Chapter 26, Problem 2ASA

Silver nitrate is added to a solution of 1 x 10-2 M sodium acetate (Ksp AgC2H3O2 = 1.9 x 10-3): a) At what concentration of Ag+ does a precipitate start to form? b) What is the concentration of acetate ion in solution if [Ag+] = 0.500 M ?

Will a precipitate form when 25 mL of 0.020M AgNO3 is mixed with 35 mL of 0.020M Na2SO4? (Ksp Ag2SO4 = 1.2 x 10-5 )

Will a precipitate form when 100.0 mL of a 4.6 ✕ 10-4 M Mg(NO3)2 is added to 100.0 mL of 5.1 ✕ 10-4 M NaOH? (Hint: Ksp for Mg(OH)2 = 8.9 ✕ 10-12)   Yes   Give the value of Q, to support your answer.   __________________________________

1) a)Calculate the value of the ion product of PbCl2 (Ksp = 1.6 ×10-5) when 255 mL of 0.016 M KCl (aq) are added to 245 mL of 0.175M Pb(NO3)2. b) The solubility product of magnesium flouride (MgF2) is 7.4x10-11 mol3/L3. What is the molar concentration of Mg2+ ions in mol/L in an equilibrium mixture of magnesium flouride? c) The solubility product of barium sulphate (BaSO4) is 1.1x10-10 mol2/L2 . What is the molar concentration of SO42- ions in mol/L in an equilibrium mixture of this salt? need all 3 or else I will downvote

Chromium (III) iodate, Cr(IO3)3, has a solubility product of 5.0 x 10^-6 . Calculate the solubility of chromium (III) iodate in 0.25 M KIO3. Will precipitate form if 12.0 mL 9.60 x 10^-3 M Cr(NO3)3 and 6.50 mL 0.175 M NaIO3 are combined? *only need help with bold

What is the solubility product expression and the Ksp value of silver sulfate, Ag2SO4 (MM=312), if the solubility of the salt is 5.7x10-3 g/mL? (Ans. Ksp = 2.3x10-5)

PART 2: A solution is prepared by mixing 150.0 mL of 0.0010 M magnesium nitrate and 250.0 mL of 0.100 M sodium fluoride (Ksp = 7.4x10-11). Is Ksp greater than , equal to, or lower than Qsp?   Will a precipitate form, Y/N?   What is the fluoride ion concentration (in solution) after mixing is complete? Give your answer in exponential form and to three sig. figs. (e. g. 1.23E-3).   What is the magnesium ion concentration (in solution) after mixing is complete? Give your answer in exponential form and to three sig. figs. (e. g. 1.23E-3).

A solution contains 0.018 mole each of I-, Br-, and Cl-. When the solution is mixed with 200. mL of 0.24 M AgNO3, what mass of AgCl(s) precipitates out, and what is [Ag+]? Assume no volume change. Agl: Ksp = 1.5 x 10-16  AgBr: Ksp  = 5.0 x 10-13 AgCI: Ksp  = 1.6 x  10-10

1.Given that the solubility products (Ksp) of silver chloride(AgCl),silver iodide(AgI) and silver bromide (AgBr) are 1.82×10^-10,1×10-16,5.2×10^-13 and 1.82×10^-10 respectively.Plot an arbitrary titration curve of pAg versus volume of AgNO3 for each of the above on the same set of axis.You may assume that the concentration and volume of starting materials the same. 2.Using the information above,predict the order in which each species would precipitate from first to last