50ml = .05L of HCL 1.0 M = 1mol / 1L of HCL simply multiply - .05 by 1.0, and get your answer!
Yes m 0552 is generic roxycodone 5 mg
Since HCl is a strong acid it completely dissociates. Therefore [H+] = [HCl] and this case = 0.25 M. pH = -log [H+] = 0.602
About 13M. You can assume it is 13M if you don't need an exact concentration (like if you need a ~1M HCl solution for an extraction or whatever) but if you need an exact concentration (for a titration, for example) then you will need to standardize your HCl first.
Add 200 mls of the 1.0N HCl solution to a 1 liter volumetric flask. Make up to the mark with water. Standardize against a known weight of Sodium Carbonate.
50ml = .05L of HCL 1.0 M = 1mol / 1L of HCL simply multiply - .05 by 1.0, and get your answer!
Yes m 0552 is generic roxycodone 5 mg
HCl is a gas. It's therefore very difficult to accurately weigh out the proper amount to use to make a solution of any given concentration, and as the solution sits, some HCl may escape as gas. In contrast, it's very easy to weigh out a solid base to high precision, and use a solution made from it to standardize the only-approximately-known HCl concentration.
Since HCl is a strong acid it completely dissociates. Therefore [H+] = [HCl] and this case = 0.25 M. pH = -log [H+] = 0.602
1 m HCl is not more reactive than 4m HCl, but 4m HCl is more concentrated.
About 13M. You can assume it is 13M if you don't need an exact concentration (like if you need a ~1M HCl solution for an extraction or whatever) but if you need an exact concentration (for a titration, for example) then you will need to standardize your HCl first.
Add 200 mls of the 1.0N HCl solution to a 1 liter volumetric flask. Make up to the mark with water. Standardize against a known weight of Sodium Carbonate.
- log(0.00450 M HCl)= 2.3 pH=======
33.3 ml of 3.0 M HCl should be filled up and mixed with water up to 100.0 ml of a 1.0 M HCl solution.
0.1 M HCl =============
(7 mL)(X M HCl) = (27.6 mL)(0.170 M NaOH)7X = 4.692X = 0.7 M HCl==========
HCl is a gas. It's therefore very difficult to accurately weigh out the proper amount to use to make a solution of any given concentration, and as the solution sits, some HCl may escape as gas. In contrast, it's very easy to weigh out a solid base to high precision, and use a solution made from it to standardize the only-approximately-known HCl concentration.