Table 9.1: Behavior of Anions in the Presence of Several Metal Ions Anion Ag Solubie Ba" Soluble Ca Soluble Ph3 Soluble NO, cr, Br, I AgCl, white; AgBr, cream; Agl, yellow. All insoluble in HNO,. In NH,OH AgCl soluble, AgBr slightly soluble and Agl insoluble. PbCl2 and PbBr, white. Both soluble in hot water. Pblz, yellow. Slightly soluble in hot water. Soluble Soluble so, Moderately soluble. BasO, white, insoluble in HNO CaSO4, white, slightly soluble in HNO3 PbSO4, white, insoluble in HNO, so, Ag,SO, white, soluble in NH,OH and HNO, BaSO, white, soluble in HNO3 CaSO3, white, soluble in HNO PbSO,, white, soluble in HNO, Ag,S, black, soluble in hot, conc. HNO3. PbS, black, soluble in HNO, Soluble Soluble PO, Ag,PO4, yellow, soluble in NH,OH and HNO, Ba;(PO4)2, white, soluble in HNO, Ca3(PO)2, white, soluble in HNO, Pb;(PO)2, white, soluble in HNO, co,- Ag;CO,, white, soluble In NH,OH and HNO, BACO, white, soluble in HNO, CACO, white, soluble in HNO3 PbCO3, white, soluble in HNO3

Table 9.1: Behavior of Anions in the Presence of Several Metal Ions Anion Ag Solubie Ba" Soluble Ca Soluble Ph3 Soluble NO, cr, Br, I AgCl, white; AgBr, cream; Agl, yellow. All insoluble in HNO,. In NH,OH AgCl soluble, AgBr slightly soluble and Agl insoluble. PbCl2 and PbBr, white. Both soluble in hot water. Pblz, yellow. Slightly soluble in hot water. Soluble Soluble so, Moderately soluble. BasO, white, insoluble in HNO CaSO4, white, slightly soluble in HNO3 PbSO4, white, insoluble in HNO, so, Ag,SO, white, soluble in NH,OH and HNO, BaSO, white, soluble in HNO3 CaSO3, white, soluble in HNO PbSO,, white, soluble in HNO, Ag,S, black, soluble in hot, conc. HNO3. PbS, black, soluble in HNO, Soluble Soluble PO, Ag,PO4, yellow, soluble in NH,OH and HNO, Ba;(PO4)2, white, soluble in HNO, Ca3(PO)2, white, soluble in HNO, Pb;(PO)2, white, soluble in HNO, co,- Ag;CO,, white, soluble In NH,OH and HNO, BACO, white, soluble in HNO, CACO, white, soluble in HNO3 PbCO3, white, soluble in HNO3

Principles of Modern Chemistry

8th Edition

ISBN:9781305079113

Author:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Publisher:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Chapter16: Solubility And Precipitation Equilibria

Section: Chapter Questions

Problem 50P

See similar textbooks

Similar questions

Which of the following anions will separate Ag* from Pb** by precipitating one of them, leaving the other in solution? (A) CATIONS High Solubility (aq) Low Solubility (s) OOH™ O cr O C₂H30₂ 3- PO4³- Cl, Br, I Halides SO4²- Most Ag+, Pb²+, Tl+, Hg₂²+, Hg, Cu Solubility Table $2. Group 1, Nhì, Group 2 Most ANIONS OH Group 1, NH4*, Sr²⁰, Ba²+, Tl. Most SO4²- Most Ag+, Pb²+, Ca²+, Ba²+, Sr², Ra² CO32, C₂H3O2 NO3 PO4³-, SO3²- Group 1, NH4 Most All Group 1 compounds, including acids, and all ammonium compounds are assumed to have high solubility in water. Most All Ag+ None
al 38% 8:42 . Pharmaceutical Inorganic Chemistr... (Ph... O Calcium Sulfate O Strontium Sulfate The following are expected to be precipitated out of their solutions, except: Lithium Hydroxide O Zin Hydroxide O Aluminum Hydroxide Ferric Hydroxide O Magnesium Hydroxide The following are not properties of acids except:
Calculate the concentration of cobalt(III) ions in a solution formed by mixing 200 mL of o.10o M Co(NO,), with 150 ml. of 6.00 M NH, solution given K, of [Co(NH),13 is 4.5x103, [Co3 1- M
96% [4) Wed 3:41 AM Jarissa Collado Q A cvg.cengagenow.com My Home OWLV2 | Online teaching and learning resource from... [Review Topics] (References] Use the References to access important values if needed for this question. M Solid lead nitrate is slowly added to 75.0 mL of a 0.0486 M sodium iodide solution. The concentration of lead ion required to just initiate precipitation is s 2req M. Es M ts M Submit Answer Retry Entire Group ts 2req 8 more group attempts remaining Previous Next problem set O Focus 92%
How does the solubility of AgBr in 1.0 M NH, compare with its solubility in 1.0 M hypo? K, of Ag(NH,),* is 1.7X10".
Which of these statements about the common-ion effect ismost correct? (a) The solubility of a salt MA is decreased ina solution that already contains either M+ or A-. (b) Commonions alter the equilibrium constant for the reaction ofan ionic solid with water. (c) The common-ion effect doesnot apply to unusual ions like SO32- . (d) The solubility of asalt MA is affected equally by the addition of either A- or anoncommon ion.
Compare the solubility of silver sulfate in each of the following aqueous solutions: Clear All 0.10 M AGNO3 More soluble than in pure water. 0.10 M (NH4)2SO4 Similar solubility as in pure water. 0.10 M NH,CH,COO Less soluble than in pure water. 0.10 M KNO3
O KINETICS AND EQUILIBRIUM 三 Calculating the solubility of an ionic compound when a commo... olh Data Formula Ksp Calculate the solubility at 25 °C of CaF, in pure water and in a 0.0180M NaF solution. BaCro4 1.17x10-10 BasO4 1.08x10-10 Round both of your answers to 2 significant digits. CaCO3 3.36x10-9 CaF2 3.45x10-11 solubility in pure water: Co(OH)2 5.92x10-15 CuBr 6.27x10-9 CuCO3 1.4x10-10 solubility in 0.0180 M NaF solution: Fe(OH)2 4.87x10-17 PBCO3 7.40x10-14 PbCrO4 2.8x10-13 PBF2 3.3x10-8 Mg(OH)2 5.61x10-12 Ni(OH)2 5.48x10-16 AgBrO3 5.38x10-5 Ag2CO3 8.46x10-12 AgCI 1.77x10-10 Ag2Cr04 1.12x10-12 SrC03 5.60x10-10 ZnCO3 1.46x10-10 Zn(OH)2 3.0x10-17 AgBr 5.35x10-13 AuCl 1.77x10-10 Check O2021 McGraw-Hill Education. All Rights Reserved Temms of Use
Compare the solubility of barium carbonate in each of the following aqueous solutions: Clear All 0.10 M Ba(NO,)2 More soluble than in pure water. 0.10 M Na,CO, Similar solubility as in pure water. 0.10 M NH,NO3 Less soluble than in pure water. 0.10 M NACH;CO0
Calculate the solubility of Pb: (P0.), in 0.2M of H,SO4 ( Note that: K = 1.1 × 10¬17 ) sp
Salt (X) When conc. H2SO, is added to unknown solid salt with heating, an orange red fumes will be separated turns a paper wet with starch yellow, and when ammonium hydroxide solution added to solution of this salt a white gelatinous ppt. is formed which soluble in dil. Acids, Salt (X) represents............. a) Aluminum bromide b) Aluminum iodide c) Iron II bromide d) Potassium iodide
the amount remainning of Mn2+ ion dissolved in a solution when MnS precipitate at pH =5.5,, (k . s .p = 1x10-15) is