Sodium hypochlorite (NaOCI) is a weak base made from reacting chlorine with a sodium hydroxide solution. Sodium hypochlorite, commonly referred to as bleach, has a variety of uses and is an excellent disinfectant/antimicrobial agent. As part of exploring titration of weak base with strong acid, a 53.0 mL solution of 0.136 M sodium hypochlorite (NaOCI) is titrated with 0.258 M HCl. (The pK, of hypochlorous acid, HOCI, is 7.350.) 1. Calculate the pH of the solution after the addition of 10,3 ml. of 0.258 HCI. 2. Calculate the pH of the solution after the addition of 29.6 mL of 0.258 M HCl. 3. Calculate the pH of the solution at the equivalence point with 0.258 M HC.

Sodium hypochlorite (NaOCI) is a weak base made from reacting chlorine with a sodium hydroxide solution. Sodium hypochlorite, commonly referred to as bleach, has a variety of uses and is an excellent disinfectant/antimicrobial agent. As part of exploring titration of weak base with strong acid, a 53.0 mL solution of 0.136 M sodium hypochlorite (NaOCI) is titrated with 0.258 M HCl. (The pK, of hypochlorous acid, HOCI, is 7.350.) 1. Calculate the pH of the solution after the addition of 10,3 ml. of 0.258 HCI. 2. Calculate the pH of the solution after the addition of 29.6 mL of 0.258 M HCl. 3. Calculate the pH of the solution at the equivalence point with 0.258 M HC.

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

Potassium hydrogen phthalate is a solid, monoprotic acid frequently used in the laboratory to standardize strong base solutions. It has the unwieldy formula of KHC3H,04. This is often written in shorthand notation as KHP. What volume of a 0.438 M sodium hydroxide solution is needed to exactly neutralize 3.48 grams of KHP ?
6. A student titrated 30.00 mL of a hydrochloric acid solution with 1.00 M sodium hydroxide. The sodium hydroxide was initially tilled to the 2.30 mL mark on the burette. Once the level in the burette reached 50.00 mL, the student was forced to refill the burette and did so to the 5.06 mL mark. The endpoint was finally reached when the sodium hydroxide level dropped to 32.09 mL on the burette. What is the molarity of the acid solution? Show work.
Three acid samples are prepared for titration by 0.03 M NaOH: Sample 1 is prepared by dissolving 0.03 mol of HCl in 20 mL of water. Sample 2 is prepared by dissolving 0.03 mol of HCl in 30 mL of water. Sample 3 is prepared by dissolving 0.03 mol of HCl in 40 mL of water. a Without performing a formal calculation, compare the concentrations of the three acid samples (rank them from highest to lowest). O3>2>1 O1>3> 2 O3>1> 2 O2>1>3 O1>2>3 O2>3>1 Submit Submit Answer Try Another Version 6 item attempts remaining
A titration is performed to determine the amount of sulfuric acid, H2SO4,, in a 6.5mL sample taken from a car battery. About 50mL of water is added to the sample, and then it is titrated with 43.37mL of standard 0.5824 molar NaOH solution. How many moles of sulfuric acid are present in the original sample?
O Chemical Reactions Standardizing a base solution by titration 3/5 Bis A chemistry student needs to standardize a fresh solution of sodium hydroxide. He carefully weighs out 36. mg of oxalic acid (H2C2O4), a diprotic acid that can be purchased inexpensively in high purity, and dissolves it in 250. mL of distilled water. The student then titrates the oxalic acid solution with his sodium hydroxide solution. When the titration reaches the equivalence point, the student finds he has used 35.1 mL of sodium hydroxide solution. Calculate the molarity of the student's sodium hydroxide solution. Round your answer to 2 significant digits. Ом OP G
One of the main acidic components of acid rain is sulfuric acid, H₂SO4. Assuming sulfuric acid is the only acid in the acid rain, what volume (in mL) of 0.000915 M KOH would be required to titrate a 45.00 mL sample of acid rain with an H₂SO4 concentration of 1.230 × 10-4 M? Volume mL
Many chemical compounds contain impurities. Crude potassium carbonate (K2CO3) obtained from the chemical supplier is assayed for purity in the following way: 8.450 g of crude potassium carbonate is weighed out into a flask and dissolved in water. The final volume was completed to 0.500 L with distilled water. 20.00 mL sample is taken from this solution and placed in a flask. Potassium carbonate is then titrated to the equivalence point with 17.80 mL of 0.2050 M HCl solution. What is the percent purity of potassium carbonate in this sample? K2CO3 + HCl  KCl + H2O + CO2
The antacid found in Tums™ has the active ingredient calcium carbonate, which undergoes a reaction when mixed with hydrochloric acid to produce water, calcium chloride and carbon dioxide. A tablet of this antacid had a mass of 1.774g and was dissolved completely in an excess of 30.0mL of 0.794M HCl. The resulting solution was then titrated with 0.995M NaOH. The initial buret reading was 11.05mL and the final buret reading was 28.52mL. The listed mass of active ingredient on the bottle is 325mg. a. What is the calculated mass of active ingredient in this tablet? b. What is the percent error from the listed mass? c. What percent of the tablet is inert (non-active) ingredients? explain in detail
what is the Molarity of the NaOH solution? Mass of H2C2O4·2H2O=1.32191 g Volume of the H2C2O4·2H2O solution=250.0 mL Volume of NaOH solution used in titration=21.45 mL
Give detailed Solution with explanation needed
A 50.0 mL solution of Ca(OH)₂ with an unknown concentration was titrated with 0.340 M HNO₃. To reach the endpoint, a total of 16.8 mL of HNO₃ was required. Write the balanced chemical equation based on the following description: solid calcium hydroxide reacts with aqueous nitric acid to produce the aqueous calcium nitrate and liquid water. Ca(OH)2(aq)+HNO3(aq)------
A solution contains one or more of the following ions: Ag+, Ca2+, and Co2+. Lithium bromide is added to the solution and no precipitate forms. An excess of lithium sulfate is then added to the solution and a precipitate forms. The precipitate is filtered off and lithium phosphate is added to the remaining solution, producing a precipitate. Which ions are present in the original solution? Ag+ O Ca2+ O Co2+ Write a net ionic equation for the formation of the precipitate observed after the addition of lithium sulfate. Include physical states. net ionic equation: Write a net ionic equation for the formation of the precipitate observed after the addition of lithium phosphate. Include physical states. net ionic equation: