QI/A-Fill in the blanks 1- 2- is the collection of all of the components in the sample containing an analyte. indicates the amount of cach substance in a sample. ........ 3- is the process of determining the proportionality between analyte concentration and a measured quantity. 4- is the ratio of its mass to the mass of an cqual volume of water at 4C. 5- A compound produced by an internal acid / base reaction consisting of positive and negative charge is.. ........ rinאalaftha

QI/A-Fill in the blanks 1- 2- is the collection of all of the components in the sample containing an analyte. indicates the amount of cach substance in a sample. ........ 3- is the process of determining the proportionality between analyte concentration and a measured quantity. 4- is the ratio of its mass to the mass of an cqual volume of water at 4C. 5- A compound produced by an internal acid / base reaction consisting of positive and negative charge is.. ........ rinאalaftha

Introductory Chemistry: An Active Learning Approach

6th Edition

ISBN:9781305079250

Author:Mark S. Cracolice, Ed Peters

Publisher:Mark S. Cracolice, Ed Peters

Chapter3: Measurement And Chemical Calculations

Section: Chapter Questions

Problem 99E

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A blood concentration of 0.065 M ethyl alchohol is sufficient to induce a coma. Blood alcohol content is a measure of alcohol in the blood as a percentage. It is calculated in grams per 100mL of blood, so a BAC os 0.08 means your blood is 0.08% alcohol by volume. a) What is the total mass of alcohol (in grams) that it represents for the same adult male whose total blood volume is 5.6L? b) What percentage does it represent from the coma induced level?
You are checking the accuracy of a volumetric flask marked 10.00 mL . To calculate the volume of water contained in the flask, you first measure the mass of the empty flask and the mass of the flask filled with water and take the difference. Then, you correct for the buoyancy factor and divide by the density of the water. The result of 8 such measurements is given in the table. Calculate the 95% confidence interval for these measurements with a mean of 10.03.
A volume of 25.00 mL of the original solution was diluted to a total volume of 100.0 mL and then 10.00 mL of that diluted solution was diluted to a total volume of 15.00 mL to make the sample for analysis. If a student in lab found that the solution for spectroscopic analysis had a concentration of (4.0x10^-5) M, what was the concentration of the original solution, in units of M?
Stock iron(II) solution (200Ug mL-1 Fe) ferrous ammonium sulfate hexahydrate mass= 0.1437g, transfer it to a 100 ml beaker. add 15 ml approx of water and 15m1 'approx of dilute sulphuric acid (2M H2SO.). then transfer FeII to 100 ml flask makeup to the mark with water. calculate the moles of ferrous ammonium sulfate hexahydrate solution in unit ug/mL.
1. Which of the following is not a step in preparing a water sample container?a. All sample containers must be dark in colorb. The type of sample container and the level of cleaning required depend on the type of sample to be takenc. All sample containers must be thoroughly cleaned in the laboratory before sampling is carried outd. The number of containers prepared must always be in excess of what is needed, for quality assurance, quality control and reserves 2. The purpose of environmental sample analysis is..a. To determine the origin and concentration of chemicals in the environmentb. To determine the origin, concentration of chemicals and/or pollutants in the environmentc. To determine the concentration of a chemical in the environmentd. To determine the cause and concentration of pollutants in the environment
4. Gasoline can be reasonably approximated as C9H20 with a density of 0.718 g/mL. Diesel can be reasonable approximated as C14H30 with a density of 0.763 g/mL. (Both gasoline and diesel are complicated mixtures. These formulas are something like weighted averages of the formulas of the different components, where the weighting is based on various quantifiable behaviors. That is, using these artificial formulas for gasoline and diesel allows one to calculate average properties that match what petroleum engineers might measure.) The enthalpy change from burning one mole of gasoline is -6160 kJ. The enthalpy change from burning one mole of diesel is -7940 kJ. Determine which fuel generates the biggest enthalpy change per gram burned, and which generates the biggest enthalpy change per mL burned.
1.) A dense plastic-like shape has a mass of 42.985 g and has a volume of 41.96 mL. What is the density of the substance? 2.) Another plastic-like piece has a mass of 65.389 grams and displaces 53.652 grams of water (measured at 24.6 ⁰C). Is this piece likely to be composed of the same material as the sample in problem 1? Explain using the Claim-Evidence-Reasoning process.
At 20oC 25.0 ml of concentrated nitric acid solution was found to have a mass of 32.503 g. What is the calculated density of this solution at 20oC? Show your calculation set-up and result using correct significant figures and proper units
In the UV assay of paracetamol you are required to weigh tablet powder “…containing 0.150 g of Paracetamol…”. If the stated content of paracetamol per tablet is 500 mg and the weight of 20 tablets is 11.267 g then the amount of paracetamol tablet powder to be weighed is
Please explain me each step with words and show me the formula and the substitution with the units. Then anything that you know can be important that I can learn from the process. Ethylene glycol, commonly used as automobile antifreeze, has a specific gravity of 1.1088 at room temperature. What is the volume of 1.00 kgkg of ethylene glycol? What is the volume of 2.00 lblb of ethylene glycol? A 500 gg sample of mercury and a 360 gg sample of iron are at an initial temperature of 25.0∘C∘C. 250 calcal of heat is applied to each sample. SUBSTANCE SPECIFIC HEAT [cal/(g⋅∘C)][cal/(g⋅∘C)] Iron 0.106 Mercury 0.033 What is the final temperature of mercury sample? Express your answer using two significant figures.
The chlorine content of a pool with a capacity of 1.80×104 L was discovered to be 0.00145% by mass, which is well below the sanitary level of 0.00305%. How much chlorine needs to be added in order for the pool to meet the health regulation standard of 0.00305%? First draw a flowchart, then given that the pool consists of fresh water and chlorine, write the total mass (or alternatively chlorine mass) and fresh water balance equations, and then calculate the mass of chlorine in grams that needs to be added to the pool. Assume that the density of the pool water is the same as that of fresh water (1.00 kg/L), the pool is filled to its rated capacity (1.80×104 L), and that the required chlorine can be added to this capacity.
It is recommended that drinking water contain 1.6ug/ml (parts per million) flouride (F-) for prevention of tooth decay. Consider a reservoir with a depth of 30.0 m and a diameter (diameter = 2 r) of 7.60 x10^4 m. (The volume is pi r^2 h) Calculate the amount of F- in grams that were added to the reservoir to give 1.6 ug/ml. How many grams of sodium flouride NaF, contain this much flouride? Note: NaF ---- Na+ + F- Please explain in depth and an easy to follow step by step process on how to solve. Thanks