While working in a laboratory, you are attempting to minimize the acid-base properties of an unknown solution. In the first step of your experiment, you mix 100.0 mL of 0.250 M NaOH with 250.0 mL of an unknown concentration of HCl solution. You analyze the solution and find that the base is completely neutralized. In the second step of your experiment, you treat the solution leftover from the first step with an excess of aqueous lead (II) nitrate. You observe the formation of 55.62 grams of precipitate. What is the concentration of the original HCl solution? a. If the base is completely neutralized after the first step, what reactant is in excess? Write the chemical formula of the reactant here. b. What is the precipitate that forms in the second step of your experiment? Write the chemical formula of the precipitate here. c. How many moles of excess reactant remains after the first step and before the second step of your experiment? Show your calculation work below and circle the amount of moles. d. What is the concentration of the original HCl solution? Show your calculation work below and circle the concentration. Hint: Draw a picture or diagram to help you visualize what is happening at each step of the experiment. What reactions are occurring at each step? What remains in the system after each step of the experiment?
While working in a laboratory, you are attempting to minimize the acid-base properties of an unknown solution. In the first step of your experiment, you mix 100.0 mL of 0.250 M NaOH with 250.0 mL of an unknown concentration of HCl solution. You analyze the solution and find that the base is completely neutralized. In the second step of your experiment, you treat the solution leftover from the first step with an excess of aqueous lead (II) nitrate. You observe the formation of 55.62 grams of precipitate. What is the concentration of the original HCl solution?
a. If the base is completely neutralized after the first step, what reactant is in excess? Write the chemical formula of the reactant here.
b. What is the precipitate that forms in the second step of your experiment? Write the chemical formula of the precipitate here.
c. How many moles of excess reactant remains after the first step and before the second step of your experiment? Show your calculation work below and circle the amount of moles.
d. What is the concentration of the original HCl solution? Show your calculation work below and circle the concentration. Hint: Draw a picture or diagram to help you visualize what is happening at each step of the experiment. What reactions are occurring at each step? What remains in the system after each step of the experiment?
Trending now
This is a popular solution!
Step by step
Solved in 2 steps with 1 images
