A student titrates 10.00 milliliters of hydrochloric acid of unknown molarity with 1.000 m naoh. it takes 21.17 milliliters of b
1 answer:
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Explanation:
1. In the first column
<u>INCREASE CONCENTRATION</u>: these are the items that needs to be placed in this bin
a. Add drink mix solid to a diluted mixture of drink mix in pure water
b. Add drink mix solution to a diluted mixture of drink mix in pure water
c. Add drink mix solid to pure drink mix solution
d Evaporate water from a diluted mixture of drink mix in pure water
e Evaporate water from pure drink mix solution
2. The items below are what should be placed in this bin,<u>DECREASE CONCENTRATION:</u>
a. Add water to a diluted mixture of drink mix in pure water
b. Add water to pure drink mix solution
3. These items here should be placed here. <u>DOES NOT AFFECT CONCENTRATION:</u>
a. Add pure drink mix solution to pure drink mix solution
b. Drain the pure drink mix solution
c. Drain the diluted mixture
Answer:
The mass of Mg consumed is 21.42g
Explanation:
The reaction is
As per balanced equation, three moles of Mg will react with one mole of nitrogen to give one mole of magnesium nitride.
as given that mass of nitrogen reacted = 8.33g
So moles of nitrogen reacted =
moles of Mg required = 3 X moles of nitrogen taken = 3X0.2975 = 0.8925mol
Mass of Mg required = moles X molar mass = 0.8925 X 24 = 21.42 g