Reasons for controlling pH within certain specified limits are:Chemically stabilityO Patient's comfortO Solubility of the drugO Two of theseO All of these

pH has a specific affect on solubility of drugs and chemically stability and patient comfort So…

Answered: Reasons for controlling pH within…

Introductory Chemistry: An Active Learning Approach

6th Edition

ISBN:9781305079250

Author:Mark S. Cracolice, Ed Peters

Publisher:Mark S. Cracolice, Ed Peters

Chapter16: Solutions

Section: Chapter Questions

Problem 11E

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Similar questions

Which of the following will affect the total amount of solute that can dissolve in a given amount of solvent? a. The solution is stirred. b. The solute is ground to fine particles before dissolving. c. The temperature changes.
If 55 mg of lead(II) sulfate is placed in 250 mL of pure water, does all of it dissolve? If not, how much dissolves?
7. Describe a buffered solution. Give three examples of buffered solutions. For each of your examples, write equations and explain how the components of the buffered solution consume added strong acids or bases. Why is buffering of solutions in biological systems so important?
Sketch the titration curve for a weak acid titrated by a strong base. When performing calculations concerning weak acidstrong base titrations, the general two-slep procedure is to solve a stoichiometry problem first, then to solve an equilibrium problem to determine the pH. What reaction takes place in the stoichiometry part of the problem? What is assumed about this reaction? At the various points in your titration curve, list the major species present after the strong base (NaOH, for example) reacts to completion with the weak acid, HA. What equilibrium problem would you solve at the various points in your titration curve to calculate the pH? Why is pH 7.0 at the equivalence point of a weak acid-strong base titration? Does the pH at the halfway point to equivalence have to be less than 7.0? What does the pH at the halfway point equal? Compare and contrast the titration curves for a strong acidstrong base titration and a weak acidstrong base titration.
. Teeth and bones are composed, to a first approximation, of calcium phosphate. Ca3(PO4)2(s). The K for this salt is 1.31032at 25 °C. Calculate the concentration of calcium ion in a saturated solution of Ca3(PO4)2.
The box below represents one liter of a saturated solution of the species , where squares represent the cation and circles represent the anion. Water molecules, though present, are not shown. Complete the next three figures below by filling one-liter boxes to the right of the arrow, showing the state of the ions after water is added to form saturated solutions. The species represented to the left of the arrow is the solid form of the ions represented above. Do not show the water molecules.
Potassium hydrogen phthalate is a solid, monoprotic acid frequently used in the laboratory as a primary standard. It has the formula KHC8H4O4. This is often written in the short-hand notation as KHP. If 25.0mL of a potassium hydroxide solution are needed to neutralize 2.26g of KHP, what is the molarity of the potassium hydroxide solution? Potassium hydrogen phthalate sometimes called potassium biphthalate, as shown on this bottle is an acid that is convenient to store and use because it is a solid.
The solubility product constant for calcium oxalate is estimated to be 4 109. What is its solubility in grams per liter?
In Exercise 12.49, what is the allowed concentration of AgCl in g per 100 g of water? The Safe Drinking Water Act of 1974 established the maximum permitted concentration of silver ion at 0.05 ppm. What is the concentration of Ag+ in parts per million in a saturated solution of AgCl? (NOTE: 1 ppm = 1 mgofsolute/L of solution.)

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Reasons for controlling pH within certain specified limits are: Chemically stability Patient's comfort O Solubility of the drug O Two of these All of these