280 mL of 1.08 M CrCl₂ is mixed with with 160 mL of 2.2 M KOH. Write out the balanced molecular, ionic, and net ionic equations. Then determine what mass of precipitate will form.

Consider two aqueous solutions: one of ammonium carbonate and one of barium nitrate.  List the ions present in each.  Is a precipitate formed when the two solutions are mixed?  If so, write the molecular, ionic and net ionic equation. Identify the spectator ions

A 25.00 mL sample of sodium hydroxide was titrated (neutralized) with 36.4 mL of 0.125 M sulfuric acid.  What is the concentration of the sodium hydroxide solution? Group of answer choices 0.364 M 0.728 M 1.46 M 0.091 M 0.182 M

a) The addition of 0.3800 L of 1.150 M KCl to a solution containing Ag+ and Pb2+ ions is just enough to precipitate all of the ions as AgCl and PbCl2. The total mass of the resulting precipitate is 61.60 g. Find the masses of PbCl2 and AgCl in the precipitate. b) A solution contains Al3+ and Co2+ The addition of 0.3533 L of 1.847 M NaOHNaOH results in the complete precipitation of the ions as Al(OH)3 and Co(OH)2. The total mass of the precipitate is 23.08 g Find the masses of Al3+ and Co2+ in the solution.

7) A sample of an unknown alkaline earth metal hydroxide is dissolved in 100.0 mL of water. The resulting solution is titrated to an indicator endpoint with 1.008 M aqueous All Sections b) If the sample amount is 1.042 g, what is the molar mass of the unknown metal hydrochloric acid. The indicator changes color after 17.00 mL of the acid has been added. a) Write the generic equation. hydroxide? hsoc) What is the identity of the metal?

Complete the table below by deciding whether a precipitate forms when aqueous solutions A and B are mixed. If a precipitate will form, enter its empirical formula in the last column. Does a precipitate form when A and B empirical formula of solution A solution B precipitate are mixed? olo manganese(II) iodide cadmium acetate O yes no silver nitrate sodium bromide yes no 18 Ar sodium sulfide zinc nitrate O yes no

Titration is a type of experiment that can be performed to investigate a neutralization reaction. The equivalence point is when all of the acid and base is fully neutralized. A sample of 0.869 M aqueous potassium hydroxide was titrated against a standard solution of hydrochloric acid. What was the volume of the potassium hydroxide solution if 77.5 mL of 1.50 M hydrochloric acid was needed to reach the equivalence point? Enter a numerical answer only, in terms of mL.

Determining the volume of base needed to titrate a given mass of acid.

Complete and balance the precipitation reactions. Include physical states. Refer to the solubility rules as necessary. K3PO4(aq)+MgCl2(aq)

When excess lead(II) nitrate was added to 225 mL of a solution of potassium iodide, a solid precipitate formed. The dry precipitate had a mass of 7.25 g. What was the concentration of iodide ions in the solution of potassium iodide? a)  0.193 mol/L   b)  0.140 mol/L   c)  0.280 mol/L   d)  0.070 mol/L   e)  0.096 mol/L