2 Fll in the table of hypothetical bases below. Remember the relationship between pH and pOHdiscussed earlier.Calculating the pH of BasesTubeMolarity ofDegree of[OH] M[H] MBaseIonization11×10-³100%21x10-³10%31×10-8100%41×10-5100%S1100%b) Which of the "bases" above isn't actually a base? Explain.3. Why are buffers important to biological systems?HupHРОН

Step 1: Step 2: Step 3: Step 4:

Answered: 2 Fll in the table of hypothetical…

Fundamentals Of Analytical Chemistry

9th Edition

ISBN:9781285640686

Author:Skoog

Publisher:Skoog

Chapter15: Complex Acid/base Systems

Section: Chapter Questions

Problem 15.1QAP

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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.
Sketch two graphs: (a) percent dissociation for weak acid HA versus the initial concentration of HA ([HA]0) and(b) H+ concentration versus [HA]0. Explain both.
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.
Use Table 13-2 to order the following from the strongest to the weakest acid. HClO2,H2O,NH4+,HClO4
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.
Rank the compounds in each of the following groups in order of increasing acidity or basicity, as indicated, and explain the order you assign. (a) acidity: HCI, HBr, HI. (b)basicity: H2O, OH-, H-, CI-. (c) basicity: Mg(OH)2, Si(OH)4, ClO3(OH) (Hint: Formula could also be written as HCIO4). (d) acidity: HF, H2O, NH3, CH4
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)?
8-62 What is the pH of a buffer solution made by dissolving 0.10 mol of formic acid, HCOOH, and 0.10 mol of sodium formate, HCOONa, in 1 L of water?
Several acids and their respective equilibrium constants are: Which is the strongest acid? Which is the weakest acid? Which acid has the weakest conjugate base? Which acid has the strongest conjugate base?
Each box represents an acid solution at equilibrium. Squares represent H+ ions, and circles represent the anion. Water molecules are not shown. Which figure represents a strong acid? Which figure is a weak acid?
Consider two separate solutions: one containing a weak acid. HA, and one containing HCl. Assume that you start with 10 molecules of each. a. Draw a molecular-level picture of what each solution looks like. b. Arrange the following from strongest to weakest base: Cl- H2O. A- . Explain.
Using the diagrams shown in Problem 10-37, which of the four acids is the weakest acid?

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