millan Learning A sample of drinking water was tested for Pb²+ and was found to have a Pb2+ concentration of 17.49 ppb. A 9.00 mL sample of the drinking water was spiked with 1.00 mL of a 2.29 ppb Pb²+ standard. Analysis of the spiked sample gave a concentration of 15.92 ppb Pb²+. Find the percent recovery of the spike.

millan Learning A sample of drinking water was tested for Pb²+ and was found to have a Pb2+ concentration of 17.49 ppb. A 9.00 mL sample of the drinking water was spiked with 1.00 mL of a 2.29 ppb Pb²+ standard. Analysis of the spiked sample gave a concentration of 15.92 ppb Pb²+. Find the percent recovery of the spike.

Appl Of Ms Excel In Analytical Chemistry

2nd Edition

ISBN:9781285686691

Author:Crouch

Publisher:Crouch

Chapter7: Neutralization Titrations And Graphical Representations

Section: Chapter Questions

Problem 8P

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Part A: Standardization of a Sodium Hydroxide Solution Titration 1 Titration 2 Titration 3 Mass of 125 mL flask 45.849g 46.715g 44.953g Mass of flask and KHP 46.849g 47.745g 46.003g Initial buret reading (mL) 0.5 ml 0.5 ml 0.5 ml Final buret reading (mL) 27.8 ml 26.5 ml 26.7 ml Volume of NaOH used (mL) 45.11 ml 45.06 ml 45.14 ml Calculations Titration 1 Titration 2 Titration 3 Moles of KHP Moles of NaOH Molarity of NaOH Average Molarity of NaOH: _______________
Titration of a 0.492-g KH₂PO4 used 25.6 mL of 0.112M NaOH. What is the percent purity of KH₂PO4? MW KH₂PO4 = 136.1 g/mol H₂PO4¹ + OH¹ HPO4² + H₂O
Direct titration: 10.90 ± 0.02 mL of an unknown KHP solution required 11.72 ± 0.02 mL of 0.1090 ± 0.0006 M NaOH to reach the end point. What is the concentration of KHP in the unknown solution reported with absolute uncertainty? If the unknown solution was prepared by dissolving 5.128 g of the unknown KHP (204.22 g/mol) in 100.00 mL of water, what is the weight percent of KHP in the sample?
Do the argentometric titration according to given data and fill in the blanks. Ag+ (aq) + Cl- (aq) → AgCl (s) (White) NaCl » Na* + Cl- SET 2 Measured Weight of NaCl, (gr) 2.5 g Measured Weight of Cl- , (g) Volume of Stock Solution, (mL) 200 mL Amount of Sample taken from the stock solution, (mL) 9mL Normality of AgNO3, (N) 0.1 N Initial burette reading, (mL) O mL Final burette reading, (ml) 6.85 mL Volume of AgNO; Consumed, (mL) 6.85 mL Amount of AGNO3 Consumed, (mg) Calculated Weight of NaCI in stock Solution, (g) Calculated Weight of CI- in stock Solution, (g) Error in Calculating Amount of CI-(%)
A sodium hydroxide (NaOH) solution was standardized with KHP primary standard. The concentration was found to be 0.1022 M. What is the concentration of a 25.0-ml hydrochloric acid (HCl) solution if it required 32.6 ml of NaOH to reach the phenolphthalein end point?
1. Commercial vinegar was titrated with NaOH solution to determine the content of acetic acid, CH3COOH. For 20.0 cm3 of the vinegar, 26.7 cm3of 0.60 mol dm-3 NaOH solution was required.What was the concentration of acetic acid in the vinegar if no other acid was present? (Thanks for your help) A. 0.45 mol dm-3B. 0.60 mol dm-3C. 0.80 mol dm-3D. 1.60 mol dm-3
3. A buffer solution after the addition of 20.0 mL of 1.00 M NaOH solution to 500.0 mL of a buffer solution containing 0.20 M acetic acid (CH3COOH) and 0.30 M sodium acetate (CH3COONa). [Ka= 1.8 x 10–5] What is the new concentration of NaOH after dilution? a 0.0273 b 0.0439 c 0.0185 d 0.0267 e 0.0385
A titrant solution of KMnO was standardized with 0.2000 grams of Na2C2O4 and consumed 27.75 mL to reach end point. Calculate the standardized NORMAL concentration of the titrant.
Given the following data during the potentiometric titration of 75.00 mL unknown NaCl solution by 0.01000 AgNO3, what is the concentration of the NaCl present in the solution (NaCl = 58.44 g/mol) Ag+ + Cl- à AgCl(s)?
4. In an experiment to determine the concentration of an HCI sample of unknown concentration, 0.1 M NaOH solution was prepared in the first step. Then, 50 mL of NaOH prepared as 0.1 M and 5 drops of methylorange indicator were added to a 250 mL flask and titrated with H2C204 prepared as 0.05 M. The turning point was observed when 26 mL of H2C204 was consumed in the titration process. In the second step, 50 mL of a non-concentrated HCI solution and 5 drops of phenolphthalein solution were added to a 250 mL flask and titrated with the adjusted NaOH solution. Calculate the concentration of an HCI sample with an unknown concentration, since it is determined that 16 mL of NaOH solution was consumed after titration.
D. Acid-Base Titrations A 0.1558 g of primary-standard-grade benzoic acid, C6H$COOH, was used to standardize a solution of Mg(OH)2. Calculate the normality of this solution if it needed 19.15 mL of this base to reach the end point of the titration. A solution of an unknown monoprotic acid was found in a laboratory. When titrated, 25.00 mL of this unknown solution needed 28.44 mL of the same base to reach the endpoint. The remaining solution of unknown monoprotic acid amounting 15.00 mL was left in an Erlenmeyer flask uncovered to recover the acid crystals. After 5 days, the mass of the unknown monoprotic acid left on the flask weighed 0.0967 g. Determine the equivalent weight of this unknown acid. FW: C6HSCOOH: 122.12 Mg(OH)2 = 58.32
what is the maximum amount of sodium sulfate that can be added to 450 ml of .0015 M CA(NO3)2 before precipitation of calcium sulfate begins? Ksp= 2.4*10-5