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Ch.4 - Reactions in Aqueous Solution

Chapter 4, Problem 60b

You make 1.000 L of an aqueous solution that contains 35.0 g of sucrose (C12H22O11). (b) How many liters of water would you have to add to this solution to reduce the molarity you calculated in part (a) by a factor of two?

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Hi everyone here we have a question telling us that a student prepared an acquis glucose solution by dissolving 9.50 g of glucose and ml of water. Calculate the polarity of the prepared solution if the student wishes to obtain a solution that has one third the concentration of the original solution, calculate how much water she should add to the original solution. So it's important information. The molar mass of glucose is 180 0. grams per mole. Now we want to calculate our polarity and polarity is in moles per leader. So we're going to start off with our 9.50 g of glucose over milliliters of solution times one more of glucose over .16 g of glucose times one middle leader of solution over 10 To the negative 3rd leaders of solution. So our grams are canceling out and our milliliters of solution are canceling out, leaving us with moles over leaders which is what we wanted. And that equals 0.117 moller so that is the answer to the first part. And now moving on to the second part. We want three times dilution. So 0.117 molar divided by three equal zero point 0390 More. And now we're going to use the formula 1st Polarity Times 1st vol equal second polarity times second volume. And we want our second volume. So to isolate that Our 2nd volume is going to equal the first volume time. The first polarity times the first volume over the second polarity. And now plugging in what we know V two equals 0 .117 Moller Times 450 ml over 0. ml. And that equals 1350 ml. And now we want to take our And subtract what we originally had, so -450 ml because this is our volume added. And that's going to equal 900 ml. And that is our final answer for the second part. Thank you for watching. Bye.