Chem Lab Exam Part 1

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Chemicals of Experiment 4

0.1 M KOH, AgNO3, BaCl3, NaCl, Na2SO4 0.15 M NH3 0.2 M Na2S 0.5 M H2SO4

Materials of Experiment 2

10 mL pipette large paper clips paper weighing cup methanol waste container spatula 600 mL beaker 100 mL beaker 50 mL graduated cylinder thermometer stirring rod metal cylinders

Chemicals of Experiment 5

20 g red cabbage 30 mL pH 7 buffer phenolphthalein indicator 200 mL HCl acid solution 65 mL Ca(OH)2 unknown solution molarity

Chemicals of Experiment 6

275 mL of 1 M NaOH 100 mL of 2 M NaOH 50 mL of 3 M Na OH 175 mL of 1 M HCl 50 mL of 1 M HNO3 50 mL of 2 N H2SO4 150 mL of 3 N H3PO4 50 mL of 1 M NH3

Materials of Experiment 5

50 mL burette 10 mL pipette 75mm filter paper cabbage waste container safety goggles 100 mL beaker two 250 mL beakers 600 mL beaker two 125 mL erlenmeyer flasks 250 mL erlenmeyer flask long steam funnel 10 mL graduated cylinder

Chemicals of Experiment 2

7.5 g sodium hydroxide (NaOH) 10 mL methanol (CH3OH)

Pink; Clear

Phenolphthalein in base is ____ in color; when neutralized, the solution will become ______ in color

Zinc and Copper

Since 1962, the US penny has been made of only...

97.5%; 2.5%

Since 1982 the penny has been made of ____ zinc and ____ copper

Labeled

The axises of a graph should always be appropriately.....

Logger Pro

What is the software program that we have used to make graphs?

Scale

When creating a graph, the ______ chosen should fill as mich of the available space as possible.

Don't

When drawing a line of best fit, _______ force the cureve to pass through each point

Inversely Proportional

When two variables are ___________ ____________, a plot of y verse 1/x will give a straight line.

Same

When weighing something in the lab, it is important to use the ____ balance each time to reduce the amount of error in your measurement

Never

When weighing something on a balance, ____ weigh anything directly on the balance pan; always use a weighing boat or beaker

Neutral

a pH of 7 is...

Line of Best Fit

a smooth line that is drawn on graphs that shows the general trend of the data

Precipitate

a solid that forms and settles out of a liquid mixture

Strong Acids

acids that dissociate almost completely in aqueous solutions; pH 3 or less (HCl, HNO3, H2SO4, H3PO4, HClO4)

Weak Acids

acids that do not completely dissociate in aqueous solutions; pH 3-7 (Fe(NO3)3, FeCl3, ZnSO4, Al2(SO4)3)

Brass

an alloy consisting of essentially copper and zinc in variable proportions

Caustic Soda

another name for NaOH is...

Proportionality Constant

another name for the slope of a line (m) is....

Analytical Balances

balances found near the windows in the lab that measure to 0.1mg or 0.0001g

Metler Balances

balances found on the bench tops in the lab that measure to 1mg or 0.001g

Strong Bases

bases that completely dissociate in aqueous solutions; pH 11 or higher (NH3, KOH, NaOH, Ca(OH)2

Weak Bases

bases that do not completely dissociate in aqueous solutions; pH 7-11 (Na2CO3, Na2S, Na3PO4)

Materials of Experiment 4

clean 3" test tubes

Blue

color of Cu^2+ ion in aqueous solutions

Yellow

color of Fe^2+ ion in aqueous solutions

Green

color of Ni^2+ ion in aqueous solutions

Red

color of the calorimeter used for acids

Blue

color of the calorimeter used for bases

Acids

compounds that increase the concentration of the H+ ion when they dissolve in water

Bases

compounds that increase the concentration of the OH- ion when they dissolve in water

Materials of Experiment 6

computer with LoggerPro and temperature probes 2-50 mL graduated cylinders 250 mL beaker 2 thermos

Goals of Experiment 2

develop weighin and pipetting skills demonstrate items difficult to weigh accurately perform a density calculation

Hand Drawn

for the graph in Part 4 of Experiment 1, the line of best fit was...

D = m/v

formula for calculating density

M1V1 = M2V2

formula for dilution

q = mc∆T

formula for heat

qCal = -(qHot + qCool)

formula for heat of the reaction

pH = -log H+

formula for pH

m = (y2 - y1)/(x2 - x1)

formula for slope

Ccal = qCal/∆T

formula for the calorimeter constant

xy = m

formula for two variable which are inversely proportional

Absolute Uncertainty

instrumental error; instruments and lab equipment have inherent limitations in the accuracy of their measurements

Digital Equipment

lab equipment (electronic balances) that has an absolute uncertainity in measurement of +/- 2 in the last reported decimal

Analog Equipment

lab equipment (graduated cylinders, beakers) that has an absolute uncertainty in a measurement of 1/5 of the smallest division

Calculations Performed in Experiment 6

moles of water produced in each reaction molarity of water ∆T = Tfinal - Tinitial ∆Hneutralization = -(ms∆T + Ccal∆T)

mg/L

ppm =

Goals of Experiment 5

preparation of an acid/base indicator from cabbage gaining practice in acid/base titration technique find the molarity of unknown Calcium Hydroxide solution

Preparation of Indicator from Cabbage

procedure carried out in Part 1 of Experiment 5; involved boiling cabbage, filtering out the solution, and using the solution as a pH indicator

Calibrating the Calorimeter

procedure carried out in Part 1 of Experiment 6; involved mixing hot DI water with room temperature DI water to determine the calorimeter constant

Titration with Phenolphthalein as the Indicator

procedure carried out in Part 2 of Experiment 5; involved the neutralization of Ca(OH)2 by HCl with a stock indicator, using a burette to perform three titrations

Measuring Reaction Temperatures

procedure carried out in Part 2 of Experiment 6; involved mixing various volumes and concentrations of acid and bases to measure the heat for reaction

Titration with Cabbage Indicator

procedure carried out in Part 3 of Experiment 5; involved the neutralization of Ca(OH)2 by HCl with a homemade indicator, using a burette to perform three titrations

Svante Arrhenius

scientist who proposed that certain compounds, commonly known as salts, dissolve in water by dissociating into positive and negative ions

NH3; Na2S

solutions of _____ and ______ in water have characteristic odors

H2S

solutions that contain ____ will produce gas and an odor of rotten eggs

CO3^2-; HCO3^-

solutions that contain _____ or _____ will produce carbon dioxide

Aqueous Solutions

solutions where dissociated ions are bound tightly to neighboring water molecules

Bright Green; Light Blue

the cabbage indicator in base is ________ in color; when neutralized, the solution will become ________ in color

Brown

the color of the nitrogen dioxide given off by the copper blue solution as the penny dissolved

Vertical

the dependent variable is plotted on the ________ axis

y = mx + b

the equation for a linear relationship when the dependent variable does not equal zero when the independent variable does

y = mx

the equation for the simplest form of a straight-line relationship that indicates that two variables are directly proportional

Horizontal

the independent variable is plotted on the _________ axis

Observation and Deduction

the keys to success in Experiment 4 are _____ and _____; must be able to _____ what happens when two reagents are mixed and ____ what ions might be present in the unknown sample

pH vs Volume

the one graph produced in Part 4 of Experiment 1 compared...

67%; 33%

the percent composition of brass is ___ copper and ____ zinc

Relative Uncertainty

the percentage of the absolute uncertainty compared to the measurement

Identification of Five Unknowns

the procedure carried out in Experiment 4; involved testing five compounds (strong acid, strong base, chloride salt, nitrate salt, sodium salt) by creating chemical solutions

Weighing Paper Clips

the procedure carried out in Part 1 of Experiment 2

Weighing high vapor pressure liquid

the procedure carried out in Part 2 of Experiment 2; involved methanol and the Matler balance

Weighing cold and hygroscopic materials

the procedure carried out in Part 3 of Experiment 2; involved NaOH and the Metler balance

Dipensing known volumes of liquid

the procedure carried out in Part 4 of Experiment 2; involved deionized water, pipette, burette, and graduated cylinder

Density determination

the procedure carried out in Part 5 of Experiment 2; involved NaOH and an unknown metal cylinder

Dissolving Pennies to Find PPM Copper

the procedure followed for Part 1 of Experiment 3; involved weighing a penny, dissolving it in Nitric Acid, diluting it in DI water, and using the atomic absorption spectrophotometer

Making Brass Pennies

the procedure followed in Part 2 of Experiment 3; involved weighing two pennies, immersing the pennies in hot 6M NaOH, and then using a bunsen burner

P vs V P vs 1/V V vs 1/P

the three graphs produced in Part 1 of Experiment 1 compared...

Io/I vs concentration log (Io/I) vs concentration

the two graphs produced in Part 2 of Experiment 1 compared...

V vs T 1/V vs T

the two graphs produced in Part 3 of Experiment 1 compared...

Goal of Experiment 6

to see that the amount of heat produced by a reaction depends upon the number of molecules involved

Goals of Experiment 4

use simple observations about the behavior of acids, bases and salts to identify the contents of an unknown solution

95%; 5%

From 1962 until 1982, a penny was ____ copper and ____ zinc

Origin

If the value of the dependent variable is zero when the value of the independent variable is also zero, the graph must pass through the...

Goal of Experiment 3

Measuring composition of alloys

262 mg/m^3

Methanol TLV =

2 mg/m^3

NaOH TLV =


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