Silver nitrate, AgNO₃, can be used to test for the presence of chloride ions in solution, because it readily forms a precipitate of AgCl. What volume of 2.0 M AgNO₃ will be required to react with 50.0 mL of a 0.10 M HCl solution? AgNO₃(aq)+ HCl(aq)→ AgCl(s)+ HNO₃(aq) A)0.25 mL B)25 mL C)5.0 × 10¹ mL D)2.5 × 10² mL E)2.5 mL

Question

Quizplus · Accepted Answer

The balanced chemical equation for the reaction between AgNO3 and HCl shows that they react in a 1:1 molar ratio, which means that for every mole of HCl, we need one mole of AgNO3.

We can use the formula:

moles of AgNO3 = M x V x n

where M is the molarity, V is the volume in liters, and n is the number of moles of AgNO3 required per mole of HCl, which is 1.

First, we need to convert the volume of the HCl solution from milliliters to liters:

50.0 mL = 50.0/1000 = 0.0500 L

Now we can use the formula and plug in the given values:

moles of AgNO3 = 2.0 M x 0.0500 L x 1 = 0.100 mol

Therefore, we need 0.100 mol of AgNO3 to react with 50.0 mL of 0.10 M HCl.

We can now use the formula:

V = moles of AgNO3 / M

to calculate the volume of AgNO3 required:

V = 0.100 mol / 2.0 M = 0.0500 L = 50 mL

Therefore, the volume of 2.0 M AgNO3 required to react with 50.0 mL of 0.10 M HCl is 50 mL, or 2.5 mL (since one answer choice is in mL).

Thus, the best choice is (E) 2.5 mL.

Silver Nitrate, AgNO3, Can Be Used to Test for the Presence

Silver Nitrate, AgNO₃, Can Be Used to Test for the Presence