Here are the steps I have done, and my written results. The questions I need aid

Question

Here are the steps I have done, and my written results. The questions I need aid with are at the bottom of this post.

Calculate how much NaOH solution should be needed to exactly neutralize the acid solution (write the balanced equation between NaOH and HCl and use stoichiometry to find the volume of NaOH needed to react with all the HCl).

Then sketch a verticel line corresponding to the volume of NaOH solution on your graph - where does it meet the titration curve?

Part A: Getting to Know Titrations Plotting a Titration Curve l. During this (800 ml or 1 as a waste receptacle. Pour all experiment, use a large beaker aste solutions into this flask as you proceed. At the end of the lab session, pour this waste into the special waste container provided by the instructor (let the instructor know if the container is too full 2. obtain about 40 mL of standardized HCl solution (provided) in a 100 mL beaker. Use a conditioned 25.00 mL volumetric pipet to quantitatively transfer an aliquot of the HCl solution into a 250 mL beaker (write down the HCl molarity in your lab notebook) 3. Use a graduated cylinder to add 50.0 mL of DI water to the beaker. Carefully slide a magnetic stir bar into the beaker so that no reagent splashes out 4. Place the beaker on a magnetic stir plate and dip the pH electrode into the solution (after rinsing with DI water and blotting dry). Turn the stir plate on slowly, so that no splashing occurs and no air is being drawn into the solution. After this point, do not remove the electrode from the solution until you have finished the titration and do not add any more water (except for a small amount used to rinse down the inside of the beaker) 5. Set up a buret (follow correct procedures make sure there is no air bubble in the buret tip) and fill with standardized NaOH (get about 100 mL of NaOH from the container using a 150 mL beaker, and write the actual NaOH molarity in your lab notebook). Your initial reading should be between 0.00 mL and 2.00 mL. Read and record the actual starting point to the nearest 0.02 mL (split the space between markings into 5, use a card to help see the meniscus, and remember to read from the bottom of the meniscus If your buret readings are not recorded to the nearest 0.02 mL, you will lose points 6. Record the initial pH and buret readings 7. Add approximately 45 mL of NaOH solution in-1 mL increments. Record the buret reading and pH after each addition of the base 8. Sketch a graph in your lab notebook showing volume of NaOH solution added (x-axis) and mixture pH (y-axis). Note: a "sketched" graph should include a title, labeled axes, and a hand-drawn line showing the approximate shape of the curve. Do not precisely plot every data point

Explanation / Answer

The balanced reaction is as shown below:

HCl + NaOH ----> NaCl + H2O

.Since the reactants react in a 1:1 molar ratio, at the exact neutralization point the moles of acid and base are equal.

Using the relation:

Macid*Vacid = Mbase*Vbase

0.1006*(40 mL) = 0.1269*('x' mL)

Solving we get:

x = 31.71 mL

Revert back if you have any queries.

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