please help me with both. I keep getting it wrong (References]This question has multiple parts. Work all the parts to get the most polnts.You require 34.54 mL of 0.0105 M HCl to reach the equivalence point in the titration of 25.0 mL of aqueous ammonia.a What was the concentration of NH, in the original ammonia solution?Concentration = 0.0145b What are the concentrations of H3Ot, OH, and NH,t at the equivalence point?K, (NH,+) = 5.6 x 10 10M.[OH ] =M[NH, | =Submit[References]This questlon has multIple parts. Work all the parts to get the most polnts.The pH of a solution of Ba(OH)2 is 10.77 at 25 °C.a What is the hydroxide ion concentration in the solution?[OH] = 5.88x10^4b If the solution volume is 212 mL, what mass of Ba(OH)2 must have been dissolved?Mass =Submit

Given as 34.54 mL of 0.0105 M HCl is required to reach the equivalence point in the titration of…

This question has multlple parts. Work all the parts to get "ou require 34.54 mL of 0.0105 M HCl to reach the equivalence point in the titration of 25.0 mL of aqueous ammo a What was the concentration of NH3 in the original ammonia solution? Concentration = 0.0145

This question has multlple parts. Work all the parts to get "ou require 34.54 mL of 0.0105 M HCl to reach the equivalence point in the titration of 25.0 mL of aqueous ammo a What was the concentration of NH3 in the original ammonia solution? Concentration = 0.0145

Introductory Chemistry For Today

8th Edition

ISBN:9781285644561

Author:Seager

Publisher:Seager

Chapter9: Acids, Bases, And Salts

Section: Chapter Questions

Problem 9.99E

See similar textbooks

Similar questions

An acid is titrated with NaOH. The following beakers are illustrations of the contents of the beaker at various times during the titration. These are presented out of order. Note: Counter-ions and water molecules have been omitted from the illustrations for clarity. (a) (b) (c) (d) (e) a. Is the acid a weak or strong acid? How can you tell? b. Arrange the beakers in order of what the contents would look like as the titration progresses. c. For which beaker would pH = pKa? Explain your answer. d. Which beaker represents the equivalence point of the titration? Explain your answer. e. For which beaker would the Ka value for the acid not be necessary to determine the pH? Explain your answer.
One half liter (500. mL) of 2.50 M HCl is mixed with 250. mL of 3.75 M HCl. Assuming the total solution volume after mixing is 750. mL, what is the concentration of hydrochloric acid in the resulting solution? What is its pH?
Consider the following two acids: In two separate experiments the pH was measured during the titration of 5.00 mmol of each acid with 0.200 M NaOH. Each experiment showed only one stoichiometric point when the data were plotted. In one experiment the stoichiometric point was at 25.00 mL added NaOH, and in the other experiment the stoichiometric point was at 50.00 mL NaOH. Explain these results. (See Exercise 113.)
Consider the nanoscale-level representations for Question 111 of the titration of the aqueous strong acid HA with aqueous NaOH, the titrant. Water molecules and Na+ ions are omitted for clarity. Which diagram corresponds to the situation: (a) After a very small volume of titrant has been added to the initial HA solution? (b) Halfway to the equivalence point? (c) When enough titrant has been added to take the solution just past the equivalence point? (d) At the equivalence point? Nanoscale representations for Question 111.
A 5.36-g sample of NH4Cl was added to 25.0 mL of 1.00 M NaOH and the resulting solution diluted to 0.100 L.. (a) What is the pH of this buffer solution?. (b) Is the solution acidic or basic?. (c) What is the pH of a solution that results when 3.00 mL of 0.034 M HCl is added to the solution?
The equivalence point for the titration of a 25.00-mL sample of CSOH solution with 0.1062 M HNO3 is at 35.27 mL. What is the concentration of the CsOH solution?
A solution is prepared by dissolving 10.8 g ammonium sulfate in enough water to make 100.0 mL of stock solution. A 10.00- mL sample of this stock solution is added to 50.00 mL of water. Calculate the concentration of ammonium ions and sulfate ions in the final solution.
The titration below was performed by placing 10.00 mL solution in an Erlenmeyer flask and titrating it with 0.1000 M HCl. What is the concentration of the solution being titrated? 0.02500 M 0.0500 M 0.0750 M 0.100 M 0.200 M
In the second titration, the molar mass of an unknown monoprotic acid is calculated. If 0.100 grams of unknown solid are dissolved in water and titrated with 4.68 mL of the NaOH, what is the molar mass of the solid? HINTS: Molar mass is grams / moles. We have grams from the weighed mass, we can calculate moles of acid from the titration. Monoprotic means that it produces 1 H+ per molecule. This means that our moles of NaOH added and moles of acid are the same. You will need to use your concentration of NaOH from the previous question
MnO4 (aq) + H2O2 (aq) → Mn2+ (aq) + O2 (g) (a) Sketch a flask containing an analyte solution before any potassium permanganate KMnO4 is added, list out all species present. (b) Once a stoichiometric amount of permanganate ion is added to the analyte solution (the equivalence point of the titration!), sketch the beaker with all the species remaining after the reaction goes to completion. (c) Sketch the flask one more time, past the equivalence point. How do you know when you have passed the equivalence point?
During the titration of an HClO4 solution with 0.10320 M NaOH, a student, Lovely became distracted and overshot the endpoint. A fellow student Ashley suggested that he should record the present volume of NaOH added and titrate the excess with a standard acid solution. If the original sample volume was 25.000 mL, the volume of NaOH added was 28.060 mL. It took 3.4700 mL of 0.10940 M HCl to back-titrate the NaOH and calculate the molar concentration of the original HClO4
In this experiment, you will determine the amount (percent) of potassium hydrogen phthalate (KHP) that is in an impure sample. You will determine the percent of KHP via titration using NaOH with known molarity. The reaction will follow, KHC8H4O4 (aq) + NaOH (aq) ---------> KNaC8H4O4 (aq) + H2O (l) At the endpoint, the moles of KHP will equal the moles of NaOH. You will use phenolphthalein as the indicator. The endpoint of the reaction will be a light pink solution color. How will you know the reaction is over? About how much KHP will be used in the titration? Which 3 substances go into the 250 mL Erlenmeyer flask for the titration? What is the mole to mole ratio in the reaction of KHP and NaOH? What solution goes into the buret?