A 1.0 M solution of a compound with 2 ionizable groups (pKa’s = 6.2 and 9.5; 100 mL total) has a pH of 6.8. If a biochemist adds 60 mL of 1.0 M HCl to this solution, the solution will change to pH: A) 5.60 B) 8.90 C) 9.13 D) 9.32 E) The pH cannot be determined from this information.

A 1.0 M solution of a compound with 2 ionizable groups (pKa’s = 6.2 and 9.5; 100 mL total) has a pH of 6.8. If a biochemist adds 60 mL of 1.0 M HCl to this solution, the solution will change to pH: A) 5.60 B) 8.90 C) 9.13 D) 9.32 E) The pH cannot be determined from this information.

Principles of Modern Chemistry

8th Edition

ISBN:9781305079113

Author:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Publisher:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Chapter15: Acid–base Equilibria

Section: Chapter Questions

Problem 55P

See similar textbooks

Related questions

Q: 5. The pK,'s for phosphoric acid represent the following ionizations: H;PO4 2 H2PO4 + H* pK = 2.14…

A: Chemical reaction between H3PO4 and NaOH is: H3PO4+3NaOH→Na3PO4+H2O

Q: The pka values of a compound with two ionizable groups are pk1 = 4.10 and pk2 between 7 and 10. A…

A: Given, pK1=4.10 pK2 = between 7 and 10 Calculating the values of pK2. By using the…

Q: Please calculate the pKa of hydrofluoric acid given that HF(aq) and hydrogen cyanide (HCN). HF(aq):…

A: Molarity of HF = 5nM Molarity of HCN = 5nM

Q: A primary amine R-NH2 has pKb=5.15 at 25°C. A buffer solution is made by adding 1.27 moles of R-NH2…

Q: The following observations are made about a diprotic acid H2A: (i) A 0.10 M solution of H2A has…

A: pH of a 0.10 M solution of H2A is 3.10 and 0.10 M solution of a salt NaHA is acidic.

Q: Question 1

A: From the given dissociation of sodium formate-

Q: A 11 mM solution of a compound with a pKa = 6.5(1L total) has a pH of 7.5.If a biochemist adds 9…

Q: The pH of an aqueous solution of weak monoprotic acid is 3.15. What is the initial…

A: All the details are explained in handwritten solution.

Q: Strong acid and strong base Strong acid and weak base C. Weak acid and their conjugate base D. Weak…

A: Buffers are mixture of either weak acid and it's conjugate base or weak base and it's conjugate…

Q: 2. Lakes that have been acidified by acid rain can be neutralized by liming, the addition of…

A: The concentration of hydronium ions of the lake, pH=-log[H3O+] Given, pH is 5.5.…

Q: = Report - Goog X ed Scholarship Ap CovalentActivity.do?locator-assignment-take NGLSync Porta OWLv2…

Q: a. In the laboratory a student measures the percent ionization of a 0.537 M solution of formic acid…

A: The question is based on the concept of equilibrium. we have been given a weak acid formic acid…

Q: Write your answer in the space provided. Show your calculations to get full credit. A 1.0 M…

Q: 28. What is the pH of a 0.62 M NH;NO3 solution at 25 °C? * [Kb for NH, is 1.76 × 10*] A. 2.48 В.…

A: Ammonium nitrate is a slat of weak base, ammonium hydroxide and strong acid, nitric acid.…

Q: Calculate the pH of a 1000 mL solution prepared by dissolving in water 0.600 mol of a weak acid HA…

Q: ver 80 % industry area has reported acid rain due to harmful gases emissions. Josephine collected a…

A: Ans. a) pH of the rainwater sample = 4.35 -log[H+] = pH…

Q: An analytical chemist is titrating 178.7 mL of a 0.8900 M solution of trimethylamine ((CH3),N) with…

A: Given: Molarity of triimethyl amine = 0.8900 M Volume of trimethyl amine = 178.7 ml Molarity of HNO3…

Q: 40. 0.05 mol of ammonium nitrate, NH-NCs was dissolve in water in a mL volumetric flask. Compute the…

A: Number of moles of ammonium nitrate, NH4NO3 = 0.05 mol Volume of the flask = 100 mL = 0.100 L (1 L =…

Q: A 1.482 g sample of N-2-acetamido-2-aminoethane-sulfonic acid potassium salt (ACES¯K*, MW = 220.29…

A: The reaction is, From the above equation, 1 mole of HCI reacts with 1 mole of ACES-K to produce 1…

Q: 0.270 M monoprotic weak acid solution has a pH of 2.50. What is the pKa of this acid? a. 4.43 b.…

A: Given: Concentration of weak acid = 0.270 M pH of solution = 2.50

Q: a) If the pH value of an aqueous solution of trimethylamine [(CH3)3N] is 10.75, what should be the…

A: Given, pH of the solution = 10.75 molarity of the solution = ? Kb = 6.3 × 10-5 The balance chemical…

Q: 1,2-diaminoethane, H2N-CH2-CH2-NH2, is used extensively in the synthesis of compounds containing…

A: The dissociation reaction is given as, H2N-CH2-CH2-NH2 + H2O →H2N-CH2-CH2-NH3+ + OH-

Q: Solutions of calcium salts of the acids in the following table are prepared with an initial…

Q: 2,What is the pH of the solution with hydronium ion concentration of 6.3 x 10-12 M? Group of…

A: We’ll answer the first question since the exact one wasn’t specified. Please submit a new question…

Q: Ethylamine (C2H5NH2) has a Kb value of 4.5x10–4. Calculate the pH of a buffer solution that is…

Q: Calculate the pH of a 0.005 M Na2HPO4 solution. pKa1 = 2.15, pKa2 = 7.2, pKa3 = 12.35 Make no…

A: For amphiprotic salt having pH = (Ka1 + Ka2)/2 Where Ka1 is dissociation constants for acid from…

Q: Methylamine CH3NH2 is a weak base with pKb =3.36. What is the value of Ka for the trimethylammonium…

A: Answer: This question is based on conjugate acid-base pair.

Q: LiF has a pKsp of 2.77. HF has a pKa of 3.17. LiF is dissolved at 0.250 F after addition of strong…

A: Formality is the number of formula mass in gram present per litre of a solution. Formula mass of…

Q: A 1.384 g sample of N-2-acetamido-2-aminoethane-sulfonic acid potassium salt (ACES¬K*, MW = 220.29…

A: The reaction is ACES-K + HCI ACES + KCI One mole of HCl reacts with one mole of ACES-K to give one…

Q: A 1.305 g sample of N-2-acetamido-2-aminoethane-sulfonic acid potassium salt (ACES-K+, MW = 220.29…

Q: Chemistry can you answer it with full steps PLEASE DO NOT USE ice to solve it Q3- How many…

A: 2,2'-bipyridinium ion is a weak acid with Ka = 4.6*10-5 2,2'-bipyridine is the conjugate base of…

Q: A 1.083 g sample of N-2-acetamido-2-aminoethane-sulfonic acid potassium salt (ACES K*, MW = 220.29…

Q: Consider a solution initially containing 0.30 M of CH3NH2 mixed with 0.50 M of CH3NH3Cl in water.…

Q: Calculate the pH of a 1000 mL solution prepared by dissolving in water 0.600 mol of a weak acid HA…

A: Interpretation - To determine the pH of a 1000 mL solution prepared by dissolving in water 0.600…

Q: Calculate the pH of a 0.105 M solution of ethylenediamine (H,NCH,CH,NH,). The pKa values for the…

A: The pH of 0.105 M ethylene diamine solution is needed to calculated given that the pKa values of…

Q: Calculate the pH of a 0.10 M solution of potassium acetate. The pKa for acetic acid = 4.76 (at…

A: Given, 0.10 M solution of potassium acetate. The pKa for acetic acid = 4.76 (at 25°C)

Q: The pKa of MOPS is 7.20. Draw the equilibrium involved in the dissociation of the proton. 1. Suppose…

A: Hi, as you have posted multiple questions and have not mentioned which question you want us to solve…

Q: Calculate the pH of each of the following buffered solutions. Ka of acetic acid = 1.8 x…

A: Since you are asked for multiple sub parts, we are entitled to solve first three only.

Q: How many mL of 0.600 M NaOH should be added to 5.38 g of carbonic acid (H2CO3, FW = 60.02) (pKa1 =…

Q: Calculate how many milliliters of 0.140 M HNO3 should be added to 200 mL containing 2.00 g K2CO3…

A: Here we have to determine the volume in ml of HNO3 solution of 0.140M to be added to 200ml of so2 g…

Q: The pH of an aqueous solution of weak monoprotic acid is 3.15. What is the initial…

A: Given that pH of weak monoprotic acid = 3.15 pKa for weak monoprotic acid = 5.74 For weak acid, pH…

Q: In the laboratory, a general chemistry student measured the pH of a 0.423 M aqueous solution of…

Q: Calculate the pH of a solution formed by mixing 200.0 mL of 0.30 M HClO with 100.0 mL of 0.20 M…

A: We have 200 ml of weak acid of 0.3M We have 100 ml of 0.2 M of KClO We have to calculate the pH of…

Q: If the pH value of an aqueous solution of trimethylamine [(CH3) 3N] is 10.75, what should be the…

Q: 1. a. Tris (C4H6(OH)3NH2) has a Ka of 7.94 x 10−9. Calculate the Kbfor this compound. b. If a…

A: 1. a. Given that : Ka of Tris (C4H6(OH)3NH2) = 7.94 x 10−9 We have to calculate the Kb for this…

Q: A solution A contains 0.02mol/dm3 CH3COOH(aq) and 0.2mol/dm3 CH3COONa(aq) Calculate the PH of the…

A: pH: pH of solution tells about neutrality of solution. pH is a scale that determine whether given…

Q: Ex 2) Acids and Bases: A solution is obtained by completely dissolving 900 g of sodium hypochlorite…

A: Answer:- This question is answered by using the simple concept of calculation of pH of solution…

Q: Calculate the pH values of the following solutions: a. a 1.0 M solution of acetic acid (pKa = 4.76)…

A: From given data For part (a) pKa=4.76 [CH3COOH]=1.0 M For part (b)…

Q: The pKa of HX is 9.34. Calculate the pH of a 0.418 M solution of HX.

A: We are authorized to answer one question at a time, since you have not mentioned which question you…

Question

100%

A 1.0 M solution of a compound with 2 ionizable groups (pKa’s = 6.2 and 9.5; 100 mL total) has a pH of 6.8. If a biochemist adds 60 mL of 1.0 M HCl to this solution, the solution will change to pH:

A) 5.60

B) 8.90

C) 9.13

D) 9.32

E) The pH cannot be determined from this information.

I believe the answer is A, but I am saying this based on a guess: adding acid will lower the value of 6.8, and out of all the answers only 5.60 is lower than 6.8. But what are the maths and chemistry behind this? I'm not sure.

Thank you for your help.

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 with 7 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

1,2-diaminoethane, H2N-CH2-CH2-NH2, is used extensively in the synthesis of compounds containing transition-metal complexes in water. If pKp1 = 3.29 and pKp2 = 6.44, what is the pH of a 1.66x10-4 M solution of diaminoethane?
The pH of a solution that is 0.5 in MA and 0.3 in HA is 5.40; determine the pKa of the acid.
10) An aqueous solution has [HC/HsO₂) = 0.100 M and (Ca(C7H5O2)2] = 0.200 M. K. = 6.3 × 105 for HC-H₂O₂. The solution volume is 5.00 L. What is the pH of the solution after 10.00 mL of 5.00 M NaOH is added?
23) Consider the titration of a 100.00 mL sample of 0.500 M methylamine, CH,NH, with 1.00 M HC1 (aq., 25 °C). The K, CH,NH,= 4.40 x 10*. Calculate the pH of the solution after 50.00 mL NaOH has been added. a) 4.87 b) 5.56 e) 9.75 c) 7.00 f) 6.46 d) 8.44
The acid dissociation constants for sulfurous acid are: Ka = 1.2 x 10-2 and Kaz = 6.6 x 10-8. (i) Calculate the pH of a solution of 0.100 M H2SO3. (ii) Calculate the pH of a solution of 0.100M NazSO.. (iii) Calculate the pH of a solution resulting when equal volumes of the solutions described in parts (i) and (ii) are mixed.
A compound has two carboxyls and one aminium group. The pKas of the groups are 1.9, 4.2, and 9.3, respectively. A biochemist has 100 mL of a 0.10 M solution of this compound at a pH of 5.6. She adds 39 mL of 0.1 M NaOH. To the nearest hundredth of a unit, what will be the pH of the solution after addition of the NaOH (assume full stirring to reach a new equilibrium)?
What is the resulting pH if 2.0 mL of a 100 mM HCl solution is added to 100 mL of a 10.0 mM solutionof phosphoric acid at pH = 7.0? (The pKa values of phosphoric acid are 2.1, 7.2, and 12.3.)
We dissolve 2.77 g of an unknown acid, HA, in enough water to produce 25.0 mL of solution. The pH of this solution of HA(aq) is 1.33. We titrate this solution with a 0.250 M solution of NaOH. It takes 41.8 mL of the NaOH solution to reach the equivalence point. (a) What is the molar mass of HA? (b) What is the pKa value of HA(aq)? (c) What is the pH at the equivalence point? (d) What is the pH one third along the titration when you still have twice as much HA(aq) as A-(aq)?
Phenylacetic acid (C6H5CH2COOH, simplified here to HPAc is a monoprotic acid. It builds up in the blood of persons with phenylketonuria, that if untreated, causes mental retardation and death. A study of the acid shows that the pH of 0.120 M HPAc is 2.62. What are (a) the Ka and (b) pKa of phenylacetic acid?
In the laboratory, a general chemistry student measured the pH of a 0.532 M aqueous solution of diethylamine, (C₂H5)2NH to be 12.436. Use the information she obtained to determine the K, for this base. K(experiment) =
: pH Titration A student is titrating 150.0 mL of a 0.300 M solution of lactic acid (pka of lactic acid is 3.85) with a 0.250 M solution of NaOH. . NOTE: You can use the generic formula of HA for lactic acid and A- for the conjugate base. 3.1 added. Round your answer to 2 decimal places. Calculate the initial pH of the lactic acid solution, before any NaOH has been pH = 3.2 Calculate the pH of the acid solution after the chemist has added 100.0 mL of the 0.2500 M NaOH solution to it. Round your answer to 2 decimal places. pH = 3.3 Calculate the pH of the acid solution after the chemist has added 200.0 mL of the OH solution to it. Round your answer to 2 decimal places. 0.2500 M pH =
4. Calculate the pH of a salt solution of NH,CI with molar concentration 0.1 M (Kh = 5.71 x 1o1")