20.01 Error from technique If you were to overshoot the endpoint by just 1 drop while you were standardizing the NaOH solution, what would be your % error? Assume the actual volume is 20.00 mL and there are exactly 20 drops in 1.00 mL ( find the value of 1 drop) for the sake of this calculation. Y20 = 0.05 %3D % error = |measured value - actual value|/actual value x 100% %3D 20.05ML-20. mx100 =0.25% coml 20. C0ML vill ve as (4) e, our II + TI-30XIS TEXAS INSTRUMENTS SCI/ENG INS 2nd DRG DEL 10* LOG PRB ex ADIC dle STAT EXIT STAT Ablc DATA STATVAR CLEAR SIN- COS-1 TAN- SIN COS TAN EE ( ) 8. RCL 4. 6. STO OFF ON RESET

20.01 Error from technique If you were to overshoot the endpoint by just 1 drop while you were standardizing the NaOH solution, what would be your % error? Assume the actual volume is 20.00 mL and there are exactly 20 drops in 1.00 mL ( find the value of 1 drop) for the sake of this calculation. Y20 = 0.05 %3D % error = |measured value - actual value|/actual value x 100% %3D 20.05ML-20. mx100 =0.25% coml 20. C0ML vill ve as (4) e, our II + TI-30XIS TEXAS INSTRUMENTS SCI/ENG INS 2nd DRG DEL 10* LOG PRB ex ADIC dle STAT EXIT STAT Ablc DATA STATVAR CLEAR SIN- COS-1 TAN- SIN COS TAN EE ( ) 8. RCL 4. 6. STO OFF ON RESET

Principles of Instrumental Analysis

7th Edition

ISBN:9781305577213

Author:Douglas A. Skoog, F. James Holler, Stanley R. Crouch

Publisher:Douglas A. Skoog, F. James Holler, Stanley R. Crouch

Chapter1: Introduction

Section: Chapter Questions

Problem 1.10QAP

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You determine the acetic acid (HOAc) content of vinegar by titrating with a sodium hydroxide standard solution to a phenolphthalein (an indicator) end point. An approximately 5-mL sample of vinegar is weighed on an analytical balance in a weighing boat and this is found to be 5.0268 g. The standard deviation in making a single weighing is 0.2 mg. The sodium hydroxide must be accurately standardised (this means its concentration must be accurately determined) by titrating known mass of high-purity potassium hydrogen phthalate, and three such titrations give molar concentrations of 0.1167, 0.1163 and 0.1164 mol L-1. A volume of 36.78 mL of sodium hydroxide is used to titrate each sample. The standard deviation of the burette used is 0.02 mL. Calculate the percentage of acetic acid in the vinegar and its standard deviation.
You are provided with a stock standard with a concentration of 100 mg/L, and a solution of unknown concentration. Prepare calibration standards using a 10 mL volumetric flask and a 1 mL piston pipette, and measure on the UV/Vis spectrophotometer (400 nm). Determine the concentration of the unknown after a 1:40 dilution, and provide the concentration of the initial solution. i need to learn how to do the calculations and draw a calibration curve to find concentration of unknown sample after i find the absorbances.
In a chromatography experiment, a solution containing 0.083 7 M X and 0.066 6 M S gave peak areas of AX = 423 and AS 5 347. (Areas are measured in arbitrary units by the instrument.) To analyze the unknown, 10.0 mL of 0.146 M S were added to 10.0 mL of unknown, and the mixture was diluted to 25.0 mL in a volumetric flask. This mixture gave the chromatogram in Figure 5-8, with peak areas AX = 553 and AS = 582. Find the concentration of X in the unknown.
An excess of 0.34 mg Pb is obtained from an assay test determined in an analysis. What is the percent relative error in ppt if the mass of the sample is 550 g?
Standardization of EDTA Solution Weight of pure CaCO3: 0.2514 g % Purity of CaCO3: 98.0% Total volume of standard CaCO3 solution: 250.00 mL Using the information given in the table, show a step-by-step process to compute the missing values. Take note of the % purity and total volume. Trial 1 2 3 Volume of standard CaCO3 solution (ml) 25.00 25.00 25.00 Final Volume Reading EDTA (ml) 24.30 47.95 24.72 Initial Volume Reading EDTA (ml) 0.00 24.30 0.20 Volume of titrant, EDTA (ml) Molarity of EDTA (M)
Standardization of Sodium Thiosulfate Solution Primary Standard used: Potassium Dichromate Formula mass of 1o standard: __________________ % Purity of 1o standard: 99.80% Trials 1 2 3 Weight of K2Cr2O7 (g)Weight of K2Cr2O7 (g) 0.0315 0.0331 0.0380 Final Volume Reading Na2S2O3 (ml) 27.50 27.50 34.90 Initial Volume Reading Na2S2O3 (ml) 1.10 0.00 1.00 Net Volume Na2S2O3 used (ml) Molarity of Na2S2O3
The color change of a chemical requires an overtitration of 0.04 mL. Calculate the percent relative error if the total volume of the titrant is 50 mL.
A 50.00 (±0.03) mL portion of an HCl solution required 29.71(±0.03) mL of 0.01963(±0.0030) M Ba(OH)2 to reach an end point with bromocresol green indicator. The molar concentration of the HCl is calculated using the equation below (attached image): a.) Calculate the uncertainty of the result (absolute error). M=0.02333(±?????) M b.) Calculate the coefficient of variation for the result. CV= (Sy/y) x 100%
A volume of 250 ml of a 0.05 M solution of a reagent of formula weight (relative molecular mass) 40 was made up, the weighing being done by difference. The standard deviation of each weighing was 0.0001 g. The standard deviation of the volume of solvent used was 0.05 ml. Express this as a relative standard deviation. Hence calculate the relative standard deviation of the molarity of the solution.
A stock solution of 0.225 +/- 0.003 M NaNO2 was transferred to a 100 mL volumetric flask (class A) and diluted to the mark. If 7 mL of the stock solution was transferred using one 5-mL and two 1-mL volumetric pipettes, what is the new concentration of the solution and the uncertainty?
A method for the detection of morphine is used to generate a calibration curve in which the assay response (y) is plotted versus morphine concentration (x, in mg/L). This gives a straight line with a slope (m) of 0.241 and a y-intercept (b) of 0.011, where y = mx + b. The slope of this line has a standard deviation of ±0.007, and the standard deviation of the intercept is ±0.006. If the sample from an athlete gives a response of 0.506 ± 0.013 in this method, what is the concentration of morphine in the sample and estimated precision of this concentration?
Standardization of EDTA Solution Weight of pure CaCO3: 0.2517 g % Purity of CaCO3: 98.0% Total volume of standard CaCO3 solution: 250.00 mL Trial 1 2 3 Volume of standard CaCO3 solution (ml) 25.00 25.00 25.00 Final Volume Reading EDTA (ml) 24.30 47.95 24.72 Initial Volume Reading EDTA (ml) 0.00 24.30 0.20 Volume of titrant, EDTA (ml) Molarity of EDTA (M)