Please correct answer and don't use hand rating 2. What are the pH values of the following solutions? For each solution below, make a list of the bulleteditems given below and construct a log C-pH diagram spanning the range of log C from 0 to -14 and pHfrom 0 to 14. Solve for the pH of the solution and concentration of each of the species graphically andsolve for the pH mathematically. Assume that the solutions are ideal (Y; ≈1), that the temperature is25°, and that the solutions are closed (no atmospheric exchange).ingredients。 species that will be present at equilibrium。 mass action laws (equilibrium constant equations)。 mole balances。 charge balancea. 10-6.0 M acetic acidAnswers: graphical pH 6.0; mathematical pH 6.02b. 10-2.0 M phenolAnswers: graphical pH 6.0; mathematical pH 5.99c. 10-2.8 M ammonium chlorideAnswers: graphical pH 6.0; mathematical pH 6.02

Analyzing the ProblemGiven:Three solutions: 10^-6 M acetic acid, 10^-2 M phenol, and 10^-2.8 M…

Answered: 2. What are the pH values of the…

Appl Of Ms Excel In Analytical Chemistry

2nd Edition

ISBN:9781285686691

Author:Crouch

Publisher:Crouch

Chapter8: Polyfunctional Acids And Bases

Section: Chapter Questions

Problem 4P

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Similar questions

. Using Fig. 16.3, list the approximate pH value of live “everyday” solutions. How do the familiar properties (such as the sour taste for acids) of these solutions correspond to their indicated pH?
Why have chemists not tabulated the fraction ionized for different acids? Such a table would make problems such as calculating the pH of an acid solution quite simple.
How do the components of a conjugate acid—base pair differ from one another4? Give an example of a conjugate acid—base pair to illustrate your answer.
Write equations to illustrate the acid-base reaction when each of the following pairs of Brnsted acids and bases are combined: Acid Base a.HOCl H2O b.HClO4 NH3 c.H2O NH2 d.H2O OCl e.HC2O4 H2O
Novocaine, C13H21O2N2Cl, is the salt of the base procaine and hydrochloric acid. The ionization constant for procaine is 7106. 15 a solution of novocaine acidic or basic? What are [H3O+], [OH-], and pH of a 2.0% solution by mass of novocaine, assuming that the density of the solution is 1.0 g/mL.
Using the diagrams shown in Problem 10-37, which of the four acids is the weakest acid?
. Consider 0.25 M solutions of the following salts: NaCl. RbOC1, KI, Ba(ClO4),, and NH4NO3. For each salt, indicate whether the solution is acidic, basic, or neutral.
In a particular solution, acetic acid is 11% ionized at 25 C. Calculate the pH of the solution and the mass of acetic acid dissolved to yield 1.00L of solution.
A solution is made by dissolving 15.0 g sodium hydroxide in approximately 450 mL water. The solution becomes quite warm, but after it is allowed to return to room temperature, water is added to bring the volume to 500.0 mL of solution. (a) Calculate the pH and pOH in the final solution. (b) Why would we wait for it to return to room temperature? (c) If the mass of the water used to initially dissolve the sodium hydroxide were exactly 450 g and the temperature of the water increased by 8.865 C, how much heat was given off by the dissolution of 15.0 g of solute? Assume the specific heat of the solution is 4.184 J/g. K. What is the molar heat change for the dissolution of sodium hydroxide (known as the enthalpy of solution, Hsol)?
Use Table 13-2 to order the following from the strongest to the weakest base. ClO2,H2O,NH3,ClO4
You are asked to determine whether an unknown white solid is acidic or basic. You also need to say whether the acid or base is weak or strong. You are given the molar mass of the solid and told that it is soluble in water. Describe an experiment that you can perform to obtain the desired characteristics of the white solid.
Write a formula for the conjugate base formed when each of the following behaves as a Brnsted acid: a. HSO3 b. HPO42 c. HClO3 d. CH3NH3+ e. H2C2O4

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