In photography, unexposed silverbromide is removed from film bysoaking the film in a solution ofsodium thiosulfate, Na,S,Os Silverion forms a soluble complex withthiosulfate ion, 5,0,2, that has theformula Ag(S,Os), and formationof the complex causes the AgBrinthe film to dissolve. The Ag(5:03)complex has K-2.0x 1013 Howmany grams of AgBr (K-5.4 x1013) will dissolve in 243 mL of 1.55MNa2S2O3 solution?mass of AgBr =ih

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Answered: In photography, unexposed silver…

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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4. A solution is 0.0350 M in Na2SO4 and 0.0350 M Na2CO3. Solid Pb(NO3)2 is added without changing the volume of the solution. Which salt will precipitate first, PbSO4 or PbCO3? Explain clearly.
.2+ In aqueous solution the Ni ion forms a complex with four cyanide anions. Write the formation constant expression for the equilibrium between the hydrated metal ion and the aqueous complex. Under that, write the balanced chemical equation for the first step in the formation of the complex. K₁ = ☐ Write the First Step: First Step: ロ→ロ ☑ ك
R456
Aluminumcan 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.
An aqueous solution at 25°C is 0.10 M in both Mg2+ and Pb2+ ions. We wish to separate the two kinds of metal ions by taking advantage of the different solubilities of their oxalates, MgC2O4 and PbC2O4.(a) What is the highest possible oxalate ion concentration that allows only one solid oxalate salt to be present at equilibrium? Which ion is present in the solid—Mg2+ or Pb2+?(b) What fraction of the less soluble ion still remains in solution under the conditions of part (a)?
1. 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.
A solution contains 0.0010 mol of KI and 0.10 mol of KCl per liter. AgNO3 is gradually added to this solution. Which forms first, solid AgI or solid AgCl?
CN 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?
12. = a The solubility product constant for the salt silver chromate, Ag₂CrO4 is Ksp 1.9 × 10-¹². If 1.00 mmol of Ag+ is combined with 1.00 mmol of CrO4²- to produce 1.00 L of solution upon mixing: a. A precipitate will form since Qsp > Ksp b. [Ag+] [CrO2-]o = 0 c. [Ag+] [CrO²-] = d. More than one response is correct b. Which of the following salts is not more soluble in an acidic solution than in pure water? a. CaF2 b. Ag3PO4 c. PbCl₂ d. Fe(OH)3
Calculate the concentration of metal ions, M³+, in a solution that initially contains 0.20 M M(NO3)3 and 1.60 M lit cyanide which produces the complex ion [M(CN)6]³, Kf = 2.47 × 10³1
Please explain steps.
Silver carbonate has a K = 5.65×10-¹2 and a solubility of 0.0001122 M in water. Solid silver sp carbonate is placed into a silver nitrate solution. What concentration of silver nitrate is necessary to reduce the solubility of the silver carbonate to 1×109 M? [AgNO,]= M

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