HX is a weak monoprotic acid with Ao = 1.79 x 104 µS/cm M. At equilibrium, the concentration of HX was experimentally determined to be 7.28 x 103 M. If the initial concentration of HX is 6.59 x 102 M and Ablank is 3 µS/cm, calculate the experimental conductivity of the weak acid along with the following necessary values. 1. Calculate [H3O+] concentration and [X]. 2. Calculate a. 3. Calculate Am. 4. Calculate Acorr. 5. Calculate Aexp. Report in proper SF.

HX is a weak monoprotic acid with Ao = 1.79 x 104 µS/cm M. At equilibrium, the concentration of HX was experimentally determined to be 7.28 x 103 M. If the initial concentration of HX is 6.59 x 102 M and Ablank is 3 µS/cm, calculate the experimental conductivity of the weak acid along with the following necessary values. 1. Calculate [H3O+] concentration and [X]. 2. Calculate a. 3. Calculate Am. 4. Calculate Acorr. 5. Calculate Aexp. Report in proper SF.

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

HX is a weak monoprotic acid with Λ0 = 1.79 x 104 μS/cm•M. At equilibrium, the concentration of HX was experimentally determined to be 7.28 x 10-3 M. If the initial concentration of HX is 6.59 x 10-2 M and Λblank is 3 μS/cm, calculate the experimental conductivity of the weak acid along with the following necessary values. 1. Calculate [H3O+] concentration and [X-]. 2. Calculate α. 3. Calculate Λm. 4. Calculate Λcorr. 5. Calculate Λexp. Report in proper SF.
The average daily dose recommended by hematologists for drugs is no more than 200 mg in terms of elemental iron. What mass of а) FeSO4·7H2O b) FeCl2·4H2O should be taken to ensure the daily requirement for iron. Will pH of solutions of salts mentioned in a) and b) basic, acidic or neutral. Write equations of hydrolysis.
In which of the following solutions would PbBr₂ be the most soluble? O 0.10 M Pb(NO3)2 O 0.20 M KNO3 0 0.15 M NaBr
A 0.2585 gram amount of H₂C₂O4 is dissolved in approximately 100 mL of 0.5 M H₂SO4. A KMnO4 solution is added to a burette and added to the H₂C₂O₂ solution. A faint colour persists when 22.35 mL of KMnO solution has been added. slowly Calculate the molarity of the KMnO4 solution. A) 0.2294 M B) 0.02235 C) 0.05139 M 0.02927 M
1) For an open system with PCO2=10−3.5 atm what fraction of the total carbonate is in the form of CO32− at pH 10.63? 2) Using paleolimnological methods it is possible to estimate past pH values of surface waters. If the estimate of pH is 5.787 , what is the corresponding PCO2? in atm.
0.28g 0f MBr is dissolved in distilled water and made up to 250mL mark in a volumetric flask. 25 mL of this solution is titrated against 0.019 M silver nitrate solution using eosin as indicator. The end point was obtained at 12.4 mL of AgNO3 solution . Calculate the molar mass of the metal bromide.
A fertilizer railroad car carrying 34,300 gallons of commercialaqueous ammonia (30% ammonia by mass)tips over and spills. The density of the aqueous ammoniasolution is 0.88 g>cm3. What mass of citric acid,C(OH)(COOH)(CH2COOH)2, (which contains three acidicprotons) is required to neutralize the spill? 1 gallon = 3.785 L.
Which has the highest conductivity and why? 0.1 M BaCl2 or 0.1 M NaCl.
Balance the equation and choose the coefficient of the (?) Na2CO3 + HCl → NaCl + H20 + CO2 -> (x)NA2CO3 + (?)HCl → (x)NaCl + (x)H20 + (x)CO2
Magnesium trisilicate, Mg2Si3O8·H2O in medicine is an antacid. Explain theuse of magnesium silicate as an antacid to reduce acidity in the stomach. Give theequation of reaction. For titration of 5 ml of gastric juice, 10 ml of a 0.15 Msodium hydroxide solution were used. Does the patient need to takeMg2Si3O8·H2O (The concentration of hydrochloric acid in the stomach of a healthy person is constant and amounts to 160 mmol/L)?
A sample of impure tin of mass 0.535 g is dissolved in strong acidto give a solution of Sn2+. The solution is then titrated with a0.0448 M solution of NO3-, which is reduced to NO(g). Theequivalence point is reached upon the addition of 0.0344 L of theNO3- solution. Find the percent by mass of tin in the originalsample, assuming that it contains no other reducing agents.
The first step in purifying the urine collected on the ISS is to treat every liter of urine with 20 mL of 1.0 M H2SO4. To simplify the calculations, lets assume that urine is water. a) What is the pH of a solution of 20. mL of 1.0 M H2SO4 added to 1.00 L water? To determine this, you can safely assume that 100% of the H2SO4 reacts to form H3O+ and HSO4- ions. Use pKa2 (1.92) to determine if any more protons are added to the solution from HSO4-.