Question: The solubility of Agl in water is 1.22×10-8 M, but increases in the presence of thiosulfate ion. Calculate the solubility of Agl when the solid is added to a solution that is 0.655 M in thiosulfate ion. For Agl, Ksp = 1.50×10-16 and for Ag(S203)23-, Kf = 2.00×1013. Solubility = M?
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- Calculate the solubility of Au2CrO4 in a 0.13 M solution of Na2CrO4. Ksp for Au2CrO4 is 7.3x10^-40Calculate the molar solubility of calcium oxalate in a solution that has been buffered so that its pH is constant and equal to 4.00. Data: Kps of CaC2O4 = 1.7x10 -9 ; Ka1 of H2C2O4 = 5.60x10-2 and Ka2 = 5.42x10-5 . Use systematic treatment.From a 50.0 mL drink sample suspected to be spiked with cyanide (CN-), an 10.0-mL aliquot was taken for analysis. It was mixed with 10.0 mL 1% (m/v) HCl to prevent metal precipitation and diluted to 25.0 mL with distilled water. The concentration of this 25.0 mL dilution is 0.02089062 M. What is the concentration of CN- (M) in the 50.0 mL sample? Does the addition of 10.0 mL HCl affect the problem solving?
- Question 4 For the aqueous [Ag(NH3)2]^+ complex =Kf×1.7107 at 25°C.Suppose equal volumes of 0.0082M AgNO3 solution and 0.20M NH3 solution are mixed. Calculate the equilibrium molarity of aqueous Ag+ ion. Round your answer to 2 significant digits.The value of Ksp for Cd(OH)2 is 2.5 x 10-14. (a) Whatis the molar solubility of Cd1OH22? (b) The solubilityof Cd(OH)2can be increased through formation of thecomplex ion CdBr42 - (Kf = 5 x 103). If solid Cd(OH)2 isadded to a NaBr solution, what is the initial concentrationof NaBr needed to increase the molar solubility of Cd(OH)2to 1.0 x 10-3 mol/L?Buffer Preparation A researcher in Biochemistry is isolating α-glucosidase enzyme from malted wheat flour. The protocol requires the use of 2.00L of 0.225 M of lactate buffer with pH of 4.25. How will he/she prepare this buffer from 2.00 M lactic acid solution and solid sodium lactate (NaC3H5O3) The Ka of lactic acid is 1.38 x 10-4. [ Na=23.0, C=12.0, H=1.01, O=16.0 g/mol]
- Someone else on here solved this one wrong. The answer is not .37x10-6 Silver chromate is sparingly soluble in aqueous solutions. The ?sp of Ag2CrO4 is 1.12×10−12. What is the solubility (in mol/L) of silver chromate in 1.00 M potassium chromate aqueous solution? solubility:What is the silver ion concentration for a saturated solution of Ag2CO3 if the Ksp for Ag2CO3 is 8.4x10-12?If the molar solubility of PbCrO4 at 25 oC is 5.48e-07 mol/L, what is the Ksp at this temperature?Ksp = (b) It is found that 1.08e-09 g of Fe(OH)3 dissolves per 100 mL of aqueous solution at 25 oC. Calculate the solubility-product constant for Fe(OH)3.Ksp = (c) The Ksp of Mg3(PO4)2 at 25 oC is 1.04e-24. What is the molar solubility of Mg3(PO4)2?solubility = mol/L
- Calculate the molar solubility of Ni(OH)2 (Ksp = 2.0 × 10-15) in a solution which is buffered at pH = 9.75. Enter your answer as scientific notation with the correct number of sig figs. Use the #e# format.Questions 3-7 relate to the use of a 0.0322 M EDTA solution as the titrant in the titration of a 50.00 mL solution that is 0.0129 M in Cu2+. The solution is held at pH = 10.00 by a buffer that is 0.050 in ammonia (NH3). What is the concentration of free copper (II) cation (expressed as pCu) when 25.00 mL of titrant have been added?29) The following concentrations are found in mixtures of ions in equilibrium with slightly soluble solids. From the concentrations given, calculate Ksp for each of the slightly soluble solids indicated: (d) Ag2SO4: [Ag+] = 2.40 ×× 10–2 M, [SO42−][SO42−] = 2.05 ×× 10–2 M (e) BaSO4: [Ba2+] = 0.500 M, [SO42−][SO42−] = 4.6 ×× 10−8 M