12:19 1 Jessica - Chemical Acid-Base Equilibria 回Q K = (b) Calculate the pH of 0.1mol dm potassium hydroxide (KOH() pH = 3.2 10. Explain briefly the effect of temperature on Kw. 11 (a) Define a buffer solution (b) What are the components of (i) an acidic buffer ? (ii) a basic buffer ? 4.2 (b) Using the equation below, explain what happens to maintain the pH of the solution: HA (u A' (aw (i) when an acid is added (meaning more H* ions added) (ii) when a base added (meaning more OH ions added)

12:19 1 Jessica - Chemical Acid-Base Equilibria 回Q K = (b) Calculate the pH of 0.1mol dm potassium hydroxide (KOH() pH = 3.2 10. Explain briefly the effect of temperature on Kw. 11 (a) Define a buffer solution (b) What are the components of (i) an acidic buffer ? (ii) a basic buffer ? 4.2 (b) Using the equation below, explain what happens to maintain the pH of the solution: HA (u A' (aw (i) when an acid is added (meaning more H* ions added) (ii) when a base added (meaning more OH ions added)

Principles of Modern Chemistry

8th Edition

ISBN:9781305079113

Author:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Publisher:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Chapter15: Acid–base Equilibria

Section: Chapter Questions

Problem 99AP

See similar textbooks

Similar questions

Calculate the molar solubility of lead(II) iodide in water at 25°C, given that its Ksp = 7.1 × 10−9 .
10. 50 cm3 of 0.05 M weak acid solution is titrated with 0.1 M NaOH solution. The measured pH valuesare 7.345 and 7.497 at the consumptions of 6.0 and 6.1 cm3, respectively. What value of the buffer capacity can be calculated in the solution at pH = 7.421?11. Based on the data given in question 10, what is the total concentration of the anion of the weak acid atthe given point?
2. You are studying an unusual enzyme that produces hydronium ions (H3O+) during the courseof the reaction.You wish to maintain pH = 8.5 for the enzyme-catalyzed reaction. Which weak acid will serveas the better 0.1 M buffer for the reaction: HEPPS with pKa = 8.0, or, AMPSO with pKa = 9.0?Justify your answer by describing how the buffer “resists” change in pH and the chemical logicof why you chose the buffer you did.
CdF2(s)⇄Cd2+(aq)+2F−(aq) A saturated aqueous solution of CdF2 is prepared. The equilibrium in the solution is represented above. In the solution, [Cd2+]eq=0.0585M and [F−]eq=0.117M. Some 0.90MNaF is added to the saturated solution. Which of the following identifies the molar solubility of CdF2 in pure water and explains the effect that the addition of NaF has on this solubility? a. The molar solubility of CdF2 in pure water is 0.0585M, and adding NaF decreases this solubility because
Suppose that a 1000 mL buffer (pH=5) solution will be prepared using 2.6g C6H5COOH (its Ka is 6x10-5) and 2.6g NaC6H5COOH in H2O. How much (in g) of the component of the buffer should be added in the 1000mL buffer so that its pH will be 3?
A solution was found to have a PH of 6.3 with the acid 100x in excess of it conjugate base. What is the pKa of the solution would it be considered a buffer
For a titration to be effective, the reaction must be rapid and the yield of the reaction must essentially be 100%. Is Kc > 1, < 1, or ≈ 1 for a titration reaction? Kc is the product of all reaction products (choose from: Multiplied by, added to, divided by, subtracted from) the product of the reactants, with all concentrations of reactants and products raised to their respective stoichiometric powers. As the titration proceeds, the amount of reactants (choose from: Increases, decreases, remains the same) and the amount of products (choose from: Increases, decreases, remains the same). Because the value of the numerator is (Choose from much greater than, much less than, approximately equal to) the value of the denominator, the value of Kc will be (Choose from much greater than, much less than, approximately equal to)1 for an effective titration reaction.
What is the proper unit of molar ratio of weak acid and its conjugate base in a buffer solution? Is it mol to mol or part to part? Or is it unitless? I need to express the answer 1.45/1 = [A]/[HA] to the right unit. See image for more details. the buffer is acetic acid/sodium acetate buffer.
If the molar solubility of CaF2 at 35 °C is 1.24 * 10-3 mol/L, what is Ksp at this temperature?
Many chemical reactions are carried out in the presence of buffers. Use the Henderson-Hasselbalch equation to provide a recommendation for a suitable acete/acetic acid buffer under the following reaction conditions. a) If a checial reaction produces hydroxide ion, OH-, what would be the range for the target pH of a buffer soution that would favor pH stabilizatoin under these conditions? Explain.
What is the solubility of silver iodide in grams per milliliter at a temperature at which the Ksp of AgI is 1.52×10-16?
A buffer solution is prepared from an unknown weak acid (HA) and its conjugate salt (NaA). If 500.00 ml of this buffer solution contains 0.025 moles of HA and 0.066 moles NaA, and has a measured pH of 4.61, what is the pKa of the unknown weak acid?