X Incorrett. Did you calculate the molarity before setting up your ICE table? Did you use the correct equilibrium expression? Some people who take megadoses of ascorbic acid will drink a solution containing as much as 70g of ascorbic acid dissolved in a glass of water. Assuming the volume to be 0.4001, calculate the pH of this solution pH- 355 Assistance Used

X Incorrett. Did you calculate the molarity before setting up your ICE table? Did you use the correct equilibrium expression? Some people who take megadoses of ascorbic acid will drink a solution containing as much as 70g of ascorbic acid dissolved in a glass of water. Assuming the volume to be 0.4001, calculate the pH of this solution pH- 355 Assistance Used

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 16.58QE

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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)?
Two students were asked to determine the Kb of an unknown base. They were given a bottle with a solution in it. The bottle was labeled aqueous solution of a monoprotic strong acid. They were also given a pH meter, a buret, and an appropriate indicator. They reported the following data: volume of acid required for neutralization = 21.0 mL pH after 7.00 mL of strong acid added = 8.95 Use the students' data to determme the Kb of the unknown base.
Consider a weak organic base (nonelectrolyte) with molar mass 281 g/mol. An aqueous solution of the base has a pH of 8.73 and an osmotic pressure of SS mm Hg at 25C. What is Kb for the weak base?
Enough water is added to the buffer in Question 30 to make the total volume 5.00 L. (a) Calculate the pH of the buffer. (b) Calculate the pH of the buffer after adding 0.0250 mol of HCl to 0.376 L of the buffer. (c) Calculate the pH of the buffer after adding 0.0250 mol of KOH to 0.376 L of the buffer. (d) Compare your answers to Question 30 (a-c) with your answers to (a-c) of this problem. (e) Comment on the effect of dilution on the pH of a buffer and on its buffer capacity. Â
How many grams of NH4Cl (53.49 g/mol) must be dissolved in 4.670 L of solution in order to obtain a solution that has a pH equal to 5.46? The Kb of NH3 at the temperature in this problem is 5.2 × 10-5. The Kw can be assumed to equal 1.0 x 10-14. Report your answer to the tenths place and do not include units. Tip: What is the reactant? Start by writing the reaction with water that is taking place and the corresponding Keq expression. You do not need an ICE table.
In the laboratory, a general chemistry student measured the pH of a 0.362 M aqueous solution of ammonia to be 11.389. Use the information she obtained to determine the Kb for this base. Kb(experiment) =
Grams of Sodium Formate required to add to 400ml of 0.1M Formic acid to make the pH of solution by 4, ionization constant for Formic acid is 1.74 ×10-4 . [M.wt of Sodium Formate] 68 g/mole *