To an aqueous solution originally containing 1.0 x 10^-4 mol/L Ag+ was added enough of the weak acid HCN to reach an equilibrium concentration of [HCN] = 3.0 x 10^-4 mol/L. What must be the pH of the solution in order to observe a precipitate of AgCN? (Hint: Assume any change in pH will not change the value of [HCN]). Ksp of AgCN = 1.2 × 10-16 Ka of HCN = 6.2 × 10-10

To an aqueous solution originally containing 1.0 x 10^-4 mol/L Ag+ was added enough of the weak acid HCN to reach an equilibrium concentration of [HCN] = 3.0 x 10^-4 mol/L. What must be the pH of the solution in order to observe a precipitate of AgCN? (Hint: Assume any change in pH will not change the value of [HCN]). Ksp of AgCN = 1.2 × 10-16 Ka of HCN = 6.2 × 10-10

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Similar questions

Suppose that an aqueous solution is in equilibrium with solid calcium sulfate and solid barium sulfate. What are the concentrations of calcium ion and barium ion in the solution? Ksp for CaSO4 is 2.4x10^-5, Ksp for BaSO4 is 1.1x10^-10. [Ca^2+] = M [Ba^2+]= M
You have a solution that is 0.25M Ca2+ and .18M Ag+. You begin to add CO32- (carbonate ion) to form CaCO3 , and Ag2CO3. Which will precipitate first? Second? What is the concentration of the first ion at the point when the second begins to precipitate? What percentage of the first ion has been removed?
In this lab, we will experimentally determine the titration curve for the titration of a weak acid solution against a strong base solution. The weak acid we will use is potassium hydrogen phthalate, KHP, its chemical structure is shown below. KHP is an ionic compound composed of a potassium cation K+ and a hydrogen phthalate anion HP–. HP– is a weak acid and upon dissolving in water, can lower the pH of the solution. (a) Suggest the chemical reaction(s) when a solid sample of KHP is dissolved in water, writing out the chemical equations for them. (b) Sketch the structure of KHP from above and circle the hydrogen atom that is responsible for its acidity. (c) Calculate the pH of a solution made of 0.50 g of KHP and 50 mL of water. KHP has a molar mass of 204.2 g and at 25 °C has a pKa of 5.4.
NaCl (s) ⇌ Na+(aq) + Cl-(aq) When adding 6M HCl, the solid white precipitate is observed. When adding 0.1M HCl, no change is observed, no solid white precipitate is observed in the NaCl solution. Explain the similarities and differences by using Le Chatlier's principle.
A student prepared a saturated solution of magnesium hydroxide for analysis of the equilibrium of dissolution of this sparingly soluble solid. Titration was used to determine the concentration of hydroxide in solution after filtering the excess solid that persisted in the solution. If 30.0 mL of Mg(OH)2solution were titrated using 4.83 mL 0.0020 M HCl, what is the value of Ksp for magnesium hydroxide?
A friend tells you: " The constant K sp of a salt is called the sol ubility product constant and is calculated from the concentra tions of ions in the solution . Thus, if salt A dissolves to a greater extent than salt B , salt A must have a higher K sp than salt B. Do you agree with your friend ? Explain . Explain the following phenomenon You a test tube with
What you expect to observe on mixing 0.1M Ba(NO3)2 with HCl. Will there be a color? Will bubbles form? Will the solution turn hot? Will a precipitate form and if so, what will its color be?
Photoelectron spectroscopy applies the principle of the photoelectric effect to study orbital energies of atoms and molecules. High-energy radiation (usually UV or X-ray) is absorbed by a sample and an electron is ejected. The orbital energy can be calculated from the known energy of the radiation and the measured energy of the electron lost. The following energy differences were determined for several electron transitions: ΔE2 →1 = 4.098 ×10−17 J ΔE3 →1 = 4.854 × 10−17 JΔE5 → 1 = 5.242 ×10−17 J ΔE4 → 2 = 1.024 ×10−17 J Calculate the energy change and the wavelength of a photon emitted in the following transitions. Enter your answers in scientific notation. Use 6.626 ×10−34 J·s for Planck's constant. (a) Level 3 to 2: ______J ______m (b) Level 4 to 1: _____J_____ m (c) Level 5 to 4: _____J _____m
What you expect to observe on mixing 0.1M Pb(NO3)2 with HCl. Will there be a color? Will bubbles form? Will the solution turn hot? Will a precipitate form and if so, what will its color be?
Complete the following solubility constant expression for Fe(OH)2. Kn 0 sp 010
A buffer solution contains 0.305 M hydrocyanic acid and 0.379 M sodium cyanide. If 0.0518 moles of potassium hydroxide are added to 225 mL of this buffer, what is the pH of the resulting solution ? (Assume that the volume does not change upon adding potassium hydroxide. ) pH %3D
Solid NaBr is slowly added to a solution that is 0.012 M in Cu+ and 0.012 M in Ag+ Which compound will begin to precipitate first? AgBr NaBr What percent of Ag remains in solution at the point when CuBr just begins to precipitate?