To draw the deformation curve resulting from 10 mL of 0.1 normal sodium hydroxide with 0.1 normal hydrochloric acid at the following points: 1- Before the start of deformation. b- Halfway to the equivalence pH point. C-at the equivalence point. D-After adding 1 ml of the acid after the equivalence point. The values of the will be as follows 13. 12.5.7.1.2 O13-12.5.7.2.3 13.9.2.7-23

To draw the deformation curve resulting from 10 mL of 0.1 normal sodium hydroxide with 0.1 normal hydrochloric acid at the following points: 1- Before the start of deformation. b- Halfway to the equivalence pH point. C-at the equivalence point. D-After adding 1 ml of the acid after the equivalence point. The values of the will be as follows 13. 12.5.7.1.2 O13-12.5.7.2.3 13.9.2.7-23

Appl Of Ms Excel In Analytical Chemistry

2nd Edition

ISBN:9781285686691

Author:Crouch

Publisher:Crouch

Chapter9: Complexometric And Precipitation Titrations

Section: Chapter Questions

Problem 16P

See similar textbooks

Similar questions

in a container with HCl solution with volume 400 ml and pH = 1, add the salt of PbCl2. Calculate how many grams of PbCl2 can be dissolved in this container, when we know that Kpt of PbCl2 = 1.6 × 10-⁵?
It is necessary to prepare 0.100 liters of buffer pH 4.70 with a concentration of 0.250 M, from a solution of acetic acid at 55.0% m/m (density = 1.010 g/mL) and sodium acetate of purity 97.0 %, how many g of salt do I need? (Ka = 1.78 x 10-5) (Note significant figures).
Determine the [H3O+] of the eight buffer solutions made by mixing 1.10 M acetic acid and 0.900 M sodium acetate solutions according to the following volumes. The pKa for acetic acid, CH3CO2H (HAc), is 4.745. To enter exponential values, use the format 1.0e-5.
calculations for acetate buffer solutions 1. moles of sodium acetate in in 250.0 mL acetate buffer (below is the data to answer the answer) Deionized water Acetate Buffer Ammonia Buffer pH of solution 6.62 4.59 9.49 Ph of solution after addition of 1 mL of 0.6 M NaOH 12.41 4.71 9.50 pH of solution after addition of 1 mL of 0.6 M HCl 1.38 3.87 9.24 Preparation of Buffer solutions Mass of sodium acetate in acetate buffer ~ 1.1981 Volume of 3.0 M acetic acid in acetate buffrer ~ 3.81 Mass of ammonium chloride ~ 1.2721 Volume of 5.0 M NH4OH ~ 6.00
A titration system is set up as follows: the bottom flask contains a sample solution of 50.0-mL 0.50 M C2H3NH2 (ethylamine), the burette is filled with 0.20 M HCl as titrant. Kb of C2H3NH2 = 6.5 ´ 10-4 What is the initial pH of above sample solution before titration starts?
A 25.00-mL sample of vinegar is diluted with deionized to 100.0 mL. Then a 10.00-mL aliquot (portion) of the dilute vinegar solutionis titrated with 0.1055MNaOHsolution using phenolphthalein as theindicator. (a) If 19.60mL of the base solution is required to reach the end-point, calculate the molar concentration of acetic in dilute vinegar solution. (b) What is the molar concentration of acetic acid in the original (undiluted) vinegar? At the end-point, the volume of NaOH consumed was found to be 32.00 mL. The acid-base reaction occurs as follows: HC2H3O2(aq) + NaOH(aq) --> H2O(l) + NaC2H3O2(aq)
Consider a 0.10 M solution of a weak polyprotic acid (H2A) with the possible values of Ka1 and Ka2 given here.a. Ka1 = 1.0 * 10-4; Ka2 = 5.0 * 10-5b. Ka1 = 1.0 * 10-4; Ka2 = 1.0 * 10-5c. Ka1 = 1.0 * 10-4; Ka2 = 1.0 * 10-6Calculate the contributions to [H3O+] from each ionization step. At what point can the contribution of the second step be neglected?
A 4.0520g sample of HCl, specific Gravity 11.18, required 44.15ml of 0.9035M of Sodium Hydroxide in titration, compute for percent purity. Please explain thoroughly. I have an answer of more than 100% concentration and I'm not sure I just want to double check. Thank you and have a great day.
Please answer it ALL ASAP and CORRECTLY for an upvote. PROVIDE YOUR FULL SOLUTION. You prepared a buffer solution by mixing 68 ml of 0.17 M ammonia and 42 ml of 0.13 M ammonium chloride. The dissociation constant of ammonia is 1.8x10^-5 What is the total volume of the buffer? What is the final concentration of the base? What is the final concentration of the salt? What is the acid strength of the solution? What is the pH of the buffer solution?
Please calculate the pH of a buffer solution made up of citric acid and potassium citrate. The solution was made by dissolving 0.800 mol of sodium citrate, and 0.800 mol of citric acid in 1.5 liters of water. (Please assume the total volume of the solution is also 1.5 L) (The Ka for this system = 7.41 x 10-4) (Please answer with 3 sig. figs.)
A mixture of HCl and H3PO4 is titrated with 0.100 M NaOH. The first end point (methyl red) occurs at 35.00 mL, and the second end point (bromthymol blue) occurs at a total of 50.00 mL (15.00 mL after the first end point). Calculate the millimoles HCl and H3PO4 present in the solution.
A titration system is set up as follows: the bottom flask contains a sample solution of 50.0-mL 0.50 M C2H3NH2(ethylamine), the burette is filled with 0.20 M HCl as titrant. Kb of C2H3NH2 = 6.5 ´ 10-4 what is the pH at the equivalent point?