Multiply .3631 and 1.185 together and take that answer and multiply it by 175. That's your answer.
10 ml of concentrated HCl added to 90 ml of water.
The concentration of the diluted solution will be 15(300/1000) = 4.5 %, if the percent is expressed on a weight/volume basis.
pH = ZERO - very strong acid
Add 57.25 g of water to 100 g of 31.45%HCl solution,because [(31.45/20)*100]-100 = 57.25 g
1.3
10 ml of concentrated HCl added to 90 ml of water.
The concentration of the diluted solution will be 15(300/1000) = 4.5 %, if the percent is expressed on a weight/volume basis.
6M
pH = ZERO - very strong acid
There will be movement of water by osmosis from the less-concentrated solution (left) to the more-concentrated solution (right). Water will tend to flow from a more-dilute state to a less-dilute state.
Add 57.25 g of water to 100 g of 31.45%HCl solution,because [(31.45/20)*100]-100 = 57.25 g
The direction will be towards the more concentrated side so the 10% solution with go towards the 20% solution in an attempt to reach equilibrium.
1.3
My best guess is about pH = 12 to 12.5, it is a rather concentrated but weak base.
32% hydrochloric acid is 10.2 M. You must dilute it to the desired molar concentration. For safety, be careful to add the acid to water and to wear appropriate protection.
The water volume is 212,5 mL.
Acetic Acid is a weak acid in that it is only partially dissociated. Hydrocholric acid is highly corrosive and is much stronger