IQ4
This intermolecular force is responsible for alcohols having much higher boiling points than alkanes of similar molecular mass.
hydrogen bonding
OH bond and carbon chain is what?
alcohol
200 free points
lets go
If things are going swimmingly for you in the UK, you might exclaim, "Bob's your" this.
uncle
who was in the winning titration team?
Yukai, Finn, AJ
When ethanol is heated with concentrated sulfuric acid at 170°C, this class of organic compounds is produced
alkenes
conditions needed for bromination of alkane
uv light or heat
-200 points
rip
This Australian prime minister disappeared while swimming and was never found.
Harold Holt
What is plasmodium falciparum?
protist (pathogen) that causes malaria
This is the product formed when a primary alcohol undergoes complete oxidation under reflux conditions.
carboxylic acid
what do you get when esterification with butan-1-ol and a twice oxidised dodecan-1-ol
butyl dodecanoate
free 300 points
nice
This prime number is the sum of the first seven primes minus the seventh prime.
41
What was the favourite movie mentioned yesterday?
BRGvengers BRGZfinity war
In this process, yeast converts glucose into ethanol and carbon dioxide under anaerobic conditions
fermentation
what are the top 3 highest priority functional groups in order
carboxylic acid, ester, amide
no points change
lol
Bananas are naturally radioactive because they contain this element.
potassium
translate to english from french:
je ne crois pas que vous avez compris ce que j'ai dit
I don't believe you understood what I said
The hydroxyl (-OH) group in alcohols can form hydrogen bonds, while the carbon chain contributes these intermolecular forces that increase with chain length.
London dispersion forces
what indicator can be used in titration (name one)
brogothymol blue
lose 500
that's unfortunate
This acorn-obsessed critter from the Ice Age films caused a "continental crack-up."
Scrat
A student prepares a buffer by mixing 250.0 mL of 0.200 mol L⁻¹ ethanoic acid (Ka=1.8×10−5K_a = 1.8\times10^{-5}Ka=1.8×10−5) with 250.0 mL of 0.200 mol L⁻¹ sodium ethanoate.
To this buffer, 0.0100 mol of solid sodium hydroxide is added and allowed to dissolve completely.
The resulting solution is then diluted to exactly 1.000 L and analysed using a colorimeter. The absorbance of the ethanoate ion at a particular wavelength is found to be exactly 0.602 in a 1.00 cm cuvette. Under these conditions, the molar absorptivity of the ethanoate ion is 1.50×103 L mol−1cm−11.50\times10^3\ \text{L mol}^{-1}\text{cm}^{-1}1.50×103 L mol−1cm−1.
Assuming all equilibria are established and all solutions behave ideally:
Question (8 marks)
""Determine the pH of the final solution.""
Why this is evil
To solve it, you must realise that:
This looks like a buffer question, but it secretly combines:
pH=4.92