Write out what data and information you plan to collect during the experiment of identification of a weak diprotic acid using titration to answer how can a weak diprotic acid be identified when titrated with a strong base?Then list the equations and formulas you plan to use to manipulate that data.Also list how many trials you plan to do? If it's just one or more?

) In a titration involving sodium hydroxide and hydrochloric acid, if significantly less acid were added to the reaction flask than what was called for, what affect would this have on the accuracy of the concentration of the reactants?   A) The sodium hydroxide would have a decreased concentration. B) The sodium hydroxide would have an increased concentration. C) The hydrochloric acid would have a decreased concentration. D) The hydrochloric acid would have an increased concentration. E) There would be no affect on the concentration of either reactant.

Can you confidently dtermine if the molarities are precise? Explain why or why not.

Please type this, do not write it on a paper.

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I need help with 1a, 1c, 2c

Part C – Acid–base and solubility equilibria 1. Rinse 4 regular size test tubes and a 10 mL measuring cylinder thoroughly with water. Number the test-tubes from 1 to 4 in a test tube rack. 2. Into each of test tubes 1 – 3 put a small amount of solid benzoic acid (put the same amount – about the size of a pea – in each test tube). 3. Add 2 mL (use the measuring cylinder) of water to tube 1 and shake to mix the contents. 4. Add 2 mL (measuring cylinder) of 2 M HNO3 to tube 2 and shake to mix the contents. 5. Rinse the measuring cylinder with water, then use it to add 2 mL of 2 M NaOH to tube 3 and shake for about 10 seconds to mix the contents. Rinse the measuring cylinder. 6. Pour about half of the solution from tube 3 into tube 4, than add 2 mL of 2 M HNO3 to tube 4. 7. Allow the test tubes to stand for 2 or 3 minutes then record the appearance of the mixtures in each test tube. 8. Answer the questions on the results page relating to this equilibrium system.

Answer both questions regarding Acids and Bases. After adding 50 mL of NaOH solution, the sample in the flask still had not turned pink. What error did the student make? and then, compare your percentage of HCI to the manufacturer’s percentage for the toilet bowl cleaner. We’re your results close? What might account for any differences? (Use the second photo for reference)

1. Obtain the actual molarity of the HCI solUlUII ITUII Include in your formal lab report this value and possible sources of error for your experiment. 2. Why is it important that the color change occurs by the addition of a single drop? Explain in terms of its effect on the calculated molarity of the acid. 3. Why is an Erlenmeyer flask preferred over a beaker when performing a titration? 4. Suppose calcium hydroxide was used in this experiment instead of sodium hydroxide. Assuming all experimental data was the same, what would be the molarity of the acid? Explain. 5. Suppose there was a large air bubble in the tip of the acid burette during the titration and it was dislodged toward the end of your titration. Explain the effect that this would have on the calculated value of the acid's molarity. 6. A student titrated 30.00 mL of a hydrochloric acid solution with 1.00 M sodium hydroxide. The sodium hydroxide was initially filled to the 2.30 mL mark on the burette. Once the level in the…

When you calculate the unknown concentration of an acid based upon your titration, you determine that it is too high compared to the actual value disclosed to you by the professor. What went wrong during your titration?