5. Use YOUR stock of 0.50 M sodium acetate and your stock of 0.50 M acetic acid to make each of the solutions below: Note: You can just give your graduated cylinder (and any other glassware) a quick rinse with tap water and deionized water between making each of these solutions. Since they are variations on the same idea you don't need to wash with soap and water between uses. a. Buffer A: 100 mls of a solution of 0.010 M acetic acid and 0.090 M sodium acetate i. What volume of stock acetic acid will you use to make this solution? ii. What volume of stock sodium acetate will you use to make this solution? iii. If I had wanted to, I could have given you the directions for making buffer A in terms of dilution factors. In that case what would be the dilution factor for the acetic acid?

5. Use YOUR stock of 0.50 M sodium acetate and your stock of 0.50 M acetic acid to make each of the solutions below: Note: You can just give your graduated cylinder (and any other glassware) a quick rinse with tap water and deionized water between making each of these solutions. Since they are variations on the same idea you don't need to wash with soap and water between uses. a. Buffer A: 100 mls of a solution of 0.010 M acetic acid and 0.090 M sodium acetate i. What volume of stock acetic acid will you use to make this solution? ii. What volume of stock sodium acetate will you use to make this solution? iii. If I had wanted to, I could have given you the directions for making buffer A in terms of dilution factors. In that case what would be the dilution factor for the acetic acid?

Introductory Chemistry For Today

8th Edition

ISBN:9781285644561

Author:Seager

Publisher:Seager

Chapter9: Acids, Bases, And Salts

Section: Chapter Questions

Problem 9.109E

See similar textbooks

Similar questions

A bottle of concentrated hydroiodic acid is 57% HI by weight and has a density of 1.70 g/mL. A solution of this strong and corrosive acid is made by adding exactly 10.0 mL to some water and diluting to 250.0 mL. If the information on the label is correct, what volume of 0.988 M NaOH is needed to neutralize the HI solution? Suggest an indicator for the titration.
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?
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.
Another way to treat data from a pH titration is to graph the absolute value of the change in pH per change in milliliters added versus milliliters added (pH/mL versus mL added). Make this graph using your results from Exercise 61. What advantage might this method have over the traditional method for treating titration data?
Calculate the sodium ion concentration when 70.0 mL of 3.0 M sodium carbonate is added to 30.0 mL of 1.0 M sodium bicarbonate.
Part C – Acid–base and solubility equilibria 1. Rinse 4 regular size test tubes and a 10 mL measuring cylinder thoroughly with water. Number the test-tubes from 1 to 4 in a test tube rack. 2. Into each of test tubes 1 – 3 put a small amount of solid benzoic acid (put the same amount – about the size of a pea – in each test tube). 3. Add 2 mL (use the measuring cylinder) of water to tube 1 and shake to mix the contents. 4. Add 2 mL (measuring cylinder) of 2 M HNO3 to tube 2 and shake to mix the contents. 5. Rinse the measuring cylinder with water, then use it to add 2 mL of 2 M NaOH to tube 3 and shake for about 10 seconds to mix the contents. Rinse the measuring cylinder. 6. Pour about half of the solution from tube 3 into tube 4, than add 2 mL of 2 M HNO3 to tube 4. 7. Allow the test tubes to stand for 2 or 3 minutes then record the appearance of the mixtures in each test tube. 8. Answer the questions on the results page relating to this equilibrium system.
A 1.00 liter solution contains 0.45 M hydrocyanic acid and 0.58 M sodium cyanide. If 0.15 moles of barium hydroxide are added to this system, indicate whether the following statements are true or false. (Assume that the volume does not change upon the addition of barium hydroxide.) A. The number of moles of HCN will decrease. B. The number of moles of CN will remain the same. BC. The equilibrium concentration of H3O+ will remain the same. D. The pH will remain the same. E. The ratio of [HCN] [CN] will increase.
A 1.00 liter solution contains 0.36 moles hydrofluoric acid and 0.28 moles sodium fluoride .If 0.14 moles of hydroiodic acid are added to this system, indicate whether the following statements are true or false.(Assume that the volume does not change upon the addition of hydroiodic acid.) A. The number of moles of HF will remain the same. B. The number of moles of F- will decrease. C. The equilibrium concentration of H3O+ will increase. D. The pH will remain the same. E. The ratio of [HF] / [F-] will remain the same.
Answer the following three questions based on the information given below. Consider a buffer made with 34.0 mL of 0.25 M butanoic acid (HC4H702) and 16.0 mL of 0.46 M sodium butanoate (NaC4H7O2). The K, for butanoic acid (HC4H-02) is 1.5 X 105. Round all numerical answers to the 100n place (2 decimal places). Assume 298 K. What is the pH, if 2.0 mL of 1.0 M NAOH is added to this buffer? Type your answer..
Volume of acetic acid (HC2H3O2) in the first titration (L) 10 mL Volume of acetic acid (HC2H3O2) in the second titration (L) 10 mL Normality of sodium hydroxide (NaOH) (N) 0.1 N Volume of sodium hydroxide (NaOH) in the first titration (L) 10 mL = ……..L Volume of sodium hydroxide (NaOH) in the second titration (L) 10 mL = ……..L Normality of acetic acid (HC2H3O2) in the first titration (N) Normality of acetic acid (HC2H3O2) in the secondtitration (N) Average normality of acetic acid (HC2H3O2) (N) Mass % of acetic acid (HC2H3O2) (%)
A 1.00 liter solution contains 0.43 M potassium cyanide and 0.56 M hydrocyanic acid. If 0.14 moles of calcium hydroxide are added to this system, indicate whether the following statements are TRUE or FALSE. (Assume that the volume does not change upon the addition of calcium hydroxide.) A. The number of moles of of CN will decrease. O True False B. The number of moles of of HCN will increase. True False C. The equilibrium concentration of H3O* will increase. O True False D. The pH will increase. True False E. The ratio of [CN] / [HCN] will remain the same. True False
A 1.00 liter solution contains 0.59 M ammonia and 0.45 M ammonium bromide.If 0.23 moles of perchloric acid are added to this system,indicate whether the following statements are true or false.(Assume that the volume does not change upon the addition of perchloric acid.) A. The number of moles of NH3 will increase. B. The number of moles of NH4+ will remain the same. C. The equilibrium concentration of H3O+ will decrease. D. The pH will remain the same. E. The ratio of [NH3] / [NH4+] will remain the same.