10x -- split this amount into 4 semi-equal amounts for 4 different tests.

Despite the fact that this Ruthernium is powdered metal it is nonetheless very difficult to dissolve in Aqua-Regia. In fact it took 4 A-R digestions to get most of each sample into solution.
Aqua-Regia (A-R) is 1 drop HNO3 & 3 drops HCl.
This A-R was premixed and then placed on the powdered Ruthenium metal. Because there was no digestion after several minutes heat was added, which still did not dissolve all of the Ru powder. A-R was added to the Ru metal 3 more times and most of the metal final dissolved.
The A-R vapors while dissolving the Ru with heat has a bitter citric and chlorine odor and has a tendency to sting the eyes. The Air color while dissolving the Ru has a slight greenish-yellow color and appears a little like oil.
After the A-R has dissolved the Ru and brought to dry a drop of HCl is added to the dried solution area. It heated to dry and the process repeated at least 2 more times, which should have driven off any remaining nitrates and rendering the solution to a chloride.

When heating the Ruthenium chloride solution the vapor odors slightly resemble the other PGMs in similar conditions.

40x – A magnified view of the preceding image of the Ruthenium metal powder.
Individual Ru particles measure on average between 0.001” & 0.004” and has a strong tendency to form clumps.

10x – A single crystal of K2Cr2O7 (potassium dichromate) was inserted into the Ruthenium chloride solution.
A slow forming orange color occurred as the K2Cr2O7 dissolved in the otherwise essentially colorless solution.
No precipitants formed, so gentle heat was applied to see if heat would initiate a precipitation, which it did not.

40x – A magnified view of the preceding upper right image to better illustrate the effects of K2Cr2O7.Obviously K2Cr2O7 is not a reagent that will indicate the presence of Ruthenium in this chloride solution.

10x – A single crystal of ammonium chloride was inserted into another Ruthenium Chloride solution, which produced no precipitants.

40x – A magnified view of the preceding image, near center of the dried Ruthenium chloride solution showing this interesting crystal pattern.
Although these crystal formations might be clues I would not consider using ammonium chloride to help identify the presence of Ruthenium in a chloride solution.

40x – Another magnified view of the center area of the dried RuCl solution, focusing upon some of the crystals that can be seen in the 10x image.
I do not consider these crystal formations as being particularly beneficial in helping identify Ruthenium in a chloride solution.

40x – Another magnified view showing some of the crystals that form at the perimeter of solution as well as some nearly transparent cubic looking crystals. I would not use any of these crystal formations to help me determine if Ruthenium was present in a chloride solution.

40x – In another solution of Ruthenium chloride a single crystal of potassium Iodide (KI) was inserted and slowly brought to dry.

No precipitant formed.
This less than definable crystal pattern is not what I would ever use to determine the presence of Ruthenium in a chloride solution.

Note: None of the reagents used and shown here were of any value. Furthermore, getting this finely divided ruthenium metal to dissolve in Aqua-Regia is really a difficult and time consuming chore. Many more microchems are required before I can claim any thorough understanding of Ruthenium in a chloride solution.

Zinc cementation seems to have some practical application.

10x – This toothpick tip was dipped in the original, heated Aqua-Regia solution. Oddly, there are 2 different colored metal formations – white and reddish.
It’s possible, even likely that the silvery colored metal is un-dissolved particles of Ruthenium that the toothpick soaked-up, whereas the reddish metal was actually dissolved and was reduced in the hottest part of the cigarette lighter flame.

10x – This toothpick tip was dipped in the original, heated Aqua-Regia solution. Oddly, there are 2 different colored metal formations – white and reddish.
It’s possible, even likely that the silvery colored metal is un-dissolved particles of Ruthenium that the toothpick soaked-up, whereas the reddish metal was actually dissolved and was reduced in the hottest part of the cigarette lighter flame.