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Chemistry
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ISBN: 9781305957404
Author: Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher: Cengage Learning
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The copper(I) ion forms a complex ion with CN2 according to the following equation:
Cu+(aq) + 3CN-(aq) ↔ Cu(CN)32-(aq) K = 1.0 * 1011
1. Calculate the solubility of CuBr(s) (Ksp = 1.0 * 10-5) in 0.80 L of 1.30 M NaCN.?
2. Calculate the concentration of Br- at equilibrium.?
3. Calculate the concentration of CN- at equilibrium.?
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- If a solution containing 0.10 M Cl-, Br, I-, and CrO2 is treated with Ag+, in what order will the anions precipitate? Salt AgCI AgBr Agl Ag₂ CrO 4 Ksp 1.8 × 10-10 5.0 × 10-13 8.3 × 10-17 1.2 × 10-12arrow_forwardAluminumcan form two complex ions with fluoride, AlF63–(Kf= 2.4x10^4), which forms in solutions with [F–] > 1.5M and AlF4–(Kf= 2.0x10^8), which forms when [F–] is between 0.5 M and 1.5M. 100 mL of 0.20 M Al(NO3)3is combined with 500 mL of a pH 4.25 HF/NaF buffer (total concentration of 2.0M). Given that the sodium salt of the complex ion has a solubility of 0.042 g/100 mL, will the sodium salt precipitate from the equilibrium mixture? Why or why not? If AlF63–forms, the sodium salt would be Na3AlF6; if AlF4–forms, the sodium salt would be NaAlF4.arrow_forward1. The Ksp of gold (I) chloride is 2.0 x 10-13. The Kr of the gold (I)-cyanide complex ion is 2.0 x 103%. A. Write the balanced net ionic equation for the reaction between AuCl and NaCN that produces the gold (I)-cyanide complex ion. B. Determine the value of K for the above chemical reaction. C. Determine the solubility of AuCl in a 0.20 M solution of NaCN.arrow_forward
- Cdf2 (s) = Cd²+ (aq) + 2 F- (aq) 1. A saturated solution of CdF2 is prepared. The equilibrium in the solution is represented above. In the solution [Cd2+] eq = 0.0585 M and [F-] eq = 0.117 M. a. Determine the solubility of CdF2. b. Some 0.90 M NaF is added to the saturated solution. Does the solubility of CdF2 increase, decrease, or remain the same? Justify your answer based on Q. 2. Is the solubility of AgCI(s) greater in distilled water or in tap water where the [CI-] = 0.010 your answer based on Q. M? Justifyarrow_forwardCN A buffer solution made from HCN and NaCN has a pH of 9.71. If pK for HCN is 9.40, what is the [HCN] [CN-1 [HCN] in the buffer?arrow_forwardThe formation constant* of [M(CN)4]² is 7.70 × 10¹6, where M is a generic metal. A 0.130 mole quantity of M(NO3)2 is added to a liter of 0.870 M NaCN solution. What is the concentration of M²+ ions at equilibrium? [M²+] = 0.130 Incorrect Marrow_forward
- What is the maximum concentration of Ag+ that can be added to a 0.00250 M solution of Na2CO3 before a percipitate will form? (Ksp for Ag2CO3 is 8.10 x 10-12)arrow_forwardWhich of the following statements is true? Select one: All sulfate salts are completely soluble. A supersaturated solution contains the maximum concentration of dissolved ions. Co(OH)2 (Ksp=5.9×10-15) is more soluble than PbI2 (Ksp=9.8×10-9). The solubility of AgCN increases in acidic conditions. The solubility of SrCO3 is greater in a solution of Na2CO3.arrow_forwardWhat is the value of the formation constant of the complex ion formed below? Equilibrium concentrations: [M3+] = 0.025 M; [L] = 0.015 M; [ML4] = 3.5 x 10-6 M %3D M3+ (aq) + 4L (aq) ML4 (aq) Select one: A. 2.8 x 103 B. 3.6 x 10-4 C. 6.0 x 102 D. 2.8 x 103arrow_forward
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