Concept explainers
(a)
Interpretation:
The largest
Concept Introduction:
Solubility product constant:
The equilibrium constant of a more soluble ionic compound in water at the higher solubility is known as solubility product constant.
The equilibrium constant of more soluble ionic compound is given by
(a)
Interpretation:
The smallest
Concept Introduction:
Solubility product constant:
The equilibrium constant of a more soluble ionic compound in water at the higher solubility is known as solubility product constant.
The equilibrium constant of more soluble ionic compound is given by
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General Chemistry: Atoms First
- A saturated solution of silver oxalate. Ag2C2O4. contains 6.9 105-M C2O42 at 25 C. Calculate the Ksp of silver oxalate at that temperature, assuming that the ions do not react with water and the dissociation is complete.arrow_forward• A mixture is prepared by combining 3.0 mL of 0.0050 M NaSCN (in 0.10 M HNO3) solution with 4.0 mL of 0.0030 M Fe(NO3)3 solution, and 3.0 mL of 0.10 M HNO3 solution. Based on your average Kf value, determine the equilibrium concentrations of Fe 3+, SCN, and FeSCN2+ in the solution. You cannot apply a small x approximation.arrow_forwardCalculate the molar solubility of Ag2SO4 in each solution below. The Ksp of silver sulfate is1.5 × 10−5. (a) 0.40 M AgNO3: (b) 0.40 M Na2SO4:arrow_forward
- Consider a beaker containing a saturated solution of CaF2 in equilibrium with undissolved CaF2 (s). (a) If solid CaCl2 is added to this solution, will the amount of solid CaF2 at the bottom of the beaker increase, decrease or remain the same? (b) Will the concentration of Ca2+ ions in solution increase or decrease?arrow_forwardWhich of the following pairs of solution would you use to prepare a buffer with pH = 7.45? (A) Acetic acid + sodium acetate; (CH3CO2H has Ka = 1.8 x 10–5) (B) Sodium dihydrogen phosphate + sodium hydrogen phosphate; (H2PO4– has Ka = 6.2 x 10–8) (C) Ammonium chloride + ammonia; (NH3 has Kb = 1.8 x 10–5) (D) Sodium hydrogen carbonate + sodium carbonate; (HCO3– has Ka = 5.6 x 10–11)arrow_forward7. In each of the following questions, assume that there is no volume change when HCI is added to the phosphate buffer in part (c). (c) Calculate the pH when 0.052 moles of HCI are added to 1.000 liters of a buffer containing 0.184 M KH2PO4 and 0.437 M K2HPO4arrow_forward
- Consider a buffer solution containing HCN and NaCN where the concentration of HCN is double the concentration of NaCN. Which statement about the buffer solution is true? (A) The pH of this solution is equal to the pK, value of HCN. (B) The pKa value of HCN will decrease if a strong acid is added. (C) The cyanide ion concentration will increase if a strong base is added. (D) The buffer capacity of this solution will improve if a strong acid is added.arrow_forwardWhat is the pH of a buffer that is .1 Molar in H2CO3 and 1M in NaHCO3?arrow_forwardBe sure to answer all parts. Tris [tris(hydroxymethyl)aminomethane] is a common buffer for studying biological systems. (K = 5.01 × 10 and pK = 8.3) (a) Calculate the pH of the Tris buffer after mixing 11.0 mL of 0.20 M HCl solution with 25.0 mL of 0.10 M Tris. (b) This buffer was used to study an enzyme-catalyzed reaction. As a result of the reaction, 0.00019 mol of H* was produced. What is the pH of the buffer at the end of the reaction? (c) What would be the final pH if no buffer were present?arrow_forward
- Cadmium carbonate, CdCO3, is a sparingly soluble salt whose Ksp = 2.5x10^-14. It is also known that Cd2+ forms the [Cd(NH3)4]^2+ complex ion that has a formation constant, Kf = 1.0x10^7. (a) Calculate the molar solubility of CdCO3 in 6.0M NH3. (b) What NH3 concentration would be required to dissolve 4.00 mol of CdCO3 in one liter of the solution?arrow_forwardScenes A to D represent tiny portions of 0.10 M aqueous so-lutions of a weak acid HA (red and blue; Kₐ=4.5X10⁻⁵), its conjugate base A⁻(red), or a mixture of the two (only these species are shown): (a) Which scene(s) show(s) a buffer?(b) What is the pH of each solution?(c) Arrange the scenes in sequence, assuming that they represent stages in a weak acid–strong base titration.(d) Which scene represents the titration at its equivalence point?arrow_forwardHuman blood contains one buffer system based on phos-phate species and one on carbonate species. Assuming that blood has a normal pH of 7.4, what are the principal phosphateand carbonate species present? What is the ratio of the two phosphate species? (In the presence of the dissolved ions andother species in blood, Kₐ₁of H₃PO4=1.3X10⁻², Kaₐ₂=2.3X10⁻⁷, and Kₐ₃=6X10⁻¹²; Kₐ₁ of H₂CO₃=8X10⁻⁷ and Kₐ₂=1.6X10⁻¹⁰.)arrow_forward
- Chemistry: The Molecular ScienceChemistryISBN:9781285199047Author:John W. Moore, Conrad L. StanitskiPublisher:Cengage LearningChemistry: An Atoms First ApproachChemistryISBN:9781305079243Author:Steven S. Zumdahl, Susan A. ZumdahlPublisher:Cengage LearningChemistryChemistryISBN:9781305957404Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCostePublisher:Cengage Learning