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Calculate the molar mass of the following substances: (a) Ethyne, C 2 H 2 (b) Sulphur molecule, S 8 (c) Phosphorus molecule, P 4 (atomic mass of phosphorus = 31) (d) Hydrochloric acid, HCl (e) Nitric acid, HNO 3
What volume of a concentrated hydrochloric acid solution, which is 36.0% hydrochloric acid by mass and has a density of 1.179g/mL, should you use to make 5.00L of a hydrochloric acid solution with a pH of 1.8?
Calculate the molar mass of the following substances. (a) Ethyne, C 2 H 2 (b) Sulphur molecule, S 8 (c) Phosphorus molecule, P 4 (Atomic mass of phosporus = 31) (d) Hydrochloric acid, H C l (e) Nitric acid, H N O 3
The balanced chemical equation is: Mg_((s))+ 2HCl_((aq))rarrMgCl_(2(aq)) + H_(2(g) The reaction between magnesium and hydrochloric acid combine to form a salt of magnesium chloride and release hydrogen gas. This single replacement reaction is a classic example of a metal reacting in an acid to release hydrogen gas. I hope this was helpful. SMARTERTEACHER You can watch this reaction in the ...
Step 3. Calculate the moles of HCl. 448.6g HCl × 1 mol HCl 36.46g HCl = 12.30 mol HCl. Step 4. Calculate the molarity of the HCl. molarity = moles of HCl litres of solution = 12.30 mol 1 L = 12.3 mol/L. Here's a summary of the types of calculations we were using above. And here's a video about converting mass % to molarity.
Calculate the molecular mass of the following substances: (a) Ethyne (C 2 H 2) (b) Sulphur molecule (S 8) (c) Phosphorus molecule (P 4) (d) Hydrochloric acid (H C l) (e) Nitric acid (H N O 3) View Solution
The molar mass of CaCI2 is 111.0 g/mol and the molar mass of water is 18.02 g/mol. How many moles of MgCl2 are produced from 3 moles of HCl? An experiment asks that you use 1.0 g of p-aminobenzoic acid. The molar mass of p-aminobenzoic acid is 137.136 g/mol. Exactly 1.0 g of acid is ____ moles.
In this context, hydrochloric acid's specific gravity tells you what the density of a specific hydrochloric acid solution is compared with that of water. More specifically, the density of your hydrochloric acid solution will be equal to. SG = ρHCl ρwater ⇒ ρHCl = SG ×ρwater. ρHCl = 1.08 × 1.00 g/mL = 1.08 g/mL.
"12.3 M" As you know, molarity is defined as moles of solute, which in your case will be hydrochloric acid, "HCl", divided by liters of solution. This means that you can make the calculations easier by picking a "1.00-L" sample of this concentrated hydrochloric acid solution. In this particular case, the molarity of the solution will be equal to the number of moles of solute. So, use the ...
0.1 and 0.9, respectively. You know that your solution is 20% hydrochloric acid by mass, which means that every "100 g" of this solution contain "20 g" of hydrochloric acid, the solute. To make the calculations easier, pick a sample of this solution that has a mass of exactly "100 g". Since you already know that this sample contains "20 g" of hydrochloric acid, you can say that the mass of ...