You perform a titration by measuring 23.98 mL of 0.09876 molar HCl and titrate to completion with 31.2 mL of NaOH. What is the molarity of the NaOH?
You perform a titration by measuring 23.98 mL of 0.09876 molar HCl and titrate to completion...
5. In a titration similar to the one you will perform today, it is found that 24.66 mL of 0.1012 M NaOH is required to titrate 0.2524 g of an unknown dicarboxylic acid. What is the molar mass of this unknown dicarboxylic acid?
If you have 50 mL of 0.1255 M HCl and titrate it with 22.15 mL of 0.1466 M NaOH, what is the pH of the solution? If you titrate another 47.21 mL of 0.1466 M NaOH, what is the pH of the new solution?
You titrate 25.0 mL of 0.100 M HCl solution with 0.086 M NaOH. What is the limiting reactant?You titrate 25.0 mL of 0.100 M HCl solution with 0.086 M NaOH. What is the final [H3O+]?You titrate 25.0 mL of 0.100 M HCl solution with 0.086 M NaOH. What is the final pH of the solution?
A titration of 25.00 mL of O.1550 M HCl solution with a solution of NaOH of unknown molarity starts at a buret reading for NaOH of 0.33 mL The phenolphthalein indicator turns light pink the acid solution for over 30 seconds at a buret reading of 24.19 mL 2) What was the volume of HCl you started with? 3) How many moles of HCl were in the original solution? 4) Write the balanced chemical equation for the titration reaction. 5)...
I'm attempting to perform some calculations on a backwards titration. After HCl has completeley reacted with all CO32- in solution, we have excess HCl which we then titrate with NaOH to determine how much carbonate was in solution to begin with. Th process was simulated by adding 2 mL of 3 M HCl to a flask and titration with NaOH. We are to assume all HCl added reacted with carbonate and are to subtract the number of mols H+ consumed...
In a titration experiment, 12.7 mL of an aqueous HCl solution was titrated with 0.6 M NaOH solution. The equivalence point in the titration was reached when 11.1 mL of the NaOH solution was added. What is the molarity of the HCl solution?
In a titration experiment, 12.6 mL of an aqueous HCl solution was titrated with 0.2 M NaOH solution. The equivalence point in the titration was reached when 9.6 mL of the NaOH solution was added. What is the molarity of the HCl solution?
In a titration experiment, 11.4 mL of an aqueous HCl solution was titrated with 0.4 M NaOH solution. The equivalence point in the titration was reached when 13.0 mL of the NaOH solution was added. What is the molarity of the HCl solution?
47 mL of 0.02M of HCl is used to titrate 25mL of Ca(OH)2. a) What is the molarity of the hydrochloric acid? b) What is the molarity of the hydroxide ions in the Ca(OH)2? c) Calculate the solubility product from the titration. Answer needs to be written using Engineering notation, where 3.14 x 10-5 = 3.14E-5.
2. (5 pts) You perform an acid-base titration to standardize an HCl solution by placing 50.00 mL of 0.100M HCI in a flask with a few drops of indicator solution. You put 0.1292 M Ba(OH)2 into the buret, how many mL of the Ba(OH)2 are necessary to titrate the HCI?