate the pH of a solution that is 0.60M HF and 1.00M of KF
Which statement best describes why a buffer solution cannot be made with a strong acid. a The conjugate acid of a strong acid is too strong. b The conjugate base of a strong acid is not a strong enough base to neutralize other acids.
It was assumed: a) Before any acetic acid was added, essentially all the indicator was in the In- form. b) After the HCl was added, essentially all the indicator was in the HIn form. Justify these assumptions using the measured pH of these solutions and your experimental value for pKHIn to determine: 1) The fraction fo the indicator in the HIn form in solution B before any of solution A was added 2) The fraction of the indicator in the In- form after the HCl was added.
A 25.000 mL aliquot of weak base that has a concentration of 0.30 M will be titrated with 0.80 M HCl. Calculate the pH of of the solution upon the addition of 9.375 mL of HCl. The Kb of the base is 4.6×10-6. Report your answer to the hundredths place.
A 31.1 mL sample of a 0.190 M solution of NaCN is titrated by 0.230 M HCl. Kb for is CN- is 2.0x10^-5 Calculate the pH of the solution: 1. after the addition of 35.7 mL of 0.230 M HCl
Phosphorous acid, H3PO3(aq), is a diprotic oxyacid that is an important compound in industry and agriculture. ???1 ???2 1.30 6.70 Calculate the pH for each of the points in the titration of 50.0 mL of 2.4 M H3PO3(aq) with 2.4 M KOH(aq). 1. Before any addition of KOH 2. After addition of 25 mL of KOH 3. After addition of 50 mL KOH
Give correct answer with explanation?.
An analytical chemist is titrating 187,7 ml. of a 0.4400M solution of isopropylamine ((CH,), CHNH,) with a 0.6800M solution of HNO,. The pK, of isopropylamine is 3.33. Calculate the pH of the base solution after the chemist has added 18.5 ml. of the HNO, solution to it. Note for advanced students: you may assume the final volume equals the initial volume of the solution plus the volume of HNO, solution added. Round your answer to 2 decimal places.
TRUE OR FALSE Acid neutralizing capacity is a measure of overall buffering capacity against alkalinization for a solution
If 50mL of 0.10M NaOH is added to 50mL of 0.10M monoprotic weak acid, the resulting pH of the solution will be?
Give answer all sub parts if you not then don't give answer. I will give you upvote