1) Suppose that, instead of using NaOH, a base such as Ba(OH)2 had been used. What changes in the calculations would then have to be done to determine the molar concentrations of the base? Answer this question in words, and illustrate your answer by calculating molarity from the following data: mol KHP used 0.040 mol Ba(OH)2 Initial buret level = 0.020 mL Final buret level 36.70 mL

1) Suppose that, instead of using NaOH, a base such as Ba(OH)2 had been used. What changes in the calculations would then have to be done to determine the molar concentrations of the base? Answer this question in words, and illustrate your answer by calculating molarity from the following data: mol KHP used 0.040 mol Ba(OH)2 Initial buret level = 0.020 mL Final buret level 36.70 mL

Chemistry: Principles and Reactions

8th Edition

ISBN:9781305079373

Author:William L. Masterton, Cecile N. Hurley

Publisher:William L. Masterton, Cecile N. Hurley

Chapter14: Equilibria In Acid-base Solutions

Section: Chapter Questions

Problem 37QAP: Given three acid-base indicatorsâ€”methyl orange (end point at pH 4), bromthymol blue (end point at...

See similar textbooks

Similar questions

If 350.0 mL of 0.450 M Ca(OH)2 are added to 380.0 mL of 0.550 M HCl. Ca(OH)2 + 2HCl → CaCl2 + 2H2O i. Will the resulting mixture be acidic or basic? Defend your answer by providing the number of moles of HCl or Ca(OH)2 that are left over in solution. Report your answer to 3 significant figures and don’t forget units. ii. Calculate the [H+] or [OH-]of the resulting solution, depending on which one is left over. Report your answer to 3 significant figures and don’t forget units. (Assume total volume of solution = volume of acid + base) iii. Find the pH of the resulting solution. Report your answer to 2 decimal places. *Add your answers to the section below i. The solution will be ________________ and the amount of moles left over is ___________ (remember to indicate HCl or Ca(OH)2) ii. The concentration of [H+] or [OH-] in solution is__________ (remove the [ ] that does not apply)
In the determination of the water hardness of a river water sample, the pH of the sample was adjusted to 12 instead of 10. Is there a positive error, negative error, no effect, or error could not be determined In terms of the ppm CaCO3 of sample?
A student prepared two solutions: 1 @ (water + cabbage extract) and 1 @ (buffet + cabbage extract). The student adjusted the solutions to pH = 7 but forgot to label each of them so both were indistinguishable. The student decided to test one of the two solutions and split the solution into two beakers: Sol1 and Sol2. The student was really struggling that day and forgot to label the HCL and the NaOH solutions. Continuing with the experiment, the student added SolA into Sol1 and the color turned light red. What is the identity of SolA? What will the color of Sol2 be after SolB is added? What must the initial solution contain?
This is a dilution lab of acetic acid. There is 1.0M acetic acid with ph of 2.297, 0.1M acetic acid with ph of 2.69897, and 0.01M acetic acid with ph of 3.69897. They were all filled up to 50ml in a volumetric flask. How do you build the ICE table for the different concentrations?I have attached some images for extra information if needed.
it is time for the titration. You measure 15.0 mL of the H2C2O4 solution with a 100-mL graduated cylinder and add it to a 125-mL Erlenmeyer flask. Then you add two drops of the indicator, phenolphthalein, to the oxalic acid solution in the flask. You dispense the NaOH solution from the buret into the flask (while swirling the flask) until you reach the endpoint. At the endpoint, the solution in the flask turns light pink. You repeat the titration two additional times for a total of three trials. H2C2O4 (aq) + 2 NaOH (aq) --> Na2C2O4 (aq) + 2 H2O (l) (I) (II) (III) Volume of H2C2O4 used 15.00 mL 15.00 mL 15.00 mL Initial Buret Reading 0.00 mL 0.05 mL 0.10 mL Final Buret Reading 14.45 mL 14.38 mL 15.40 mL what Volume of NaOH is used ?
it is time for the titration. You measure 15.0 mL of the H2C2O4 solution with a 100-mL graduated cylinder and add it to a 125-mL Erlenmeyer flask. Then you add two drops of the indicator, phenolphthalein, to the oxalic acid solution in the flask. You dispense the NaOH solution from the buret into the flask (while swirling the flask) until you reach the endpoint. At the endpoint, the solution in the flask turns light pink. You repeat the titration two additional times for a total of three trials. H2C2O4 (aq) + 2 NaOH (aq) --> Na2C2O4 (aq) + 2 H2O (l) (I) (II) (III) Volume of H2C2O4 used 15.00 mL 15.00 mL 15.00 mL Initial Buret Reading 0.00 mL 0.05 mL 0.10 mL Final Buret Reading 14.45 mL 14.38 mL 15.40 mL Volume NaOH used ________mL ________mL ______mL Moles NaOH _______M ________M _________M…
How many mls of 1 M NaOH titront are needed to react with 5 mls of 0.1 KHT? (Use the ml*M/ coefficient= ml*m/coefficient formula to solve this problem)
In Experiment 4, we used titration to determine the total acid content of samples, which we reported in terms of molarity. Reporting acidity through pH measurements is quite different, in that we can only measure the amount of the acid in its ionized form. You were tasked to investigate a clear aqueous solution of an unknown monoprotic acid. You decided to use two Chem 16.1 methods to gather data.Method 1 – TITRATION: A 10. mL aliquot of the sample was diluted with 25 mL distilled water. Two drops of phenolphthalein were added and then it was titrated 3.54 mL of 0.048 M standardized NaOH to the endpoint.Method 2 – pH STRIP: You took 1 mL of the sample and used a pH strip to estimate the pH, which turned out to be around 3.3. Another 1 mL of the sample was diluted with 9 mL of water. The pH was taken again and is now around 3.8 a) Calculate the molarity of the acid using the titration data.b) If we assume that the titrated unknown is a strong acid, predict the pH of the sample.c) Using…
In Experiment 4, we used titration to determine the total acid content of samples, which we reported in terms of molarity. Reporting acidity through pH measurements is quite different, in that we can only measure the amount of the acid in its ionized form. You were tasked to investigate a clear aqueous solution of an unknown monoprotic acid. You decided to use two Chem 16.1 methods to gather data.Method 1 – TITRATION: A 10. mL aliquot of the sample was diluted with 25 mL distilled water. Two drops of phenolphthalein were added and then it was titrated 3.54 mL of 0.048 M standardized NaOH to the endpoint.Method 2 – pH STRIP: You took 1 mL of the sample and used a pH strip to estimate the pH, which turned out to be around 3.3. Another 1 mL of the sample was diluted with 9 mL of water. The pH was taken again and is now around 3.8 d) Based on your answer in a) and c), do you think the unknown is really a strong acid or is it a weak acid instead? Defend your answer in one sentence.e)…
Suppose you add 20 drops of 0.2M NaOH to 17 drops of 0.2M HCl. Phenolphthalein has been added to the HCl. What color do you suspect the resulting solution will be? Why? I think that I need to find the pH, because phenolphthalein turns pink at pHs 7-10, and NaOH is a base and HCl is an acid.
You mix 50.0 mL of 0.250 M CH3COOH with 1.00 mL of 0.500 M NaOH. Calculate the pH of the mixture. The total volume is 51.0 mL. Use two stages method to solve this problem (I. stoichiometric reaction between acid and base, II. Acid-Base Equilibrium, ICE). Ka of CH3COOH = 1.8 x 10-5.
Need help filling this out. It is the Data Sheet for Ch. 2 Qualitative Analysis. Very much appreciated!