Precipitation Rea CASO,(aq) + K₂S(aq) → CdS(s) + K₂SO4(aq) Using the information in the table below, identify the limiting reagent for each trial performed: Trial 1 2 3 4 5 0.100 M CdSO (mL) 50.0 50.0 50.0 50.0 50.0 0.100 M K₂S (mL) 20.0 40.0 50.0 60.0 80.0 CdS (grams) 0.289 0.578 0.722 0.722 0.722 Limiting Reactant

Precipitation Rea CASO,(aq) + K₂S(aq) → CdS(s) + K₂SO4(aq) Using the information in the table below, identify the limiting reagent for each trial performed: Trial 1 2 3 4 5 0.100 M CdSO (mL) 50.0 50.0 50.0 50.0 50.0 0.100 M K₂S (mL) 20.0 40.0 50.0 60.0 80.0 CdS (grams) 0.289 0.578 0.722 0.722 0.722 Limiting Reactant

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...

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20.
Barium sulphate is a relatively insoluble salt used for medical radiographs of the gastrointestinal tract: BaSO4 (s) Ba2+ (aq) + SO4²- (aq) The concentration of Ba2+ ions in a saturated aqueous solution is 1.05×105 M. Determine Ksp for barium sulphate dissolving in water. O 1.12 x 10-5 O 1.05 x 1025 O 2.12 x 10-5 1.10 x 10-25 O 1.10 x 10-10
11. The Kf for [AIF6]³- is 7.0 x 101⁹ and the corresponding equilibrium is shown below. Calculate the concentration of Al³+ ions in a solution that is initially 0.83 M in [AlF6]³-. Al³+ (aq) + 6 F-(aq) [AIF6]³(aq)
A student combines Fe(NO3)3 solution and KSCN solution to produce a solution in which the initial concentrations of Fe3+(aq) and SCN–(aq) are both 5.58 × 10–2 M. The chemical equilibrium forms FeSCN2+(aq): Fe3+ + SCN- <=> FeSCN2+ The absorbance of this solution (from FeSCN2+) is measured as 0.161, and Beer's law equation (the trend line from best fitting) as Absorbance = 189 x Concentration of FeSCN2+ + 0.02 Determine the equilibrium concentration for SCN- in mol/L.
Identify the spectator ion(s) in the following reaction.Zn(OH)2(s) + 2K+(aq) + 2OH–(aq) → 2K+(aq) + Zn(OH)4–(aq) Zn(OH)2 K+ and OH- K+ K+ and Zn(OH)4 -2 Zn(OH)4– Provide explanation for answer.
Barium hydroxide, Ba(OH)2, dissolves in water to the extent of 18.5 g per liter. What is the value of Ksp for Ba(OH)2 ? Ba(OH)2(s) ⇒ Ba²+ (aq) + 2 OH¯(aq) K sp =
A student was asked to identify a compound. In an effort to do so, he first dissolved the compound in water. He found that no precipitate formed when hydrochloric acid was added, but when H2S was bubbled into this acidic solution, a precipitate formed. Which one of the following could be the precipitate? NiS AgCl HgS BaS
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14.5-3 Silver bromide, a solid used in photographic film, can be prepared by mixing solutions of silver nitrate and potassium bromide: Ag+ (aq) + Br(aq) AgBr(s) Keq = 1.87 × 10¹² Calculate the concentrations of Ag and Brions remaining in solution after mixing 2.50 L of 0.100 M AgNO3 solution with 2.50 L of 0.500 M KBr solution.
A saturated solution of the hypothetical salt, M2A3, has an initial salt concentration of 0.000466 M. What is the value of Ksp with 3 significant figures. M2A3 → 2 M3+ + 3 A2-
17. In which of the following solutions, Mn(OH)2 has the greatest solubility? (by assuming sufficient Mn(OH)2 (s) present in solution). Ksp (Mn(OH)2) 2.0 × 10-13. a) 0.20 M HNO3 b) 0.20 M NaNO3 c) b) 0.20 M Mn(NO3)2 e) same solubility for all