Aqueous sulfuric acid (H2SO4) reacts with solid sodium...

Aqueous sulfuric acid ($H_2SO_4$) reacts with solid sodium hydroxide ($NaOH$) to produce aqueous sodium sulfate ($Na_2SO_4$) and liquid water ($H_2O$). If 3.12 g of sodium sulfate is produced from the reaction of 3.9 g of sulfuric acid and 2.2 g of sodium hydroxide, calculate the percent yield of sodium sulfate. Be sure your answer has the correct number of significant digits in it.

Transcript

00:01 For this question, we have a reaction between sulfuric acid and sodium hydroxide to produce sodium sulfate and water.

00:06 We want to know if 1 .58 grams of sodium sulfate was actually produced in a lab, what is the percent yield? so what we're going to do is we're going to determine the theoretical yield, and we were given the starting amounts of both reactants, so one of them is going to be limiting.

00:20 But we'll determine the theoretical yields, and then we'll be able to calculate the percent yield.

00:24 First thing we have to do, though, is balance the reaction.

00:27 We were given the formulas for the reactants in the products.

00:29 I already have those written out.

00:32 Because we're converting between substances, we're going to need a multiple ratio, and that comes from a balanced chemical reaction.

00:38 So we have to balance this first.

00:40 To do that, we're going to put a two in front of sodium hydroxide and then a two in front of water.

00:45 And at this point, it's balanced.

00:48 So now we're going to start converting from each of our reactants to our product of sodium sulfate.

00:55 So starting out, we've got 3 .9 grams of sulfuric acid.

01:02 In order to convert between substances, we have to be in moles.

01:05 So we're going to use sulfuric acid's molar mass to get to moles.

01:09 So we'll have one mole on top, and then we'll have its molar mass on the bottom, which is 98 .08 grams.

01:20 Now that we're in moles, we can convert between substances.

01:23 And so we're going to use a mole ratio.

01:25 And this just comes from the balanced chemical reaction and the coefficients for each compound we're looking at.

01:30 So we're going to have one mole of sodium sulfate on top.

01:34 And then one mole of sulfuric acid on the bottom.

01:40 And then lastly, we're going to use sodium sulfate's molar mass to get to grams.

01:45 So we'll have 142 .04 grams of sodium sulfate on top and one mole on the bottom.

01:59 One multiply everything across the top and then divide by the things on the bottom and we're going to get 5 .6 grams of sodium sulfate.

02:06 So this is our first possible answer.

02:08 We're going to get two answers...

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