Consider the titration of 25.0 mt. of 0.070 M HCN with 0.080 H NaOH, what volume of base, in matters, is required to reach the equivalence point? Volume-21.871 m The equivalence point for a reaction is the point at which one reactant has been completely consumed by addition of another reactant. Thus n(HCN) = n(NaOH) [HCN] × V(HCN)-[NaOH] × V(NaOH) V(NaOH)-22 mL Consider the titration of 25.0 ml of 0.070 M HCN (K, -4.0 x 10) with 0.080 M NaOH. what is the pH before any NaOH is added? pH initial- what is the pH at the halfway point of the titration? pH at halfway- What is the pet when 95% of the NaOH required to reach the equivalence point has been added pH when 95% is added- What is the pit at the equivalence point? pet at the equivalence point- Correct Submit

Consider the titration of 25.0 mt. of 0.070 M HCN with 0.080 H NaOH, what volume of base, in matters, is required to reach the equivalence point? Volume-21.871 m The equivalence point for a reaction is the point at which one reactant has been completely consumed by addition of another reactant. Thus n(HCN) = n(NaOH) [HCN] × V(HCN)-[NaOH] × V(NaOH) V(NaOH)-22 mL Consider the titration of 25.0 ml of 0.070 M HCN (K, -4.0 x 10) with 0.080 M NaOH. what is the pH before any NaOH is added? pH initial- what is the pH at the halfway point of the titration? pH at halfway- What is the pet when 95% of the NaOH required to reach the equivalence point has been added pH when 95% is added- What is the pit at the equivalence point? pet at the equivalence point- Correct Submit

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

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Similar questions

In a titration, 20.0 g of oxalic acid dihydrate was dissolved in a flask and neutralized with 31.2 mL of NaOH. Determine the molarity of the NaOH. 2NaOH(aq) + H2C2O4 ⋅ 2H2O(s) --> Na2C2O4(aq) + 4H2O(l)
An analytical chemist weighs out 0.066 g of an unknown monoprotic acid into a 250 mL volumetric flask and dilutes to the mark with distilled water. She then titrates this solution with 0.1700M NaOH solution. When the titration reaches the equivalence point, the chemist finds she has added 8.4 mL of NaOH solution. Calculate the molar mass of the unknown acid. Be sure your answer has the correct number of significant digits. g mol x10 X S
A 0.2897-g sample of an unknown monoprotic acid is dissolved in water and titrated with standardized barium hydroxide. The equivalence point in the titration is reached after the addition of 28.65 mL of 6.189×10-2 M barium hydroxide to the sample of the unknown acid. Calculate the molar mass of the acid.
The flask contains 10.0 mL10.0 mL of HClHCl and a few drops of phenolphthalein indicator. The buret contains 0.110 M NaOH.0.110 M NaOH. It requires 31.4 mL31.4 mL of the NaOHNaOH solution to reach the end point of the titration. What is the initial concentration of HClHCl?
The amount of nitrogen in an organic substance can be determined by an analytical method called the Kjeldahl method, in which all the nitrogen in the organic substance is converted to ammonia. The ammonia, which is a weak base, can be neutralized with hydrochloric acid, as described by the equation NH3(aq) + HCl(aq) ->> NH₂Cl(aq) If 6.0 mL of 0.150 M HCl(aq) is needed to neutralize all the NH3(g) from a 2.25 g sample of organic material, calculate the mass percentage of nitrogen in the sample.
In a laboratory experiment, a student is conducting a titration. In this titration, a 0.250 M solution of Sodium Hydroxide (NaOH) is added to 30.0 mL of an HCl solution with an unknown concentration. After adding the sodium hydroxide, the student determined that 15.0 mL of NaOH was needed to reach the equivalence point. Based on this information, what was the original concentration of the HCl solution? (Please provide your answer to 3 decimal places.)
55.0 mL of 1.20 M H2SO4 is added to a 39.5 mL of 2.00 M LiOH. The balanced chemical equation for the reaction is: H2SO4 (aq) + 2LiOH (aq) --> Li2SO4 (aq) + 2H2O (l) What kind of reaction is this? If a phenolphthalein indicator was included in the reaction flask, what color will it be after the 55.0 mL of 1.20 M H2SO4 and 39.5 mL of 2.00 M LiOH have reacted? Clear or pink? Explain your answer and include any relevant calculations.
A chemist needs to determine the concentration of a solution of nitric acid, HNO3. She puts 905 mL of the acid in a flask along with a few drops of indicator. She then slowly adds 0.200 mol L Ba(OH)2 to the flask until the solution turns pink, indicating the equivalence point of the titration. She notes that 225 mL of Ba(OH)2 was needed to reach the equivalence point. Solution map In this titration, the concentration of base is known and can be used to calculate the unknown acid concentration: concentration of base → moles of base → moles of acid → concentration of acid Part A How many moles of Ba(OH)2 are present in 225 mL of 0.200 mol L-1 Ba(OH)2? Express your answer numerically in moles. • View Available Hint(s) Vo AEO ? mol Ba(OH)2 Submit
For the titration of an aqueous ammonia solution, NHalag), with an aqueous hydrobromic acid solution, HBr(ag), which of the following chemical species will be present in highest concentration at the equivalence point? O NH,(ag) OH laa) O NH, "(ag) O All of these chemical species will be present in highest concentration at the equivalence point. O H(ag)
Solid sodium sulfide is slowly added to 125 mL of a 0.0536 M iron(II) acetate solution. The concentration of sulfide ion required to just initiate precipitation is M.
Calculate the number of grams of AgCl will precipitate out of solution if 125 mL of 0.500 M AgNO3 is combined with 275 mL of 0.235 M NaCl according to the following AgNO3 (aq) + NaCl (aq) --> AgCl (s) + NaNO3 (aq)
If the concentration of the NaOH that was added was 1.0 M and the volume of oxalic acid being titrated was 75 ml, then what is the unknown concentration of the oxalic acid in this titration. The volume of NaOH is 29ml.