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orchidwasp82Lv1
28 Sep 2019
1.) Assuming complete dissociation, what is the pH of a 3.51mg/L Ba(OH)2 solution?
**Is there a specific formula for this, please help!
2.) Enough of a monoprotic acid is dissolved in water to produce a0.0177 M solution. The pH of the resulting solution is 2.32.Calculate the Ka for the acid.
**For Ka I got .56 and then converting that into pK I got .252, butI don't believe this is right
1.) Assuming complete dissociation, what is the pH of a 3.51mg/L Ba(OH)2 solution?
**Is there a specific formula for this, please help!
2.) Enough of a monoprotic acid is dissolved in water to produce a0.0177 M solution. The pH of the resulting solution is 2.32.Calculate the Ka for the acid.
**For Ka I got .56 and then converting that into pK I got .252, butI don't believe this is right
**Is there a specific formula for this, please help!
2.) Enough of a monoprotic acid is dissolved in water to produce a0.0177 M solution. The pH of the resulting solution is 2.32.Calculate the Ka for the acid.
**For Ka I got .56 and then converting that into pK I got .252, butI don't believe this is right
guruborude24Lv6
13 Apr 2023
Trinidad TremblayLv2
28 Sep 2019
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