4. a. A buffer is prepared by mixing 0.900 mole of ammonia and 0.850 mole of ammonium chloride to form an aqueous solution with a total volume of 0.500 litre. b. 30.0 ml of 1.00 M NaOH was added to 350 ml of this solution. What is the pH of the solution before and after the addition of NaOH? Show Transcribed Text Alternatively, how many moles of NaOH are required to react with 0.850 mol of ammonium chloride to form an aqueous buffer solution with a total volume of 0.500 litres, and a pH of 9.00?

4. a. A buffer is prepared by mixing 0.900 mole of ammonia and 0.850 mole of ammonium chloride to form an aqueous solution with a total volume of 0.500 litre. b. 30.0 ml of 1.00 M NaOH was added to 350 ml of this solution. What is the pH of the solution before and after the addition of NaOH? Show Transcribed Text Alternatively, how many moles of NaOH are required to react with 0.850 mol of ammonium chloride to form an aqueous buffer solution with a total volume of 0.500 litres, and a pH of 9.00?

Chemistry for Today: General, Organic, and Biochemistry

9th Edition

ISBN:9781305960060

Author:Spencer L. Seager, Michael R. Slabaugh, Maren S. Hansen

Publisher:Spencer L. Seager, Michael R. Slabaugh, Maren S. Hansen

Chapter9: Acids, Bases, And Salts

Section: Chapter Questions

Problem 9.128E

See similar textbooks

Similar questions

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 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?
How much solid NaCH3CO23H2O must be added to 0300 L of a 0.50-M acetic acid solution to give a buffer with a pH of 5.00? (Him: Assume a negligible change in volume as the solid is added.)
A chemist needs a buffer with pH 4.35. How many milliliters of pure acetic acid (density = 1.049 g/mL) must be added to 465 mL of 0.0941 M NaOH solution to obtain such a buffer?
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.
When titrating 50mL of 0.2MHCl, what quantity of 0.5M NaOH is needed to bring the solution to the equivalence point? a.80mL b.40mL c.20mL d.10mL
A friend asks the following: Consider a buffered solution made up of the weak acid HA and its salt NaA. If a strong base like NaOH is added, the HA reacts with the OH to form A. Thus the amount of acid (HA) is decreased, and the amount of base (A) is increased. Analogously, adding HCI to the buffered solution forms more of the acid (HA) by reacting with the base (A). Thus how can we claim that a buffered solution resists changes in the pH of the solution? How would you explain buffering to this friend?
Some K2SO3 and KHSO, are dissolved in 250.0 mL of solution and the resulting pH is 6.88. Which is greater in this buffer solution, the concentration of So, or the concentration of HSO3-? K.(HSO3-) = 1.0 x 10-7 Oconcentration of SO3²- Oconcentration of HSO3 Oboth are equal If (so.] HSO,. = 0.80 M in this solution, calculate the concentration of [HSO,-] =
10. How many mililiters of 0.085 M NaOH are required to titrate the following solution to the equivalence point: 40.0 mL of 0.0900M HNO3 Group of answer choices A) 42.4 mL NaOH soln B) 23.6 mL C.) 37.8 mL D.) 40.0 mL
8. A 100. mL sample of 0.10 MHCI is mixed with 50. mL of 0.12 M NH.. What is the resulting pH? (K, for NH3 = 1.8 × 10-- 3.07 10.93 1.57 12.43 1.40
What is pH of 200. mL of 0.25 M CHOONa solution after addition of ... The pka of the conjugate acid ( CHOOH) is 3.75. no HCI