Which of the following describes what happens to the solubility of a slightly soluble ionic compound when a common ion is added to the solution? There is no effect on the solubility of the ionic compound. More of the ionic compound dissolves. The solubility of the ionic compound is reduced. The solubility of the ionic compound is increased.

In an acid-base titration experiment, the equivalence point on the titration curve was at a pH of 6.0. Based on this information, which of the following is represents the titration experiment that was conducted? It was a titration conducted between a strong base and strong acid It was a titration conducted between a weak acid and a strong base. It was a titration conducted between a strong acid and a weak base

1. Using the solubility chart, explain whether or not this double replacement reaction will occur. FeSO4 + NaCl  ->  Na2SO4  + FeCl2   2. In order for a double replacement reaction with precipitate to occur, what must be true. Select all that apply The ion doing the replacing must be more reactice than the ion it replaces   Both reactants must be soluble in water   Both products must be soluble in water   One of the reactants must be insolube in water   One of the products must be insoluble in water

Some soluble compounds are listed in the table below. Classify each compound using the checkboxes. type of compound (check all that apply) name strong weak strong weak ionic molecular acid acid base base ammonia potassium hydroxide sodium hydroxide sodium perchlorate

CaCl2(aq) + 2 AgNO3(aq) ⟶Ca(NO3)2 + 2 AgCl   Fill in the blanks with either an (s) or an (aq) to indicate the phase of each product. Use the Solubility Rules.

The Solubility Product Constant for silver phosphate is 1.3 x 10^-20. The maximum amount of silver phosphate that will dissolve in a 0.270 M sodium phosphate solution is ________M.

Be sure to answer all parts. Solid NaI is slowly added to a solution that is 0.0099 M Cu+ and 0.0081 M Ag+. Which compound will begin to precipitate first?    NaI    CuI    AgI Calculate [ Ag+ ] when CuI just begins to precipitate.    × 10   M   Enter your answer in scientific notation. What percent of Ag+ remains in solution at this point?    %

Determine the compound that is expected to be more soluble in acidic solution than in neutral or basic solution. О KBr O BaCl2 O Ni(OH)2 O Cu(NO3)2

Which of the following best describes why magnesium hydroxide, found in milk of magnesia, is soluble in acidic solution? O According to Le Chatelier's principle, the acid will react with hydroxide ions in the solution, forming water and thereby decreasing the concentration of hydroxide ions in solution causing more magnesium hydroxide to dissolve. O Magnesium hydroxide does not dissolve in acidic solutions. O According to Le Chatelier's principle, the acid will react with magnesium ions in the solution, forming magnesium hydride and causing more magnesium hydroxide to dissolve. O According to Le Chatelier's principle, the acid will react with water in the solution, forming hydroxide ions and thereby decreasing the concentration of magnesium ions in solution causing more magnesium hydroxide to dissolve. O According to Le Chatelier's principle, the acid will react with hydroxide ions in the solution, forming a precipitate.

According to the solubility chart, is MgCO3 soluble or insoluble?