Question
What is the freezing point of each solution?
a)1.40mol Na2SO4 in 1750 g H2O
Are these the right steps?
1.40mol Na2SO4 / 1.75kg = .8m
3 * 1.86 degrees C * .8m = 4.46 degrees C
4.46 degrees C - 1.86 degrees C = 2.6 degrees C
a)1.40mol Na2SO4 in 1750 g H2O
Are these the right steps?
1.40mol Na2SO4 / 1.75kg = .8m
3 * 1.86 degrees C * .8m = 4.46 degrees C
4.46 degrees C - 1.86 degrees C = 2.6 degrees C
Answers
DrBob222
a)1.40mol Na2SO4 in 1750 g H2O
Are these the right steps?
1.40mol Na2SO4 / 1.75kg = .8m
3 * 1.86 degrees C * .8m = 4.46 degrees C
<b>OK to here. The next step is wrong.</b>
4.46 degrees C - 1.86 degrees C = 2.6 degrees C
<b>Why is it wrong? The normal freezing point of water is zero C; therefore, the freezing point of this solution is 4.46 degrees lower than that OR 0-4.46 = -4.46<sup>o</sup> C. </b>
Are these the right steps?
1.40mol Na2SO4 / 1.75kg = .8m
3 * 1.86 degrees C * .8m = 4.46 degrees C
<b>OK to here. The next step is wrong.</b>
4.46 degrees C - 1.86 degrees C = 2.6 degrees C
<b>Why is it wrong? The normal freezing point of water is zero C; therefore, the freezing point of this solution is 4.46 degrees lower than that OR 0-4.46 = -4.46<sup>o</sup> C. </b>