The following data are for a series of extemal standards of Cd² buffered to a pH of 3.7. [Cď*], nM Signal intensity 15.4 15.0 30.4 42.7 44.9 58.5 59.0 77.0 72.7 101 86.0 118 unknown 66.3 Plot the calibration curve and calculate the linear least-squares equation for the data. Determine the concentration of Cd²* in the unknown sample.

The following data are for a series of extemal standards of Cd² buffered to a pH of 3.7. [Cď], nM Signal intensity 15.4 15.0 30.4 42.7 44.9 58.5 59.0 77.0 72.7 101 86.0 118 unknown 66.3 Plot the calibration curve and calculate the linear least-squares equation for the data. Determine the concentration of Cd² in the unknown sample.

Appl Of Ms Excel In Analytical Chemistry

2nd Edition

ISBN:9781285686691

Author:Crouch

Publisher:Crouch

Chapter5: Equilibrium, Activity And Solving Equations

Section: Chapter Questions

Problem 5P

See similar textbooks

Similar questions

•The pKa for acetic acid is 4.756 and the pKa for NH4+ is 9.245. What pH do you expect for the solutions with [A-]init [HA]init? Explain this by referring to the acid = dissociation constant expressions (Ka) for NH4+ and CH3COOH as well as your answer to part (a). Do your measurements agree with your expectations (make specific reference to your experimental data and consider uncertainty)?
25.0 cm3 of sodium hydroxide solution is tritrated against 0.2 mol dm–3 hydrochloric acid until the indicator just changes colour. 27.5 cm3 of the acid are required to reach the end point.Phenolphthalein is used as an indicator in the above experiment. What will be its colour change at the end point? From pink to yellow From pink to colourless From yellow to colourless From yellow to pink
Arthur Wen, a CHEM 18.1 student, was tasked to make a 250mL solution of NaCH3CO0 with pH = 9.022 for their laboratory class. However, he forgot to take note of the initial concentration needed and was too shy to ask Mr. Lee, his teacher. He knows that the conjugate acid of one of the salt's ions has a Ka = 1.8 x 10-5. 1. Compute for the initial concentration (M) of NACH3COO: M 2. Compute the mass (g) of solid NaCH3COO to prepare the said solution: g
A.) The value of Ka for hydrocyanic acid is 4.00×10-10.What is the value of Kb, for its conjugate base, CN-? B.) In the laboratory, a general chemistry student measured the pH of a 0.589 M aqueous solution of benzoic acid, C6H5COOH to be 2.199.Use the information she obtained to determine the Ka for this acid.Ka(experiment) =
What conclusion can be derived from the following sentences regarding analytical methods: I. Classical methods (gravimetry and volumetric methods) are no longer useful in analytical chemistry. II. Volumetric methods do not require calibration if a primary standard is used as titrant. III. Instrumental methods are useful with analyte solutions that are less than 1.00 mM. IV. Classical methods yield high precision and accuracy at concentrations greater than 1.00 mM. What conclusion can be derived from the following sentences regarding analytical methods: Two statements are incorrect. All statements are correct. One statement is incorrect. Only one statement is correct. All statements are incorrect.
4. To perform a certain activity assay it is necessary to have 0.25 mL of an enzyme at a concentration of 0.2 mgml¹ in the presence of 0.4 mM substrate and 200 mM NaCl in a suitable buffer. The stock solutions of enzyme, substrate and NaCl are 4 mgmL-¹, 40 mM and 1 M all in the same type of buffer. What volumes of the stock solutions and buffer are required for each assay?
Please check if my second data table is correct. I don't think the molar mass is correct
A second calibration standard solution of an iron(III) salicylate complex was prepared in two steps. First, 10.0 mL of a 0.100 M stock solution was added to 90.0 mL of solvent to make 100.0 mL of the first calibration standard solution and, secondly, 80 mL of that first calibration solution plus 20.0 mL of solvent were mixed to make the second calibration standard. What is the concentration of the second calibration standard solution?
The course is specifically quantitative analysis, I figured that would just fall under chemistry. The issue I'm having with this one is that I have absolutely no idea how to even begin. I figure benzoic acid wouldn't affect the pH of NaOH that much since it's a weak acid and NaOH is a strong base, but I don't think it'd be right to just take the pH using solely the concentration of NaOH. What approach should I take to solve this? 220 mL of 0.03 M NaOH were added to 200 mL of 0.03 M benzoic acid (pKa = 4.2). What is the pH of the resulting solution?
The calcium ion binds to a certain protein to form a 1:1 complex. The following data were obtained in an experiment. Total Ca2+/µM 60.9 122 186 250. 536 Ca2+ bound to Protein/µM 31.4 51.4 63.6 71.0 83.6 Determine graphically the dissociation constant of the Ca²+-protein complex. The protein concentration was kept at 97 µM for each run. (1 µM = 1x10-6 M.) Kd =
What are the applications of re-crystallization in gravimetric analysis? answer at your own words and answer should be to the point, not any irrelevant words
25.0 cm3 of sodium hydroxide solution is tritrated against 0.200 mol dm–3 hydrochloric acid until the indicator just changes colour. 27.5 cm3 of the acid are required to reach the end point.Which of the following pieces of apparatus should be used to transfer 25.0 cm3 of the sodium hydroxide solution?a. Burette b. Pipette c. Measuring cyclinder d. Volumetric flask