![SOLVED:Calculate the percent ionization of hydrofluoric acid at these concentrations: (a) 0.60 M, (b) 0.080 M (c) 0.0046 M, (d) 0.00028 M . Comment on the trends. SOLVED:Calculate the percent ionization of hydrofluoric acid at these concentrations: (a) 0.60 M, (b) 0.080 M (c) 0.0046 M, (d) 0.00028 M . Comment on the trends.](https://cdn.numerade.com/previews/ebb10fca-ce9e-431e-9ec1-7301de23d8ae.gif)
SOLVED:Calculate the percent ionization of hydrofluoric acid at these concentrations: (a) 0.60 M, (b) 0.080 M (c) 0.0046 M, (d) 0.00028 M . Comment on the trends.
![Worked example: Finding the percent ionization of a weak acid | AP Chemistry | Khan Academy - YouTube Worked example: Finding the percent ionization of a weak acid | AP Chemistry | Khan Academy - YouTube](https://i.ytimg.com/vi/_jEe0Tkyn3w/maxresdefault.jpg)
Worked example: Finding the percent ionization of a weak acid | AP Chemistry | Khan Academy - YouTube
![pH = -log[H+] assuming 100 percent dissociation; if given percent ionization, multiply by the molarity… | Chemistry lessons, Teaching chemistry, Chemistry education pH = -log[H+] assuming 100 percent dissociation; if given percent ionization, multiply by the molarity… | Chemistry lessons, Teaching chemistry, Chemistry education](https://i.pinimg.com/originals/99/80/05/998005d7b3fbb74f7a91222f3209e7c5.png)