With which of the following solutions would a 3.5 × 10⁻⁴ M solution of Ag⁺ ions NOT form a precipitate? Formula Ksp AgCl 1.8 x 10⁻¹⁰ Ag₃PO₄ 8.9 x 10⁻¹⁷ AgBr 5.0 x 10⁻¹³ Ag₂CO₃ 8.1 x 10⁻¹² A 5.0 × 10⁻⁵ M Cl⁻ B 5.0 × 10⁻⁵ M PO₄³⁻ C 5.0 × 10⁻⁵ M Br⁻ D 5.0 × 10⁻⁵ M CO₃²⁻

A student is asked to identify the metal nitrate present in an aqueous solution. The cation in the solution can be either Na+, Ba2+, Ag+, or Ni2+. Results of solubility experiments are as follows: unknown + chloride ions—no precipitate unknown + carbonate ions—precipitate unknown + sulfate ions—precipitate What is the cation in the solution?

Consider the following generic equation OH(aq)+HB(aq) B(aq)+H2OFor which of the following pairs would this be the correct prototype equation for the acid-base reaction in solution? If it is not correct, write the proper equation for the acid-base reaction between the pair. (a) hydrochloric acid and pyridine, C5H5N (b) sulfuric acid and rubidium hydroxide (c) potassium hydroxide and hydrofluoric acid (d) ammonia and hydriodic acid (e) strontium hydroxide and hydrocyanic acid

Describe in words how you would prepare pure crystalline AgCl and NaNO3 from solid AgNO3 and solid NaCl.