Q1 In redox titration involving potassium permanganate, if the contents of the conical flask turn brown, it means _____was added
Insufficient acid catalyst
Insufficient base catalyst
Insufficient catalyst
all of the above
Q2 Potassium permanganate is a self-indicating reagent because of its different characteristic _______ in either the acidic or basic medium
Colour change
Colour stability
solubility
oxidation state
Q3 Potassium permanganate can be used to estimate the ________of a substance
Valency
water of hydration
reactivity
percentage purity
Q4 IO$${_3}{^2-}$$ + SO$${_3}{^2+}$$ ­­�?? I +SO$${_4}{^2-}$$ The oxidation state of oxygen in the product�??s equation is______
+3
+6
-3
+6
Q5 IO$${_3}{^2-}$$ + SO{_3}{^2}$$+ the oxidation state of oxygen in the equation is ______
-2
-4
+4
+2
Q6 A substance which loses water of hydration upon exposure to atmosphere is called?
Deliquescent substance
Efflorescence substance
Anhydrous substance
Hygroscopic substance
Q7 Volumetric analysis involving iodine are usually referred to as___________
iodotitration
iodine acid titration
halogenmetry
iodometry
Q8 In the _____, standard solutions of iodine are used to estimate directly the concentrations of some oxidizable species.
Direct method
indirect method
standard method
calibrated method
Q9 Of all the oxidizable species available for use, iodine titration are usually used with the___
sulphate ions
Thiopsulphate
hydrogensulphate
thioesters
Q10 The colour changes accompanying the varying change in oxidation states of iodine and its ion can be used to indicate the________
Iodine complxity
iniyial point
end point
all of the above
Q11 The most commonly used external indicator for iodine titration is_________
Glucose solution
hydrogen chloride
Protein solution
starch solution
Q12 The starch solution forms a _______complex with the tri-iodide ion during the titration that is rapidly discharge at the end point
Light blue
Blue
Blue black
Brick red
Q13 Thus using starch as indicator, the colour variations of the solution depend on ______formation of the starch with iodide ion formed in the last stage of the titration.
Complex
Coloid
Hydrolysed
non of the above
Q14 For this reason and in order to avoid complications in the end point detection, the starch indicator is added at the______ colouration of the solution which is near the end point
Yellow
Light yellow
Colourless
Dark yellow
Q15 Complete the colour change in iodometry analysis. _______(initially)�??
Red-orange
Dark-brown
Brown
Red-brown
Q16 Light yellow colouration is observed at near end point of the iodometry analysis. True or false___
True
False
Partially true
Indifferent
Q17 During iodometry analysis the blue black colouration appear at the end of the titration. True or false_____
True
False
Partially true
Indifferent
Q18 The oxidation potentials of Na is________
11
23
271
2.71
Q19 The study of thermal changes in chemical and physical processes is known as________
thermochemistry
Thermodynamics
A and B
B only
Q20 The _________is the amount of heat released or observed for a given amount of reactants or products
heat of reaction
heat of combustion
heat of neutralization
heat of formation
Q21 Predict the colour of methyl orange when $$p{^H}$$ is 8?
Pink
Orange
Yellow
Blue
Q22 At complete neutralization point, the litmus paper colour turns?
Yellow
Red
Blue
Purple
Q23 At neutralization point the $$P{^H}$$ value is?
seven
zero
fourteen
one
Q24 What is a $$P{^H}$$ of a solution?
It is the measure of base concentration in the solution
It is the measure of hydrogen ions concentration in the solution
It is the measure of acid concentration in the solution
It is the measure of hydroxyl ions concentration in the solution
Q25 In an acid base titration conducted by a student the colour of the solution in the beaker changed from colourless to pink when phenolphthalein was used as an indicator, what went wrong?
The base was stronger than the acid
The acid base ions are at equilibrium
The beaker was occupied by acid solution instead of base.
The titration time was overdue
Q26 Which of the following options is an indicator use for acid-base titration?
Methylbenzene
Bromohexane
phenol
Methyl orange
Q27 The point at which stoicheometrically equivalent quantities of substance have been brought together is known as?
Equivalence point of titration
Saturated point of titration
End point of titration
Neutralization point of titration
Q28 The concentration of pure HCl 11.7 Molar if $$20 cm{^3}$$ of the acid is diluted to $$250 cm{^3}$$ to give concentration of $$0.936 mol.dm{^3}$$ substitute this values on this equation; CIVI=C2V2?
12.636 X 270 = C1 X 20
11.7 X 20 = 0.936 X 250
0.936 X 250 = 11.7 X 20
11.7 X 250 = 0.936 X 20
Q29 Give reason why water should not be added to acid during carrying out acid-base titration?
The procedure can cause explosion
The acid is hygroscopic and will cause explosion when added to water
The dissolution of acid in water is exothermic which may cause explosion
The acid is corrosive and can destroy the glass ware
Q30 A table of requirement for laboratory experiment contains the following except?
Quantity of apparatus
List of apparatus
List of chemicals
List of weight of each reagents
Q31 A substance which takes in only moisture upon exposure to atmosphere is refer to as?
Deliquescence substance
Anhydrous substance
Efflorescence substance
Hygroscopic substance
Q32 A substance which loses water of hydration upon exposure to atmosphere is called?
Deliquescent substance
Efflorescence substance
Anhydrous substance
Hygroscopic substance
Q33 If 2 cm3 of a stoke solution contains 1 mole of an acid how would you prepare 1 molar concentration of that acid in 250 cm3 of water?
Dissolve $$2 cm{^3}$$ of the stoke solution in 250 cm3 of water
Dissolve $$1 cm{^3}$$ of the stoke solution in $$250 cm{^3}$$ of water
Dissolve $$2 cm{^3}$$ of the stoke solution in $$248 cm{^3}$$ of water
Dissolve $$1 cm{^3}$$ of the stoke solution in $$249 cm{^3}$$ of water
Q34 In a chemistry laboratory a stoke bottle of acid solution reads, �??1.25 specific gravity�?�; what does that mean?
It means $$100 cm{^3}$$ of that solution weight 12500 g
It means $$1 cm{^3}$$ of that solution weight 1250 g
It means $$1 cm{^3}$$ of the weight 125 g
$$1 cm{^3}$$ of that solution weight 1.25 g
Q35 A solution contains 1.2 Molar concentration, what volume of it must be diluted with water to give 600 mls of 0.5 Molar solution?
25 mls
300 mls
600 mls
575 mls
Q36 In preparing a standard solution, two factors must be considered?
1. The solute must be solid and 2. the solvent must be liquid
1.The solute must be pure and 2. a suitable solvent be measured todefinite volume
1.The solvent must be water and 2. the solute must be crystal form
1.The solute�??s nature must be known and 2. the solvent can be unknown
Q37 Define standard solution?
A solution of which the concentration is partially known
Concentration which has 1 mol dissolved in 1 dm3 of solvent
A solution of which the concentration is accurately known
A solution containing a pure substance dissolve in a known volume of solvent
Q38 What is the w/v percentage concentration of 300ml of NaCl(aq) containing 5 g NaCl?
$$1.66 % w/v$$
$$305 % w/v$$
$$150 % w/v$$
$$60 % w/v$$
Q39 Calculate the mass of NaCl in 450 g of NaCl solution containing NaCl w/w %?
485 g
450 g
35 g
157.5 g
Q40 What is the percentage w/w % ethanol if 5 g of ethanol is dissolved in 20 g of water?
$$72 % w/w$$
$$20 % w/w$$
$$5 % w/w$$
$$25 % w/w$$
Q41 One of the disadvantages of acid-base titration is?
Large quantity of the sample(s) is required
Takes longer time for reaction to start
The acid need to be handled with care
Requires careful attention to reach end point accurately
Q42 All are advantages of acid base titration except?
Simple to do
Less accuracy and precision
Cost effective
Do not need high expertise
Q43 The equation NaOH + HCl $$�??$$NaCl + H2O is a ____?
Acid base reaction
Oxidation reaction
Neutralization reaction
Reduction reaction
Q44 When performing acid-base titration, one should first?
Rinse the burette twice with acid solution
Fill the burette twice with acid solution
Fill the burette twice with base solution
Rinse the burette twice with base solution
Q45 Which of these is a method of finding the equivalence point?
PH indicator
Amperometry
Thermometric titrametry
All of the above
Q46 What is a titrant in titration analysis?
Unknown concentration and volume of an analyte
Known concentration and volume of an analyte
Partially unknown concentration and volume of acid
Partially known concentration and volume of an analyte
Q47 What is a titrand in titration analysis?
Known concentration of an analyte
Partially known concentration of an analyte
Partially unknown concentration of acid
Unknown concentration of an analyte
Q48 During acid-base titration sulphuric acid would be dissociated into what ions?
$$H{^+} + SO{_4}$$
$$H{^-} + SO{_4}{^-}$$
$$2H{^+} + SO{_4}{^-}$$
$$H{_2} + SO{_4}$$
Q49 Both molarity and normality are measures of concentration. True or false?
True
Partially true
false
Indifferent
Q50 Choose the most suitable water for use in acid base titration?
Distilled water
Deionised water
Temporary hard water
Permanent hard water
Q51 A student used a hard tap water and performed and acid base titration. In few lines explain what would happen to his result?
The starting solution would be more acidic as such it would consume more base to achieve the equivalence point
the student cannot get an equivalence point owing to the fact that tap water was used not distilled water
The solution would require more of indicator at the beginning of the experiment
the starting solution would be more alkaline therefore it would require more volume of acid than expected
Q52 A 25 ml solution of 0.5 M NaOH is titrated until neutralized into a 50 ml sample of HCl?
50 mol
0.125 mol
0.25 mol
0.5 mol
Q53 What is the importance of back titration?
To determine the concentration of a substance that is in excess after a chemical reaction.
To determine the base in excess.
To determine the acid in excess.
To determine the average value of acid base titration.
Q54 What is the implication of adding a phenolphthalein as an indicator during the titration of HCl against Na2CO3?
The end point will appear when only half of Na2CO3 has been used
The end point will appear at the first drop of the acid.
The end point will appear when half of the HCl has been used.
The indicator will be sensitive to the acid alone
Q55 Which of these indicators will be suitable for use in titration involving a weak acid and a strong base?
Any indicator
Phenolphthalein
Methyl orange
No suitable indicator
Q56 What type of indicator will be suitable for use in a titration involving H2SO4 + NH3(ag)?
Phenolphthalein
Methyl orange
Any indicator
No suitable indicator
Q57 An example of a strong acid is?
$$H{_2}SO{_3}$$
$$CH{_3}COOH$$
$$H{_2}C{_2}O{_4}$$
$$H{_2}SO{_4}$$
Q58 What is a strong acid?
Any acid that ionizes completely in solution
Any acid which turns blue litmus paper red
Any acid that is highly corrosive and can cause burn to the skin
Any acid whose pH is less than 3
Q59 An indicator X was added to an acid solution in a beaker but no colour change was observed give the name of the indicator X?
Methyl orange
Bromothymol
Phenolphthalein
Litmus paper
Q60 What is the colour of bromothymol when added to an acid solution?
Blue
Red
Yellow
Colourless
Q61 The unit µg is equivalent to?
$$10{^-3}$$ Kg
$$10{^-6}$$ Kg
$$10{^-12}$$ Kg
$$10{^-9}$$ Kg
Q62 When filtration is carried out under reduced pressure is called?
Pressure filtration
Simple filtration
Ordinary filtration
Suction filtration
Q63 The unit of a volume express in $$dm{^3}$$ is equivalent to?
1 litre or 100 ml
$$10{^3}$$ cm or 1 litre
100 $$cm{^3}$$ or 1 litre
1000 ml or 10 litre
Q64 Define precipitation in respect to wet chemical analysis?
A method of converting ions in solution into an insoluble compound
The process of separating solid (crystals or precipitate) from the liquid (mother liquor)
A method of reducing the volume of by heating
A method of converting water vapour in to liquid water
Q65 What is a mole?
The amount of substance which contains as many element as there are atoms in 12 g carbon 12
The amount of substance which is contain in a solution
The amount of substance equivalent to carbon 12 atom present in a solution
All the options are correct
Q66 Why do we heat precipitates during gravimetric analysis?
To obtain a compound of constant composition
To increase the solubility of the precipitates
To dry the precipitates
To speed the reaction rate of the precipitates
Q67 The Avogadro number $$6.02 X 10{^23}$$ is equivalent to?
Number of atoms, ions or molecules in a mole
Number of mole of an atom equivalent to carbon atom
Number of elementary units in a mole of a substance
All options above are correct
Q68 Choose from the list of chemicals given and determine which has negative effect on skin?
Tetraoxosulphate(VI)and hydrogensulphide
Esters and ethanols
Benzene and benzoylchloride
Phenols and hydrogenfloride
Q69 Calculate the molar mass of 1 mole of a pure substance weighting X g?
M=2X g $$mol{^-1}$$
M=1/X g $$mol{^-1}$$
M=X g $$mol{^-1}$$
M=1 g $$mol{^-1}$$
Q70 Which of these hazardous chemicals are likely to cause dizziness and are carcinogenic?
Ethanol
benzene
Silvernitrate
Phenol
Q71 Calculate the mass of 0.5 moles of water?
9.408 g
18.016 g
18.071 g
4.504 g
Q72 The hazardous effect of chlorinated alkanes is?
Highly oxidizing
irritant
Skin burns
Causes mental confusion
Q73 Calculate the number of moles in 24 g of oxygen gas?
281 mol
265 mol
7.8 mol
3.8 mol
Q74 All are laboratory safety tips except?
Wearing lab coat or apron
Close all windows and doors
Never work alone in the laboratory
Be familiar with the position of some safety equipment
Q75 Calculate the molar mass of a pure substance if 2 moles of the substance has a mass of 35 g?
17.5 $$g mol{^-1}$$
70 g $$mol{^-1}$$
35 g $$mol{^-1}$$
37 g $$mol{^-1}$$
Q76 Qualitative analysis helps in determining what in a given solution?
How long it will take for reactant to react to form products
How much of a component is present in that solution
The quantity of the solvent required to form solution with the component
What type of component is present in that solution
Q77 Define molality of a solution?
Weight in grams of a substance per formula weight in kilograms of that substance
The number of moles of solute per $$dm{^3}$$ of a solution
The number of moles of solute in one kilogram of solution
Moles of solute per volume of solution express in litre
Q78 Quantitative methods help in determining what in a solution?
How much of a component is present in the solution
What type of component is present in a solution
The quantity of a solvent required to form a solution with the component
How long will take for reactant to react in order to form products
Q79 Normality can be defined as?
Moles of solute in 1 $$dm{^3}$$ of solution
Weight in gram of a substance per formula weight in kilo gram of substance
Number of gram equivalent weight of a solute in one litre of solution
All the options are correct
Q80 The various method of quantitative analysis include?
Acid �??base titration and Oxidative analysis
Gravimetric, spectrophotometric and volumetric methods
Titration, Gravimetric, and Volumetric
Spectrophotometric, Oxidative and Neutralization methods
FOR YOUR LATEST CHM191 TMA SOLUTIONS as well as PAST QUESTIONS AND ANSWERS CONTACT 08039407882 on whatsapp.
YOU CAN NOW GET YOUR EXAM SUMMARY FOR ALL YOU E-EXAMS FROM US.
What is exam summary? Click here to learn more.

Q1 In redox titration involving potassium permanganate, if the contents of the conical flask turn brown, it means _____was added
Insufficient acid catalyst
Insufficient base catalyst
Insufficient catalyst
all of the above
Q2 Potassium permanganate is a self-indicating reagent because of its different characteristic _______ in either the acidic or basic medium
Colour change
Colour stability
solubility
oxidation state
Q3 Potassium permanganate can be used to estimate the ________of a substance
Valency
water of hydration
reactivity
percentage purity
Q4 IO$${_3}{^2-}$$ + SO$${_3}{^2+}$$ ­­�?? I +SO$${_4}{^2-}$$ The oxidation state of oxygen in the product�??s equation is______
+3
+6
-3
+6
Q5 IO$${_3}{^2-}$$ + SO{_3}{^2}$$+ the oxidation state of oxygen in the equation is ______
-2
-4
+4
+2
Q6 A substance which loses water of hydration upon exposure to atmosphere is called?
Deliquescent substance
Efflorescence substance
Anhydrous substance
Hygroscopic substance
Q7 Volumetric analysis involving iodine are usually referred to as___________
iodotitration
iodine acid titration
halogenmetry
iodometry
Q8 In the _____, standard solutions of iodine are used to estimate directly the concentrations of some oxidizable species.
Direct method
indirect method
standard method
calibrated method
Q9 Of all the oxidizable species available for use, iodine titration are usually used with the___
sulphate ions
Thiopsulphate
hydrogensulphate
thioesters
Q10 The colour changes accompanying the varying change in oxidation states of iodine and its ion can be used to indicate the________
Iodine complxity
iniyial point
end point
all of the above
Q11 The most commonly used external indicator for iodine titration is_________
Glucose solution
hydrogen chloride
Protein solution
starch solution
Q12 The starch solution forms a _______complex with the tri-iodide ion during the titration that is rapidly discharge at the end point
Light blue
Blue
Blue black
Brick red
Q13 Thus using starch as indicator, the colour variations of the solution depend on ______formation of the starch with iodide ion formed in the last stage of the titration.
Complex
Coloid
Hydrolysed
non of the above
Q14 For this reason and in order to avoid complications in the end point detection, the starch indicator is added at the______ colouration of the solution which is near the end point
Yellow
Light yellow
Colourless
Dark yellow
Q15 Complete the colour change in iodometry analysis. _______(initially)�??
Red-orange
Dark-brown
Brown
Red-brown
Q16 Light yellow colouration is observed at near end point of the iodometry analysis. True or false___
True
False
Partially true
Indifferent
Q17 During iodometry analysis the blue black colouration appear at the end of the titration. True or false_____
True
False
Partially true
Indifferent
Q18 The oxidation potentials of Na is________
11
23
271
2.71
Q19 The study of thermal changes in chemical and physical processes is known as________
thermochemistry
Thermodynamics
A and B
B only
Q20 The _________is the amount of heat released or observed for a given amount of reactants or products
heat of reaction
heat of combustion
heat of neutralization
heat of formation
Q21 Predict the colour of methyl orange when $$p{^H}$$ is 8?
Pink
Orange
Yellow
Blue
Q22 At complete neutralization point, the litmus paper colour turns?
Yellow
Red
Blue
Purple
Q23 At neutralization point the $$P{^H}$$ value is?
seven
zero
fourteen
one
Q24 What is a $$P{^H}$$ of a solution?
It is the measure of base concentration in the solution
It is the measure of hydrogen ions concentration in the solution
It is the measure of acid concentration in the solution
It is the measure of hydroxyl ions concentration in the solution
Q25 In an acid base titration conducted by a student the colour of the solution in the beaker changed from colourless to pink when phenolphthalein was used as an indicator, what went wrong?
The base was stronger than the acid
The acid base ions are at equilibrium
The beaker was occupied by acid solution instead of base.
The titration time was overdue
Q26 Which of the following options is an indicator use for acid-base titration?
Methylbenzene
Bromohexane
phenol
Methyl orange
Q27 The point at which stoicheometrically equivalent quantities of substance have been brought together is known as?
Equivalence point of titration
Saturated point of titration
End point of titration
Neutralization point of titration
Q28 The concentration of pure HCl 11.7 Molar if $$20 cm{^3}$$ of the acid is diluted to $$250 cm{^3}$$ to give concentration of $$0.936 mol.dm{^3}$$ substitute this values on this equation; CIVI=C2V2?
12.636 X 270 = C1 X 20
11.7 X 20 = 0.936 X 250
0.936 X 250 = 11.7 X 20
11.7 X 250 = 0.936 X 20
Q29 Give reason why water should not be added to acid during carrying out acid-base titration?
The procedure can cause explosion
The acid is hygroscopic and will cause explosion when added to water
The dissolution of acid in water is exothermic which may cause explosion
The acid is corrosive and can destroy the glass ware
Q30 A table of requirement for laboratory experiment contains the following except?
Quantity of apparatus
List of apparatus
List of chemicals
List of weight of each reagents
Q31 A substance which takes in only moisture upon exposure to atmosphere is refer to as?
Deliquescence substance
Anhydrous substance
Efflorescence substance
Hygroscopic substance
Q32 A substance which loses water of hydration upon exposure to atmosphere is called?
Deliquescent substance
Efflorescence substance
Anhydrous substance
Hygroscopic substance
Q33 If 2 cm3 of a stoke solution contains 1 mole of an acid how would you prepare 1 molar concentration of that acid in 250 cm3 of water?
Dissolve $$2 cm{^3}$$ of the stoke solution in 250 cm3 of water
Dissolve $$1 cm{^3}$$ of the stoke solution in $$250 cm{^3}$$ of water
Dissolve $$2 cm{^3}$$ of the stoke solution in $$248 cm{^3}$$ of water
Dissolve $$1 cm{^3}$$ of the stoke solution in $$249 cm{^3}$$ of water
Q34 In a chemistry laboratory a stoke bottle of acid solution reads, �??1.25 specific gravity�?�; what does that mean?
It means $$100 cm{^3}$$ of that solution weight 12500 g
It means $$1 cm{^3}$$ of that solution weight 1250 g
It means $$1 cm{^3}$$ of the weight 125 g
$$1 cm{^3}$$ of that solution weight 1.25 g
Q35 A solution contains 1.2 Molar concentration, what volume of it must be diluted with water to give 600 mls of 0.5 Molar solution?
25 mls
300 mls
600 mls
575 mls
Q36 In preparing a standard solution, two factors must be considered?
1. The solute must be solid and 2. the solvent must be liquid
1.The solute must be pure and 2. a suitable solvent be measured todefinite volume
1.The solvent must be water and 2. the solute must be crystal form
1.The solute�??s nature must be known and 2. the solvent can be unknown
Q37 Define standard solution?
A solution of which the concentration is partially known
Concentration which has 1 mol dissolved in 1 dm3 of solvent
A solution of which the concentration is accurately known
A solution containing a pure substance dissolve in a known volume of solvent
Q38 What is the w/v percentage concentration of 300ml of NaCl(aq) containing 5 g NaCl?
$$1.66 % w/v$$
$$305 % w/v$$
$$150 % w/v$$
$$60 % w/v$$
Q39 Calculate the mass of NaCl in 450 g of NaCl solution containing NaCl w/w %?
485 g
450 g
35 g
157.5 g
Q40 What is the percentage w/w % ethanol if 5 g of ethanol is dissolved in 20 g of water?
$$72 % w/w$$
$$20 % w/w$$
$$5 % w/w$$
$$25 % w/w$$
Q41 One of the disadvantages of acid-base titration is?
Large quantity of the sample(s) is required
Takes longer time for reaction to start
The acid need to be handled with care
Requires careful attention to reach end point accurately
Q42 All are advantages of acid base titration except?
Simple to do
Less accuracy and precision
Cost effective
Do not need high expertise
Q43 The equation NaOH + HCl $$�??$$NaCl + H2O is a ____?
Acid base reaction
Oxidation reaction
Neutralization reaction
Reduction reaction
Q44 When performing acid-base titration, one should first?
Rinse the burette twice with acid solution
Fill the burette twice with acid solution
Fill the burette twice with base solution
Rinse the burette twice with base solution
Q45 Which of these is a method of finding the equivalence point?
PH indicator
Amperometry
Thermometric titrametry
All of the above
Q46 What is a titrant in titration analysis?
Unknown concentration and volume of an analyte
Known concentration and volume of an analyte
Partially unknown concentration and volume of acid
Partially known concentration and volume of an analyte
Q47 What is a titrand in titration analysis?
Known concentration of an analyte
Partially known concentration of an analyte
Partially unknown concentration of acid
Unknown concentration of an analyte
Q48 During acid-base titration sulphuric acid would be dissociated into what ions?
$$H{^+} + SO{_4}$$
$$H{^-} + SO{_4}{^-}$$
$$2H{^+} + SO{_4}{^-}$$
$$H{_2} + SO{_4}$$
Q49 Both molarity and normality are measures of concentration. True or false?
True
Partially true
false
Indifferent
Q50 Choose the most suitable water for use in acid base titration?
Distilled water
Deionised water
Temporary hard water
Permanent hard water
Q51 A student used a hard tap water and performed and acid base titration. In few lines explain what would happen to his result?
The starting solution would be more acidic as such it would consume more base to achieve the equivalence point
the student cannot get an equivalence point owing to the fact that tap water was used not distilled water
The solution would require more of indicator at the beginning of the experiment
the starting solution would be more alkaline therefore it would require more volume of acid than expected
Q52 A 25 ml solution of 0.5 M NaOH is titrated until neutralized into a 50 ml sample of HCl?
50 mol
0.125 mol
0.25 mol
0.5 mol
Q53 What is the importance of back titration?
To determine the concentration of a substance that is in excess after a chemical reaction.
To determine the base in excess.
To determine the acid in excess.
To determine the average value of acid base titration.
Q54 What is the implication of adding a phenolphthalein as an indicator during the titration of HCl against Na2CO3?
The end point will appear when only half of Na2CO3 has been used
The end point will appear at the first drop of the acid.
The end point will appear when half of the HCl has been used.
The indicator will be sensitive to the acid alone
Q55 Which of these indicators will be suitable for use in titration involving a weak acid and a strong base?
Any indicator
Phenolphthalein
Methyl orange
No suitable indicator
Q56 What type of indicator will be suitable for use in a titration involving H2SO4 + NH3(ag)?
Phenolphthalein
Methyl orange
Any indicator
No suitable indicator
Q57 An example of a strong acid is?
$$H{_2}SO{_3}$$
$$CH{_3}COOH$$
$$H{_2}C{_2}O{_4}$$
$$H{_2}SO{_4}$$
Q58 What is a strong acid?
Any acid that ionizes completely in solution
Any acid which turns blue litmus paper red
Any acid that is highly corrosive and can cause burn to the skin
Any acid whose pH is less than 3
Q59 An indicator X was added to an acid solution in a beaker but no colour change was observed give the name of the indicator X?
Methyl orange
Bromothymol
Phenolphthalein
Litmus paper
Q60 What is the colour of bromothymol when added to an acid solution?
Blue
Red
Yellow
Colourless
Q61 The unit µg is equivalent to?
$$10{^-3}$$ Kg
$$10{^-6}$$ Kg
$$10{^-12}$$ Kg
$$10{^-9}$$ Kg
Q62 When filtration is carried out under reduced pressure is called?
Pressure filtration
Simple filtration
Ordinary filtration
Suction filtration
Q63 The unit of a volume express in $$dm{^3}$$ is equivalent to?
1 litre or 100 ml
$$10{^3}$$ cm or 1 litre
100 $$cm{^3}$$ or 1 litre
1000 ml or 10 litre
Q64 Define precipitation in respect to wet chemical analysis?
A method of converting ions in solution into an insoluble compound
The process of separating solid (crystals or precipitate) from the liquid (mother liquor)
A method of reducing the volume of by heating
A method of converting water vapour in to liquid water
Q65 What is a mole?
The amount of substance which contains as many element as there are atoms in 12 g carbon 12
The amount of substance which is contain in a solution
The amount of substance equivalent to carbon 12 atom present in a solution
All the options are correct
Q66 Why do we heat precipitates during gravimetric analysis?
To obtain a compound of constant composition
To increase the solubility of the precipitates
To dry the precipitates
To speed the reaction rate of the precipitates
Q67 The Avogadro number $$6.02 X 10{^23}$$ is equivalent to?
Number of atoms, ions or molecules in a mole
Number of mole of an atom equivalent to carbon atom
Number of elementary units in a mole of a substance
All options above are correct
Q68 Choose from the list of chemicals given and determine which has negative effect on skin?
Tetraoxosulphate(VI)and hydrogensulphide
Esters and ethanols
Benzene and benzoylchloride
Phenols and hydrogenfloride
Q69 Calculate the molar mass of 1 mole of a pure substance weighting X g?
M=2X g $$mol{^-1}$$
M=1/X g $$mol{^-1}$$
M=X g $$mol{^-1}$$
M=1 g $$mol{^-1}$$
Q70 Which of these hazardous chemicals are likely to cause dizziness and are carcinogenic?
Ethanol
benzene
Silvernitrate
Phenol
Q71 Calculate the mass of 0.5 moles of water?
9.408 g
18.016 g
18.071 g
4.504 g
Q72 The hazardous effect of chlorinated alkanes is?
Highly oxidizing
irritant
Skin burns
Causes mental confusion
Q73 Calculate the number of moles in 24 g of oxygen gas?
281 mol
265 mol
7.8 mol
3.8 mol
Q74 All are laboratory safety tips except?
Wearing lab coat or apron
Close all windows and doors
Never work alone in the laboratory
Be familiar with the position of some safety equipment
Q75 Calculate the molar mass of a pure substance if 2 moles of the substance has a mass of 35 g?
17.5 $$g mol{^-1}$$
70 g $$mol{^-1}$$
35 g $$mol{^-1}$$
37 g $$mol{^-1}$$
Q76 Qualitative analysis helps in determining what in a given solution?
How long it will take for reactant to react to form products
How much of a component is present in that solution
The quantity of the solvent required to form solution with the component
What type of component is present in that solution
Q77 Define molality of a solution?
Weight in grams of a substance per formula weight in kilograms of that substance
The number of moles of solute per $$dm{^3}$$ of a solution
The number of moles of solute in one kilogram of solution
Moles of solute per volume of solution express in litre
Q78 Quantitative methods help in determining what in a solution?
How much of a component is present in the solution
What type of component is present in a solution
The quantity of a solvent required to form a solution with the component
How long will take for reactant to react in order to form products
Q79 Normality can be defined as?
Moles of solute in 1 $$dm{^3}$$ of solution
Weight in gram of a substance per formula weight in kilo gram of substance
Number of gram equivalent weight of a solute in one litre of solution
All the options are correct
Q80 The various method of quantitative analysis include?
Acid �??base titration and Oxidative analysis
Gravimetric, spectrophotometric and volumetric methods
Titration, Gravimetric, and Volumetric
Spectrophotometric, Oxidative and Neutralization methods
YOU CAN NOW GET YOUR EXAM SUMMARY FOR ALL YOU E-EXAMS FROM US.
What is exam summary? Click here to learn more.
FOR YOUR LATEST CHM191 TMA SOLUTIONS as well as PAST QUESTIONS AND ANSWERS FOR EXAMS CONTACT 08039407882 on whatsapp.