For each of the salts on the left, match the salts on the right that can be compared directly, using Ksp values, to estimate solubilities. (If more than one salt on the right can be directly compared, include all the relevant salts by writing your answer as a string of characters without punctuation, e.g, ABC.) fill in the blank 1 1. nickel(II) sulfide                          A. CuCO3 fill in the blank 2 2. nickel(II) hydroxide   B. Zn3(PO4)2         C. BaF2         D. Cu(OH)2 Write the expression for K in terms of the solubility, s, for each salt, when dissolved in water. nickel(II) sulfide                          nickel(II) hydroxide Ksp =     Ksp =

A 50.0 mL aliquot of a 0.00100M solution of acetic acid (K, = 1.8 x 10-5) is titrated with 0.00993M NaOH. Use the Indicator Table below to decide which of the indicators listed would most accurately signal the equivalence point for this titration. Properties of Several Indicators Write the letter corresponding to your choice of indicator in the box

Cons Praseodymium(II) hydroxide, Pr(OH)3, has a Ksp of approximately 3.39×10-24. Part A Calculate the molar solubility of praseodymium(II) hydroxide in an aqueous solution buffered at pH = 6.60.

(Asking this question again because I'm getting 2 different answers.)

Suppose that you want to titrate a sample of vinegar with standard sodium hydroxide solution to determine the concentration of acetic acid in it, and you want to use an indicator to help you determine the end-point. Which of the following indicator would be suitable?           (A) Bromocresol Green (Ka ~ 2.0 x 10–5; color: yellow in acid; blue in base)          (B) Methyl Red (Ka ~ 5.0 x 10–6; color: red in acid; yellow in base)          (C) Bromothymol Blue (Ka ~ 6.0 x 10–8; color: yellow in acid; blue in base)          (D) Any of them

Tris(hydroxymethyl)aminomethane [(HOCH2)3CNH2, MW = 121.14] is commonly referred to as Tris or THAM.  THAM is a weak base frequently used to prepare buffers in biochemistry.  Its Kb is 1.2 x 10−6. What weight of THAM must be taken with 100. mL of 0.50 M HCl to prepare 1 L of a pH 7.4 buffer?  (Assume no volume change.)

a) One liter of solution contains 0.10 mol of Ag+ and 0.10 mol of Ba2+. If a highly concentrated solution of K2CrO4 is added drop by drop, which will precipitate first, Ag2CrO4 or BaCrO4? (Ksp for Ag2CrO4 = 2.0 x 10-12; Ksp for BaCrO4 = 1.2 x 10-10) %3D %3D b) If the solution in part “a" contains 0.0010 mol of Ag+ and 0.0010 mol of Ba2+ instead, which will precipitate first, Ag2CrO4 or BaCrO4?

What is the pH of a buffer that is 0.200M HC2H3O2 and 0.100M NaC2H3O2 (Ka =1.8 x 10-5).