Prepare a buffer by direct addition.Close ProblemConsider how best to prepare one liter of abuffer solution with pH = 7.66 using one ofthe weak acid/conjugate base systems shownhere.Weak AcidConjugate BaseКаpKaHC204¯ C204²-6.4 x 10-5 4.19Н2РОД НРОД2-2-6.2 x 10-8 7.21HCO34.8 x 10-1110.32How many grams of the potassium salt of theweak acid must be combined with how manygrams of the potassium salt of its conjugatebase, to produce 1.00 L of a buffer that is 1.00M in the weak base?grams potassium salt of weak acid =grams potassium salt of conjugate base =

Henderson-Hasselbalch equation The equation that is used to find the pH of a buffer solution is…

Prepare a buffer by direct addition. Close Problem Consider how best to prepare one liter of a buffer solution with pH = 7.66 using one of the weak acid/conjugate base systems shown here. %3D Weak AcidConjugate Base Ка pka HC2O4¯ C2042- H2PO4 HPO42- HCO3 CO3²- 6.4 x 10-5 4.19 6.2 x 10-8 7.21 4.8 x 10-1110.32 How many grams of the potassium salt of the weak acid must be combined with how many grams of the potassium salt of its conjugate base, to produce 1.00 L of a buffer that is 1.00 M in the weak base? grams potassium salt of weak acid = %3D grams potassium salt of coniugate base =

Prepare a buffer by direct addition. Close Problem Consider how best to prepare one liter of a buffer solution with pH = 7.66 using one of the weak acid/conjugate base systems shown here. %3D Weak AcidConjugate Base Ка pka HC2O4¯ C2042- H2PO4 HPO42- HCO3 CO3²- 6.4 x 10-5 4.19 6.2 x 10-8 7.21 4.8 x 10-1110.32 How many grams of the potassium salt of the weak acid must be combined with how many grams of the potassium salt of its conjugate base, to produce 1.00 L of a buffer that is 1.00 M in the weak base? grams potassium salt of weak acid = %3D grams potassium salt of coniugate base =

Chemistry: Principles and Practice

3rd Edition

ISBN:9780534420123

Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Publisher:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Chapter16: Reactions Between Acids And Bases

Section: Chapter Questions

Problem 16.89QE

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Similar questions

A diprotic acid, H2B(MM=126g/moL), is determined to be a hydrate, H2B xH2O. A 10.00-g sample of this hydrate is dissolved in enough water to make 150.0 mL of solution. Twenty-five milliliters of this solution requires 48.5 mL of 0.425 M NaOH to reach the equivalence point. What is x?
Amino acids are an important group of compounds. At low pH, both the carboxylic acid group (CO2H) and the amine group (NHR) are protonated. However, as the pH of the solution increases (say, by adding base), the carboxylic acid proton is removed, usually at a pH between 2 and 3. In a middle range of pHs, therefore, the amine group is protonated, but the carboxylic acid group has lost the proton. (This is called a zwitterion.) At more basic pH values, the amine proton is dissociated. What is the pH of a 0.20 M solution of alanine hydrochloride, [NH3CHCH3CO2H]Cl?
What is an acidbase indicator? Define the equivalence (stoichiometric) point and the end point of a titration. Why should you choose an indicator so that the two points coincide? Do the pH values of the two points have to be within 0.01 pH unit of each other? Explain.
. 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?
Determine the dominant acid-base equilibrium that results when each of the following pairs of solutions is mixed. Indicate the equilibrium by writing 1 for a strong acid, 3 for a weak acid, 4 for an acidic buffer, 7 for a neutral solution, 10 for a basic buffer, 11 for a weak base, and 13 for a strong base. (a) 10.0 mL of 0.15 M NaOH + 15.0 mL of 0.10 M HNO3 (b) 25.0 mL of 0.10 M HCl + 10.0 mL of 0.25 M NH3 (c) 50.0 mL of 0.050 M NaOH + 50.0 mL of 0.10 M NH3 (d) 50.0 mL of 0.10 M NH3 + 50.0 mL of 0.05 M HCl
Calculate the pH after mixing 15 mL of 0.12 M acetic acid with 15 ml of 0.12 M NaOH. What are the major species in solution at equilibrium (besides water), and what are their concentrations?
Sketch a titration curve for the titration of potassium hydroxide with HCl, both 0.100 M. Identify three regions in which a particular chemical species or system dominates the acid-base equilibria.
In dilute aqueous solution HF acts as a weak acid. However, pure liquid HF (boiling point = 19.5 C) is a strong acid. In liquid HF, HNO3 acts like a base and accepts protons. The acidity of liquid HF can be increased by adding one of several inorganic fluorides that ale Lewis acids and accept F- ion (for example, BF3 or SbF5]. Write balanced chemical equations for the reaction of pure HNO3 with pure HF and of pure HF with BF3.
8-60 How is the buffer capacity affected by the ratio of the conjugate base to the conjugate acid?
A solution has a pH of 4.5. What would be the color of the solution if each of the following indicators were added? (See Fig. 14-8.) a. methyl orange b. alizarin c. bromcresol green d. phenolphthalein