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How do you remove gold from a computer?
If you identify gold color, remove unnecessary parts, grind (IC's) and soak in 10% HCL, then add a little hydrogen peroxide, this will lift the gold
How many molecules of HCI will be required to have 10 grams of it?
To calculate the number of molecules of HCl in 10 grams, you first need to determine the molar mass of HCl, which is about 36.5 g/mol. Next, use the formula n = m/M, where n is the number of moles, m is the mass in grams, and M is the molar mass. Finally, use Avogadro's number (6.022 x 10^23 molecules/mol) to convert moles to molecules.
How do you convert 36 percent hcl to 10 percent hcl?
Take 100 grams of 36% HCl-sol'n and add it up with (260 g) water to total weight of 360 gram 10% HCl-sol'n.Don't use volumetrics, because the density is not linearally changing and there is no 'Law of conservation' for 'volumes' (only for mass).
What about a 10 panel test?
have to test a employee need to know what test to use
What is N10 HCL and how will you prepare it?
N10 HCl would be 10 M HCl. You might mean N/10 which would be 0.1 M. (N or normal is an old-fashioned way to define chemical concentrations. Most chemists prefer M or molar concentrations.) Just take some higher-concentration HCl and dilute it to get the desired concentration. Use the dilution formula C1V1 = C2V2 to figure out how much high-concentration HCl to use for the volume of dilute HCl you want to make. If anything here doesn't make perfect sense, you probably shouldn't be working unsupervised with chemicals, and if you don't know what HCl is then you definitely shouldn't do whatever it is you are trying to do. 10 M HCl is a caustic liquid that gives off caustic vapors so wear goggles and be careful with it.
How do you get 0.1M from 1M HCL?
To make a 0.1M solution from a 1M HCL solution, you would dilute the 1M HCL with 10 parts of water (or whatever solvent you are using). For example, mix 1 mL of 1M HCL with 9 mL of water to obtain a 0.1M HCL solution.
How many moles of HCl are represented by 1.0 x 1019 HCl molecules?
The number of Avogadro states that 1 mole equals 6.02214179*10^23 mole. So if you have 1*10^19 HCl molecules, you have: 1*10^19 / 6.02214179*10^23 = 1.660538783*10^-5 mole of HCl. Which equals 0.0166053878 milimole.
23.74cm3 0.0147 mol dm-3NaOHare required to neutralize 25.00 cm3 of HCl calculate concentration of HCl acid in moldm-3and g dm-3?
HCl + NaOH ― NaCl + H2O nNaOH = c*v = 0.01470 * 23.74*10-3L = 3.49*10-4 mol 1 mol HCl reacts with 1 mol NaOH therefore nHCl = 3.49*10-4mol CHCL= nNaOH /VNaOH = 3.49*10-4 / 25.00*10-3 = 13.96 * 10-3 mol.dm-3
How do you prepare 10 M HCL from 37 percent HCL?
37% HCl = { [ 37 (gHCl) / 100 (g sol'n) ] / 36.46 (gHCl/molHCl) } * 1,18 (g sol'n/mL sol'n) * 1000 (mL/L) = about 12 M HClTo prepare V Litres of 10M sol'n you should dilute [10*V]/12 Litre of 37% HCl solution to the total volume of V. Be very carefull with this addition of water.
What is ghr on jewelry mean?
for the love of god buy a test kit. it is 10 kt gold
Calculate the molarity of HCl of pH 5.7?
To calculate the molarity of a solution from its pH, use the formula: pH = -log[H+]. In this case, pH 5.7 corresponds to [H+] = 1 x 10^-5.7 M. Given that HCl is a strong acid and dissociates completely in water, the molarity of HCl is also 1 x 10^-5.7 M.
Calculate the molarity of a 10 percent aqueous solution of HCl?
molarity = mol / litre The concentration is 10% HCl in water, assuming this is expressed in w/v (weight to volume) as this is the normal way. The density of 10% HCl is unknown but will be estimated to be the same as water (although slightly incorrect), since no data is given. 1 L of which 10% are HCl is assumed to weigh 1000 grams. 10% HCl x 1000g = 100g of HCl. 100g of HCl is present in 1 L. The mw of HCl = 36.5g/mol, 100g/(36.5g/mol) = 2.74mol is present in 1 L. The molarity is 2.74mol / 1 L = 2.7 M (two significant figures) (Looking up hydrochloric acid in wikipedia tells us that the density of a 10% solution is actually 1048g/L and the actual molarity becomes 2.87M. The calculated number was close enough, but it shows that the density is important. Molality on the other hand is mol/kg, so with molality we can skip the unknown density problem. For practical purposes, molarity is still the mostly used one, because volume is easier to measure than weight in the laboratory when handling toxic solvents that are unhealthy to inhale.)
