A solution originally contains 0.140 mol thioglyoxylic acid (pKg 3.68), a monoprotic acid, and 0.136 mol sodium thioglyoxylate. What is the pH of this solution after the addition of 0.0550 moles of HBr to 1.00 L of this solution? Assume the volume of the solution does not change. Enter your answer to the hundredths place. Your Answer: Answer

A solution originally contains 0.140 mol thioglyoxylic acid (pKg 3.68), a monoprotic acid, and 0.136 mol sodium thioglyoxylate. What is the pH of this solution after the addition of 0.0550 moles of HBr to 1.00 L of this solution? Assume the volume of the solution does not change. Enter your answer to the hundredths place. Your Answer: Answer

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

Similar questions

The pKa of NH3 is estimated to be 35. Its conjugate base, the amide ion (NH2−), can be isolated as an alkali metal salt, such as sodium amide (NaNH2). Calculate the pH of a solution prepared by adding 0.100 mol of sodium amide to 1.00 L of water. Does the pH differ appreciably from the pH of a NaOH solution of the same concentration? Why or why not?
Calculate the pKa of the weak acid HA, given that a solution that is 0.357 in HA and 1.24 in A- has pH = 5.32.Provide your answer rounded to 2 decimal digits.
The simplest amino acid is glycine ( molar mass = 75.1 g/mol), whose structure is shown above. An aqueous solution of glycine is prepared by dissolving 0.329 g in 150 mL of water at a temperature of 25 C. The resulting solution has a pH of 2.02. Calculate the molarity of the solution. Calculate the percent ionization of this solution of glycine. Calculate the Ka for glycine. Glycine is water soluble. On a structural formula like the one above, draw one water molecule that shows how glycine and water can form hydrogen bonds with each other.
A new potential cure for the common cold, code-named Z-123, is being tested by a pharmaceutical company. As a research technician, you are told that Z-123 is a monoprotic weak acid, and the company is interested in the drug's Ka value.To find the pKa of Z-123, you prepare a 0.091 mol/L test solution of the drug. The pH of the solution is determined to be 2.77.What is the pKa of Z-123?Express your answer to two decimal places.pKa = === What is pKb of the conjugate base of Z-123?Express your answer using two decimal places.pKb =
Phosphoric acid is a triprotic acid with the pKa values pKa1=2.148, pKa2=7.198, and pKa3=12.375. You wish to prepare 1.000 L of a 0.0100 M phosphate buffer at pH 7.780. To do this, you choose to mix the two salt forms involved in the second ionization, NaH2PO4, and Na2HPO4, in a 1.000 L volumetric flask and add water to the mark. What mass of each salt will you add to the mixture? What other combination of phosphoric acid and its salts could be mixed to prepare this buffer? H3PO4 and Na3PO4 H3PO4 and Na2HPO4 NaH2PO4 and Na3PO4 Na2HPO4 and Na3PO4 H3PO4 and NaH2PO4
1. Arrange the following in order of increasing pH of their corresponding solutions. a. CH3NH3Cl, NaCH3COO, RbBr b. K2C2O4, C2H5NH3Br, Ba(ClO4)2 2. Oleic acid (which can be denoted as HOL), is a weak acid. Considering its sodium salt, sodium oleate (NaOL), calculate the pKa of HOL given that a 0.100 M solution of NaOL has a pH of 9.01. (hint: Kw=Ka * Kb).
A weak acid HA, has a pKa of 5.0. If 1.0 mol of this acid and 0.1 mol of NaOH were dissolved in one liter of water, what is the final pH?
:::::(((((((( The PH of a 0.2 M solution of a monoprotic acid is 3.45. Calculate the pKa for this acid. What is the percent ionization of acid?
A solution is made by mixing 50.0 mL of a stock solution of 2.0 M K2HPO4 and 25.0 mL of a stock solution of 2.0 M KH2PO4. The solution is diluted to a final volume of 200.0 mL. What is the pH of the resulting solution given that the pKa of H2PO4- is 6.82?
Determine the pH of 0.01 M solutions of Citric Acid, Sodium Dihydrogen Citrate, Sodium Hydrogen Citrate, and Sodium Citrate solutions. Citric Acid has pKas of 3.13, 4.76, and 6.40. For situations where this cannot be done with ICE/small-x approximation, list the simultaneous equations you could have a computer program solve to arrive at the answer.
A 0.015 M solution of hydrogen cyanate (HOCN) has a pH of 2.67. Calculate the hydrogen cyanate concentration, hydronium ion concentration, and cyanate ion concentration in the solution. Calculate the Ka and pKa for the acid.
1. a. The surface of Venus is quite inhospitable with an average temperature of 450 ̊C and a pressure of 92 atm (earth). Under these delightful conditions, the pKw of water is estimated to be 24. What is the pH of neutral water on Venus? b. An aqueous acetic acid (HOAc) solution is 1.00 % dissociated. What will the concentration of H3O+ be if 0.82 g of sodium acetate (NaO2C2H3) is added to 100.mL of solution?