Question 1 The simplest carboxylic acid is methanoic acid (or formic acid), HCOOH, which occurs naturally in ants. When an ant bites, it injects an aqueous solution of 50% (by volume) methanoic acid, typically injecting around 6.0 × 10-3 mL of this solution. a) For each sting, the ant does not inject all of its methanoic acid but keeps a little in reserve. Assuming that a typical ant injects 80% of its methanoic acid, what is the total volume of pure methanoic acid contained in a ‘typical ant’? b) How many ‘typical’ ants would have to be distilled to produce 1 L of pure methanoic acid? Sodium hydrogencarbonate, NaHCO3, is often used to treat ant stings. The reaction between methanoic acid and sodium hydrogencarbonate is: HCOOH + NaHCO3 → HCOO- + Na+ + H2O + CO2 c) Given that the density of methanoic acid is 1.2 g mL-1 , how many moles of methanoic acid does a typical ant inject?
Question 1 The simplest carboxylic acid is methanoic acid (or formic acid), HCOOH, which occurs naturally in ants. When an ant bites, it injects an aqueous solution of 50% (by volume) methanoic acid, typically injecting around 6.0 × 10-3 mL of this solution. a) For each sting, the ant does not inject all of its methanoic acid but keeps a little in reserve. Assuming that a typical ant injects 80% of its methanoic acid, what is the total volume of pure methanoic acid contained in a ‘typical ant’? b) How many ‘typical’ ants would have to be distilled to produce 1 L of pure methanoic acid? Sodium hydrogencarbonate, NaHCO3, is often used to treat ant stings. The reaction between methanoic acid and sodium hydrogencarbonate is: HCOOH + NaHCO3 → HCOO- + Na+ + H2O + CO2 c) Given that the density of methanoic acid is 1.2 g mL-1 , how many moles of methanoic acid does a typical ant inject?
Question 1 The simplest carboxylic acid is methanoic acid (or formic acid), HCOOH, which occurs naturally in ants. When an ant bites, it injects an aqueous solution of 50% (by volume) methanoic acid, typically injecting around 6.0 × 10-3 mL of this solution. a) For each sting, the ant does not inject all of its methanoic acid but keeps a little in reserve. Assuming that a typical ant injects 80% of its methanoic acid, what is the total volume of pure methanoic acid contained in a ‘typical ant’? b) How many ‘typical’ ants would have to be distilled to produce 1 L of pure methanoic acid? Sodium hydrogencarbonate, NaHCO3, is often used to treat ant stings. The reaction between methanoic acid and sodium hydrogencarbonate is: HCOOH + NaHCO3 → HCOO- + Na+ + H2O + CO2 c) Given that the density of methanoic acid is 1.2 g mL-1 , how many moles of methanoic acid does a typical ant inject?
Question 1 The simplest carboxylic acid is methanoic acid (or formic acid), HCOOH, which occurs naturally in ants. When an ant bites, it injects an aqueous solution of 50% (by volume) methanoic acid, typically injecting around 6.0 × 10-3 mL of this solution. a) For each sting, the ant does not inject all of its methanoic acid but keeps a little in reserve. Assuming that a typical ant injects 80% of its methanoic acid, what is the total volume of pure methanoic acid contained in a ‘typical ant’? b) How many ‘typical’ ants would have to be distilled to produce 1 L of pure methanoic acid? Sodium hydrogencarbonate, NaHCO3, is often used to treat ant stings. The reaction between methanoic acid and sodium hydrogencarbonate is: HCOOH + NaHCO3 → HCOO- + Na+ + H2O + CO2 c) Given that the density of methanoic acid is 1.2 g mL-1 , how many moles of methanoic acid does a typical ant inject? d) What mass (g) of sodium hydrogencarbonate would be required to completely neutralise a typical ant sting?
Transcribed Image Text:Question 2
Sherbet lemons are sweets which consist of a flavoured sugar (sucrose, C12H22O11) shell filled
with sherbet. The sherbet contains sodium hydrogencarbonate, NaHCO3 and tartaric acid (2,3-
dihydroxybutanedioic acid):
a) Write an equation for the complete combustion of sucrose in excess oxygen, which gives
carbon dioxide and water.
H₂C₂H4O6 + 2NaHCO3
Sodium
Bicarbonate
Tartaric Acid
b) The standard enthalpy change of combustion (i.e. the heat change) of sucrose is -5644 kJ
mol-¹. Calculate the energy released when one sweet containing 6.70 g of sucrose is completely
burnt.
c) A man needs to consume about 2500 dietary calories (i.e. 2500 kcal) per day. Given that 1 kJ
= 0.239 kcal, how many sweets would a man have to consume in order to meet his daily
calorific requirement?
Sherbet produces a fizzing sensation in the mouth when its two main components, tartaric acid
and sodium hydrogencarbonate, react together in aqueous solution to make carbon dioxide gas.
The reaction is given below:
a)
b)
In a laboratory experiment, one sherbet lemon sweet produced 6.00 mL of carbon dioxide.
d) Calculate the minimum mass (g) of tartaric acid necessary to produce this 6.00 mL volume of
carbon dioxide. (Assume that 1 mole of carbon dioxide occupies 24.0 L at room temperature
and pressure).
c)
e) By making the appropriate substitutions for tartaric acid's H (hydrogen) and OH (hydroxyl)
groups among positions A, B, D and E in the structure shown below, how many different
stereoisomers of tartaric acid are possible?
e)
Question 3
Name the following organic compounds:
HO
(b)
T
H
Question 4
HO₂C
HO
f) Citric acid, sometimes used to flavour sherbet lemons, has a condensed formula that may be
written as:
How many single C-O bonds does a citric acid molecule contain'?
Question 5
0.0
2.0
H
H₂C
Η Ο
4.0
6.0
8.0
10.0
Tartaric acid
12.0
CH₂CI
OH
HH
H-C-C-0-C-C-H
HO₂C
B
II
HH
Concentration of Glucose/mmol L-¹
A
Na₂C4H406 + 2H₂O +
Water
Sodium
Tartarate
HOOC-CH2-C(OH)(COOH)-CH2-COOH
Use Markovnikov's Rule to predict the organic products of the following reactions:
(a)
CO₂H
OH
H
For your answers provide the correct systematic IUPAC names.
+
An analyst was told to determine the amount of glucose in blood using a colorimetric method.
The analyst prepared a series of standards containing known amounts of glucose and obtained
the results given in the table below by UV/visible spectroscopy.
0.11
E
0.25
0.45
CO₂H
0.63
D
0.87
Absorbance
1.05
1.24
2002
Carbon
Dioxide
H-CI
Use the data in the table to plot a graph of absorbance against glucose concentration.
a) Is Beer's Law obeyed?
b) From the best fit line, calculate the molar absorptivity, &, and its units.
c) If a urine sample has absorbance = 0.53, use your graph (not any individual data
points) to determine its glucose concentration.
Definition Definition Class of organic compounds that contain a carboxyl group ( - COOH ) and has a general formula R - COOH or R - CO 2 H , where R refers to the alkyl, alkenyl, aryl, or other groups. They can undergo different chemical reactions, such as acid-base reactions, esterification, and oxidation. These are essential components of living organisms, playing important roles in metabolic processes, signaling, and as pharmaceuticals.
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