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.

......................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.

Did you know?

Did you know that pOH is a measure of the hydroxide ion concentration in a solution? In this given scenario, 50.0 mL of 0.185M Sr(OH)2 is reacted with 35.0 mL of a solution containing 0.120g of HCl. By performing the necessary calculations, you can determine the pOH resulting from this mixture. Now, let's move on! When choosing an indicator for an incomplete titration like this, it is crucial to select one that undergoes a color change in a pH range close to the equivalence point, where the reaction is nearly complete. In this case, the equivalence point occurs when all of the hydroxide ions in Sr(OH)2 react with the available HCl. Considering this, a suitable indicator for this incomplete titration would be phenolphthalein. Phenolphthalein transitions from colorless to pink around a pH of 8.2 to 10.0, which is close to the pH range near the equivalence point. This range ensures that the indicator remains colorless until the reaction is almost complete, and then undergoes a clear color change as the hydroxide ions are neutralized.