Answered: What quantity in moles of CH3NH;CI need…

What quantity in moles of CH3NH;CI need to be added to 200.0 mL of a 0.500 M solution of CH3NH2 (Kb for CH;NH2 is 4.4 x 10-4) to make a buffer with a pH of 10.85?

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: What is the pH of a buffer that is composed of 121 mL of 0.10 M CH3COOH and 81 mL of 0.10 M…

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: How many grams of solid potassium butanoate (CH,CH;CH;CO,K, 126.196 g/mol) would have to be added to…

A: Given : Volume of solution = 325 mL = 0.325 L (Since 1…

Q: how many grams of NH4Cl must be added to 1 liter of 1.0 M NH4OH solution to prepare a buffer…

Q: A beaker with 2.00×10² mL of an acetic acid buffer with a pH of 5.000 is sitting on a benchtop. The…

A: Henderson-Hasselbalch equation is used for the pH of buffer solution. pH =pKa +log[CH3COO-][CH3COOH]…

Q: What is the [H3O+] and the pH of a benzoic acid-benzoate buffer that consists of 0.12 M C6H₂COOH and…

A: Recall the data from the question, Molarity of C6H5COOH=0.12 M Molarity of C6H5COONa=0.43 M Ka of…

Q: A buffer is prepared by adding 150mL of KOH 1.00M to 250mL of KH2PO4 1.00M. Calculate the moles of…

A: A buffer is prepared by adding 150mL of KOH 1.00M to 250mL of KH2PO4 1.00M. after adding HCl the pH…

Q: A chemistry graduate student is given 300. mL of a 1.10M dimethylamine ((CH3)2NH) solution.…

Q: what is the pH of a buffer made from 0.350 mol of HBrO (ka = 2.5 * 10^-9) and 0.120 mol of KBrO in a…

A: Given,moles of HBrO = 0.350 molmoles of KBrO = 0.120 molvolume of solution = 2.0 LKa of HBrO = 2.5 x…

Q: How many grams of dry NH,Cl need to be added to 2.00 L of a 0.800 M solution of ammonia, NH3, to…

A: Given, Concentration of NH3, [NH3] = 0.8 MVolume of solution, V = 2 LpH = 8.64Base dissociation…

Q: Which is the best solution to buffer at pH = 10.50? (A) A buffer solution containing 0.25…

A: Henderson-Hasselbalch equation The equation that is used to calculate the pH of a buffer solution is…

Q: Suppose that a 1000 mL buffer (pH=5) solution will be prepared using 2.6g C6H5COOH (its Ka is…

A: Molecular weight of C6H5COOH = 122 So, 2.6 g of C6H5COOH = 2.6122mole = 0.021 mole Thus,…

Q: 6. A buffer solution contains 0.10M benzoic acid (C6H5COOH, Ka = 6.3 x 105) and 0.10M potassium…

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: What is the pH of a buffer that is 0.41 M HCN(aq) and 0.87 M NaCN(aq)? The Ka of HCN is 6.2 x 10-10.…

A: A numerical problem based on Henderson equation, which is to be accomplished.

Q: A solution contains 0.329 M HA (K₂ = 5.65 · 10−4) and 0.551 M NaA. What is the pH of this solution?…

Q: A chemistry graduate student is given 300. mL of a 1.70M trimethylamine ((CH3), N) solution.…

Q: а A chemistry graduate student is given 450. mL of a 0.90M chloroacetic acid (HCH2CICO₂) solution.…

A: The image contains a detailed chemistry problem with the following information:A chemistry graduate…

Q: What is the pH of the buffer 0.13 M Na₂HPO4/0.16 M KH₂PO4? Round your answer to 2 decimal places.…

A: A buffer is a solution which resist any change in pH on adding a small amount of acid or base . it…

Q: If you have 50.0 mL of a 0.125 M acetic acid, HC,H,O, what mass of sodium acetate, NaC,H,O,, should…

A: Given: pH of the solution= 5.25 Volume ov the solution= 50 mL=0.05 L pKa of acetic acid = 4.76…

Q: What ratio of NaCN to HCN is needed to prepare a pH 9.90 buffer? (Ka of HCN is 4.9 × 10-10)

Q: 6. How many grams of KOH must be added to 500.0 mL of 2.0 M CH3COOH to prepare a 30 [1] sri…

Q: What is the pH of a buffer prepared by mixing 20.0 g of ethylamine CH3CH2NH2, and 20.0 g of…

Q: A chemistry graduate student is given 100. mL of a 1.80M trimethylamine ((CH3),N) solution.…

A: Data given: Volume of triethylamine ((CH3)3N) solution = 100 mL = 0.1 L (1 L = 1000 mL)…

Q: What will be the pH of the solution prepared by dissolving 8.35 g of aniline hydrochloride (C6H5NH3…

Q: Lactic acid, (CH3CH(OH)COOH) is a common biomolecule which can accumulate inmuscles during intense…

A: The objective of this question is to calculate the pH of a buffer solution prepared by mixing lactic…

Q: HEPES is commonly used to make physiological buffers and undergoes the following dissociation:…

A: Given: Concentration of buffer = 0.1000 M pH of buffer = 7.20 Volume of buffer = 2.000 L Molar mass…

Q: 50ml of 1.00M acetic acid, CH3COOH, is tritated with 2.00 M NaOH . find the PH of the solution at…

A: We would use Henderson-Hasselbalch to calculate the pH ate half equivalence point. The volume of…

Q: What mass (in g) of sodium formate, HCOONa, must be added to 10.0 L of a 0.483 M aqueous solution of…

A: Here, we have to find the mass of sodium formate that must be added to 10.0 L of a 0.483 M aqueous…

Q: What is the pH of a buffer that is 0.41 M HCN(aq) and 0.87 M NaCN(aq)? The Ka of HCN is 6.2 x 10-10.

A: Using Henderson Hasselbalch equation we can calculate pH of a buffer

Q: 50.0 ml of 0.1 M NaOH is added to 100.0 ml of 0.2 M HCN (Ka=6.2x10-10). What is the pH of the…

A: A buffer solution is a mixture of weak acid and its conjugate base or weak base and it's conjugate…

Q: A student made a mistake while preparing an acetic acid/acetate buffer. They intended to prepare…

Q: What is the pH of a buffer solution with 0.21 M Pyridine (C5 H5 N) and 0.35 M pyridine chloride ( C5…

A: • Given that the concentration of pyridine base is 0.21 M in buffer solution. • And the…

Q: A buffer solution contains 0.19 mol of hypochlorous acid (HClO) and 0.63 mol of sodium hypochlorite…

Q: 12 a C Consider a buffer made by adding 132.8 g of NaC,H₂O₂ to 300.0 mL of 1.51 M HC₂H₂O₂ (Ka = 6.3…

A: A buffer is a solution which resists any change in pH on adding a small amount of acid or base. It…

Q: The pH of a bicarbonate-carbonic acid buffer is 6.18. Calculate the ratio of the concentration of…

A: The ratio of [H2CO3] to that of [HCO3-] is determined by using Henderson-Hasselbalch equation.

Q: 6. A buffer solution contains 0.1OM benzoic acid (C,H5COOH, Ka = 6.3 x 10) and 0.10M potassium…

A: pH can be calculated by using henderson equation pH = pka + log (salt/ acid) Pka = - log 6.3 x10-5…

Q: How many grams of dry NH4 Cl need to be added to 2.10 L of a 0.100 M solution of ammonia, NH3, to…

A: Given: Volume of ammonia solution = 2.10 L Molarity of ammonia solution = 0.100 M pH of buffer…

Q: a) What is the pH of a buffer prepared by adding 0.506 mol of the weak acid HA to 0.507 mol of NaA…

A: the solution is as follows:

Q: What volume in mL of 0.2572 M NaOH must be added to 500.0 mL of 0.1000 M chlorous acid (HClO2, Ka =…

A: Given: pH = 2.25 Concentration of HClO2 = 0.100 M Volume of HClO2 = 500.00 mL Concentration of NaOH…

Q: What are the [H₃O⁺] and the pH of a propanoic acid–propanoate buffer that consists of 0.35 M…

A: First of all write the equation for given compound: CH3CH2COONa→CH3CH2COO-+Na+ CH3CH2OOH=0.15…

Q: buffer consists of 0.30 M ethylamine (C2H5NH2) and 0.40 M C2H5NH3Cl. What is the pH after 5.04 g of…

Q: How many mL of 1.0 M NaOH must be added to 100. mL of 0.050 M HC2H3O2 to make a buffer with a pH =…

A: We have given that pH = 5.0 Ka = 1.8×10-5 Pka = -log(1.8×10-5) = 4.74 Concentration of Acetic Acid =…

Q: Calculate the pH of a buffer that is 0.208 M lactic acid, HC3H5O3, and 0.208 M sodium lactate,…

A: Given that: Molarity of lactic acid = 0.208 M…

Question

100%

What quantity in moles of CH3NH;CI need to be added to 200.0 mL of
a 0.500 M solution of CH3NH2 (Kb for CH3NH2 is 4.4 x 10-4) to make
a buffer with a pH of 10.85?

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

SEE SOLUTION Check out a sample Q&A here

Similar questions

A buffer solution contains 0.53 mol of hydrosulfuric acid (H2S) and 0.10 mol of sodium hydrogen sulfide (NaHS) in 8.70 L.The Ka of hydrosulfuric acid (H2S) is Ka = 9.5e-08.(a) What is the pH of this buffer?pH = ____(b) What is the pH of the buffer after the addition of 0.44 mol of NaOH? (assume no volume change)pH = ____(c) What is the pH of the original buffer after the addition of 0.02 mol of HI? (assume no volume change)pH = ____
2. What is the pH of a buffer prepared by mixing 5.0 g of ammonia (NH3) and 20.0 g of ammonium chloride (NH4CI) in enough water to form 2.50L of solution. The Kb of ammonia is 1.76 x 10-5.
You have 150 mL of 1 M ammonia solution (pKa=9.25). What volume of 1 M hydrochloric acid is needed to prepare buffer with pH=9.5?
How many moles of CH3NH3CI need to be added to 200.0 mL of a 0.500 M solution of CH:NH2 (Kb for CH:NH2 is 4.4 × 10 4) to make a buffer with a pH of 11.00?
A chemistry graduate student is given 125. mL of a 1.20M dimethylamine ((CH3)₂NH) solution. Dimethylamine is a weak base with K₁=5.4 × 10-4. What mass of (CH3)NH₂Br should the student dissolve in the (CH3) NH solution to turn it into a buffer with 2 pH = 11.05? You may assume that the volume of the solution doesn't change when the (CH3)NH₂Br is dissolved in it. Be sure your answer has a 2 unit symbol, and round it to 2 significant digits.
A 25.0 mL sample of 0.450 M (CH3)2NH is titrated with HBr. What is the pH of the solution after 30.0 mL of 0.375 M HBr have been added to the methylamine solution? ((CH3)2NH; Kb Give answer to 2 decimal places. = 5.9×10-4)
Please don't provide handwritten solution...
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 buffer with a pH of 4.20? Ka (HC2H3O2) = 1.8 x 10-5
The Ka of bromoacetic acid is 2.00 ×10–3. What masses of bromoacetic acid (CH2BrCOOH) and sodium bromoacetate (CH2BrCOONa) are needed to prepare 1.00 L of pH = 2.100 buffer if the total concentration of the two components is 0.200 M? ? g of bromoacetic acid ? g of sodium bromoacetate
A chemistry graduate student is given 300. mL of a 1.60M pyridine (C H,N) solution. Pyridine is a weak base with K,=1.7 × 10 What mass of CH,NHC1 should the student dissolve in the CH,N solution to turn it into a buffer with pH = 5.16? 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 to 2 significant digits.
Caleulate the pH of the following two buffer solu- tions: (a) 2.0 M CH;COONA/2.0 M CH3COOH, (b) 0.20 M CH;COONA/0.20 M CH;COOH. Which is the more effective buffer? Why? 16.12
Which of the following 1.0 L solutions would produce a buffer with a pH of approximately 3.2? O A solution of 6.3 x 104 moles of HNO3. O A solution of 0.100 moles of NH3 (Kp 1.8 x 10-5) and 0.100 moles of NH,CI. O A solution of 0.100 moles of HBr and 0.099 moles of NaOH. O A solution of 0.100 moles of HF (K, = 6.4 x 10 4) and 0.100 moles of KF. O A solution of 0.100 moles of CH;CO,H (K, 1.8 x 10-) and 0.100 moles of NACH,CO2.