The ionization constant (Ka ) equation of a monoportic weak, HA, acid is given by ca2 K = (1-0) The use of conductivity meter to test a 0.106 M solution of this weak acid gives a specific conductance, K, 20.24 uS.cm-1. What would be the pKa, (-long Ka), of the acid, if its limiting molar ionic conductivities are A+ = 243 and A. = 74 S.cm2 mol-1? OA 4.41 OB. 6.00 OC 5.53 OD.3.12 OE3.62

The ionization constant (Ka ) equation of a monoportic weak, HA, acid is given by ca2 K = (1-0) The use of conductivity meter to test a 0.106 M solution of this weak acid gives a specific conductance, K, 20.24 uS.cm-1. What would be the pKa, (-long Ka), of the acid, if its limiting molar ionic conductivities are A+ = 243 and A. = 74 S.cm2 mol-1? OA 4.41 OB. 6.00 OC 5.53 OD.3.12 OE3.62

Chemistry: The Molecular Science

5th Edition

ISBN:9781285199047

Author:John W. Moore, Conrad L. Stanitski

Publisher:John W. Moore, Conrad L. Stanitski

Chapter12: Chemical Equilibrium

Section12.3: Determining Equilibrium Constants

Problem 12.3PSP

See similar textbooks

Similar questions

If a solution of dissolved acid has pH = 2.5 and the pka for the acid chemical is 4.3 and you measure the concentration of the conjugate []-base to be 10mm, what is the concentration of the acid in the solution? pH = pka + logi [HA]
The value of Ksp for Mg3(AsO4)2 is 2.1 x 10-20. TheAsO43 - ion is derived from the weak acid H3AsO4 (pKa1 =2.22; pKa2 = 6.98; pKa3 = 11.50). (a) Calculate the molarsolubility of Mg3(AsO4)2 in water. (b) Calculate the pH of asaturated solution of Mg3(AsO4)2 in water.
Calculate the volume, in liters, of 1.666 M KOH that must be added to a 0.129 L solution containing 9.42 g of glutamic acid hydrochloride (H3Glu Cr, MW = 183.59 g/mol) to achieve a pH of 10.39. Glutamic acid (Glu) is an amino acid with pK, values of pK1 = 2.23, pK2 = 4.42, pK3 = 9.95. NH, CH-CH2-CH2- OH Glutamic Acid Hydrochloride
One strategy for dealing with the acidification of lakes is periodically to add powered limestone (CaCO3) to them, resulting in pH of 10.95. Calculate the Ca2+ concentration in the lake. CO2 in atmosphere 370 ppm KH,CO2 = 0.033 mol/(L∙atm) Ka1 = 10-6.3 Ka2 = 10-10.3 Ksp,CaCO3 = 4.57 x 10-9
The value of Ksp for Mg3(AsO4)2 is 2.1 * 10-20. The AsO43- ion is derived from the weak acid H3AsO4 (pKa1 = 2.22; pKa2 = 6.98; pKa3 = 11.50). Calculate the pH of a saturated solution of Mg3(AsO4)2 in water.
Phosphate-buffered saline (PBS) is a solution commonly used in studies of animal tissues and cells. Its composition is 137 mM NaCl, 2.7 mM KC1, 10 mM Na, HPO, (pK, = 2.14), and 1.8 mM KH₂PO, (pK, = 6.86). Calculate the pH and osmolarity of PBS. Give the osmolarity in units of osmoles per liter (osm/L). pH = 7.605 osmolarity 313.0 Incorrect osm/L
An aliquot of 20 ml of skim milk was placed in an Erlenmeyer flask. To the flask was added 3 to 4 drops of phenolphthalein. The sample was titrated in triplicate using a previously standardized NaOH solution 0.101M. The volumes of NaOH spent in the three experiments to reach chemical equivalence were 3.6ml, 3.7ml and 3.5ml. 1) Express the acidity of milk in g/L of lactic acid. 2) Assuming that the only acid present in milk is lactic acid, would you expect the pH corresponding to the equivalence point was 7?.
Write the Henderson-Hasselbalch equation for a propanoic acid solution (CH;CH,CO,H, pKa=4.874) using the symbols HA and A, and the given pka value for propanoic acid in the expression. pH = + log - Using the equation to calculate the quotient [A-]/[HA] at three different pH values. pH = 5.321 ГА УНА] - pH = 4.079 [А УНА] 3 pH = 4.874 [А УНА] %3
A biochemist working with bacteria requires a culture buffered at a pH of 3.6. Which of the following acid/conjugate base pairs is best for preparing this solution? НCО2Н/КСO2Н; Ка - 1.8х10-4 HC2H3O2/NAC2H3O2; Ka = 1.8x10-5 KH2PO4/K2HP04; Ka2 = 6.2x108 O H2CO3/NAHCO3; Ka1 = 4.5x10-7
12a. In the laboratory, a general chemistry student measured the pH of a 0.493 M aqueous solution of benzoic acid, C6H5COOH to be 2.271. Use the information she obtained to determine the Ka for this acid. Kalexperiment) = 12b. In the laboratory, a general chemistry student measured the pH of a 0.493 M aqueous solution of acetic acid to be 2.542. Use the information she obtained to determine the Ka for this acid. Kalexperiment) = 12c. In the laboratory, a general chemistry student measured the pH of a 0.493 M aqueous solution of nitrous acid to be 1.813. Use the information she obtained to determine the Ka for this acid. Ka(experiment) %3D
Strong base is dissolved in 715 mL of 0.600 M weak acid (Ka = 4.12 x 10-5) to make a buffer with a pH of 4.09. Assume that the volume remains constant when the base is added. HA(aq) + OH¯(aq) → H₂O(l) + A¯(aq) Calculate the pKa value of the acid, and determine the number of moles of acid initially present. pKa = initial amount: When the reaction is complete, what is the concentration ratio of conjugate base to acid? [A-] [HA] = How many moles of strong base were initially added? amount added: mol HA mol OH-
Strong base is dissolved in 685 mL of 0.400 M weak acid (K, = 4.21 × 10-) to make a buffer with a pH of 3.98. Assume that the volume remains constant when the base is added. HA(aq) + OH (aq) H, O(1) + A¯(aq) Calculate the pKą value of the acid, and determine the number of moles of acid initially present. pKa initial amount: mol HA When the reaction is complete, what is the concentration ratio of conjugate base to acid? [A ] [HA] How many moles of strong base were initially added? amount added: mol OH-