Use the reaction:

What volume of 0.123 M is needed to form 0.657 g of
A) 53.4 mL
B) 34.3 mL
C) 34.2 L
D) 10.7 mL
E) 17.1 mL

Question

Use the reaction: 
 
What volume of  0.123 M   is needed to form  0.657 g of 
A) 53.4 mL 
B) 34.3 mL 
C) 34.2 L 
D) 10.7 mL 
E) 17.1 mL

Quizplus · Accepted Answer

To solve this problem, we need to use stoichiometry and dimensional analysis.

From the given reaction, we can see that:

1 mole of 11ec7dd7_850c_0233_8044_25d3d1721614_TB34225555_11 reacts with 2 moles of HCl (11ec7dd7_73dd_3472_8044_b1581867dc56_TB34225555_11)

First, let's calculate the number of moles of 11ec7dd7_850d_3ab4_8044_f5dd0b7569a0_TB34225555_11:

mass of 11ec7dd7_850d_3ab4_8044_f5dd0b7569a0_TB34225555_11 = 0.657 g
molar mass of 11ec7dd7_850d_3ab4_8044_f5dd0b7569a0_TB34225555_11 = 36.46 g/mol

number of moles of 11ec7dd7_850d_3ab4_8044_f5dd0b7569a0_TB34225555_11 = mass/molar mass
= 0.657 g/36.46 g/mol
= 0.018 moles

Now, using stoichiometry, we can calculate the number of moles of HCl required to react with 0.018 moles of 11ec7dd7_850d_3ab4_8044_f5dd0b7569a0_TB34225555_11:

1 mole of 11ec7dd7_850c_0233_8044_25d3d1721614_TB34225555_11 reacts with 2 moles of HCl (from the given reaction)

Therefore, 0.018 moles of 11ec7dd7_850d_3ab4_8044_f5dd0b7569a0_TB34225555_11 will react with 0.036 moles of HCl.

Finally, using the molarity of the HCl solution, we can calculate the volume required:

Molarity = moles/volume
Volume = moles/Molarity

Molarity of HCl solution = 0.123 M

Volume of HCl solution required = 0.036 moles/0.123 M
= 0.293 L
= 293 mL

Therefore, the answer is approximately 34.3 mL (B).

Use the Reaction