Which one of the following indicators is best suited for titrating 0.40 M ammonia (pKb = 4.74) with 0.40 M HCl?   A.  Alizarin yellow, pKa = 11.2   B.  Phenol red, pKa = 7.9   C.  Bromocresol purple, pKa = 6.3   D.  Methyl red, pKa = 5.0   E.  Bromophenol blue, pKa = 3.9

What is the solubility of magnesium fluoride in a butter solution containing 0.45 M HC2H3O2 (acetic acid) and 0.20 M NaC2H3O2? The Ksp for magnesium fluoride is 6.5 109 (See the hint for Problem 17.131.)

Lactic acid (CH3CHOHCO2H) is found in sour milk, in sauerkraut, and in muscles after activity. (Ka for lactic acid = 1.4 104.) (a) If 2.75 g of NaCH3CHOHCO2, sodium lactate, is added to 5.00 102 mL of 0.100 M lactic acid, what is the pH of the resulting buffer solution? (b) Is the pH of the buffered solution lower or higher than the pH of the lactic acid solution?

The salt MX has a solubility of 3.17 108 mol/L in a solution with pH = 0.000. If K4 for HX is 1.00 1015, calculate the Ksp value for MX.

What reagent might be used to separate the ions in each of the following mixtures, which are 0.1 M with respect to each ion? In some cases it may be necessary to control the pH. (Hint: Consider the KSP values given in Appendix J.) (a) Hg22+ and Cu2+. (b) SO42- and Cl-. (c) Hg2+ and CO2+. (d) Zn2+ and Sr2+. (e) Ba2+ and Mg2+. (f) CO32- and OH-

Assuming that the solubility of Ca3(PO4)2(s) is 1.6 107 mol/L at 25c, calculate the Ksp for this salt. Ignore any potential reactions of the ions with water.

You are browsing through the Handbook of Hypothetical Chemistry when you come across a solid that is reported to have a Ksp value of zero in water at 25C. What does this mean?

What is the molar solubility of Pb(OH)2 (Ksp = 2.8 x 10−16) in a buffer solution containing the same amount of NH3 and NH4+?  (Kb = 1.8 x 10−5) 7.9 x 10−6 4.3 x 10−6 8.6 x 10−7 1.2 x 10−5 4.3 x 10−7

Phosphoric acid is a triprotic acid (Kal = 6.9 x 10-3, K₁2 = 6.2 x 10-8, and K₁3 = 4.8 x 10-13). a2 To find the pH of a buffer composed of H₂PO (aq) and HPO2 (aq), which pKa value should be used in the Henderson-Hasselbalch equation? O pKal = 2.16 O pK ₁2 = 7.21 a2 OpK₂3 = 12.32 Calculate the pH of a buffer solution obtained by dissolving 17.0 g of KH₂PO4(s) and 28.0 g of Na₂HPO4(s) in water and then diluting to 1.00 L. pH =

A buffer is formed by dissolving 0.105 moles of HCIO, hypochorous acid; and 0.115 moles of NaCIO, sodium hypochlorite; in 200 ml of water. Ka 3.0 X 10-8. a) Find the pH of the buffer. b) How does the pH compare with the pka? c) How much does the pH change when 2.00 ml of 0.50 M NaOH is added to the buffer? d) What would be the pH change if 2.00 ml of 0.50 M NaOH was added to 200 ml of pure H2O? e) How does this pH change compare to the addition of the same amount of 0.50 M NaOH to the buffer solution (as in c)?