Question

6. A student in a lab adds 20.0 mL of 0.150M Al2(SO4)3 solution to 30.0 mL of 0.200M
BaCl2 solution, a precipitate forms.
a. Write a balanced equation for the double replacement reaction that occurs.
(hint: review Ch 7 on Precipitation reactions)
b. What is the formula of the insoluble salt (the precipitate) that forms?
c. Which reactant is the limiting reactant? (Show calculations to support your answer.)
d. How many grams of the precipitate are formed? Molar mass of BaSO4 is 233.4 g/mol
Molar mass of AlCl3 is 133.33 g/mol (hint: you are only calculating grams of 1 of these

Answer 1

Answer on Question #52396 - Chemistry - Other

Question

41.0 g of barium hydroxide, $\mathrm{Ba(OH)_2}$ is dissolved in water. The final volume of the solution is 2.00 L. What is the molarity of the solution? The molar mass of $\mathrm{Ba(OH)_2}$ is 171.3 g/mol.

Answer:

Molarity (molar concentration) of the solution is:

$$C = \frac{n}{V} = \frac{m}{M \cdot V}$$ $$C = \frac{m}{M \cdot V} = \frac{41.0}{171.3 \cdot 2.00} = 0.12 \, \text{mol/L}$$

Answer: 0.12 M

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