Type your answer here...
For AuCl, Ksp = 2.0 x 10-13 at 25°C. What is the solubility of AuCl at this temperature?
4.5 x 10<sup> -7 </sup>
4.5 x 10<sup>-7</sup> to simplify 4.5 x 10-7
(AuCl has Ksp = 2.0 x 10-13)-1.0 x 10-12
Gold (I) Chloride.
Gold (I) Chloride.
Most commonly it is AuCl3 for gold(III) chloride. Gold(I) chloride would be AuCl.
Examples: AuCl3, AuCl, HAuCl4, Au2(SO4)2 etc.
There is no chemical with the formula AuC1. You most likely mean AuCl, which is gold I chloride.
The chemical symbol for gold is Au. An example of a chemical formula for a chemical compound of gold is AuCl.
There is not chemical compound with the formula AuCI. You most likely mean AuCl, with a lowercase L. This is gold I chloride.
Gold chloride AuCl. The electronegativivty difference (0.62) is less than in RbCl (2.34)
I'm not certain this will work, never having tried it myself, but I think it's worth a try. I think your best bet to change AuCl into pure gold is to try electrolysis. First dissolve the AuCl in water. It would work best with distilled water but regular water will work too; the gold just won't be as pure. Cover the solution with plastic wrap or something that you can puncture. Obtain two nails. These will act as electrodes. Set them up in a way such that the point of each nail is in the solution and the head is sticking out of the solution. That's what the plastic wrap is for. Also, it might be a good idea to saw off the points of the nails because the gold metal will be attatching to one of the nails and it would be difficult to remove if the nail still had a tip. Make sure the two nails aren't touching. Next, get a battery, 9 volt or better. Attach a wire from the cathode to one of the electrodes and attach another wire from the anode to the other electrode. Let it sit. If everything worked out well, there should be a deposit of solid gold at the end of one of the nails. I don't know of a test for gold salts, but if the water changes color when you dissolve the AuCl, all gold salts, regardless of the anion will cause the same color change.
There are two types of replacements in Chemistry. There are single and double replacements. A single replacement is when an element replaces another element within a compound, but in order for this reaction to occur the elemet that is being replaced must be less active than the element that is being replaced. This can be determined using an activity series. A double replacement is when two compounds switch their elements: NaF + AuCl --> NaCl + AuF. (This reaction may not actually occur, it is just a demonstration of how the elements replace eachother). Finally, within these reactions if pure water (H2O) is formed the reaction is classified as a neutralization and a no reaction. !
Gold is called a noble metal because it resists reacting with stuff. But it can be "convinced" to react, and it forms numerous compounds. It's oxidation states range from -1 to +5, with +1 and +3, Au(I) and Au(III), far and away the most common. Gold will dissolve in mercury, but creates an amalgam rather than react with it to create a compound. Aurum (gold) resists most acids, though aqua regia (a 3:1 mix of concentrated hydrochloric and nitric acids) will attack gold, as will cyanide. In the unusual -1 state, gold will form compounds like CsAu (cesium auride). It will hook up with the most reactive of the Group 1 and Group 2 elements, the Alkali and Alkaline Earth elements. Remember that the activity of these elements increases as you go down the column. That's just the opposite of the Group 17 elements, the halogens (fluorine, chlorine, etc.), whose reactivity increases as you go up the column. Speaking of the halogens, the Group 17 elements, will react with gold (Au), and auric fluoride (gold fluoride, AuFl) and auric chloride (gold chloride, AuCl) would be examples. Gold will form compounds in its +1 oxidation state with other ions, and it will also similarily form a number of compounds in the +3 oxidation state. There are also compounds (cluster compounds) where gold will form a compound that includes both the +1 and +3 oxidation states of the metal. It has "dual" (fractional) oxidation states in a single compound. Links are provided for more information.