Using the table of the weak base below, you have chosen Ethylamine as your weak base in the buffer solution. You have already added enough of the conjugate acid salt to make the buffer solution concentration at 0.52 M in this salt. The desired pH of the buffer should be equal to 10.1. Values of K, for Some Common Weak Bases Conjugate Name Formula Acid Ammonia Methylamine Ethylamine NH, CH NH," CH&NH, CH,NH," CH NH 1.8 x 10- 4.38 x 10- 5.6 x 10 3.8 x 10-10 1.7 x 10- NH, CH NH; CH NH, CH,NH, C,H.N Aniline Pyridine 3. Compute the concentration of the weak base in Molarity. (round off final answer to 4 decimal places)

Using the table of the weak base below, you have chosen Ethylamine as your weak base in the buffer solution. You have already added enough of the conjugate acid salt to make the buffer solution concentration at 0.52 M in this salt. The desired pH of the buffer should be equal to 10.1. Values of K, for Some Common Weak Bases Conjugate Name Formula Acid Ammonia Methylamine Ethylamine NH, CH NH," CH&NH, CH,NH," CH NH 1.8 x 10- 4.38 x 10- 5.6 x 10 3.8 x 10-10 1.7 x 10- NH, CH NH; CH NH, CH,NH, C,H.N Aniline Pyridine 3. Compute the concentration of the weak base in Molarity. (round off final answer to 4 decimal places)

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 solution is prepared by combining 3.58 milliliters of 0.3312 M formic acid,128.3 milligrams of…

A: The number of moles of KOH is calculated as shown below.

Q: A 0.1-L unbuffered solution needs the pH adjusted from 3.5 to 2. How many microliters of a 12 molar…

A: pH is used to determine the concentration of hydronium ion.

Q: how to determine the pH

Q: Each row of the table below describes an aqueous solution at 25 °C. The second column of the table…

Q: pH = 6.9 small can be neutralized can not be neutralized is not dissolved large Reset Help When…

A: Buffer solution — A solution which prevents change in pH on adding small amount of any acid or base…

Q: Give a sentence or two on what you would do to complete the preparation of your buffer. You add 0.20…

A: Calculation of pKa of the acid: Calculation of the concentration of the conjugate base (salt):

Q: Answer the following three questions based on the information given below. Consider a buffer made…

A: Buffer are the solution which try to resist any change in pH by addition of acid or base

Q: A solution is prepared that is initially 0.20M in trimethylamine ((CH3)2N).. a weak base, and 0.070M…

A: Step 1: Given[(CH3)3N] = 0.20 M[(CH3)3NHCl] = [(CH3)3NH+] = 0.070 MComplete the reaction table = ?…

Q: Calculate the pH of a buffer solution that is prepared by mixing 8.02 ml of a 0.200 M solution of a…

A: We have to calculate the pH of the buffer solution .

Q: You are studying a clear solution and you added the pH indicator methyl violet. The colour range of…

A: The color of a solution of pH 0.2 is needed to be determined on the addition of an acid-base…

Q: At what point (how many milliters of added acid) was the solution in beaker “B” neutralized?…

A: NaHCO3 + CH3COOH ---> CH3COONa + H2O Sodium bicarbonate reacts with acetic acid which is present…

Q: A 10.0 mL solution of 0.540 M NH, is titrated with a 0.180 M HCl solution. Calculate the pH after…

A: The objective of this question is to calculate the pH of a solution of NH3 after the addition of…

Q: None

A: Step 1: To begin answering this question, we must first determine the concentration of each species…

Q: what do I need to calculate the theoretical pH if my buffer solution has 0.50 M of a ethyl alcohol…

A: Theoretical pH of a buffer solution is calculated using the Henderson-Hasselbalch Equation written…

Q: 10mL of solution B has 10mL of water added to it, how does this effect the pH - what two solutions…

A: #Part-1: 10 mL solution-B + 10 mL water: # pH before the addition of water: Dissociation equation of…

Q: A chemist adds a chemical to pure water and there is a 100-fold incre approximation of the new pH…

A: The objective of the question is to calculate the new .

Q: The buffer from the above question was made by mixing 150.0 mL of 0.10 M HC7H502 with 100.0 mL of…

A: To calculate the pH of the solution formed by mixing HC7H5O2 (benzoic acid) and NaC7H5O2 (sodium…

Q: References Use the References to access important values if needed for this question. A 29.5 mL…

A: Given,Molarity of CH3NH2 = 0.265 Mvolume of CH3NH2 = 29.5 mLMolarity of HI = 0.330 Mvolume of HI…

Q: An analytical chemist is titrating 57.8 mL of a 0.6200M solution of methylamine (CH,NH,) with a…

Q: The phenolphthalein pH indicator is clear and colorless in an acidic solution, but it turns a pink…

A: Given: Acidic solution contains phenolphthalein and you add a drop of Solution 1 to Solution 2. A…

Q: In general, adding a strong acid or a strong base to a buffer solution _________ neutralizes the…

A: Buffer solution is the solution which resist change in pH on addition of small amount of acid or…

Q: An analytical chemist is titrating 88.9 mL of a 0.2700M solution of ammonia (NH3) with a 0.4900M…

A: Ammonia, NH3(aq) is a monoacidic weak base with pKb = 4.74 HIO3(aq) is a monoprotic strong acid.…

Q: Assuming the final solution will be diluted to 1.00 L , how much more HCl should you add to achieve…

Q: Using the table of the weak base below, you have chosen Pyridine as your weak base in the buffer…

A: We have find out the values of PKb by using formula PKb= -log kb.

Q: Which of the following is true of a buffer solution that contains equivalent amounts of acid and…

A: buffer solution that contains equivalent amounts of acid and conjugate base means [Conjugate base ]…

Q: The final volume of buffer solution must be 100.00 mL and the final concentration of the weak acid…

A: In the above question given that - Final volume of buffer solution =100.00 ml Final concentration…

Q: I don't know if it is possible, but I have to make a solution of acetic acid with a pH of 4 and a…

A: Required pH of Acetic acid solution = 4 Volume of acetic acid solution required = 250 mL Volume of…

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

Step 3

VIEW

Trending now

This is a popular solution!

Step by step

Solved in 3 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

What is a description of the salt that is used in a buffer solution? from the conjugate base from a weak acid O from the conjugate base of a weak base from the conjugate acid of a weak acid O from the conjugate acid of a strong base
A solution is prepared that is initially 0.41 M in trimethylamine ((CH N, a weak base, and 0.40M in trimethylammonium bromide ((CH,)¸NHB"). Complete the reaction table below, so that you could use it to calculate the pH of this solution. Use x to stand for the unknown change in [OH]. You can leave out the M symbol for molarity. [CH.),N] [CH),NH] [on] initial change final olo X O O
A 0.1-L unbuffered solution needs the pH adjusted from 4 to 1. How many microliters of a 12 molar HCl solution need to be added to adjust the pH? Report your answer to four decimal places. For this question: Assume the volume of HCl being added is negligible and the total volume of the solution does not change. The volume of the solution is *not* 1 L like it was in the practice pools. The question requests your answer be reported in μL (microliters)!!
7 of 21 I Review | Constants | Periodic Table Part A You need to produce a buffer solution that has a pH of 5.21. You already have a solution that contains 10. mmol (millimoles) of acetic acid. How many millimoles of acetate (the conjugate base of acetic acid) will you need to add to this solution? The pKa of acetic acid is 4.74. Express your answer numerically in millimoles. • View Available Hint(s) ΑΣφ mmol acetate
pH: 3 [H*]: 10-3 M [OH]: 10-11 M 14 1 1 7 · 10-7 10-7 10-14 10-14 Dip litmus paper into the solution or add a drop of universal indicator. Use the sliders to change the pH of the solution and observe the effect on the indicators. Click Reset to start over. Help Reset The solution turns orange when the univeral indicator is added to it. Is the solution basic, acidic, or neutral?
For each of the salts (assume at this point completely soluble), write the equation for dissociation and label the ions as acidic, basic or neutral.Each salt listed will 100% dissociate NH4C2H3O2 Al2(CO3)3 Na2HPO4 NaI For each of the following salts, determine the pH of a 2.50M solution of the salt.You will need the Ka and Kb tables to complete this problem. NaBrO CH3NH3Cl NaClO2 C6H5OK CsNO3 C6H5NH3Br
explain why the ph doesnt change significantly when a small amount of an acid or a base is added to a solution that contains equal amounts of the base NH3 and a salt of its conjugate acid NH4CL
Will 260.0 milligrams of calcium carbonate raise the pH of 75.0 milliliters of stomach fluid from a low pH of 1.00 into the normal pH range of 1.50-3.50? In the last discussion, you calculated that 260.0mg of calcium carbonate is 0.2600g of calcium carbonate. The next step is to figure out the formula of calcium carbonate and to calculate the molar mass of calcium carbonate in grams per mole. Submit a reply that that tells how you decided to approach the problem and shows the work that results in an answer. Use correct units and significant figures and correct symbols for elements and math. In addition, select another student's explanation that makes sense to you and reply with a comment about the insight you gained from their answer. Calcium carbonate is an ionic compound. Ionic nomenclature is in section 2.8. Molar mass is described on page 74 in section 2.8 of the textbook.
You have chosen Methylamine as your weak base in the buffer solution. You have already added enough of the conjugate acid salt to make the buffer solution concentration at 0.48 M in this salt. The desired pH of the buffer should be equal to 9.75. To prepare the buffer, a total volume of 550 mL is required. The stock solution of the weak base is available at 1 gallon with a concentration of 0.98 M. (Remember the lesson on dilution: C1V1=C2V2) 4. How many mL should be taken from the stock solution to prepare the desired buffer solution? (round off final answer to 1 decimal place)
A buffer solution is prepared by combining 0.848 moles of formic acid and 0.719 moles of sodium formate. What will the solution pH be if 0.126 moles of sodium hydroxide (NaOH) is added to the buffer solution? The K₂ of formic acid is 1.8 x 10-4. (Two decimal places) Type your answer...
both parts please
Suppose 90.00 mL of 0.200M HCl is added to an acetate buffer prepared by dissolving 0.100 mol of acetic acid and 0.110 mol of sodium acetate in 0.100 L of solution. What are the initial and final pH values? What would be the pH if the same amount of HCI solution were added to 190 mL of pure water? Initial pH = Final pH pH after HCl is added to water =