Asked by Asterix
50.0 mL of 0.185M Sr(OH)2 is reacted with 35.0 mL of a solution containing 0.120g of HCl. Calculate the pOH resulting from the mixture. Then suggest an indicator that will be effective for this incomplete titration and explain your choice.
Answers
Answered by
DrBob222
......................Sr(OH)2 + 2HCl ==> SrCl2 + 2H2O
millimoles Sr(OH)2 = mL x M = 50.0 x 0.185 = 92.5
millimoles HCl = don't know. The solution contains 0.120 g HCl in a solution and you take 35.0 mL of that solution but if you don't show the volume then we don't know how much of the 0.120 g was transferred.
millimoles Sr(OH)2 = mL x M = 50.0 x 0.185 = 92.5
millimoles HCl = don't know. The solution contains 0.120 g HCl in a solution and you take 35.0 mL of that solution but if you don't show the volume then we don't know how much of the 0.120 g was transferred.
There are no AI answers yet. The ability to request AI answers is coming soon!
Submit Your Answer
We prioritize human answers over AI answers.
If you are human, and you can answer this question, please submit your answer.