21:56 1Question 21 of 30SubmitA solution of phosphoric acid (H3PO4) with a knownconcentration of 0.250M H;PO. is titrated with a 0.800M NAOH solution. How many ml of NaOH are required toreach the third equivalence point with a starting volume of72.0mL H3PO. , according to the following balancedchemical equation:НРО, +3NaOH > NaзРОд +3H20XSTARTING AMOUNTADD FACTORANSWERRESET*( )7.503222.50.25072.0167.5m10000.8000.00143.26.75 x 1040.0675Tap here or pull up for additional resources

At third equivalence point, all the H3PO4 molecule get converted to PO4-3 i.e complete…

A solution of phosphoric acid (H3PO4) with a known concentration of 0.250 M H3PO4 is titrated with a 0.800 M NAOH solution. How many mL of NaOH are required to reach the third equivalence point with a starting volume of 72.0 mL H3PO4 , according to the following balanced chemical equation: H3PO4 + 3 NaOH → Na3PO4 + 3 H2O

A solution of phosphoric acid (H3PO4) with a known concentration of 0.250 M H3PO4 is titrated with a 0.800 M NAOH solution. How many mL of NaOH are required to reach the third equivalence point with a starting volume of 72.0 mL H3PO4 , according to the following balanced chemical equation: H3PO4 + 3 NaOH → Na3PO4 + 3 H2O

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

Calculate the molarity of an NaOH solution from the following titration data. Be sure the answer has the correct amount of significant figures. The chemical equation for this titration is as follows: NaOH + KHP → NaKP + H₂O NaOH buret reading, inital: 15.27 mL NaOH buret reading, final: 8.32 mL Mass of KHP (204.22 g/mol): 1.1592 g
A chemistry student needs to standardize a fresh solution of sodium hydroxide. She carefully weighs out 400. mg of oxalic acid (H,C204), 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 her sodium hydroxide solution. When the titration reaches the equivalence point, the student finds she has used 90.3 mL of sodium hydroxide solution. Calculate the molarity of the student's sodium hydroxide solution. Be sure your answer has the correct number of significant digits.
A chemistry student needs to standardize a fresh solution of sodium hydroxide. He carefully weighs out 79. mg of oxalic acid (H,C,0,), 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 23.0 mL of sodium hydroxide solution. Calculate the molarity of the student's sodium hydroxide solution. Be sure your answer has the correct number of significant digits.
Fill in the missing words With the given plot, if a 0.1000 M NaOH solution was used to fully precipitate all the Zn2+ in the form of Zn(OH)2 with the addition of 6.00 mL of NaOH, the number of moles of Zn2+ in this 10 mL brass stock solution is mmol. Therefore, there are mmol of Zn2+ in the entire 100-mL brass stock solution, which is g/mol). mg of Zn2+ (FW = 65
A chemistry student weighs out 0.106 g of ascorbic acid (H,C,H,O), a diprotic acid, into a 250. mL volumetric flask and dilutes to the mark with distilled water. He plans to titrate the acid with 0.2000M NAOH solution. Calculate the volume of NAOH solution the student will need to add to reach the final equivalence point. Be sure your answer has the correct number of significant digits. mL 19 MacBook Air DII 888 F6 F7 F8 F4 F5 F3 &
A chemistry student needs to standardize a fresh solution of sodium hydroxide. She carefully weighs out 17. mg of oxalic acid (H,C,0,), 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 her sodium hydroxide solution. When the titration reaches the equivalence point, the student finds she has used 16.4 mL of sodium hydroxide solution. Calculate the molarity of the student's sodium hydroxide solution. Round your answer to 2 significant digits. Submit Ass Continue O 2021 McGraw Hill LLC. Al Rights Reserved. Terms of Use I Privacy Center LL
A 25.00 mL aliquot is withdrawn from the liquid portion of saturated Manganese (II) hydroxide and transferred to an Erlenmeyer flask. After the addition of methyl orange, a titration with 0.0045 M HCl was performed. The endpoint was reached after 8.72 mL of the acid was added. What is the balanced chemical equation? How many moles of hydroxide ions were neutralized in the reaction? What is the molar concentration of hydroxide in the saturated solution? What is the molar concentration of Magnesium ion in solution?
A chemistry student needs to standardize a fresh solution of sodium hydroxide. He carefully weighs out 150. 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 77.1 mL of sodium hydroxide solution. Calculate the molarity of the student's sodium hydroxide solution. Round your answer to 3 significant digits. x10 M X 5 ?
A commercial vinegar was analyzed by titration to determine the percent acetic acid. Briefly, 10.00 mL of vinegar sample was diluted to 100. mL solution in volumetric flask. A 25.00 mL aliquot from the diluted vinegar required 25.55 mL of 0.1005 M NaOH to reach the phenolphthalein endpoint. Which is the correct equation between the analyte and titrant reaction? CH3COOH + NaOH → NaCH3COO + H2O 2CH3COOH + NaOH → NaCH3COO + H2O C20H14O4 + NaOH → NaC20H14O4 + H2O CH3COOH + 2NaOH → NaCH3COO + H2O
You are assigned to measure the amount of salicylic acid in a wart remover solution. Salicylate ion reacts with an Fe³+ ion to form a complex ion that strongly absorbs light at 528 nm. You prepare standard solutions of known salicylate concentration. You add 5.00 mL of 0.025 M FeCl3 to each standard solution and dilute each solution to a total of 10.00 mL. The concentration of salicylate in each solution is given in the table below. You then measure the absorbance of each standard solution. The data are shown below. What is the concentration of salicylate in mg/dL in an unknown salicylate solution whose absorbance is 0.310? (Give your answer to 2 decimal places) Salicylate solution concentration (mg/dL) 1.00 2.00 3.00 4.00 5.00 Absorbance at 528 nm 0.162 0.223 0.262 0.359 0.401
You are assigned to measure the amount of salicylic acid in a wart remover solution. Salicylate ion reacts with an Fe³+ ion to form a complex ion that strongly absorbs light at 528 nm. You prepare standard solutions of known salicylate concentration. You add 5.00 mL of 0.025 M FeCl3 to each standard solution and dilute each solution to a total of 10.00 mL. The concentration of salicylate in each solution is given in the table below. You then measure the absorbance of each standard solution. The data are shown below. What is the concentration of salicylate in mg/dL in an unknown salicylate solution whose absorbance is 0.185? (Give your answer to 2 decimal places) Salicylate solution concentration Absorbance at 528 (mg/dL) 1.00 2.00 3.00 4.00 5.00 nm 0.162 0.223 0.262 0.359 0.401
Potassium hydrogen phthalate (KHPKHP) is often used as a primary standard in acid–base titrations. If 20.05 mL NaOH20.05 mL NaOH is required to neutralize 0.397 g KHP,0.397 g KHP, what is the concentration of the NaOH?