day 1 acid-base. review of naming acids determine name: h 2 so 3 h 2 so 4 h 2 s hclo 3 hcl hclo 2
DESCRIPTION
Determine Name: H 2 SO 3 H 2 SO 4 H 2 S HClO 3 HCl HClO 2TRANSCRIPT
Day 1Acid-Base
Review of naming acids
Determine Name: H2SO3
H2SO4
H2S
HClO3
HCl
HClO2
Determine Name: H2SO3
H2SO4
H2S
HClO3
HCl
HClO2
Determine Formula
Hydrofluoric acid
Carbonic acid
Nitrous acid
Hydroselenic acid
Determine Formula
Hydrofluoric acid HFCarbonic acid
Nitrous acid
Hydroselenic acid
Characteristics of Acids & Bases
Acids are Characterized by:
OSour tasteO color of indicator ORelease of H2 gasOReacts with bases salt( ionic
compound) & H2O
Bases are Characterized by:
OBitter tasteOFeels slipperyO color of indicator OReacts with acid salt( ionic
compound) & H2OOConducts electric current ( its
an ionic compound)
What does ionization mean?
Ionization OAdding or removing
electrons (e-)OMaking a cation or anion
Strong AcidsOIonizes completely = breaks
up completely OConducts electric current
(remember electrolyte demo & PhET)
Strong AcidsExamples:
OHydrochloric Acid (HCl)
OSulfuric Acid (H2SO4) ONitric Acid (HNO3)
Strong BaseOIonizes completely = breaks up
completely OExamples: group 1 hydroxides –
sodium hydroxide, potassium hydroxide, etc.
Neutralization Reaction HCl + NaOH NaCl + HOHStrong + Strong Salt + Water Acid BaseHNO3 + KOH KNO3 + HOH
Neutralization ReactionIs a double replacement rxn b/w …
strong acid + strong base a salt (ionic compound) + water
pH ScaleDetermining strength of an Acid
or Base
pH scale 0-14 Oneutral pH = 7.0
Oacidic pH <7.0
Obasic pH > 7.0
pH Scale
Calculating pH & [H+]
pH = -log[H+]Inverse of log10 is 10^( )
[H+] = 10^(-pH)
Calculating pOH & [OH-]
pH = -log[OH-]Inverse of log10 is 10^( )
[OH-] = 10^(-pOH)
Relationship between pH & pOH
pH + pOH = 14
Now you try…
Answer
Try on your own…
Try on your own…
Practice
Now you try
Answer
Try on your own..
Answers
Other methods of determining pH
If molarity is not known, pH can be determined by…
OAcid-Base Indicators
OpH meterOTitration
Indicator SolutionsOChange color
depending on pH of test solution
Indicators
Indicators
Indicators
Problems with indicator solutions:
OIf you have a colored solution
OApprox pH value not exact
OTemperature affects color
pH meter
pH meter Oconsists of a measuring probe Oelectronic meter: measures &
displays the pH readingOhave to calibrate probe
TitrationOUse Buret, Erlenmeyer flask,
indicatorOUse M1V1 = M2V2 to determine
molarity of unknown
Titration
Titration
Answer the following questions while watching the video clips: 1. Where do you read/How do you read a
burette? 2. What hand do you use to swirl the
Erlenmeyer flask? 3. What hand do use to adjust the burette? 4. When do you know you are getting close to
the endpoint? 5. How is the standard solution added as you
get close to the endpoint? 6. When do you know you have achieved the
endpoint?
OTitration Video Clip #1 (3:15)
OTitration Video Clip # 2 ( 6:07)
Now, do the titration pre-lab