Unit Test 1 Flashcards
Accuracy
How closely a measured value agrees with the True(Reference) value.
Precision
How closely measurements agree with each other - more DPs more precise
How to fix Random Errors?
More Trials/Increase Sample Size/More Precise Device
How to Average Values with Uncerts.
Avg of Measurements + Avg of Uncerts.
Giga/Mega/Kilo/Deci/Centi/Milli/Micro/Nano
9/6/3/-1/-2/-3/-6/-9
Discrete Data
Points can be joined - plotted as bar chart
Continuous Data
Best fit line can connect data
Coefficient R
+1/Perfect Positive Linear
0/No Linear Trend
-1/Perfect Negative Linear
Error Propaagation
Slope Uncert.
Tangent
Drawn as Large as possible to minimize uncert.
Interpolation
Assume Pattern applies between points
Extrapolation
Extend Trend Beyond Measurement Range
Matter
Mass and Volume
Pure Substances
Element or Compound - (Ionic or Molecular)
Mixtures
Solutions(Steel and Brass) or Suspensions(Blood) or Mechanical
Extensive Property
Depends on Amount - Mass, Volume
Intensive Property
Depends of Nature - Density, Melting Point
Distillation
For liquid-liquid Solutions - Based on Melting Point
Gas Distilled called Distillate
Solvent Extraction
Separating Solid-Solid or Liquid-Liquid mixtures - different solubilities
Gravity Seperation
Based on Density - Centrifuge
Paper/Column Chromatography
Pen-Ink Colour Separation
1. Stationary Phase
2. Mobile Phase
3. Developing Solvent
Rule for Naming Hydrates
Name as Normal - add (prefix) hydrate
Rule for Naming Acids
Binary Acids: Hydro___ic Acid
Polyatomic Ions: ate-ic ite-ous
Laws for Chemical Reactions
Law of Conservation of Mass/Energy/Electrical Charge/Atoms
Neutralization Reaction
Hx + mOH -> H20 + mx
Combustion
CxHyOz + O2 -> CO2 + H2O
Carbonate Reactions
Hx + mCO3 -> H2O + CO2 + mx
Activity Series Gas
F
Cl
Br
I
(As Listed)
Empirical Formula (Provides Ratio) Procedure
- % to grams
- grams to moles
- divide by smallest
Percentage Composition Procedure
Molar Mass/Total Molar Mass
Molecular Formula Procedure
Empirical Formula First
1. Obtain Multiplier - Molar Mass of Compound/Empirical Molar Mass
How to obtain Density from Molarity?
Density = Molarity times Molar Mass
Molarity Procedure
Total Moles/Total Volume (L)
Dilution Procedure
m1v2 = m2v2
Charles’s Law
Volume is proportional to Temperature
Gay-Lussac’s Law
Pressure is proportional to Temperature
Combined Gas Law
P1V1/T1 = P2V2/T2
Ideal Gas Law Conditions
Pressure - Pa
Volume - m^3
Temperature - Kelvins
R - Gas Constant - 8.31
*K = C + 273.15
1 atm = 101.325kPa
1 bar = 100kPa
*kPa(dm^3) = Pa(m^3)
STP Conditions
Temperature - 273K - 0C
Pressure - 100 kPa - 1 bar
Ideal Gas Law vs Combined Gas Law?
Combined Gas Law - Changing Conditions
Ideal Gas Law - Same Gas, Solving for Unknown
Limiting/Excess Procedure
*Get How much excess left - use reagent side stoich
Use all given with stoich to convert to specified/chosen product - least product produced is LIMITING
Percentage Yield
Actual(Experiment)/Theory
Percent Purity
Pure Amount/Total Amount
Titration Setup
Base (Titrant) on top (In Burette with high precision - 2 dp)
Acid with Indicator on bottom
What is a Primary Standard and what to do with it?
Chemicals that are stable, pure, and non-hygroscopic (does not absorb water)
- Titrate the Titrant
- Use known Molarity for Actual Titration
