An analytical chemest is titrating 150.6 ml. of a 0.6600 M solution of dhethylamine (C,H,) NH) wth a 0.1500M solution of HIO, The p K, of dethylamine is 2.89. Cakculate the pH of the base solution after the chemest has added 7773 ml. of the HIO, sohuton to . Note for advanced students: you may assume the fnal vokume equals the intal volume of the solution plas the volume of HIO, sokaton added. Round your answer to 2 decimal places please explain and solvel

An analytical chemest is titrating 150.6 ml. of a 0.6600 M solution of dhethylamine (C,H,) NH) wth a 0.1500M solution of HIO, The p K, of dethylamine is 2.89. Cakculate the pH of the base solution after the chemest has added 7773 ml. of the HIO, sohuton to . Note for advanced students: you may assume the fnal vokume equals the intal volume of the solution plas the volume of HIO, sokaton added. Round your answer to 2 decimal places please explain and solvel

Chemistry

9th Edition

ISBN:9781133611097

Author:Steven S. Zumdahl

Publisher:Steven S. Zumdahl

Chapter15: Acid-base Equilibria

Section: Chapter Questions

Problem 8ALQ: You have a solution of the weak acid HA and add some of the salt NaA to it. What are the major...

See similar textbooks

Similar questions

You have a solution of the weak acid HA and add some of the salt NaA to it. What are the major species in the solution? What do you need to know to calculate the pH of the solution, and how would you use this information? How does the pH of the solution of just the HA compare with that of the final mixture? Explain.
A 10.00-g sample of the ionic compound NaA, where A is the anion of a weak acid, was dissolved in enough water to make 100.0 mL of solution and was then titrated with 0.100 M HCl. After 500.0 mL HCl was added, the pH was 5.00. The experimenter found that 1.00 L of 0.100 M HCl was required to reach the stoichiometric point of the titration. a. What is the molar mass of NaA? b. Calculate the pH of the solution at the stoichiometric point of the titration.
. How is the strength of an acid related to the fact that a competition for protons exists in aqueous solution between water molecules and the anion of the acid?
A solution of sodium acetate is prepared using 0.56 mol L-1 NaOH as the solvent. The pKapKa of acetic acid is 4.75 . The concentration of sodium acetate after mixing, before any reaction takes place is 0.44 mol L-1 . Calculate the equilibrium concentrations of all acid species: [ CH3COOH ], [ CH3COO- ], the pH and the pOH in the solution. Some assumptions may not work, on the other hand, if you do not make the correct assumptions first, the quadratic formula will give you the wrong answer. [ CH3COOH ] = ___mol L-1 , [ CH3COO- ] = ___mol L-1 , pH = ___ pOH = ____
1.00g of acetylsalicylic acid is mixed with 120 mL of water. Then, 25.00 mL of the solution is transferred to 3 flasks each. Assuming the pH is 3.00, calculate the initial concentration of , the Ka and pKa.
A titration curve is constructed by plotting the pH of the analyte solution versus the volume ofthe reagent added as the titration progresses. As the equivalence point is approached, there is arapid change in the pH. Titration curves enable us to explain how end points are detected andtheir relationship to equivalence points. They can also serve as guides for choosing the properindicators for a particular acid-base titration. Explain how each plot can be used to interpret the acid-base titration.
The pH of a 0.5L HNO2-NO2 buffer solution was determined to be 4.23. The solution was mixed with 5g of HNO2.Considering that the pKa is 4.35, what is the approximate pH of the new solution? Show all pertinent calculations.The MW of acid = 47g/mol. Illustrate the titration curve of the solution as a diprotic acid. Compute for the optimal pH if 1M of the solution isprepared. Illustrate what happens to the buffer system if additional acid or base is added to the solution. Label allparts accordingly.
Calculate the pH of a buffer prepared by dissolving 0.80 moles acetic acid (CH3COOH) and 0.40 moles of sodium acetate (CH3COONa) in enough water to make 1500 mL of buffer solution. The pKa for acetic acid is 4.74