A chemistry graduate student is given 250. mL of a 1.40M trimethylamine ((CH,) N) solution. Trimethylamine is a weak base with K,=7.4 x 10*. What mass of (CH,) NHC1 should the student dissolve in the (CH,) N solution to turn it into a buffer with pH = 10.85? You may assume that the volume of the solution doesn't change when the (CH,) NHCI is dissolved in it. Be sure your answer has a unit symbol, and round it 圖 to 2 significant digits. olo Explanation Check © 2022 McGraw Hill LLC. All Rights Reserved. Terms of Use | Privacy Center | Accessibility

A chemistry graduate student is given 250. mL of a 1.40M trimethylamine ((CH,) N) solution. Trimethylamine is a weak base with K,=7.4 x 10*. What mass of (CH,) NHC1 should the student dissolve in the (CH,) N solution to turn it into a buffer with pH = 10.85? You may assume that the volume of the solution doesn't change when the (CH,) NHCI is dissolved in it. Be sure your answer has a unit symbol, and round it 圖 to 2 significant digits. olo Explanation Check © 2022 McGraw Hill LLC. All Rights Reserved. Terms of Use | Privacy Center | Accessibility

Chemistry: Principles and Reactions

8th Edition

ISBN:9781305079373

Author:William L. Masterton, Cecile N. Hurley

Publisher:William L. Masterton, Cecile N. Hurley

Chapter14: Equilibria In Acid-base Solutions

Section: Chapter Questions

Problem 26QAP: You want to make a buffer with a pH of 10.00 from NH4+/NH3. (a) What must the [ NH4+ ]/[ NH3 ]ratio...

See similar textbooks

Related questions

Q: chemistry graduate student is given 450. mL of a 1.10M nitrous acid (HNO,) solution. Nitrous acid is…

Q: An industrial chemist studying bleaching and sterilizing pre-pares several hypochlorite buffers.…

A: Handerson Hasselbalch equation – Buffer solution is mixture of weak acid and its conjugate base.…

Q: A chemistry graduate student is given 100. mL of a 1.30 M chloroacetic acid (HCH,CICO,) solution.…

Q: A buffer solution of 300.0 mL is 0.200M in CH3COOH (acetic acid) and 0.300M in sodium NaCH3COO…

Q: A buffer solution contains 0.351 M KHSO3 and 0.344 M K2SO3. If 0.0252 moles of hydroiodic acid are…

Q: A chemistry graduate student is given 450. mL of a 0.30M diethylamine ((C₂H²)₂NH) NH solution.…

Q: A chemistry graduate student is given 500. mL of a 0.60M nitrous acid (HNO,) solution. Nitrous acid…

Q: A solution is prepared that is initially 0.36M in trimethylamine ((CH3),N), a weak base, and 0.19M…

Q: Does the concentration of HC, H,0, increase or decrease when OH is added? O increase O decrease

A: NOTE- Since you've posted multiple questions, we are solving only the first question for you. If you…

Q: A buffer solution contains 0.482 M hydrofluoric acid and 0.389 M sodium fluoride. If 0.0326 moles of…

Q: A chemistry graduate student is given 100. ml. of a 0.10M pyridine (C,H,N) solution. Pyridine is a…

Q: A buffer system is prepared by combining 0.506 moles of ammonium chloride (NH4CI) and 0.720 moles of…

A: we have to calculate the pH of the buffer solution

Q: Calculate the pH of 1.00 L of the buffer 0.92 M CH3COONa/0.97 M CH3COOH before and after the…

A: This is problem of acidic buffer where there is very little change or effect on adding acid or base.

Q: A chemistry graduate student is given 250. mL of a 0.70M dimethylamine ((CH,), NH) solution.…

Q: A chemistry graduate student is given 450. mL of a 1.40M nitrous acid (HNO,) solution. Nitrous acid…

A: Answer :- Mass Of NaNO2 = 1.8 × 102 (g) The mass of NaNO2 needs to be dissolved in 450 mL 1.40 M…

Q: A buffer is prepared by mixing 43.9 g of NH3 and 43.9 g of NH4Cl in 0.548 L of solution. What is the…

Q: A chemistry graduate student is given 300. mL of a 0.90M ammonia (NH,) solution. Ammonia is a weak…

A: GivenVolume of Soloution = 300 mL = 0.3 LMolarity of Ammonia = 0.90 MMoles of Ammonia = Molarity of…

Q: A chemistry graduate student is given 125. mL of a 0.30M benzoic acid (HC H,CO,) solution. Benzoic…

Q: A chemistry graduate student is given 100. mL of a 1.30M benzoic acid (HC,H,CO,) solution. Benzoic…

A: GivenMolarity ofbenzoic acid = HC6H5CO2 =1.30 MVolume of solution = 100 mL = 0.1 LMoles of benzoic…

Q: To fill a 500 mL volumetric flask, 40 g of ammonium chloride (NH4Cl) and 3.2 g of ammonia (NH3) are…

Q: 1. A buffer is formed by mixing 65.0 mL of 0.82 M acetic acid (CH3CO2H) with 80.0 mL of 0.64 M…

Q: A chemistry graduate student is given 250. mL of a 0.10M methylamine (CH3NH2) solution. Methylamine…

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

Q: Determine the molar solubility (?) of Ag2CO3 in a buffered solution with a pH of 5.887 using the…

A: The solubility product constant (Ksp) is a measure of the solubility of a sparingly soluble salt in…

Q: A chemistry graduate student is given 450. mL of a 1.70M hydrocyanic acid (HCN) solution.…

A: Given : Concentration of HCN = 1.70 M Volume of solution = 450 mL = 0.450 L…

Q: A chemistry graduate student is given 450. ml of a 1.10M dimethylamine (CH:) NH) solution.…

Q: A chemistry graduate student is given 450. mL of a 1.10M methylamine (CH,NH,) solution. Methylamine…

Q: A buffer contains 0.010 mol of lactic acid (pKa = 3.86) and 0.050 mol of sodium lactate per liter.…

A: Buffer solutions are solutions that can resist pH changes. Buffer solution contains a weak acid/base…

Q: pH buffer is a solution that resists changes in pH when acids or bases are added to it—typically, a…

A: Given data contains, Volume of the solution is 7.00 L. pH of the solution is 12.00. Total…

Concept explainers

Ionic Equilibrium

Chemical equilibrium and ionic equilibrium are two major concepts in chemistry. Ionic equilibrium deals with the equilibrium involved in an ionization process while chemical equilibrium deals with the equilibrium during a chemical change. Ionic equilibrium is established between the ions and unionized species in a system. Understanding the concept of ionic equilibrium is very important to answer the questions related to certain chemical reactions in chemistry.

Arrhenius Acid

Arrhenius acid act as a good electrolyte as it dissociates to its respective ions in the aqueous solutions. Keeping it similar to the general acid properties, Arrhenius acid also neutralizes bases and turns litmus paper into red.

Bronsted Lowry Base In Inorganic Chemistry

Bronsted-Lowry base in inorganic chemistry is any chemical substance that can accept a proton from the other chemical substance it is reacting with.

Question

A chemistry graduate student is given 250. mL of a 1.40M trimethylamine ((CH,) N) solution. Trimethylamine is a weak base with K, =7.4 × 10 *. What
3
mass of (CH,) NHCI should the student dissolve in the (CH, N solution to turn it into a buffer with pH =10.85?
3
You may assume that the volume of the solution doesn't change when the (CH,) NHC1 is dissolved in it. Be sure your answer has a unit symbol, and round it
to 2 significant digits.
olo
x10
Ar
?
Explanation
Check
© 2022 McGraw Hill LLC. AlL Rights Reserved.
Terms of Use | Privacy Center | Accessibility

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 with 2 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

A buffer solution is prepared by adding 5.50 g of ammonium chloride and 0.0188 mol of ammonia to enough water to make 155 mL of solution. (a) What is the pH of the buffer? (b) If enough water is added to double the volume, what is the pH of the solution?
Sketch the titration curve for a weak acid titrated by a strong base. When performing calculations concerning weak acidstrong base titrations, the general two-slep procedure is to solve a stoichiometry problem first, then to solve an equilibrium problem to determine the pH. What reaction takes place in the stoichiometry part of the problem? What is assumed about this reaction? At the various points in your titration curve, list the major species present after the strong base (NaOH, for example) reacts to completion with the weak acid, HA. What equilibrium problem would you solve at the various points in your titration curve to calculate the pH? Why is pH 7.0 at the equivalence point of a weak acid-strong base titration? Does the pH at the halfway point to equivalence have to be less than 7.0? What does the pH at the halfway point equal? Compare and contrast the titration curves for a strong acidstrong base titration and a weak acidstrong base titration.
A buffer is prepared using the butyric acid/butyrate (HC4H7O2/C4H7O2)acid-base pair. The ratio of acid to base is 2.2 and Ka for butyric acid is1.54105. (a) What is the pH of this buffer? (b) Enough strong base is added to convert 15% of butyric acid to the butyrate ion. What is the pH of the resulting solution? (c) Strong acid is added to the buffer to increase its pH. What must the acid/base ratio be so that the pH increases by exactly one unit (e.g., from 2 to 3) from the answer in (a)?
What is the pH of a buffer that is 0.175 M in a weak acid and 0.200 M in the acids conjugate base? The acids ionization constant is 5.7 104.
When 40.00 mL of a weak monoprotic acid solution is titrated with 0.100-M NaOH, the equivalence point is reached when 35.00 mL base has been added. After 20.00 mL NaOH solution has been added, the titration mixture has a pH of 5.75. Calculate the ionization constant of the acid.
Marble is almost pure CaCO3. Acid rain has a devastating effect on marble statuary left outdoors. Assume that the reaction which occurs is CoCO3(s)+ H+(aq)Ca2+(aq)+HCO3(aq) Neglecting all other competing equilibria and using Tables 15.1 and 13.2, calculate (a) K for the reaction. (b) the molar solubility of CaCO3 in pure water. (c) the molar solubility of CaCO3 in acid rainwater with a pH of 4.00.
What mass of NH4Cl must be added to 0.750 L of a 0.100-M solution of NH3 to give a buffer solution with a pH of 9.26? (Him: Assume a negligible change in volume as the solid is added.)
A buffer is made up of 239 mL of 0.187 M potassium hydrogen tartrate (KHC4H4O6) and 137 mL of 0.288 M potassium tartrate (K2C4H4O6). Ka for is (H2C4H4O6)4.55105. Assuming volumes are additive, calculate (a) the pH of the buffer. (b) the pH of the buffer after adding 0.0250 mol of HCI to 0.376 L of the buffer. (c) the pH of the buffer after adding 0.0250 mol of KOH to 0.376 L of the buffer.
A 1.0-L solution that is 4.2 M in ammonia is mixed with 26.7 g of ammonium chloride. a What is the hydroxide-ion concentration of this solution? b 0.075 mol of MgCl2 is added to the above solution. Assume that there is no volume change. After Mg(OH)2 has precipitated, what is the molar concentration of magnesium ion? What percent of the Mg2+ is removed from solution?
A buffer solution with it pH of 12.00 consists of Na3PO4 and Na2HPO4. The volume of solution is 200.0 mL. (a) Which component of the buffer is present in a larger amount? (b) If the concentration of Na3PO4 is 0.400 M, what mass of Na2HPO4 is present? (c) Which component of the buffer must be added to change the pH to 12.25? What mass of that component is required?
Consider the nanoscale-level representations for Question 110 of the titration of the aqueous weak acid HX with aqueous NaOH, the titrant. Water molecules and Na+ ions are omitted for clarity. Which diagram corresponds to the situation: After a very small volume of titrant has been added to the initial HX solution? When enough titrant has been added to take the solution just past the equivalence point? Halfway to the equivalence point? At the equivalence point? Nanoscale representations for Question 110.
The species called glacial acetic acid is 98% acetic acid by mass (d=1.0542g/mL). What volume of glacial acetic acid must be added to 100.0 mL of 1.25 M NaOH to give a buffer with a pH of 4.20?