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200ml of 0.15M H3AsO4 given

200ml of 0.15M H3AsO4 given Ka1=10^-3 Ka2=10^-7 Ka3=10^-12 50ml of 0.6M Na2HAsO4 and 100ml of 0.1M Naish are mixed. pH of
1. 3 answers
2. asked by M.koteswararao
3. 842 views
H3AsO4 reacts with water as follows:H3aso4+h20<=>h2aso4- + h30+ The conjugate base of h3aso4 in this reaction is
1. 1 answer
2. asked by Anonymous
3. 2,960 views
The oxidation of iodide ion by arsenic acid, H3AsO4, is described by the balanced equation3I−(aq)+H3AsO4(aq)+2H+(aq)→
1. 2 answers
2. asked by Joe
3. 2,316 views
The oxidation of iodide ion by arsenic acid, H3AsO4, is described by the balanced equation3I−(aq)+H3AsO4(aq)+2H+(aq)→
1. 1 answer
2. asked by Joe
3. 1,564 views
The oxidation of iodide ions by arsenic acid in acidic aqueous solution occurs according to the net reaction H3AsO4 + 3I – + 2
1. 1 answer
2. asked by Jenna
3. 3,795 views
"Arsenic acid (H3AsO4) is a triprotic acid with Ka1 = 5 10-3, Ka2 = 8 10-8, and Ka3 = 6 10-10. Calculate [H+], [OH ‾ ],
1. 2 answers
2. asked by Clur
3. 1,448 views
Arsenic acid (H3AsO4) is a triprotic acid with Ka1 = 5 10-3, Ka2 = 8 10-8, and Ka3 = 6 10-10. Calculate [H+], [OH -], [H3AsO4],
1. 15 answers
2. asked by Cab
3. 9,858 views
Arsenic acid (H3AsO4) is a triprotic acid with Ka1 = 5 10-3, Ka2 = 8 10-8, and Ka3 = 6 10-10. Calculate [H + ], [OH − ],
1. 1 answer
2. 107 views
Arsenic acid (H3AsO4) is a triprotic acid with Ka1 = 5 ✕ 10-3, Ka2 = 8 ✕ 10-8, and Ka3 = 6 ✕ 10-10. Calculate [H+], [OH
1. 0 answers
2. asked by Damian Clarke
3. 920 views
calculate the 0.4M molarity of ammoniaFrom data given, how to prepare 200ml of 0.4M ammonia solution 25%. From previous study, i
1. 2 answers
2. asked by Merlina_Lyn
3. 1,250 views