A 0.4755-g sample containing (NH,),C,O, and inert materials was dissolved in water and strongly alkaline with KOH, which converted NH,* to NH3. The liberated NH; was distilled into 50.0mL of 0.05035 M H,SO The excess H,SO, was back titrated with 11.13 mL of 0.1214 M NaOH. Calculate the following: A. The % N (14.00 g/mole)

A 0.4755-g sample containing (NH,),C,O, and inert materials was dissolved in water and strongly alkaline with KOH, which converted NH,* to NH3. The liberated NH; was distilled into 50.0mL of 0.05035 M H,SO The excess H,SO, was back titrated with 11.13 mL of 0.1214 M NaOH. Calculate the following: A. The % N (14.00 g/mole)

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter15: Acid-base Equilibria

Section: Chapter Questions

Problem 132IP: A 10.00-g sample of the ionic compound NaA, where A is the anion of a weak acid, was dissolved in...

See similar textbooks

Similar questions

The titration of Na2CO3 with HCl bas the following qualitative profile: a. Identify the major species in solution at points AF. b. Calculate the pH at the halfway points to equivalence, B and D. (Hint: Refer to Exercise 113.)
Two drops of indicator HIn (Ka = 1.0 109), where HIn is yellow and In is blue, are placed in 100.0 mL of 0.10 M HCl. a. What color is the solution initially? b. The solution is titrated with 0.10 M NaOH. At what pH will the color change (yellow to greenish yellow) occur? c. What color will the solution be after 200.0 mL NaOH has been added?
In a titration of cyanide ion, 28.72 mL of 0.0100 M AgNO3 is added before precipitation begins. [The reaction of Ag+ with CN- goes to completion, producing the Ag(CN)2- complex. Precipitation of solid AgCN takes place when excess Ag+ is added to the solution, above the amount needed to complete the formation of Ag(CN)2-. How many grams of NaCN were in the original sample?
Write an overall net ionic equation and calculate K for the reaction where Co(OH)2(Ksp=21016) is dissolved by HCI.
Isocyanic acid (HNCO) can be prepared by heating sodium cyanate in the presence of solid oxalic acid according to the equation 2NaOCN(s)+H2C2O4(s)2HNCO(l)+Na2C2O4(s) Upon isolating pure HNCO(l), an aqueous solution of HNCO can be prepared by dissolving the liquid HNCO in water. What is the pH of a l00.-mL solution of HNCO prepared from the reaction of 10.0 g each of NaOCN and H2C2O4, assuming all of the HNCO produced is dissolved in solution? (Ka of HNCO = 1.2 l04.)
A buffer is prepared in which the ratio [ H2PO4 ]/[ HPO42 ]is 3.0. (a) What is the pH of this buffer? (b) Enough strong acid is added to convert 15% of HPO42- to H2PO4-. What is the pH of the resulting solution? (c) Enough strong base is added to make the pH 7.00. What is the ratio of [H2PO4-] to [HPO42-] at this point?
Without doing detailed calculations, sketch the curve for the titration of 30.0 mL of 0.10 M NaOH with 0.10 M HCl. Indicate the approximate pH at the beginning of the titration and at the equivalence point. What is the total solution volume at the equivalence point?
A bottle of concentrated hydroiodic acid is 57% HI by weight and has a density of 1.70 g/mL. A solution of this strong and corrosive acid is made by adding exactly 10.0 mL to some water and diluting to 250.0 mL. If the information on the label is correct, what volume of 0.988 M NaOH is needed to neutralize the HI solution? Suggest an indicator for the titration.
5. A 25.00-mL portion of a H₂SO4 solution was titrated with a 0.256 M KOH solution. To reach the equivalence point required 31.2 mL of the base. a) Write a chemical equation for the titration. (pai) sling (usindost to ofgez low bocistdo 028 and daw ba b) What was the molarity of the sulfuric acid solution? ods anw red 02),A 1,004 v 20.20 alde tximo Tol ment bonisado od vlasnoor (ans: 0.160 M)
you want to separate Ni2+ and Mn2+ by precipitating the corresponding sulphidesfrom each other. What pH value must you set so that one of the twometals is precipitated quantitatively (concentration in the solution less than/equal to 10/-5 mol/l)is precipitated while the other is still in solution? Ksp (NiS): 10^-21, Kps (MnS): 10~15; Ks (H2S): 10 ~- 20,Saturation concentration of H2S in water: 0.1 mol/l
18a
The magnesium concentration in a water sample was calculated to be 12.0 mg/L. What pH is required to precipitate all but 2.0 mg/L of Mg2+ concentration? The pKs is 11.25 and the reaction is