Is equal to number of moles, number of moles, of solute per liters of solution, liters of solution. Our original solution, of our one-molar solution,ĭo we need to take out to have that many moles? And to think about how many moles, we just have to remind On how we visualize it? And then, how much of Goal solution, this one or this one, depending We just have to figure out how many moles of sodium sulfate need to be in this final We can then dilute with water to get to our goal solution? Well, to answer that question, Is, is how much of this do we have to put in, which This up to 500 milliliters, that we would then haveĪ 0.125-molar solution. Sufficient number of moles of sodium sulfate that, if we were to then fill Less than 500 milliliters of our original solution, So our intuition would tell us is that we're going to take Pause this video and think about how you would approach that. We want 500 milliliters of this new solution. So we want to createĪ 0.125-molar solution of sodium sulfate, and Is create a solution, another aqueous solutionĭifferent concentration, in this case, one that And let's say we also haveĪs much water as we need, and what we want to do Of sodium sulfate, and it's an aqueous solution. That's quite important, known as dilutions. Video, we're gonna talk about a concept in chemistry
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