What is the pH of a 0.16 M NH3 solution? Kb = 1.8 x 10-5 (at %3D the current temperature) IMPORTANT: When entering your answer: • Enter the number only (no units) • Do not leave any spaces • Use a leading zero before the decimal when necessary Report your number to 2 decimal places (regardless of the sign.cant figures) Correctly round your answer to the 2nd decimal place (allowed margin of error is only + 0.01, so always use un- rounded numbers in your calculations) Examples: 0.12 or 9.87

What is the pH of a 0.16 M NH3 solution? Kb = 1.8 x 10-5 (at %3D the current temperature) IMPORTANT: When entering your answer: • Enter the number only (no units) • Do not leave any spaces • Use a leading zero before the decimal when necessary Report your number to 2 decimal places (regardless of the sign.cant figures) Correctly round your answer to the 2nd decimal place (allowed margin of error is only + 0.01, so always use un- rounded numbers in your calculations) Examples: 0.12 or 9.87

Introductory Chemistry: A Foundation

9th Edition

ISBN:9781337399425

Author:Steven S. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Donald J. DeCoste

Chapter16: Acids And Bases

Section: Chapter Questions

Problem 7ALQ

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Similar questions

A student prepares 455 mL of a KOH solution, but neglects to write down the mass of KOH added. His TA suggests that he take the pH of the solution. The pH is 13.33. How many grams of KOH were added?
For oxyacids, how does acid strength depend on a. the strength of the bond to the acidic hydrogen atom? b. the electronegativity of the element bonded to the oxygen atom that bears the acidic hydrogen? c. the number of oxygen atoms? How does the strength of a conjugate base depend on these factors? What type of solution forms when a nonmetal oxide dissolves in water? Give an example of such an oxide. What type of solution forms when a metal oxide dissolves in water? Give an example of such an oxide.
A chilled carbonated beverage is opened and warmed to room temperature. Does the pH change and, if so, how does it change?
Consider two weak acids, HA (MM=138g/mol)and HB (MM=72.0g/mol). A solution consisting of 11.0 g of HA in 745 mL has the same pH as a solution made up of 5.00 g of HB in 525 mL. Which of the two acids is stronger? Justify your answer by an appropriate calculation.
Why have chemists not tabulated the fraction ionized for different acids? Such a table would make problems such as calculating the pH of an acid solution quite simple.
Consider an aqueous solution of HF. The molar heat of formation for aqueous HF is -320.1 kJ/mol. (a) What is the pH of a 0.100 M solution of HF at 100C? (b) Compare with the pH of a 0.100 M solution of HF at 25C.
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)?
Novocaine, C13H21O2N2Cl, is the salt of the base procaine and hydrochloric acid. The ionization constant for procaine is 7106. 15 a solution of novocaine acidic or basic? What are [H3O+], [OH-], and pH of a 2.0% solution by mass of novocaine, assuming that the density of the solution is 1.0 g/mL.
You are asked to determine whether an unknown white solid is acidic or basic. You also need to say whether the acid or base is weak or strong. You are given the molar mass of the solid and told that it is soluble in water. Describe an experiment that you can perform to obtain the desired characteristics of the white solid.
Both HF and HCN ionize in water to a limited extent. Which of the conjugate bases. F“ or CN”, is the stronger base? See Table 14.2.
How many significant figures are there in the following numbers: 10.78, 6.78, 0.78? If these were pH values, to how many significant figures can you express the [H+]? Explain any discrepancies between your answers to the two questions.
How do the components of a conjugate acid—base pair differ from one another4? Give an example of a conjugate acid—base pair to illustrate your answer.