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- Suppose you want to prepare a solution of 2.50L of 1.00M HCL solution from concentrated 12.0 M HCl (aq.) How many liters of concentrated acid is needed and how many liters of water is needed?[Dimensional Analysis is appreciated!]3 q101 Please put solutions thanksA student determined the average molarity of their sample of acetic acid to be 0.608 M. Calculate the (w/w)% of the solution. Assume the density of this solution is that of pure water, dH2O = 1000. g/L. Enter a number without the '%' symbol.
- 2. PLease don't provide handwritten solution ...a) Calculate [H3O+] of the following polyprotic acid solution: 0.115 M H2CO3. Express your answer using two significant figures. b)Calculate [H3O+] of the following polyprotic acid solution: 0.135 M H3C6H5O7. Express your answer using two significant figures.Acetic acid Ka= 1.75 x 10^-5, 5.00 M